SCIENCE - Carl Schurz High School

The best team you never saw compete.

FLASHCARD PRINTOUTS SCIENCE

Question Answer

1. What was the overarching question that characterized the explorations of early philosophers and chemists?

ʺHow does nature work?ʺ (USRG:6,1,3)

2. What was an early inhibitor to the growth of scientific knowledge?

limited means of communication (USRG:6,2,0)

3. In what year did the most recent ʺspurtʺ of growth in the field of chemistry begin?

1600 A.D. (USRG:6,2,1)

4. What example does USAD give of a Neolithic exploration into chemistry?

cooking (USRG:6,1,1)

5. In the Neolithic era, for what purpose was gold used? ornamentation (USRG:6,2,2)

6. What was likely the first known metal? gold (USRG:6,2,2)

7. What was the second metal to be discovered and used by ancient humans?

copper (USRG:6,2,2)

8. What was the earliest ore smelted? copper (USRG:6,2,2)

9. What are the two primary components of bronze? tin and copper (USRG:6,2,2)

10. According to USAD, what were the earliest metals used for weapon making?

tin and bronze (USRG:6,2,2)

11. What three metals did ancient humans use in ways similar to those in which they used tin and bronze?

silver, antimony, and lead (USRG:6,2,2)

12. How does brass differ from bronze? Both are made of copper, but bronze contains tin while brass has zinc. (USRG:6,2,2)

13. What is the major metallic component of the alloy steel?

iron (USRG:7,1,2)

14. From what source did the first iron that was found and used by humans probably originate?

meteorites (USRG:7,1,2)

15. For approximately how long have humans been creating glass?

thousands of years (USRG:7,2,2)

16. What sort of containers were used to store oils in ancient times?

ceramic containers (USRG:7,2,2)

17. Approximately what percentage of bronze is composed of copper?

90% (USIRG:3,1,1)

18. What three properties of copper ore make it conducive to metal working?

It melts easily, can be poured into a cast, and creates a hard, very useful substance good for tools and weapons.

(USIRG:3,1,1)

19. What metals composed the earliest bronze alloys prior to the use of tin?

copper and arsenic or antimony (USIRG:3,1,1)

20. In open casting, which tool is used to create the final shape of the piece?

a hammer (USIRG:3,1,3)

SCIENCE FLASHCARDS DEMIDEC RESOURCES ©2009

I A Brief History of Chemistry

21. What casting method was improved by the use of a mold made of two pieces that could be opened to remove the cast object?

open casting (USIRG:3,1,3)

22. What casting method was invented approximately one thousand years after the open casting method?

the ʺlost‐waxʺ method (USIRG:3,1,4)

23. How would ancient sculptors save expensive ores when producing large objects using the lost‐wax method?

They would make their mold with a ceramic ʺcore,ʺ so that only a thin layer of metal would define the object, not a solid

block of metal. (USIRG:3,2,1)

24. What ancient civilization produced the highest quality bronze work?

the Chinese (USIRG:4,1,2)

25. What characterized the bronze work of the Benin? highly accurate lost‐wax models (USIRG:4,2,1)

26. According to USAD, what is notable about the cave paintings from the Pyrenees in the south of France?

their brilliant red and black pigments (USIRG:4,1,3)

27. What color dye do woad seeds produce? vibrant blue (USIRG:4,1,3)

28. In the Egyptian mummification process, for what were mercury oxides used?

to create yellow or red dyes that acted as preservatives and antibacterial agents on the cloth and skin (USIRG:4,1,4)

29. What is another name for Tyrian purple? royal purple (USIRG:4,2,2)

30. What creature is the source of royal purple dye? sea snails on the coast of the Mediterranean (USIRG:4,2,2)

31. What compound has been shown to be closely related to the pigment in Tyrian purple dye?

indigo (USIRG4,2,2)

32. Who were the first people to use royal purple textiles? Minoans on Crete (USIRG:4,2,2)

33. Who was the first person to use the term ʺchemistryʺ? Diocletian in a 296 A.D. edict (USIRG:5,1,1)

34. Which regions were famous for their early alchemic research?

Rome, Egypt, and the Arab world (USIRG:5,1,1)

35. What power did the ʺphilosopherʹs stoneʺ supposedly possess?

the ability to change arsenic and copper into silver or lead and mercury into gold (USIRG:5,2,0)

36. What occurrence led alchemists to believe that they could convert base metals to gold or silver?

Lead and mercury turn yellow, like gold, when heated, and heating copper with arsenic causes them to react to form a

white substance imitating silver. (USIRG:5,1,2)

37. What important philosophical contribution did Roger Bacon make to chemistry?

He defined the difference between alchemy, which is philosophical in nature, and chemistry, which is scientific in

nature. (USIRG:5,2,1)

38. What substance results when potassium nitrate is mixed with charcoal and sulfur?

gunpowder (USIRG:5,1,3)

39. What Misc invented gunpowder? the Chinese (USIRG:5,1,3)

40. For what purpose was early gunpowder used? to fuel rockets and bombs that could be launched by catapults (USIRG:5,1,3)

41. During which century did the use of gunpowder in warfare become widespread?

the 15th century (USIRG:5,2,2)

42. How did Plato picture elements? as specific three‐dimensional geometric shapes (USIRG:5,2,3)

43. What were Aristotleʹs four primary properties? hot, cold, wet, and dry (USIRG:6,2,1)



44. What were Aristotleʹs five elements? earth, air, fire, water and his fifth element, called ether, which was immaterial and accounted for the transmission of energy

(USIRG:6,2,1)

45. How did Aristotleʹs properties relate to his elements? The four properties combined to form the four material elements. (USIRG:6,2,1)

46. Who elaborated on Aristotleʹs views of properties and elements?

Democritus (USIRG:6,2,2)

47. How did Democritusʹ views on matter differ from earlier views?

He believed matter was made of discrete particles as opposed to being continuous. (USIRG:6,2,2)

48. According to USAD, which state of matter is the easiest to understand but the hardest to capture and quantify?

gas (USRG:8,1,2)

49. What defined the transition from early chemistry to modern chemistry?

the development of extremely precise instruments that can measure all matter (USRG:8,1,2)

50. Who was the first person to use the term gas? Johann Baptista van Helmont (USRG:8,1,2)

51. What were Johann Baptista van Helmontʹs views on Misc?

He disagreed with it and refuted alchemical element transmutation (the changing of base materials into gold or

silver). (USRG:8,1,2)

52. Which law did Johann Baptista van Helmont develop and probably discover?

the law of conservation of mass (USRG:8,1,2)

53. What did Robert Boyle, Joseph Black, Henry Cavendish, Joseph Priestly, and Antoine Lavoisier have in common?

They all followed and supported the work of Johann Baptista van Helmont. (USRG:8,1,2)

54. What aspect of trees especially interested non‐medical chemists from the 17th to the 19th century?

how a tree gains mass as it grows (USRG:8,1,3)

55. What did Johann Baptista van Helmont conclude from the living tree experiment?

Trees grow solely due to their water intake. (USIRG:7,1,0)

56. What was Johann Baptista van Helmontʹs experimental design for the living tree experiment?

Johann Baptista n Helmont placed a weighed sapling in a known weight of soil. After an amount of time, he weighed

the tree and soil and compared them to their original weights. (USIRG:7,1,0)

57. What did Johann Baptista van Helmont notice about the weight of the soil in his living tree experiment?

The weight of the soil decreased by only a few ounces after five years. (USIRG:7,1,0)

58. True/False: The living tree experimentʹs conclusion is consistent with modern scientific knowledge.

False; Johann Baptista van Helmont did not know that photosynthesis involves atmospheric carbon dioxide, not

solely water. (USIRG:7,2,1)

59. Why do scientists celebrate the living tree experiment today?

It is one of the first well‐documented controlled experiments involving intense and careful scientific observations.

(USIRG:7,2,1)

60. What did Johann Baptista van Helmont do with fallen leaves in the living tree experiment?

He discarded them and did not weigh them in his final measurements. (USIRG:7,0,1)

61. Who discovered that air is made of mostly oxygen and nitrogen?

Antoine Lavoisier (USRG:8,2,2)

62. Which of Antoine Lavoisierʹs discoveries cast doubts upon the results of the living tree experiment?

the discovery that water cannot be converted into Earth (USRG:8,2,2)



63. Which side did the majority of chemists support in the French Revolution?

the new revolutionary government (USRG:9,1,1)

64. What political group particularly opposed scientists during the French Revolution?

Jacobins (USRG:9,1,1)

65. What field of science was safe from the Jacobinsʹ criticism during the French Revolution?

biology (USRG:9,1,1)

66. What did the Jacobins do to French science August 1793?

They abolished the Academy of Science through the National Convention. (USRG:9,1,1)

67. Who is considered the father of modern chemistry? Antoine Lavoisier (USIRG:7,1,1)

68. How did Antoine Lavoisier die? He was guillotined on May 8, 1794. (USIRG:7,1,1)

69. True/False: Lavoisier believed science should serve both the rich and the poor.

True; this caused him trouble, as he was caught between the aristocracy and the revolutionaries. (USIRG:7,1,2)

70. How was Antoine Lavoisier employed after 1764? as an investor, tax collector, accountant, and chemical analyst for Ferme Generale, director of the Academie de Science,

geologist, etc. (USIRG:7,1,3)

71. What were the ʺphysiocratsʺ? a group that aimed to handle finances in a way that would more fairly reward all members of the country (USIRG:7,2,2)

72. What did Lavoisier design to help the Ferme Generaleʹs customs collections?

a wall around Paris (USIRG:7,2,3)

73. What group abolished the Ferme Generale in 1791? The National Assembly (USIRG:7,2,4)

74. How did Lavoisier use his position as head of the Gunpowder and Saltpeter Commission to help the revolutionaries?

He gave gunpowder to the rebels and oversaw the demolition of the Bastille. (USIRG:8,2,0)

75. How did Antoine Lavoisier try to take part in the revolutionary government?

He tried to join the National Assembly. (USIRG:8,2,1)

76. What was the revolutionary governmentʹs response to the Ferme Generale?

It arrested and guillotined former employees of the Ferme Generale. (USIRG:8,2,2)

77. What was Madame Lavoisierʹs maiden name? Marie Anne Pierrette Paulz (USIRG:8,2,4)

78. How did Madame Lavoisier use her artistic talents to help her husband?

She took detailed notes, made sketches, and etched plates for her husbandʹs work. (USIRG:9,1,0)

79. True/False: Madame Lavoisier was put in prison because of the revolutionary governmentʹs suspicions regarding her husband.

True; she spent 65 days in prison until the government changed and she was released. (USIRG:9,1,1)

80. How did DuPont de Nemour know Madame Lavoisier?

He associated with her husband because of their shared interest in chemistry, and was later her suitor. (USIRG:9,1,2)

81. Who was Madame Lavoisierʹs second husband? Benjamin Thompson (USIRG:9,2,1)

82. Who discovered in 1896 that uranium is radioactive? Henri Becquerel (USRG:9,1,4)

83. Which two people first explained radioactive decay? Pierre and Marie Curie (USRG:9,2,1)

84. How did J.J. Thompson contribute to the field of chemistry?

He discovered the electron. (USRG:9,2,1)

85. Who discovered the atomic nucleus? Ernest Rutherford (USRG:9,2,1)



86. What did James Chadwick discover? the neutron (USRG:9,2,1)

87. What concept did Niels Bohr discover about atomic structure?

electron energy levels (USRG:9,2,1)

88. Who discovered that one element can have several different atomic weights?

Frederick Soddy (USRG:9,2,1)

89. Who found that photons can knock electrons off of the surface of a metal object?

Albert Einstein (USRG:9,2,2)

90. What equation unifies mass and energy? E=mc2 (USRG:9,2,2)

91. Who discovered that wave equations describe particles, and energy comes in discrete quanta?

Louis de Broglie and Erwin Shroedinger (USRG:9,2,2)

92. How did Henri Becquerel discover radiation? Becquerel placed uranium near undeveloped photographic plates and then developed the plates, exposing lines from the

radiation. (USIRG:9,1,3)

93. What two elements did Pierre and Marie Curie discover?

polonium and radium (USIRG:9,1,4)

94. What type of foil did Lord Rutherford use in his famous 1920 experiment?

gold foil (USIRG:9,1,5)

95. What gas did Lord Rutherford use in his 1920 experiment?

helium gas (USIRG:9,1,5)

96. How did Lord Rutherford picture the atom? as a heavy, positive nucleus with enough orbiting electrons to be neutral (USIRG:9,1,5)

97. Who originally performed the experiment that James Chadwick repeated to discover the neutron?

Marie Curieʹ daughter, Irene Joliot‐Curie and her husband, Frederic Joliot‐Curie (USIRG:9,2,2)

98. What type of foil did James Chadwick use in his experiment to discover the neutron?

beryllium foil (USIRG:9,2,2)

99. What false conclusion did Irene and Frederic Joliot‐Curie reach from their experiment regarding neutrons?

They thought they had observed gamma radiation when in fact they had seen the effects of neutrons. (USIRG:9,2,2)

100. What item visually organizes information about the elements?

the periodic table (USRG:10,1,2)

101. What is an intramolecular force? a force between atoms within a molecule (USRG:10,1,2)

102. What is an intermolecular force? a force between the molecules of a compound (USRG:10,1,2)

103. What type of force governs boiling and melting points for various chemical compounds?

intermolecular forces (USRG:10,1,2)

104. Who postulated that atoms bond together due to electrostatic forces?

Gilbert N. Lewis and Linus Pauling (USRG:10,1,3)

105. What is an electric dipole? the phenomenon that occurs when a positive and a negative charge are located a small distance apart on the same

molecule (USRG:10,1,3)

106. How do dipoles help engender intermolecular forces? Permanent or temporary dipoles attract opposite charges on other molecules. (USRG:10,1,3)

107. True/False: Dipoles only form between atoms that are entirely negative or positive.

False; dipoles can result in an overall neutral molecule as long as the charges are located on opposite sides of the molecule.

(USRG:10,1,3)



108. Who created the original periodic table? Dmitri Mendeleev (USIRG:10,1,1)

109. In what year was the periodic table first published? 1869 (USIRG:10,1,1)

110. How was each row of the earliest periodic table organized?

by increasing atomic weight (USIRG:10,1,1)

111. How is each row of the modern periodic table organized?

by increasing atomic number (USIRG:10,1,1)

112. True/False: Elements in the same column of the modern periodic table have very similar properties.

True; this is because they have the same number of valence electrons. (USIRG:10,1,1)

113. How did Mendeleev deal with elements that seemed out of place in the periodic table?

He assumed their properties were accurately measured, but their atomic weights were not. (USIRG:10,1,2)

114. What prefix did Mendeleev give to not yet discovered elements?

eka (USIRG:10,2,0)

115. What are the three pairs of ʺproblemʺ elements that were more difficult to fit into the periodic table?

Ar and K, Co and Ni, and Te and I (USIRG:10,2,1)

116. Why are the three pairs of ʺproblemʺ elements problematic?

their placement by atomic weight does not match their placement by properties (USIRG:10,2,1)

117. Who solved confusion regarding the three pairs of ʺproblemʺ elements?

Henry Moseley (USIRG:10,2,1)

118. Whose laboratory did Henry Moseley use for his 1914 experiment?

that of Rutherford (USIRG:10,2,1)

119. What was Moseleyʹs solution to the three pairs of problem elements?

He used atomic number instead of atomic mass in the table. (USIRG:10,2,1)

120. Why were the three problem pairs of elements misplaced in Moseleyʹs model?

The ratios of their isotopes in nature made them appear heavier or lighter than their adjacent elements. (USIRG:10,2,1)

121. What is periodic about the periodic table? as atomic number increases, atomic properties regularly repeat (USIRG:10,1,1)

122. What was Count Rumfordʹs real name? Benjamin Thompson (USRG:10,2,1)

123. What objects did Benjamin Thompson use to measure the heat of friction?

iron cannons (USRG:10,2,1)

124. Who discovered the exact relationship between heat and work?

James Joule (USRG:10,2,1)

125. With what mathematical subject was Josiah Gibbs concerned?

probability (USRG:10,2,1)

126. According to Gibbsʹ findings, what knowledge is necessary to determine the probability a reaction will occur?

specific measurable properties of the reactants and products (USRG:10,2,1)

127. With what subject is the field of chemical kinetics concerned?

the rate at which reactions occur (USRG:10,2,2)

128. What has happened to the field of chemical kinetics in the past century?

It has experienced immense growth. (USRG:10,2,2)

129. On what field does chemical kinetics rely in order to develop its models?

mathematics (USRG:10,2,2)



130. What establishes the maximum speed that a reaction can maintain?

the height of the energy barrier that all of its reactants must overcome (USRG:10,2,2)

131. What is responsible for the great diversity of elements? varying arrangements of a few elementary particles (USRG:11,1,1)

132. What is the smallest distinctive particle of matter? the atom (USRG:11,2,1)

133. What determines the properties and behaviors of an atom?

its internal structure (USRG:11,2,1)

134. What term is used for an atom that lost or gained electrons?

an ion (USRG:11,2,1)

135. Approximately how many elements have been discovered?

just over one hundred (USRG:11,2,1)

136. What occurs when an atom gains an electron? It becomes negatively charged. (USRG:11,2,1)

137. How did early chemists calculate the mass of one atom?

by measuring many atoms simultaneously, measuring their mass ratios in various compounds, and using these quantities

to develop a standard mass (USRG:11,2,2)

138. What is the mass ratio of hydrogen to fluorine in the compound HF?

1:19 (USRG:11,2,2)

139. What instrument can determine the relative masses of single atoms with some accuracy?

a mass spectrometer (USRG:11,2,3)

140. True/False: Scientists can use mass spectrometers to measure the masses of atoms in compounds.

True; mass spectrometers can measure both compounds and pure elements. (USRG:11,2,3)

141. For what purpose are mass spectrometers used in airports?

to determine if a substance contains explosive compounds (USRG:11,2,3)

142. What object separates ion beams by weight in a mass spectrometer?

a magnet (USRG:11,2,3)

143. True/False: In a mass spectrometer, a heavier element is bent more than a lighter element.

False; the magnet pulls them both equally, but a heavier element will have more inertia and be less affected.

(USRG:11,2,3)

144. What are the three basic components of a mass spectrometer?

an ion source, a mass analyzer, and a detector that measures the amount of each type of particle (USIRG:11,1,1)

145. How do the mass spectrometers used in airports differ from regular mass spectrometers?

In airport varieties, the pathway of the particles is straight and the magnet moves; in regular mass spectrometers, the

particles are bent by a stationary magnet. (USIRG:11,1,2)

146. What is the only state of matter mass spectrometers can measure?

gasses (USIRG:11,1,2)

147. What particles are found in an atomʹs nucleus? protons and neutrons (USRG:12,2,1)

148. What is the symbol for the negatively charged particle outside of the nucleus of an atom?

e‐ (USRG:12,2,1)

149. What is the symbol for a proton? p+ (USRG:12,2,1)

150. What is the minimum number of protons in an atom? one (USRG:12,2,1)

151. What is the symbol for a neutron? n° (USRG:12,2,1)


II The Structure of Matter

152. What is the minimum number of neutrons an atom can have?

0 (USRG:12,2,1)

153. In an elementʹs isotope notation, what does the number on the upper left of the symbol indicate?

the mass number (USRG:12,2,2)

154. How does one calculate the mass number of an isotope?

by adding its number of neutrons to its number of protons (USRG:12,2,2)

155. What is a nuclide? any arrangement of protons and neutrons which forms a nucleus (USRG:12,2,2)

156. Which carbon isotope is radioactive? carbon‐14 (USRG:12,2,2)

157. How does one calculate the number of neutrons in an atom given the mass number and the atomic number of that element?

by subtracting the atomic number from the mass number (USRG:12,2,2)

158. How many neutrons does carbon‐12 have? 6 (USRG:12,2,2)

159. How many isotopes of carbon are there? 3 (USRG:12,2,2)

160. What are the three most common carbon isotopes? carbon‐12, carbon‐13, and carbon‐14 (USRG:12,2,2)

161. What was the original standard for all atomic masses? hydrogen, which was given a mass of exactly 1 amu (USRG:12,2,3)

162. What is the modern standard for all atomic masses? the carbon atom, which was given a mass of 12 amu (USRG:12,2,3)

163. Why was the standard for atomic masses changed? as a solid, carbon is easier to use and measure than hydrogen (USRG:12,2,3)

164. What is the mass ratio of one hydrogen atom to one carbon atom?

1:12 (USRG:12,2,3)

165. What is the mass ratio of one helium atom to one carbon atom?

1:3 (USRG:12,2,3)

166. What is the weight of one helium atom in amus? 4 amus (USRG:12,2,3)

167. True/False: Changing the standard for atomic masses from hydrogen to carbon‐12 effected drastic changes.

False: there was only a minimal shift in masses. (USRG:12,2,3)

168. Why do isotopes of the same element have identical properties?

The properties of an element are determined by its number of protons, not by its number of neutrons. (USIRG:12,1,1)

169. What is deuterium? an isotope of hydrogen (USIRG:12,1,2)

170. What is the ratio of hydrogen‐2 to hydrogen‐1 in nature?

1:6500 (USIRG:12,1,2)

171. What is a common use for deuterium? It is used to trace the path hydrogen takes in chemical reactions. (USIRG:12,1,2)

172. In what type of reactions is deuterium commonly used?

fusion reactions (USIRG:12,1,2)

173. What is tritium? an isotope of hydrogen (USIRG:12,1,2)

174. How is carbon‐14 made in nature? It is formed in the upper atmosphere when cosmic rays hit atmospheric nitrogen. (USIRG:12,1,3)

175. True/False: Carbon‐14 is permanently stable. False; it slowly decays. (USIRG:12,1,3)



176. How many years long is carbon‐14ʹs half‐life? approximately 5,730 (USIRG:12,2,1)

177. What element must an object contain in order to be carbon dated?

carbon (USIRG:12,2,1)

178. What is the most common use of carbon‐14? carbon‐dating (USIRG:12,2,1)

179. If an object has half of the carbon‐14 it would have in its natural state, how old is it?

approximately 5,730 years old (USIRG:12,2,1)

180. Why does the amount of carbon‐14 in an organismʹs tissues change once the organism dies?

The organism no longer maintains equilibrium with the environment, and the carbon‐14 slowly decays.

(USIRG:12,2,1)

181. What isotope of carbon did scientists use to discover the photosynthesis reactions?

carbon‐14 (USIRG:12,2,2)

182. True/False: Carbon‐14 and hydrogen‐2 both occur in nature.

True; carbon‐14 and hydrogen‐2 both occur naturally and are in all living things. (USIRG:12,2,2)

183. Where is cobalt‐60 created? in nuclear reactors (USIRG:12,2,2)

184. What element is used to make cobalt‐60? a different isotope of cobalt (USIRG:12,2,2)

185. Approximately how many years is cobalt‐60ʹs half‐life? 5.3 years (USIRG:12,2,2)

186. What is a common use of cobalt‐60 in hospitals? as an anti‐microbial to sanitize surgery equipment (USIRG:12,2,2)

187. What aspect of cobalt‐60 is useful to the canning industry?

It is an antibacterial agent and canneries use it to sterilize some shelved foods. (USIRG:12,2,2)

188. What is cobalt‐60ʹs primary use in the human body? It is used for treating cancer with ʺradiation,ʺ where it effectively kills cancer cells. (USIRG:12,2,2)

189. Why is cobalt‐60 better than x‐rays for inspecting steel? It penetrates steel better than x‐rays. (USIRG:12,2,2)

190. What is an industrial use for cobalt‐60? It can be used to inspect welding and steel structural integrity. (USIRG:12,2,2)

191. What happens when cobalt‐60 is placed near a camera? It causes marks to appear on the film when it is developed. (USIRG:12,2,2)

192. Which isotopes are included in the atomic mass listed on the periodic table for a given element?

all of the elementʹs isotopes (USRG:13,1,1)

193. What are the two chlorine isotopes? chlorine‐35 and chlorine‐37 (USRG:13,1,1)

194. What percentage of chlorine atoms are chlorine‐35? 75% (USRG:13,1,3)

195. What is the atomic mass of natural chlorine? 35.453 amu (USRG:13,1,3)

196. What is the formula used to calculate average atomic mass?

(proportiona)(massa )+

(proportionb)(massb) . (USRG:13,1,3)

197. Who first proposed a theory about the different energy levels which electrons occupy?

Niels Bohr (USRG:13,1,4)

198. In the Bohr Model, what degree of freedom of movement are electrons postulated to have?

They are not free and must occupy specific energy levels. (USRG:13,1,4)

199. According to the Bohr Model, how do electrons move to a higher energy level?

by absorbing a quantum of energy from a photon (USRG:13,1,4)



200. According to the Bohr Model, how do electrons release photons?

by moving to a lower energy level (USRG:13,1,4)

201. What is the term for a discrete quantum of electromagnetic radiation?

a photon (USRG:13,1,4)

202. How large is a quantum of energy? It is the smallest possible unit of energy. (USRG:13,1,4)

203. What property of an atom is determined by the energy levels of the photons it emits when returning to a lower energy level?

its absorption or emission spectrum (USRG:13,1,4)

204. How do scientists determine the differences in energy between two energy levels?

by measuring the exact energies of photons emitted when an electron moves from one energy level to the other

(USRG:13,1,5)

205. Which famous scientist stated that electrons circle the nucleus of an atom in fixed orbits?

Niels Bohr (USRG:13,1,5)

206. What is the premise of Bohr Model of the atom? Electrons occupy fixed and unchanging orbits around the nucleus. (USRG:13,1,5)

207. What atomic model describes the atom as being analogous to a central sun being orbited by planets in strict patterns?

the Bohr Model of the atom (USRG:13,1,5)

208. According to the Bohr Model, how many electrons can occupy the same orbit at the same time?

2 (USRG:13,1,5)

209. True/False: According to the Bohr Model, two electrons following the same orbit necessarily exhibit the same behavior.

False; just because electrons are in the same path does not mean that they will have the same properties. (USRG:13,1,5)

210. In what direction do electrons move when they are in an unexcited state?

closer to the nucleus (USRG:13,1,5)

211. According to the Bohr Model, if an electron moved from an outer orbit to an inner orbit, what would happen?

light would be released (USRG:13,1,5)

212. According to the Bohr Model, in what direction would an electron move if it absorbed light?

outward, away from the nucleus (USRG:13,1,5)

213. What discovery led to the Quantum Mechanical Model of the atom?

Particles also exhibit wave properties. (USRG:13,1,5)

214. When an electron moves to an orbit closer to the nucleus of an atom, at what energy level will light be emitted?

one corresponding with the potential energy difference of an atom (USRG:13,1,5)

215. Where are electrons in the Quantum Mechanical Model?

somewhere outside of the nucleus‐they do not have specific or exact location (USRG:13,1,5)

216. In the Quantum Mechanical Model, what path do electrons take around the nucleus of an atom?

unpredictable oscillations rather than fixed orbits (USRG:13,1,5)

217. What model did the Quantum Mechanical Model replace?

the Bohr Model of the atom (USRG:13,1,5)

218. What phenomenon first indicated that wave‐like and particle‐like properties could simultaneously coexist?

light, which exhibits both wave and particle properties (USIRG:12,1,4)



219. What items are sometimes thought of as ʺwave packets?ʺ

particles (USIRG:13,1,0)

220. What types of matter can be represented by wave equations?

all matter (USIRG:13,1,0)

221. Before the discovery of the wave‐particle duality, what did scientists believe light to be?

waves (USIRG:13,1,0)

222. What property of light is demonstrated by the photoelectric effect?

its particle nature (USIRG:13,1,0)

223. Before the discovery of the wave‐particle duality, what did scientists believe electrons to be?

particles (USIRG:13,1,0)

224. What type of particles tends to most readily exhibit wave‐like properties?

lighter particles (USIRG:13,1,0)

225. How does the photoelectric effect demonstrate the particle nature of photons?

In the photoelectric effect, a photon transfers its energy to a particle. (USIRG:13,1,0)

226. How does the Davisson‐Germer experiment demonstrate the wave‐like nature of certain particles?

It demonstrated that, when directed at certain angles, the beam of scattered particles peaked in intensity in a manner

that suggested wavelike properties. (USIRG:13,1,0)

227. Of what aspect of photons do digital cameras take advantage?

their particle‐like properties (USIRG:13,1,0)

228. What type of crystal was used in the Davisson‐Germer experiment?

nickel crystal (USIRG:13,1,0)

229. What particle did the Davisson‐Germer observe? the electron (USIRG:13,1,0)

230. What is the term for the regions where electrons are likely to be found in the Quantum Mechanical Model?

orbitals (USRG:14,1,1)

231. According to the Quantum Mechanical Model, what does each electron generate?

an electron cloud (USRG:14,1,1)

232. What are the two simplest electron orbital shapes called?

s and p (USRG:14,1,1)

233. What determines the ability of two elements to bond? the number and shape of electron orbitals (USRG:14,1,2)

234. What pattern emerged when scientists organized elements by orbital structures?

one that matches the periodic table (USRG:14,1,2)

235. What patterns emerge when unstable elements are organized by orbital structures?

none (USRG:14,1,2)

236. What is notable about a chart of elements made based on orbital structures and one created based on physical and chemical properties?

both are atomic arrangements that match the periodic table created according to atomic number (USRG:14,1,2)

237. What is the name for a row in the periodic table? a period (USRG:14,1,3)

238. How many protons can be found in the element with the atomic number 12?

12 (USRG:14,1,3)

239. When do scientists begin a new row on the periodic table?

when atomic properties begin repeating (USRG:14,1,3)

240. What is the atomic number of the element that begins the second period on the periodic table?

3 (USRG:14,1,3)



241. How many electrons are in the first orbital? 2 (USRG:14,1,3)

242. How many orbitals surround atoms in the second period of the periodic table?

3 (USRG:14,1,3)

243. What is the maximum number of electrons that can surround an atom in the second period of the periodic table?

10 (USRG:14,1,3)

244. How many electrons total fit into the two additional orbitals that appear in the second period of the periodic table?

8 (USRG:14,1,3)

245. What is the atomic number of the element that begins the third period?

11 (USRG:14,1,3)

246. What happens to the number of columns in the periodic table as new elements are discovered?

more columns are added (USRG:14,1,3)

247. What happens to an atomʹs atomic radius as one moves from left to right on the periodic table?

it decreases (USRG:14,2,1)

248. What causes the change in the atomic radius from left to right across the periodic table?

An increase in the number of protons causes electrons to be more attracted to the nucleus and the radius of the atom to

decrease. (USRG:14,2,1)

249. What is the first element on the periodic table? hydrogen (USRG:14,2,1)

250. How many protons does nitrogen have? 7 (USRG:14,2,1)

251. What is a common measure of atomic size? atomic radius (USRG:14,2,1)

252. How does the addition of neutrons affect an atomʹs atomic radius?

It has no effect. (USRG:14,2,1)

253. What is ionization energy? the energy required to remove the most loosely held electron (USRG:14,2,2)

254. What happens to an atomʹs ionization energy from left to right across the periodic table?

It increases. (USRG:14,2,2)

255. What is the relationship between atomic radius and ionization energy?

The two are inversely related. (USRG:14,2,2)

256. What causes an atomʹs ionization energy to increase? the increased pull of additional protons, which makes it harder to remove an electron (USRG:14,2,2)

257. What is the second element on the periodic table? helium (USRG:14,2,2)

258. What is equal to the force of attraction between an electron its nucleus?

the ionization energy (USRG:14,2,2)

259. What is electron affinity? the amount of energy change that when an electron is added to a neutral atom (USRG:14,2,3)

260. What happens to electron affinity from left to right across the periodic table?


261. True/False: The left to right trend in the periodic table for electron affinity is always true.

False; there are notable exceptions to the rule due to irregularities in atomic structures. (USRG:14,2,3)

262. What element is a notable exception to the general periodic trend in electron affinity?

nitrogen (USRG:14,2,3)



263. How do scientists describe the addition of an electron to an atom at a substantially further distance from the nucleus?

ʺadding a new shellʺ (USRG:14,2,4)

264. What are two other names for a column in the periodic table?

a group or a family (USRG:14,2,4)

265. Why does the atomic radius change for atoms down the periodic table?

New shells are added, which are substantially further away from the nucleus than previous shells. (USRG:14,2,5)

266. What happens to atomic radii as one moves down the periodic table?

They increase. (USRG:14,2,5)

267. Why does ionization energy change down the periodic table?

the increased distance between the furthest electrons and the nucleus makes it easier to remove those electrons

(USRG:14,2,7)

268. What happens to ionization energy as one moves down the periodic table?

It decreases. (USRG:14,2,7)

269. What happens to electron affinity as one moves down a group on the periodic table?


270. Why does electron affinity change down the periodic table?

The increased distance between the furthest out electrons and the nucleus means that there is less residual attractive force

when there is an additional electron. (USRG:14,2,7)

271. What is electronegativity? the attraction between an atom and adjacent atomsʹ electrons (USRG:13,1,1)

272. Who devised a method for numerically measuring electronegativity?

Linus Pauling (USRG:13,1,1)

273. What is a numeric value for electronegativity called? Pauling electronegativity (USRG:13,1,1)

274. What atom has an electronegativity of 1.0? lithium (USRG:13,1,1)

275. What does a higher Pauling electronegativity indicate? increased attraction for neighboring electrons (USRG:13,1,2)

276. What is a common acronym for electronegativity? EN (USRG:13,1,3)

277. What happens when two atoms with widely different electronegativities bond?

The atom with the higher Pauling electronegativity value pulls electrons closer to it. (USRG:13,1,3)

278. From what type of differences in electronegativities do ionic bonds result?

large differences (USRG:13,1,3)

279. What type of bond occurs between sodium and fluorine?

ionic (USRG:13,1,3)

280. From what types of differences in electronegativites do polar covalent bonds result?

small or intermediate differences (USRG:13,1,3)

281. What type of bond occurs between nitrogen and oxygen?

a covalent bond with a small dipole moment (USRG:13,1,3)

282. From what type of difference in electronegativities do non‐polar covalent bonds result?

identical electronegativities (USRG:13,1,3)

283. What type of bonds form between hydrogen and hydrogen?

non‐polar covalent bonds (USRG:13,1,3)

284. What type of bonds form between F and F? non‐polar covalent bonds (USRG:13,1,3)



285. What are the five types of forces associated with atoms and molecules?

ionic bonds, covalent bonds, metallic bonds, van de Waals forces, and hydrogen bonds (USRG:15,1,4)

286. What is the source of the five types of forces associated with atoms and molecules?

the electrostatic force (USRG:15,1,4)

287. What term describes the force of attraction between positive and negative charges?

the electrostatic force (USRG:15,1,4)

288. What are the three types of intramolecular forces? ionic bonds, covalent bonds, and metallic bonds (USRG:15,2,1)

289. What is necessary to break most chemical bonds? immense amounts of energy (USRG:15,2,1)

290. Under what circumstances are most chemical bonds broken?

in chemical reactions (USRG:15,2,1)

291. When do ionic bonds form? when an electron is transferred from one atom to another (USRG:15,2,2)

292. In sodium chloride, what charge does each element take?

Na is positive and Cl is negative (USRG:15,2,2)

293. How do covalent bonds form? Two atoms share electrons which attract both nuclei. (USRG:15,2,3)

294. What happens to an electronʹs freedom of motion in a metallic bond?

It increases because electrons can easily be transferred from atom to atom. (USRG:15,2,4)

295. True/False: Metallic bonds usually form between different elements.

False; metallic bonds usually form between atoms of the same element. (USRG:15,2,4)

296. What term do scientists use for the motion of electrons in metallic bonds?

an electron sea (USRG:15,2,4)

297. Which of the three intramolecular forces fosters the greatest electrical conductivity?

metallic bonds (USRG:15,2,4)

298. What term do scientists use for a metal composed of two or more elements?

an alloy (USRG:15,2,4)

299. Which of the intramolecular forces does solid lithium exhibit?


300. Which of the intramolecular forces is present in Fe? metallic bonds (USRG:15,2,4)

301. Which of the intramolecular forces has the most energy?

ionic bonds (USRG:15,2,4)

302. Which of the intramolecular forces has the least energy?


303. True/False: Intermolecular forces are stronger than intramolecular forces.

False; intramolecular forces are much stronger than intermolecular forces. (USRG:15,2,6)

304. What two people independently described dispersion forces?

Fritz London and Johannes van der Waals (USRG:16,1,1)

305. What are two names for dispersion forces? van der Waals forces and London dispersion forces (USRG:16,1,1)

306. What are van der Waals forces? attraction between molecules resulting from either temporary or permanent dipoles (USRG:16,1,1)



307. Who was the first scientist to discover London dispersion forces?

Johannes van de Waals (USRG:16,1,1)

308. What happens when scientists place an atom with a dipole moment in an electric field?

a torque acts on the dipole (USRG:16,1,1)

309. What do scientists call a temporary polarity in a molecule?

an induced dipole (USRG:16,1,1)

310. What term do scientists use for molecules with a permanent distance between the centers of their positive and negative charges?

polar molecules (USRG:16,1,1)

311. What is the most common example of hydrogen bonding?

The temporary bonds that occur between molecules of H20. (USRG:16,1,2)

312. Between what atoms are the hydrogen bonds in water? between the hydrogen in one molecule and the oxygen in another (USRG:16,1,2)

313. What type of intermolecular forces must be broken to boil water?

hydrogen bonds (USRG:16,1,2)

314. Why does ice have a lower density than water? It has an open structure due to hydrogen bonding between atoms. (USRG:16,1,2)

315. What is a simple way to demonstrate that ice is less dense than water?

It floats on water. (USRG:16,1,2)

316. What type of bond causes water to coalesce into drops? hydrogen bonds (USRG:16,1,2)

317. What intermolecular force has the most energy? the ion‐dipole variety of van der Waals forces (USRG:16,1,chart)

318. What are the three elements with which hydrogen most commonly forms hydrogen bonds?

nitrogen, oxygen, and fluorine (USRG:16,1,chart)

319. What three elements that commonly form hydrogen bonds are present in DNA?

H, O, and N (USIRG:14,1,1)

320. What type of intermolecular force is crucial in the structure of DNA?

hydrogen bonding (USIRG:14,1,1)

321. What two scientists produced the x‐ray of DNA that James Watson and Francis Crick studied?

Rosalind Franklin and Maurice Watkins (USIRG:14,1,2)

322. Who first proposed the idea that DNA is shaped like a double helix?

James Watson and Francis Crick (USIRG:14,1,2)

323. What causes the double helix shape in DNA? hydrogen bonds (USIRG:14,1,2)

324. According to USAD, what is the most common example of an ionic lattice?

sodium chloride (USRG:16,2,2)

325. Why can ions form crystals? each atomʹs charge extends in every direction, creating a lattice (USRG:16,2,2)

326. How many covalent bonds can carbon form? 4 (USRG:16,2,3)

327. What is the smallest unit of methane? a single discrete molecule (USRG:16,2,3)

328. What element composes diamonds? carbon (USRG:16,2,3)



329. What kind of intrarmolecular force creates the structure of a diamond?

covalent bonds (USRG:16,2,3)

330. What is the smallest discrete unit of a diamond? a covalent network (USRG:16,2,3)

331. What are the structural characteristics of solids with metallic bonds?

They are dense and strong, but can be bent or hammered. (USRG:16,2,4)

332. How rigid are most solids held together with metallic bonds?

They are quite malleable, and layers can slide over each other. (USRG:16,2,4)

333. What type of motion do atoms exhibit within solids? translational motion (USRG:16,2,5)

334. What types of motion do atoms in solids not exhibit? vibrational motion and rotational motion (USRG:16,2,5)

335. Why must molecules absorb energy in order to change their states?

to overcome the intermolecular forces (USRG:16,2,5)

336. What state of matter exhibits the most motion? gases (USRG:16,2,5)

337. What is a direct measure of molecular motion? temperature (USRG:17,1,1)

338. What is an accurate predictor of the state a substance will take at room temperature?

the types of intermolecular forces present in that substance (USRG:17,1,1)

339. In what state are ionic substances likely to be at room temperature?

solid (USRG:17,1,2)

340. What is the chemical formula for quartz? SiO2 (USRG:17,1,2)

341. What is the chemical formula for diamond? C (USRG:17,1,2)

342. What is the chemical formula for methane? CH4 (USRG:17,1,2)

343. True/False: Liquids are common at room temperature. False; they are rare, because only a small range of intermediate magnitudes for intermolecular forces result in

liquids at room temperature. (USRG:17,1,2)

344. In what state of matter are compounds with only dispersion forces likely to be at room temperature?

gaseous (USRG:17,1,2)

345. What two types of bonds do water molecules exhibit? covalent bonds (intramolecular) and hydrogen bonds (intermolecular) (USRG:17,1,3)

346. What characterizes the charge on one element relative to the other element in a polar molecule?

equal in magnitude, but opposite in charge (USRG:17,1,5)

347. What type of van der Waals force does water exhibit? permanent van der Waals forces (USRG:17,1,5)

348. What type of bonds usually results in permanent van der Waals forces?

polar bonds (USRG:17,1,5)

349. Under what circumstances will scientists continue to use models they know to be incorrect?

when the models still make accurate predictions (USRG:17,2,1)

350. With which university is G. N. Lewis associated? the University of California (USRG:17,2,1)

351. What symbol represents an electron in Lewisʹ model? a dot (USRG:17,2,2)

352. What term do scientists use for the electrons in an atomʹs outermost shell?

valence electrons (USRG:17,2,2)

353. Why do Lewis structures usually depict only the outermost electrons of an atom?

An atomʹs outermost electrons are usually the only ones to take part in bonding. (USRG:17,2,2)



354. What is the simplest entity a Lewis structure can represent?

an atom (USRG:17,2,3)

355. True/False: Lewis structures can be used to draw ions. True; ions are drawn in a manner similar to atoms. (USRG:17,2,3)

356. Why are Lewis structures often used to draw atoms in compounds?

because Lewis structures are useful for modeling atoms and bonds (USRG:17,2,3)

357. True/False: Lewis structures can be used to draw atoms in fusion reactions.

False; they can only be used to show atoms and bonds (USRG:17,2,3)

358. What symbol represents a covalent bond in a Lewis diagram?

a pair of dots (USRG:17,2,3)

359. How often do Lewis structures show all the electrons in an atom?

rarely (USRG:17,2,3)

360. What is the term for a pair of valence electrons that is not involved in bonding?

a lone pair (USRG:17,2,4)

361. What is another name for a lone pair? non‐bonding electrons (USRG:17,2,4)

362. How many electrons are necessary for two atoms to form a neutral molecule?

an amount equivalent to the sum of the protons in the nuclei of the two atoms (USRG:17,2,4)

363. What happens to sodiumʹs valence electron when it bonds with chlorine?

It is transferred to chlorine, forming an ionic bond. (USRG:17,2,5)

364. What idea regarding electron bonding needed to be worked into the Lewis model shortly after its discovery?

electron orbitals (USRG:18,2,1)

365. According to the valence bond concept, what causes the force of attraction in covalence bonds?

an overlap between two atomsʹ electron orbitals (USRG:18,2,2)

366. What type of bond is formed when two atoms overlap in one orbital?

a single bond (USRG:18,2,2)

367. What is the maximum number of orbitals that can overlap between two atoms?

3 (USRG:18,2,3)

368. What type of covalent bond is present in carbon dioxide?

a double bond (USRG:18,2,3)

369. What type of covalent bond is present in nitrogen gas? a triple bond (USRG:18,2,3)

370. How are double bonds depicted in Lewis structures? as 2 parallel lines (USRG:18,2,3)

371. How are triple bonds depicted in a Lewis structure? as 3 parallel lines (USRG:18,2,3)

372. What observation led scientists to believe two orbitals could hybridize?

the observation that occasionally the interactions of two atomic orbitals did not correctly predict the shape of the

resulting molecule (USRG:18,2,3)

373. What effect is responsible for the symmetric shape of many molecules?

the hybridization of orbitals (USRG:18,2,3)

374. What happens to two orbitals when they hybridize? They combine to take on a different shape. (USRG:18,2,3)

375. How many sp3 orbitals can 1 s and 3 p orbitals hybridize to form?

4 (USRG:18,2,3)

376. What shape are sp3 orbitals? tetrahedral (USRG:18,2,3)



377. What abbreviation is commonly used for molecular orbitals?

MOs (USIRG:15,1,1)

378. What is the term for electron waves between atoms within a molecule?

molecular orbitals (USIRG:15,1,1)

379. What are molecular orbitals? the positions assumed by the electrons of bonded atoms (USIRG:15,1,1)

380. What are the two types of molecular orbitals? sigma bonds and pi bonds (USIRG:15,1,1)

381. What is a sigma bond? a molecular orbital that lies primarily upon an axis between the centers of two atoms (USIRG:15,1,1)

382. What is a pi bond? a molecular orbital that lies between two atoms, but away from the axis that runs between the two atomsʹ centers

(USIRG:15,1,1)

383. What type of molecular orbital develops from s atomic orbitals?

sigma bonds (USIRG:15,1,2)

384. What type of molecular orbital develops from p atomic orbitals?

pi bonds (USIRG:15,1,2)

385. What molecular orbital forms in F2? one sigma bond (USIRG:15,2,2)

386. How many valence electrons are there in F2? 14 (USIRG:15,2,2)

387. What molecular orbitals form in O2? one sigma bond and one pi bond (USIRG:15,2,2)

388. How many valence electrons are there in O2? 12 (USIRG:15,2,2)

389. How many valence electrons are there in N2? 10 (USIRG:15,2,2)

390. What molecular orbitals form in N2? one sigma bond and two pi bonds (USIRG:15,2,2)

391. What molecular orbitals form in CO2? one sigma bond and one pi bond with each oxygen (USIRG:16,1,1)

392. How many valence electrons are there in CO2? 16 (USIRG:16,1,1)

393. What is the maximum number of molecular orbitals that can exist between two atoms?

3 (USIRG:16,1,1)

394. How many dimensions do Lewis structures depict? 2 (USRG:18,2,5)

395. How many dimensions do VSEPR models depict? 3 (USRG:18,2,5)

396. What model is one of the most successful replacements of the Lewis model?

the VSEPR model (USRG:18,2,5)

397. What does the acronym VSEPR represent? Valence Shell Electron Pair Repulsion (USRG:18,2,5)

398. What conclusion did the VSEPR model reach regarding electron pairs?

Each pair mutually repels other pairs in all three dimensions. (USRG:18,2,5)

399. True/False: Resonance can occur between two atoms. False; it can only occur within molecules of three or more atoms. (USIRG:17,1,0)

400. What led to the discovery of resonance? the experimental observation that the length and strength of covalent bonds in an atom are equal even when there are not

enough electrons to form bonds to satisfy an atomʹs octet requirements (USIRG:17,1,0)

401. How many valence electrons does O3 have? 18 (USIRG:17,1,0)



402. According to the rules of Lewis structures, what type of covalent bonds should form in O3??

one single bond and one double bond (USIRG:17,1,0)

403. What does experimental evidence demonstrate about the different covalent bonds in O3?

They are equal in length and strength. (USIRG:17,1,0)

404. How do Lewis structures accommodate resonance? All possible bonding combinations are drawn with arrows between them. (USIRG:17,1,0)

405. How did scientists originally picture resonance? as the molecule rapidly alternating between all possible bonding patterns (USIRG:17,1,2)

406. Why did scientists use the name ʺresonanceʺ for the phenomena associated with equalizing covalent bonds in an atom?

because they believed that molecules resonated between all of the possible different forms (USIRG:17,1,2)

407. How do modern scientists picture resonance? as all bonds being of an equal intermediate length (USIRG:17,1,2)

408. What is the experimentally determined strength of each bond in O3?

1.5 (USIRG:17,1,2)

409. What is the experimentally determined strength of the bonds in SO3?

1.3333 (USIRG:17,2,1)

410. What do O3 and SO3 structurally have in common? They both exhibit resonance. (USIRG:17,2,1)

411. How do scientists describe an orbital that can bond more than two atoms together with a pair of electrons?

ʺdelocalizedʺ (USIRG:17,2,2)

412. What is an oxidation state? a numerical value that indicates whether an atom gained or lost electrons to form a bond (USRG:19,1,1)

413. What is the oxidation state of Li+? +1 (USRG:19,1,2)

414. What are the oxidation states of the hydrogen atoms in H2O?

+1 (USRG:19,1,2)

415. What is the oxidation state of the oxygen atom in H2O? ‐2 (USRG:19,1,2)

416. What is the total sum of the oxidation states in H2O? 0 (USRG:19,1,2)

417. What is the total sum of oxidation states in all neutral molecules?

0 (USRG:19,1,2)

418. What is the total sum of the oxidation states of the atoms in charged molecules?

The sum is equal to the charge of the molecule. (USRG:19,1,2)

419. What is the total sum of the oxidation states in NH4+? +1 (USRG:19,1,2)

420. What is the oxidation state of each hydrogen atom in NH4+?

+1 (USRG:19,1,2)

421. What is the oxidation state of the nitrogen atom in NH4+?

‐3 (USRG:19,1,2)

422. What shape is a methane molecule? a tetrahedron (USRG:19,1,3)

423. On what atom do VSEPR models focus when determining a moleculeʹs shape?

the central atom (USRG:19,1,3)

424. What is the most common shape of a molecule composed of a central atom with four outer atoms?

a tetrahedron (USRG:19,1,3)



425. What can scientists ascertain about the shape of a molecule with no dipole moment?

It is symmetrical. (USRG:19,1,4)

426. True/False: If the charge vectors in a molecule sum to zero, the molecule must have a significant dipole moment.

False; it must have no dipole moment. (USRG:19,1,4)

427. What can scientists ascertain about the shape of a molecule with a strong dipole moment?

It is asymmetrical. (USRG:19,1,4)

428. True/False: The C=O bonds in CO2 are polar. True; there is some charge separation. (USRG:19,2,1)

429. How much of a dipole moment does CO2 have in total? none (USRG:19,2,1)

430. What is notable about the shape of CO2? It is symmetrical. (USRG:19,2,1)

431. How polar is CO2? It is non polar. (USRG:19,2,1)

432. What shape is the CO2 molecule? linear (USRG:19,2,1)

433. On what atom would the VSEPR model focus to determine the shape of CO2?

carbon (USRG:19,2,1)

434. On what atom would the VSEPR model focus to determine the shape of NH3?

nitrogen (USRG:19,2,1)

435. How is the polarity of a molecule related to the intermolecular forces it exerts on other molecules?

more polar molecules exert stronger intermolecular forces (USRG:19,2,2)

436. Why do polar molecules have higher melting points than non‐polar molecules?

They have stronger intermolecular forces. (USRG:19,2,2)

437. What is alpha decay? the expulsion of a helium nucleus from an atom (USRG:20,1,2)

438. What is beta decay? a type of radioactive decay in which a neutron becomes a proton by emitting an electron, or a proton becomes a neutron

by emitting a positron (USRG:20,1,2)

439. What does the symbol N/Z represent in the atomic symbol for an element?

the neutron to proton ratio (USRG:20,1,2)

440. What determines if an atom will be radioactive? its ratio of neutrons to protons (USRG:20,1,2)

441. What term is used for electrons in beta decay reactions? beta minus particles (USRG:20,1,2)

442. What type of radioactive decay is positron decay? beta decay (USRG:20,1,2)

443. What is positron decay? a type of radioactive decay in which a proton transforms into a neutron, expelling a positron (USRG:20,1,2)

444. What term is used for a positron in beta decay? a beta plus particle (USRG:20,1,2)

445. What is a neutrino? a particle that shares energy with a positron (USRG:20,1,2)

446. How many neutrons are expelled from an atom during alpha decay?

2 (USIRG:17,1,2)

447. How many protons are expelled from an atom during alpha decay?

2 (USIRG:17,1,2)

448. What type of radioactive decay usually happens to extremely large atoms?

alpha decay (USIRG:17,1,2)

449. How many protons does bismuth have? 83 (USIRG:17,1,2)



450. What is the smallest element that commonly undergoes alpha decay?

bismuth (USIRG:17,1,2)

451. What is an anti‐neutrino? a particle that shares energy with an emitted electron (USIRG:17,2,3)

452. What kind of beta decay results in an anti‐neutrino? beta minus decay (USIRG:17,2,3)

453. What kind of beta decay results in a neutrino? beta plus decay (USIRG:17,2,3)

454. What kind of radioactive decay might result from too many neutrons in a small atom?

beta minus decay (USIRG:17,2,3)

455. What kind of radioactive decay does carbon‐14 experience?

beta minus decay (USIRG:17,2,3)

456. What element does carbon‐14 become after undergoing radioactive decay?

nitrogen‐14 (USIRG:17,2,3)

457. How does an elementʹs mass change in beta decay? It does not change. (USIRG:17,2,3)

458. How does an elementʹs mass change in alpha decay? It decreases by 4 amus. (USIRG:17,2,3)

459. What kind of radioactive decay might result from too many protons in a small atom?

beta plus decay (USIRG:17,2,3)

460. What kind of radioactive decay does carbon‐10 experience?

beta plus decay (USIRG:17,2,3)

461. What element does carbon‐10 become after it undergoes radioactive decay?

boron‐10 (USIRG:17,2,3)

462. What ratio of neutrons to protons within an atom is the most stable?

1:1 (USIRG:17,2,3)

463. True/False: In alpha decay, protons can change into neutrons.

False; this only occurs in beta decay. (USIRG:18,2,1)

464. What do nitrogen particles become when they collide with alpha particles?

oxygen atoms (USIRG:18,2,1)

465. Who was the first scientist to discover alpha bombardment reactions?

Ernest Rutherford (USIRG:18,2,1)

466. What types of particles are conserved in alpha bombardment reactions?

electrons, protons, and neutrons (USIRG:18,2,1)

467. How does the total mass of the reactants change in an alpha bombardment reaction?

It does not change, as mass is conserved. (USIRG:18,2,1)

468. What is the byproduct of nitrogen being bombarded with alpha particles?

hydrogen (USIRG:18,2,1)

469. What two particles react in a typical nuclear power plant?

uranium atoms and loose neutrons (USIRG:18,2,2)

470. What are the masses of the two products of uranium fission?

130 amus and 100 amus (USIRG:18,2,2)

471. What type of nuclear reaction is used to generate electricity?

fission (USIRG:19,1,1)



472. True/False: Scientists have never performed fusion reactions.

False; nuclear fusion reactions have been performed, just not on a scale large enough to generate electricity. (USIRG:19,1,1)

473. Why does nuclear fusion require a great deal of energy?

It must overcome the repulsion of the two positive nuclei. (USIRG:19,1,1)

474. What element results from the fusion of two hydrogen atoms?

helium (USIRG:19,1,1)

475. What elementary particle is released in hydrogen fusion?

1 neutron (USIRG:19,1,1)

476. What are the three main types of elementary particles? protons, neutrons, and electrons (USRG:20,2,1)

477. What distinguishes one atom from another? the number of protons in its nucleus (USRG:20,2,2)

478. What information is indicated by an elementʹs atomic symbol?

its number of protons, chemical symbol, and mass number (USRG:20,2,4)

479. What is the term given to a mixture that appears to be homogenous substance?

a solution (USRG:22,1,1)

480. True/False: Pure elements are commonly encountered in nature.

False; most substances encountered are mixtures. (USRG:22,1,1)

481. According to USAD, what do most people picture when they think of solutions?

solids or liquids dissolved in liquids (USRG:22,1,1)

482. What type of mixture is lemonade? a solution (USRG:22,1,1)

483. What term do scientists use for a homogenous combination of two or more metals?


484. What strong solid solution is often used in bicycles? steel (USRG:22,1,1)

485. What type of mixture is air? a gas in gas solution (USRG:22,1,1)

486. Which states of matter can be considered a collection of moving particles?

all states of matter (USRG:22,1,2)

487. Which model can explain the laws that govern the behavior of gases?

the Kinetic Molecular Theory (USRG:22,1,2)

488. What forms the basis the Kinetic Molecular Theory? the constant motion of gas particles and their intrinsic energy (USRG:22,1,2)

489. True/False: The Kinetic Molecular Theory preceded the laws that govern the behavior of gases.

False; the laws that govern gases were experimentally discovered prior to the Kinetic Molecular Theory.

(USRG:22,1,2)

490. At what temperature does all atomic motion cease? absolute zero (USRG:22,1,2)

491. In what era did scientists discover how to isolate gases from one another?

the Scientific Revolution (USRG:22,2,1)

492. During the Scientific Revolution, what observation did scientists make regarding the behavior of all gases?

It is highly regular. (USRG:22,2,1)

493. What are phase diagrams? diagrams that illustrate how all three states for a pure substance exist under different conditions (USRG:22,2,1)

494. What is the relationship between pressure and volume for gases in flexible containers?

inversely proportional (USRG:22,2,2)

495. What law linked the pressure of a gas to its volume? Boyleʹs Law (USRG:22,2,2)


III States of Matter

496. What is the standard abbreviation for pressure? P (USRG:22,2,2)

497. What is the standard abbreviation for volume? V (USRG:22,2,2)

498. What is the equation for Boyleʹs Law? PV=C (USRG:22,2,2)

499. In what units is the ʺCʺ in the equation for Boyleʹs Law usually measured?

liter‐atmospheres (USRG:22,2,2)

500. What is the most common unit used to measure pressure?

atmospheres (USRG:22,2,2)

501. What is the nature of the relationship between temperature and volume for a gas in a flexible container?

direct proportionality (USRG:22,2,3)

502. What law links temperature and volume for gases? Charlesʹs Law (USRG:22,2,3)

503. What is the equation for Charlesʹs law? V/T=D (USRG:22,2,3)

504. In what unit is the D in Charlesʹs law measured? liters/degree (USRG:22,2,3)

505. In a closed piston, what is the temperature in degrees Celsius that would theoretically result in no volume?

‐273°C (USRG:22,2,4)

506. When pressure is held constant, what happens to the volume of gas in a piston when its temperature decreases from 70°C to ‐100°C?

It decreases by approximately half. (USRG:22,2,4)

507. When pressure is held constant, what kind of relationship exists between volume and temperature in a closed piston?

a positive linear relationship (USRG:22,2,4)

508. What is absolute zero in degrees Celsius? ‐273°C (USRG:22,2,5)

509. What discovery sparked the invention of the Kelvin scale?

the discovery of absolute zero (USRG:22,2,5)

510. What temperature is absolute zero in Kelvin? 0 (USRG:22,2,5)

511. What equation is used to convert temperatures from Kelvin to degrees Celsius?

K‐273=°C (USRG:22,2,5)

512. What measure of temperature must be used in Charlesʹs law?

Kelvin (USRG:22,2,5)

513. What is the fundamental beginning for all temperature measurements?

absolute zero (USRG:22,2,5)

514. True/False: A temperature of ‐275°C is theoretically possible.

False; no temperature below ‐273°C can exist. (USRG:22,2,5)

515. Why is there no degree symbol accompanying measurements in Kelvin?

K is defined as degrees Kelvin. (USRG:22,2,5)

516. What equation that contains constants results from the combination of Boyleʹs and Charlesʹs laws?

PV/T=CD (USRG:23,1,1)

517. What equation without constants results from the combination of Boyleʹs and Charlesʹs laws?

P1V1/T1= P2V2/T2 (USRG:23,1,1)

518. What happens when the volume of gas in a closed piston decreases but the temperature remains the same?

pressure in the piston increases (USRG:23,1,1)



519. What happens when the temperature of gas in a closed piston decreases and the volume of the piston remains the same?

pressure in the piston decreases (USRG:23,1,1)

520. What is the scientific name for the force exerted by gas particles hitting the walls of their container?

pressure (USIRG:20,1,1)

521. What assumption must be made to calculate partial pressures of gases in a container?

the gases involved behave ideally (USIRG:20,1,1)

522. What happens to pressure within a container when more gas particles are added to the container?

It increases. (USIRG:20,1,1)

523. What is the relationship between pressure and the number of gas particles in a container?

directly proportional (USIRG:20,1,1)

524. In what units is the number of particles in a container usually measured?

moles (USIRG:20,1,1)

525. What is a mole fraction? the proportion of total particles in a container constituted by a certain gas (USIRG:20,1,1)

526. How is a gasʹs mole fraction calculated? the number of moles of the gas divided by the total number of moles of gases in the container (USIRG:20,1,1)

527. What is the equation for the ideal gas law? PV=nRT (USIRG:20,1,1)

528. What is the equation for Daltonʹs law? the mole fraction of substance

A=PA/(PA+PB+PC+.) (USIRG:20,1,1)

529. What is the term for the pressure exerted by a liquid in dynamic equilibrium in a container?

vapor pressure (USIRG:20,2,1)

530. What aspect of its surroundings determines the magnitude of waterʹs vapor pressure?

temperature (USIRG:20,2,1)

531. For what is mmHg a unit of measure? pressure (USIRG:21,1,1)

532. Given the vapor pressure of a liquid in a container and the total pressure inside the container, what formula do scientists use to calculate the partial pressure of the gas in the container?

total pressure ‐ vapor pressure = gas pressure (USIRG:21,1,1)

533. What measure of temperature must be used in the ideal gas law?

Kelvin (USIRG:21,1,1)

534. What four assumptions are made about ideal gases in the Kinetic Molecular Theory?

The volume of gas molecules is negligible, molecules are moving at varying speeds, there are no attractive or repulsive

forces between molecules, and molecules lose no kinetic energy in collisions. (USRG:23,2,1)

535. To what does the abbreviation KMT refer? Kinetic Molecular Theory (USRG:23,2,1)

536. What is the symbol for the average speed of a molecule?

u (USRG:23,2,2)

537. What equation relates the average speed of a molecule with the force it exerts on the walls of its container

Force= mu2/l per second, m being the mass of the molecule, and l being the average distance it travels between collisions

(USRG:23,2,3)

538. What portion of the gaseous molecules in a container can be assumed to be traveling in any one of the three dimensions at a time?

1/3 (USRG:24,1,1)



539. What formula is used to calculate the volume of a closed container given its length and the area of its base?

V=Al (USRG:24,1,1)

540. What equation defines pressure in terms of force? Pressure=Force/Area (USRG:24,1,1)

541. In the equation that relates pressure and volume to average molecular speed within a container, what does N represent?

the number of molecules in the container (USRG:24,1,1)

542. What equation relates pressure and volume to average molecular speed?

PV=(1/3)Nmu2 (USRG:24,1,2)

543. What was the nationality of Amadeo Avogadro? Italian (USRG:24,1,caption)

544. How many grams of helium are necessary to fill the same volume as two grams of hydrogen at a given temperature and pressure?

4 (USRG:24,2,2)

545. How many grams of methane are necessary to fill the same volume as two grams of hydrogen at a given temperature and pressure?

16 (USRG:24,2,2)

546. What is the ratio of the mass of one liter of helium to one liter of methane at a given temperature and pressure?

1:4 (USRG:24,2,2)

547. What is the molecular theory of matter? the theory that number of molecules in a substance, not the mass of the substance, determines its properties (USRG:24,2,3)

548. According to the official curriculum, how does Avogadroʹs Law relate to the molecular theory of matter?

It extends the molecular theory of matter. (USRG:24,2,3)

549. What was the original name for Avogadroʹs Law? Avogadroʹs hypothesis (USRG:24,2,3)

550. In what century was Avogadroʹs Law developed? the 19th century (ʺAvogadroʹs Law‐what is it?ʺ http://www.chemistry.co.nz/avogadro.htm)

551. Of what nation was Amedeo Avogadro? Italy (USRG:24,2,3)

552. What is Avogadroʹs law? In a container of gas at a given temperature, pressure, and volume, there is a certain constant number of molecules,

regardless of molecular mass. (USRG:24,2,3)

553. What does the acronym STP signify? standard temperature and pressure (USRG:24,2,4)

554. What pressure is indicated by STP? 1 atm (USRG:24,2,4)

555. What was the first definition of a mole? the number of molecules in 22.4 liters at 1 atmosphere and 273 K (USRG:24,2,4)

556. What is the modern definition of a mole? the number of atoms in exactly 12 grams of carbon‐12 (USRG:24,2,4)

557. True/False: Scientists know exactly how many particles are in a mole.

False; they can only make a close approximation of Avogadroʹs number. (USRG:24,2,5)

558. Approximately how many particles are in one mole? 6.022 x 1023 (USRG:24,2,5)

559. True/False: Amedeo Avogadro first approximated Avogadroʹs number.

False; though the number is named after him, he did not approximate it. (USRG:24,2,5)

560. What is the molar mass of carbon? 12 g/mol (USRG:24,2,5)



561. What is the molar mass of methane? 16 g/mol (USRG:24,2,5)

562. What is the molar mass of helium? 4 g/mol (USRG:24,2,5)

563. What is Avogadroʹs number? 6.022 x 1023 (USRG:24,2,5)

564. Approximately how many atoms are in 22.4 liters of helium at 1 atmosphere and 273 K?

6.022 x 1023 (USRG:24,2,5)

565. Approximately how many atoms are in 22.4 liters of methane at 1 atmosphere and 273 K?

6.022 x 1023 (USRG:24,2,5)

566. Approximately how much does 22.4 liters of methane at 1 atmosphere and 273 K weigh?

16 g (USRG:24,2,5)

567. Approximately how much does 22.4 liters of helium at 1 atmosphere and 273 K weigh?

4 g (USRG:24,2,5)

568. In what units are molar masses measured? grams/mole (USRG:24,2,5)

569. With what formula does one calculate a moleculeʹs molar mass?

(atomsa/molecule) x (atomic massa)+

(atomsb/molecule) x (atomic massb)+. (USRG:24,2,6)

570. What states of matter do scientists measure with moles?

all states of matter (USRG:25,1,1)

571. What is the molar mass of table salt? approximately 58.5 g/mol (USRG:25,1,1)

572. What is the molar mass of sodium? approximately 23.0 g/mol (USRG:25,1,1)

573. What is the molar mass of Cl? approximately 35.45 g/mol (USRG:25,1,1)

574. What equation relates a moving particleʹs kinetic energy to its mass and velocity?

KE=mu2/2 (USRG:25,1,2)

575. What equation relates the energy of a molecule in a gas to the temperature of the gas?

energy=3kT/2 (USRG:25,1,2)

576. What does the symbol k represent in the equation that relates the energy of a molecule in a gas to the temperature of the gas?

the Boltzman constant (USRG:25,1,2)

577. In what units must T be measured in the equation that relates the energy of a molecule in a gas to the temperature of that gas?

K (USRG:25,1,2)

578. What equation combines the two energy equations for gaseous particles?

u=(3kT/m)0.5 (USRG:25,1,3)

579. What quantity does the equation that combines the two energy equations for gaseous particles yield?

the root mean square speed of particles in the gas (USRG:25,1,3)

580. How is molar mass often abbreviated? M (USRG:25,1,4)

581. What does the symbol R represent in the equation for the root mean square speed of the molecules in one mole of gas?

the universal molar gas constant (USRG:25,1,4)

582. What equation yields the root mean square speed for molecules in one mole of gas?

u=(3RT/M)0.5 (USRG:25,1,4)

583. What is the relationship between the molecular mass of the molecules in a gas and their root mean square speed?

As the molecular mass of the molecules within the gas increases, their speed decreases. (USRG:25,1,4)



584. What is the relationship between the temperature of a gas and the root mean square speed of the molecules within that gas?

As its temperature increases, the root mean square speed of its molecules increases. (USRG:25,1,4)

585. True/False: One mile per second is an unusual speed for a gaseous particle.

False; that is approximately the root mean square speed of helium on a 25°C day. (USRG:25,1,4)

586. What variable must be held constant for the ideal gas law to become Boyleʹs and Charlesʹs laws?

n (USRG:25,2,2)

587. In the ideal gas law, what variable represents number of moles of a substance?

n (USRG:25,2,2)

588. Which symbol represents a constant in the equation PV=nRT?

R (USRG:25,2,1)

589. When the variable n is held constant, how can the equation PV=nRT be rewritten?

P1V1/T1=P2V2/T2 (USRG:25,2,1)

590. What is the ideal value of PV/RT for one mole of gas? 1 (USIRG:21,2,1)

591. What conditions can cause gases to behave non‐ideally?

very high pressures, very low volumes, or very low temperatures (USIRG:21,2,1)

592. What scientist developed an equation to model gases under non‐ideal conditions?

Johannes van der Waals (USIRG:21,2,2)

593. What is the appearance of the graph that would result from plotting an experimentally determined value of PV/RT for an ideal gas under certain pressures?

a straight line (USIRG:21,1,graph)

594. What is the van der Waals equation? P=(nRT)/(V‐nb)‐(n2a)/(V2) (USIRG:21,2,2)

595. In the van der Waals equation, what two terms must be equal to zero to indicate an ideal gas?

a and b (USIRG:21,2,3)

596. What is the appearance of the graph that would result from plotting an experimentally determined value of PV/RT for methane under certain pressures?

The graph would slope downwards, reach a minimum, and then slope upwards in a linear fashion. (USIRG:21,1,graph)

597. For what non‐ideal condition does the term ʺaʺ correct in the van der Waals equation?

attraction between particles of gas during collisions (USIRG:21,2,3)

598. For what non‐ideal condition does the term ʺbʺ correct in the van der Waals equation?

the volume of the particles of gas being considered (USIRG:21,2,3)

599. In what two states of matter are the materials a refrigerator uses to cool food?

liquid and gas (USIRG:22,1,1)

600. What mechanism makes a refrigerator cold? the evaporation of a liquid (USIRG:22,1,1)

601. How is energy conserved in a refrigerator? All of the cooling done by evaporation is negated by the heat generated during condensation. (USIRG:22,1,1)

602. Which common refrigerant has the highest ʺaʺ value for the van der Waals equation?

NH3 (USIRG:21,2,3)

603. Which gas has the highest ʺbʺ value for the van der Waals equation?

CH4 (USIRG:21,2,3)

604. If energy is conserved in the mechanism of a refrigerator, how does a refrigerator become cold?

Heat is released into area surrounding the refrigerator, whereas cold is generated inside the unit. (USIRG:22,1,1)



605. What substances were originally chosen as refrigerator liquids?

CFCs (USIRG:22,1,1)

606. In what way do CFCs damage the environment? They deplete the ozone layer. (USIRG:22,1,1)

607. True/False: Refrigerators operate best when using gases that behave nearly ideally.

False; for refrigerators, gases need to be easily turned into liquids. (USIRG:22,1,1)

608. What is heliumʹs ʺbʺ value for the van der Waals equation?

0.0273 L/mol (USIRG:22,1,table)

609. What does the acronym CFC represent? Chlorofluorocarbon (USIRG:22,1,1)

610. What two gases are used in modern refrigerators? NH3 and CO2 (USIRG:22,1,1)

611. What is the chemical formula for ammonia? NH3 (USIRG:22,1,1)

612. What concept is illustrated by a gas leak due to a puncture?

effusion (USRG:25,2,4)

613. What concept does the rate at which perfume molecules spread across a room illustrate?

diffusion (USRG:25,2,4)

614. To what does the term diffusion refer? the rate at which gas particles can spread throughout a container (USRG:25,2,4)

615. To what does the term effusion refer? the rate at which gas particles flow out of a small opening (USRG:25,2,4)

616. Why is it difficult to calculate an absolute rate of diffusion for any gas?

Gas particles collide with the air molecules and change their directions, resulting in unpredictable paths. (USRG:26,1,1)

617. Under what conditions would calculating the absolute rate of diffusion for a certain gas become much simpler?

the diffusion taking place in a vacuum (USRG:26,1,1)

618. What tool is necessary to calculate an absolute rate of diffusion of a certain gas through air?

a complex computer model (USRG:26,1,1)

619. In what terms are most rates of diffusion calculated? relative to another rate of diffusion (USRG:26,1,1)

620. What equation relates the root mean square speeds of two different molecules to their molar masses?

u1/u2=(M2/M1)0.5 (USRG:26,1,2)

621. What is the relationship between the masses of the molecules within a gas and the diffusion rate of that gas?

as the molecular masses increase, the diffusion rate decreases (USRG:26,1,2)

622. What is the chemical formula for acetone? C2H5CHO (USRG:26,1,4)

623. How fast will hydrogen molecules travel at the temperature at which the average speed of helium molecules is 1 mile per second?

1.4 miles per second (USRG:26,1,4)

624. What is the approximate molar mass of acetone? 58 grams/mole (USRG:26,1,4)

625. What is NH4ʹs ʺbʺ value for the van der Waals equation?


626. What type of gases usually exists as single atoms? the noble gases (USRG:26,1,5)

627. What is commonly the smallest distinct unit of a gas? a molecule (USRG:26,1,5)

628. How strong are the intermolecular forces in gases? almost non‐existent (USRG:26,1,5)



629. What is the term for movement from place to place? translational motion (USRG:26,1,5)

630. True/False: Particles in solids move very little. False; particles in solids move a great deal, just with little directionality. (USRG:26,1,5)

631. What is oxygenʹs ʺaʺ value for the van der Waals equation?

1.36 L2 atm/mol2 (USIRG:22,1,table)

632. Which state of matter has the most short‐range order? solids (USRG:26,1,5)

633. What state of matter has the least short‐range order? gases (USRG:26,1,5)

634. What is the term for the process in which a solid transforms into a gas?

sublimation (USRG:26,1,5)

635. What happens to a solidʹs volume when its temperature increases?

It increases slightly. (USRG:26,1,5)

636. Why does the volume of a solid change as its temperature increases?

because the solidʹs particles vibrate with greater intensity (USRG:26,1,5)

637. What is the ʺbʺ value of carbon dioxide in the van der Waals equation?


638. Which state of matter do liquids most closely resemble over a short distance?

gases (USRG:26,2,1)

639. What is methaneʹs ʺaʺ value for the van der Waals equation?

2.25 L2 atm/mol2 (USRG22,1,table)

640. What type of order do liquids exhibit? long‐range order (USRG:26,2,1)

641. In what substance is octane commonly encountered? in gasoline (USRG:26,2,1)

642. True/False: All liquids have approximately the same degree of order.

False; the amount of order in a liquid is highly dependent on the strength of intermolecular forces. (USRG:26,2,1)

643. What is carbon dioxideʹs ʺaʺ value for the van der Waals equation?

3.59 L2 atm/mol2 (USIRG:22,1,table)

644. What is a common example of a liquid that exhibits a high degree of order?

water (USRG:26,2,1)

645. Why is water a relatively ordered liquid? It has strong intermolecular forces. (USRG:26,2,1)

646. What type of intermolecular forces is most prevalent in water?

hydrogen bonds (USRG:26,2,1)

647. True/False: Octane has stronger intermolecular forces than water.

False; the intermolecular forces present in octane are far weaker than those in water, so octane tends to be far less

ordered than water. (USRG:26,2,1)

648. Of what are clouds composed? small drops of liquid water (USRG:26,2,3)

649. True/False: Clouds are composed of water vapor. False; clouds are composed of liquid water droplets; water vapor is invisible. (USRG:26,2,3)

650. What state of matter is the densest? solids (USRG:27,1,1)

651. What state of matter is the least dense? gases (USRG:27,1,1)

652. What substance is a notable exception to the relationship between states of matter and density?

water (USRG:27,1,1)

653. What holds particles in place in a solid? intermolecular forces (USRG:27,1,2)



654. What are the four types of solids? ionic lattice solids, metallic solids, molecular solids, and covalent networks (USRG:27,1,2)

655. What is another name for buckminsterfullerene? C60 (USRG:27,1,2)

656. What is an allotrope? an element that can exist in several solid forms (USRG:27,2,1)

657. What element is a common example of an allotrope? carbon (USRG:27,2,1)

658. How many allotropes of carbon are mentioned in the official curriculum?

8 (USRG:27,2,1)

659. Of what element is buckminsterfullerene an allotrope? carbon (USRG:27,2,1)

660. What element can form a single‐walled nanotube? carbon (USRG:27,2,1)

661. Of what element is lonsdaleite an allotrope? carbon (USRG:27,2,1)

662. Of what element is graphite an allotrope? carbon (USRG:27,2,1)

663. Of what element is diamond an allotrope? carbon (USRG:27,2,1)

664. True/False: Allotropes can have widely different properties.

True; allotropes of an element can be conductors or insulators, malleable or stiff, etc. (USRG:27,2,2)

665. What is carbonʹs most stable allotrope? graphite (USRG:27,2,3)

666. What form of carbon is a good conductor? graphite (USRG:27,2,2)

667. What form of carbon is a good electrical insulator? diamond (USRG:27,2,2)

668. How do scientists determine an elementʹs most stable allotrope?

by comparing the energy levels of that elementʹs allotropes (USRG:27,2,3)

669. From what form of carbon are natural diamonds formed?

graphite (USRG:27,2,3)

670. Under what conditions are diamonds formed? high pressure and temperature (USRG:27,2,3)

671. From what form of carbon are artificial diamonds formed?

graphite (USRG:27,2,3)

672. How are density and energy related in metallic solids? the denser the solid, the more energy is contained (USRG:27,2,4)

673. How are density and energy related in ionic lattice solids?

the denser the solid, the more energy it contains (USRG:27,2,4)

674. In which types of solids is a particleʹs size important in determining its arrangement?

metallic and ionic lattice solids (USRG:27,2,4)

675. What element coats the surface of galvanized objects? crystals of zinc (USRG:27,2,5)

676. What factor determines the solid form of a metal? the number of nearest neighbors each particle has (USRG:27,2,5)

677. What is a nearest neighbor? a similar particle at the nearest distance (USRG:27,2,5)

678. What type of solid has a regular crystalline structure? metals (USRG:27,2,5)

679. What type of solid is generally the densest? metals (USRG:27,2,5)

680. What are the three simplest forms of metals? body‐centered cubic, cubic closest packed, and hexagonal closest packing (USRG:27,2,6)

681. Which form of metal is zinc? hexagonal closest packing (USRG:27,2,6)



682. Which form of metal is gold? cubic closest packed (USRG:27,2,6)

683. Which form of metal is iron? body‐centered cubic (USRG:27,2,6)

684. How many nearest neighbors does each particle have in the body‐centered cubic form?

8 (USRG:27,2,6)

685. How many nearest neighbors does each particle in the cubic closest packed form have?

12 (USRG:27,2,6)

686. How many nearest neighbors does each particle in the hexagonal closest packing have?

12 (USRG:27,2,6)

687. What type of particle are an atomʹs nearest neighbors in a pure metal?

identical atoms (USRG:27,2,6)

688. What aspect of metallic structure causes metals to be lustrous, good conductors of heat, good conductors of electricity, and malleable?

Their atoms are tightly packed. (USRG:27,2,6)

689. What is the term for the effect of light reflecting off of a regular arrangement of atoms in a metal?

luster (USRG:27,2,6)

690. What shape are the lattices of atoms in buckminsterfullerene?

pentagonal (USRG:27,1,diagram)

691. To what property does the term ʺsonorousʺ refer? the proclivity to produce sound when struck (USRG:27,2,6)

692. Why are metals sonorous? sound waves easily travel through densely packed particles (USRG:27,2,6)

693. To what attribute does the term ʺmalleableʺ refer? flexibility¬the ability to be molded into shapes (USRG:27,2,6)

694. To what attribute does the term ʺductileʺ refer? the ability to be pulled into wire (USRG:27,2,6)

695. What happens to the softness of a metal as its atoms get more densely packed?

It becomes softer. (USRG:28,1,1)

696. What shape are the lattices in single‐walled carbon nanotubes?

hexagonal (USRG:27,1,diagram)

697. Why are alloys stronger than pure metals? Their impurities prevent layers of atoms from being smooth enough to slide over one another. (USRG:28,1,2)

698. Why might a blacksmith want impurities in his metals? Impurities make metals harder and stronger. (USRG:28,1,2)

699. What type of image visually summarizes the transitions between states of matter for a certain element?

a phase diagram (USRG:28,1,3)

700. What is another name for a state of matter? a phase (USRG:28,1,3)

701. What shape are the lattices of C70? pentagonal (USRG:27,1,diagram)

702. What is the term for the process in which a liquid becomes a gas?

vaporization (USRG:28,1,3)

703. What is the term for the process in which a gas becomes a liquid?

condensation (USRG:28,1,3)

704. What is the term for the process in which a gas becomes a solid?

deposition (USRG:28,1,3)



705. What state of matter generally occupies a space shaped vaguely like a triangle in the bottom and right areas of a phase diagram?

gas (USRG:28,1,3)

706. What condition is implied for the values given by a phase diagram?

The substance in question is in a vacuum. (USRG:28,1,3)

707. What state of matter generally occupies a triangular space in the upper left of a phase diagram?

solids (USRG:28,1,3)

708. What is the term for a situation in which particles are entering a phase at the same rate in which they leave it?

equilibrium (USRG:28,1,3)

709. What phase of a substance is present in small quantities at any temperature?

gas (USRG:28,1,3)

710. What term for gases is used when the majority of the substance is in solid or liquid form?

vapors (USRG:28,1,3)

711. Under what circumstance do the vapors associated with any substance have a gas pressure?

when the substance is in a sealed container (USRG:28,1,3)

712. In a phase diagram, what is plotted on the vertical axis? pressure (USRG:28,2,1)

713. In a phase diagram, what is plotted on the horizontal axis?

temperature (USRG:28,2,1)

714. How are phases represented on a phase diagram? as regions between lines (USRG:28,2,1)

715. What do the lines on a phase diagram represent? equilibrium between two states (USRG:28,2,1)

716. At how many points on a phase diagram do all three states exist in equilibrium?

1 (USRG:28,2,1)

717. What is the triple point? a point on a phase diagram at which all states of matter are in equilibrium (USRG:28,2,1)

718. What do vertical arrows on a phase diagram indicate? changing states by changing pressure (USRG:28,2,1)

719. What is one way to increase the pressure a substance experiences?

decreasing the size of the container which contains the substance (USRG:28,2,1)

720. What do the horizontal arrows on a phase diagram indicate?

changing states by changing temperature (USRG:28,2,1)

721. Under what circumstances do gases and liquids tend to exhibit similar properties?

very high temperature and pressure (USRG:28,2,1)

722. What is the critical point on a phase diagram? the end point of the equilibrium line between liquids and gases (USRG:28,2,1)

723. What is the standard pressure on the surface of the earth?

14 lbs. per square inch (USRG:29,1,2)

724. At what temperature is waterʹs critical point? 374°C (USRG:29,1,2)

725. At what pressure is waterʹs

critical point?

218 atm (USRG:29,1,2)


melting point 0°C?

1 atm (USRG:29,1,2)


boiling point 100°C?

1 atm (USRG:29,1,2)



728. What is unusual about waterʹs phase diagram? Its melting point line slants backwards. (USRG:29,1,3)

729. What happens to waterʹs melting point as pressure increases?


730. Why can two ice cubes become fused when pressed together?

The increased pressure causes them to melt and then they refreeze together when the pressure is released. (USRG:29,1,3)

731. Why do ice skates slide so easily over frozen water? The increased pressure causes some water to melt on the surface of the ice, making them glide well. (USRG:29,1,3)

732. According to the official curriculum, how is the structure of ice best described?

open (USRG:29,1,4)

733. What causes the abnormal slant of waterʹs melting point line?

its strong hydrogen bonds (USRG:29,1,4)

734. What property of water allowed life to survive Earthʹs glacial periods?

It is less dense in a solid state than a liquid state. (USRG:29,1,4)

735. True/False: Many substancesʹ melting points decrease as pressure increases.

False; substances like this are relatively rare. (USRG:29,1,4)

736. The triple point of carbon dioxide occurs at this pressure

5.11 atm (USIRG:23,1,2)

737. The triple point of carbon dioxide occurs at this temperature

‐56.4°C (USIRG:23,1,2)

738. Why is liquid carbon dioxide rare? It can only be observed in situations with extremely low temperatures and extremely high pressure. (USIRG:23,1,2)

739. What is the minimum pressure at which liquid CO2 can exist?

5.11 atm (USIRG:23,1,2)

740. Aside from differences in scale, how does the phase diagram of CO2 differ from that of water?

Its melting point line does not slant backward. (USIRG:23,1,2)

741. What type of CO2 is ideal as a solvent? supercritical CO2 (USIRG:23,1,3)

742. What are the properties of supercritical CO2? It is as dense as a liquid but it moves like a gas. (USIRG:23,1,3)

743. At what pressure is CO2ʹs critical point? 73 atm (USIRG:23,1,3)

744. At what temperature is CO2ʹs critical point? 31.1°C (USIRG:23,1,3)

745. How do industries remove of supercritical CO2 from a solution?

They reduce the pressure and the CO2 boils away. (USIRG:23,2,1)

746. True/False: The sugar at the bottom of a pitcher of lemonade is part of the solution.

False; it is not homogenous. (USRG:29,2,1)

747. What is a solvent? the substance that composes the majority of a solution (USRG:29,2,2)

748. What is a solute? the substance that composes the minority of a solution (USRG:29,2,2)

749. What is an aqueous solution? a solution whose solvent is water (USRG:29,2,2)

750. What is an organic solution? a solution whose solvent is a non‐polar substance (USRG:29,2,2)

751. What type of solution is lemonade? an aqueous solution (USRG:29,2,2)



752. What type of solution is one in whose solvent is CH4? an organic solution (USRG:29,2,2)

753. To what does the term solubility refer? the amount of solute that can be suspended in solution (USRG:29,2,3)

754. To what does the term concentration refer? the ratio of solute to solvent in a solution (USRG:29,2,3)

755. How do scientists usually distinguish between solvents?

by polarity (USRG:29,2,4)

756. According to the official curriculum, what is the most general rule of solubility?

Like dissolves like. (USRG:29,2,4)

757. What is the most important polar solvent? water (USRG:29,2,4)

758. In what type of solvent do salts dissolve? polar (USRG:29,2,4)

759. What type of solution is salt dissolved in water? aqueous (USRG:29,2,4)

760. In what type of solvent do sugars dissolve? polar (USRG:29,2,4)

761. In what type of solvent does vegetable oil dissolve? non‐polar (USRG:29,2,4)

762. What type of solution is vegetable oil dissolved in octane?

an organic solution (USRG:29,2,4)

763. What happens when NaCl dissolves in water? It breaks into Na+ and Cl‐ ions. (USRG:30,1,1)

764. Why do crystal lattices dissolve in a water solvent? Each particle is more attracted to the water molecules than to other particles in the lattice. (USRG:30,1,1)

765. To what does the term hydration refer with regards to solutions?

the circumstance in which positive and negative ions are separated and surrounded by water molecules (USRG:30,1,1)

766. Why are some salts insoluble? Their particles are more attracted to each other than to the water molecules. (USRG:30,1,3)

767. What group of elements on the periodic table forms compounds that are always soluble?

group I (USRG:30,1,3)

768. What is the solubility rule regarding ammonium compounds?

They are soluble. (USRG:30,1,3)

769. What is the solubility rule regarding nitrate compounds?


770. What is the solubility rule regarding acetate compounds?


771. What is the solubility rule regarding chlorate compounds?


772. What is the solubility rule regarding binary compounds of halogens with metals?

Most are soluble. (USRG:30,1,3)

773. What halogen is an exception to the general halogen solubility rule?

fluorine (USRG:30,1,3)

774. What metals are never soluble in binary compounds with halogens?

Ag and Hg(I) (USRG:30,1,3)

775. What metal is soluble in a binary compound with halogen only when in hot water?

Pb (USRG:30,1,3)

776. What group of elements on the periodic table is also known as the halogens?

group VII (USRG:30,1,3)



777. What is the solubility rule regarding sulfates? Most are soluble. (USRG:30,1,3)

778. What sulfates are exceptions to the solubility rules? barium, strontium, lead, silver, mercury, and calcium sulfates (USRG:30,1,3)

779. What is the solubility rule regarding carbonates? Most are insoluble. (USRG:30,1,3)

780. What is the solubility rule regarding hydroxides? Most are insoluble. (USRG:30,1,3)

781. What is the solubility rule regarding oxides? Most are insoluble. (USRG:30,1,3)

782. What is the solubility rule regarding silicates? Most are insoluble. (USRG:30,1,3)

783. What is the solubility rule regarding phosphates? Most are insoluble. (USRG:30,1,3)

784. What sorts of carbonate compounds are soluble? those that involve a group I metal (USRG:30,1,3)

785. What is the solubility rule regarding sulfides? Most are insoluble. (USRG:30,1,3)

786. What seven types of sulfides are the exceptions to the sulfide solubility rule?

calcium, barium, strontium, magnesium, sodium, potassium, and ammonium (USRG:30,1,3)

787. What is a saturated solution? a solution with the maximum possible amount of dissolved solids (USRG:30,2,1)

788. What happens when solute is added to a saturated solution?

It does not dissolve. (USRG:30,2,1)

789. What happens to the solubility of a compound as its temperature is raised?


790. What happens when a hot saturated solution is cooled? Excess solute falls out of the solution. (USRG:30,2,1)

791. How are crystals grown? A hot saturated solution with a crystalline solute is slowly and carefully cooled. (USRG:30,2,1)

792. What is a precipitate? an insoluble substance created in a solution (USRG:30,2,2)

793. What precipitate results from adding silver ions to a solution with chlorine ions?

AgCl (USRG:30,2,2)

794. What is a common method for testing if chlorine ions are present in a solution?

adding silver ions to the solution (USRG:30,2,2)

795. What principle of solutions explains the formation of stalactites and stalagmites based?

the formation of insoluble precipitates (USRG:30,2,3)

796. What ions are created when carbon dioxide dissolves in water?

carbonate ions (USRG:30,2,3)

797. What is the chemical formula for carbonate? CO32‐ (USRG:30,2,3)

798. What ions must be present in water for stalactites and stalagmites to form?

calcium ions (USRG:30,2,3)

799. What is the chemical formula for calcium ions? Ca2+ (USRG:30,2,3)

800. What compound composes stalactites and stalagmites? calcium carbonate (USRG:30,2,3)

801. What is the chemical formula for calcium carbonate? CaCO3 (USRG:30,2,3)

802. What happens when calcium ions and carbonate ions come into contact in solution?

They fall out of the solution as a precipitate. (USRG:30,2,3)

803. Why can sugar dissolve in water? It contains O‐H bonds that form hydrogen bond with water. (USRG:31,1,1)

804. How many O‐H groups does glucose have? five (USRG:31,1,1)



805. What is the solubility rule regarding alcohols? They are soluble. (USRG:31,1,1)

806. What is the solubility rule regarding glucose? It is soluble. (USRG:31,1,1)

807. For what substance were the solubility rules created? water (USRG:31,1,1)

808. What are the two main elements in non‐polar solvents? carbon and hydrogen (USRG:31,1,2)

809. What is the difference in electronegativity between carbon and hydrogen?

0.05 (USRG:31,1,2)

810. What types of solvents are commonly used in cleaning? non‐polar solvents (USRG:31,1,3)

811. What is the only way to dispose of non‐polar solvents? immolation (USRG:31,1,3)

812. What type of solvents are most greases and oils? non‐polar (USRG:31,1,3)

813. According to the official curriculum, what are modern ʺsuper solventsʺ?

supercritical fluids (USRG:31,14)

814. How do detergents work? One side of a detergent molecule binds to grime and another side binds to water, allowing the molecule and the grime to

get washed away. (USRG:31,14)

815. What are the two common shapes of detergent molecules?

long or ringlike (USRG:31,14)

816. According to the official curriculum, what is the most basic way to express the proportions of solvent and solute in a solution?

by mass (USRG:31,1,6)

817. How is the percent composition of a solution calculated?

by dividing its grams of solute by its grams of solvent (USRG:31,1,6)

818. What is the chemical formula for bleach? NaOCl (USRG:31,1,6)

819. What method of calculating concentrations is implied by a label such as ʺ7% bleachʺ?

percent composition by mass (USRG:31,1,6)

820. For what measure is weight a substitute? mass (USRG:31,2,1)

821. What does the symbol w represent in % w/w? weight (USRG:31,2,1)

822. What symbol is used for molarity? M (USRG:31,2,2)

823. In what units are molarities measured? moles/liter (USRG:31,2,2)

824. What measure of concentration would chemists use if they were concerned with the number of particles in a solution?

molarity (USRG:31,2,2)

825. What are colligative properties? properties of a solution dependent on the ratio of moles of solute to moles of solvent (USRG:31,2,3)

826. What measure of concentration involves the ratio of a solutionʹs moles of solute its moles of solvent?

the mole fraction (USRG:31,2,3)

827. In what units are molalities measured? molals (USRG:31,2,3)

828. What is a molal? one mole of solute in 1 kg of solvent (USRG:31,2,3)

829. What happens to the colligative properties of a solution when its molality doubles?

The colligative properties also double in value. (USRG:31,2,3)

830. What is the chemical formula for glucose? C6H12O6 (USIRG:23,2,2)



831. Who discovered that the colligative properties of a solution are dependent only its mole ratios?

François Raoult (USIRG:23,2,2)

832. Why does a solution tend to have a higher boiling point than a pure liquid?

The solute particles prevent the solvent from becoming a vapor. (USIRG:23,2,3)

833. Which of a solutionʹs phase changes are affected by its colligative properties?

all of its phase changes (USIRG:23,2,3)

834. What happens to the colligative properties of a solution when salts are added?

They change by a greater magnitude than they would if the same amount of a different type of compound were added.

(USIRG:23,2,5)

835. Why do salts alter the colligative properties of a solution more than do non‐ionic molecules?

They separate into ions, which multiplies the number of moles of particles in the solution and thus the solutionʹs colligative

properties. (USIRG:23,2,5)

836. What is the chemical formula for calcium chloride? CaCl2 (USIRG:23,2,5)

837. How magnified is NaClʹs effect on a solutionʹs molality?

2x (USIRG:23,2,5)

838. How magnified is CaCl2ʹs effect on a solutionʹs molality?

3x (USIRG:23,2,5)

839. How magnified is NaClʹs effect on a solutionʹs colligative properties?

2x (USIRG:23,2,5)

840. How magnified is CaCl2ʹs effect on a solutionʹs colligative properties?

3x (USIRG:23,2,5)

841. Why is salting icy roads effective? The salt forms a solution with the water, lowering its melting point. (USIRG:24,1,1)

842. Why have some groups protested the use of NaCl as a road salt?

It is damaging to plants, animals, and concrete. (USIRG:24,1,1)

843. What substance has replaced NaCl as road salt? calcium magnesium acetate (USIRG:24,1,1)

844. What is the primary problem with using calcium magnesium acetate as road salt?

It is much more expensive than NaCl. (USIRG:24,1,1)

845. What was the first substance used to salt roads? NaCl (USIRG:24,1,1)

846. True/False: The vapor above a solution contains both solute and solvent.

False; it contains only solvent. (USIRG:24,1,2)

847. What is the name of the device used to distill solutions? a still (USIRG:24,1,2)

848. How does distillation purify water? The pure vapor above a solution is collected and condensed into pure solvent. (USIRG:24,1,2)

849. What happens to the original solution during the distillation process?

It becomes more concentrated. (USIRG:24,1,2)

850. According to the official curriculum, what is the most realistic alternative to distillation?

reverse osmosis (USIRG:24,2,1)

851. What is the preferred salt water purification method of California?

reverse osmosis (USIRG:24,2,1)

852. How does reverse osmosis purify water? Water is pushed through a semi‐permeable membrane which traps impurities. (USIRG:24,2,1)



853. What advantages does distillation have over reverse osmosis?

It is easier to perform on a large scale, the equipment involved does not need to be routinely cleaned, it requires less

pretreatment processing, and it has fewer wastes. (USIRG:24,2,3)

854. What advantages does reverse osmosis have over distillation?

It requires less energy, it is less damaging to the environment, and it has purer output. (USIRG:24,2,3)

855. What term do scientists use for the rearrangement of chemical substances to form new substances with new properties?

chemical reactions (USRG:33,1,1)

856. What are the five main types of chemical reactions? synthesis, decomposition, double replacement, single replacement, and combustion (USRG:33,1,2)

857. What aspect of chemical reactions do chemists use to classify them?

the way in which atoms are to be rearranged within the reaction (USRG:33,1,3)

858. How do scientists further classify the reactions that fall within a certain type of chemical reaction?

They differentiate among the properties of the molecules and atoms involved. (USRG:33,1,3)

859. What appears on the left hand side of a chemical equation?

reactants (USRG:33,1,4)

860. What appears on the right hand side of a chemical equation?

products (USRG:33,1,4)

861. What lies between the products and reactants in a typical chemical equation?

an arrow (USRG:33,1,4)

862. What element does the atomic symbol ʺKʺ represent? potassium (USRG:33,2,4)

863. What symbol was originally used to separate products and reactants in chemical equations?

= (USRG:33,2,1)

864. Why did scientists begin to use an arrow to write chemical equations?

to express directionality (USRG:33,2,1)

865. What quantity must remain equal in chemical reactions?

the quantity of each element (USRG:33,2,1)

866. What symbol separates each of the reactants in a chemical equation?

+ (USRG:33,2,1)

867. What is another name for synthesis reactions? combination reactions (USRG:33,2,2)

868. What is the minimum number of reactants in synthesis reactions?

2 (USRG:33,2,2)

869. How many products are there in synthesis reactions? 1 (USRG:33,2,2)

870. Why type of reaction is

2Na + Cl2→2NaCl?

synthesis (USRG:33,2,2)

871. What type of reaction is

2K + Cl2→2KCl?

synthesis (USRG:33,2,2)

872. In what state of matter is Cl2 at room temperature? gas (USRG:33,2,2)

873. In what state of matter is K at room temperature? solid (USRG:33,2,2)

874. In what state of matter is KCl at room temperature? solid (USRG:33,2,2)


IV Reactions

875. How many reactants are there in decomposition reactions?

1 (USRG:33,2,3)

876. What is the minimum number of products for decomposition reactions?

2 (USRG:33,2,3)


2H2O2 → 2H2O + O2?

decomposition (USRG:33,2,3)

878. In what year was the

2H2O2→2H2O + O2

reaction discovered?

1774 (USRG:33,2,3)

879. For what purpose was the

2H2O2 → 2H2O + O2

reaction originally used?

to produce oxygen gas (USRG:33,2,3)

880. What is the chemical formula for mercury oxide? HgO (USRG:33,2,3)


2HgO → 2Hg + O2?

decomposition (USRG:33,2,3)

882. In what state of matter is HgO at room temperature? solid (USRG:33,2,3)

883. What type of compounds are the only possible reactants for a double displacement reaction?

ionic compounds (USRG:34,1,1)

884. In what substance do double replacement reactions usually occur?


885. In general, how many products are there in a double replacement reaction?

2 (USRG:34,1,1)

886. In general, how many reactants are there in a double replacement reaction?

2 (USRG:34,1,1)


Pb(NO3)2 + 2KI → PbI2 + 2KNO3?

double replacement (USRG:34,1,1)

888. True/False: 2KNO3 is soluble in water. True; 2KNO3 dissociates in water. (USRG:34,1,1)

889. What happens when PbI2 is placed in water? It remains solid because it is an insoluble molecule. (USRG:34,1,1)

890. Into what two categories are all single replacement reactions subdivided?

metallic or nonmetallic (USRG:34,1,2)

891. What is the general format for a single replacement reaction with a metallic element?

M + BC → MC + B

(M represents the metallic element) (USRG:34,1,2)

892. What is the general format for a single replacement reaction with a nonmetallic element?

N + BC → BN+C

(N represents the nonmetallic element) (USRG:34,1,2)

893. In general, how many reactants are there in single replacement reactions?

2 (USRG:34,1,2)

894. In general, how many products are there in single replacement reactions?

2 (USRG:34,1,2)


IV Reactions


Cu + 2AgNO3 → Cu(NO3)2 + 2Ag?

metallic single replacement (USRG:34,1,2)


Cl2 + 2KBr → 2KCl + Br2?

nonmetallic single replacement (USRG:34,1,2)

897. Which is the most common type of single replacement reaction?

metallic (USRG:34,1,2)

898. What is the chemical symbol for silver? Ag (USRG:34,1,2)

899. What is the chemical formula for silver nitrate? AgNO3 (USRG:34,1,2)

900. What is the chemical formula for copper nitrate? Cu(NO3)2 (USRG:34,1,2)


2AgNO3 + Cu → Cu(NO3)2 + 2Ag?

metallic single replacement (USRG:34,1,2)

902. What is the chemical formula for lithium hydroxide? LiOH (USRG:34,1,2)

903. What is the state of matter of H2 at room temperature? gas (USRG:34,1,2)


2Li + 2H2O → 2LiOH + H2?

nonmetallic single replacement (USRG:34,1,2)

905. What list do chemists use to predict the occurrence of a single replacement reaction?

the activity series (USRG:34,1,5)

906. Where must an element lie on the activity series to replace another element in a single replacement reaction?

above the element that it will replace (USRG:34,1,5)

907. What element is at the top of the activity series? Li (USRG:34,1,5)

908. What element is at the bottom of the activity series? Au (USRG:34,1,5)

909. What chemical composes natural gas? methane (USRG:34,2,1)

910. What element is necessary in a combustion reaction? O2 (USRG:34,2,1)

911. What are the products of a combustion reaction between O2 and an organic hydrocarbon?

H2O and CO2 (USRG:34,2,1)


CH4 + 2O2 → 2H2O + CO2?

combustion (USRG:34,2,1)

913. Who created the first theory about acids and bases? Svante Arrhenius (USRG:35,1,1)

914. What is the chemical symbol for hydroxide? OH‐ (USRG:35,1,1)

915. Which theory of acids and bases fails to explain the effects of NH3?

the Arrhenius theory (USRG:35,1,1)

916. What happens when a solution with NH3 is tested for acidity?

It appears basic. (USRG:35,1,1)

917. According to Svante Arrhenius, which particle is associated with all acids?

H+ (USRG:35,1,1)

918. According to Svante Arrhenius, which particle is associated with all bases?

OH‐ (USRG:35,1,1)

919. What was Svante Arrheniusʹs theory about acids and bases?

Acids yield H+ ions in water, and bases yield OH‐ ions. (USRG:35,1,1)


IV Reactions

920. Who proposed the modern theory of acids and bases? Brønsted and Lowry (USRG:35,1,3)

921. What is the Brønsted‐Lowry theory? Acids are H+ donors and bases are H+ acceptors. (USRG:35,1,3)

922. What products result when NH3 is placed in water? NH4+ and OH‐ (USRG:35,1,4)

923. True/False: Water is classified as a base in a solution of NH3?

False; water is classified as an acid because it donates a hydrogen ion to NH3. (USRG:35,1,4)

924. True/False: Water is classified as a base in a solution of acetic acid?

True; water is classified as a base because it accepts a hydrogen ion. (USRG:35,1,5)

925. What is the chemical formula for hydronium? H3O+ (USRG:35,1,5)

926. True/False: The Brønsted‐Lowry theory applies to Arrhenius acids and bases.

True; it successfully predicts Arrhenius acids and bases, in addition to those unclassified by the Arrhenius theory.

(USRG:35,1,4)

927. What is the chemical formula for acetic acid? HC2H3O2 (USRG:35,1,5)

928. What is the chemical formula for acetate? C2H3O2‐ (USRG:35,1,5)

929. What substance is added to water to make vinegar? acetic acid (USRG:35,1,5)

930. What are the products of an aqueous solution of acetic acid?

H3O+ and C2H3O2‐ (USRG:35,1,5)

931. What substances can be either acids or bases? amphoteric substances (USRG:36,1,1)

932. What is the most common amphoteric substance? water (USRG:36,1,1)

933. What scale measures acidity? the pH scale (USRG:36,1,2)

934. How do chemists usually

abbreviate [H3O+]?

[H+] (USRG:36,1,2)

935. True/False: The pH scale is exponential. False; it is logarithmic. (USRG:36,1,2)

936. What do brackets signify in chemistry? concentration (USRG:36,1,2)

937. In what units must concentrations be measured for the pH scale?

molar (USRG:36,1,2)

938. What are the units for the concentration of an acid? moles of H3O+/liter (USRG:36,1,2)

939. According to the Brønsted‐Lowry theory, what ion defines an acidic aqueous solution?

H3O+ (USRG:36,1,2)

940. What is the equation for the pH scale? pH=‐log[H3O+] (USRG:36,1,2)

941. What is the only state of matter that the pH scale can measure?

liquid (USRG:36,1,2)

942. What is the range of the pH scale? 0‐14 (USRG:36,1,3)

943. What is the concentration of hydrogen ions in a solution with a pH of 7?

1.0 x 10‐7 M (USRG:36,1,3)

944. What pH level is neutral? 7 (USRG:36,1,3)

945. What pH range is acidic? 0‐7 (USRG:36,1,3)

946. What pH range is basic? 7‐14 (USRG:36,1,3)

947. True/False: Acidic solutions contain bases. True; every solution contains both acids and bases. (USRG:36,1,4)


IV Reactions

948. Which pH level indicates equilibrium between acidic particles and basic particles?

7 (USRG:36,1,4)

949. What is a titration? the mixture of acids and bases for the purpose of observing a pH level (USRG:36,2,1)

950. What is a buret? a long tube used in titrations (USRG:36,2,1)

951. What device controls the flow of acid or base out of a buret?

a stopcock (USRG:36,2,1)

952. Into what object is the solution in the buret poured in a titration?

an Erlenmeyer flask (USRG:36,2,1)

953. What object usually contains the acid at the beginning of a titration?

an Erlenmeyer flask (USRG:36,2,1)

954. What object usually contains the base at the beginning of a titration?

a buret (USRG:36,2,1)

955. Why do scientists often use titrations? to determine the molarity of an unknown acid or base (USRG:36,2,1)

956. What is another name for the end of a titration? the equivalence point (USRG:36,2,2)

957. What is the equivalence point of a titration? the point at which the moles of acid in the flask equal the moles of base in the flask (USRG:36,2,2)

958. What is an indicator? a dye that changes color at a specific pH level (USRG:36,2,2)

959. What do some scientists use in place of an indicator for their titrations?

a pH meter (USRG:36,2,2)

960. What equation represents the equivalence point? MaVa = MbVb (USRG:36,2,3)

961. What kind of ions can a diprotic acid donate? H+ ions (USRG:36,2,3)

962. What type of acid can donate three H+ ions? a triprotic acid (USRG:36,2,3)

963. What type of acid is H2SO4? diprotic (USRG:36,2,3)

964. What type of acid is H3PO4? triprotic (USRG:36,2,3)

965. What type of chemical reactions are acid‐base reactions?

double replacement reactions (USRG:36,2,5)

966. What are the products of an acid‐base reaction? water and a salt (USRG:36,2,5)

967. How is the chemical composition of a salt different from that of an acid?

A salt contains a metal ion in place of a hydrogen ion. (USRG:36,2,5)

968. What element usually begins the chemical formula of an acid?

H (USRG:36,2,5)

969. What is a strong acid? an acid that will donate all of its H+ ions to a solution (USRG:36,2,7)

970. What is a weak acid? an acid that will donate only some of its H+ ions to a solution (USRG:36,2,7)

971. What pH levels can salts have? any pH level (USRG:36,2,7)

972. What types of acids and bases react to produce neutral salts?

strong acids and strong bases (USRG:36,2,7)

973. What is the pH level of NaCl? 7 (USRG:36,2,7)


IV Reactions

974. Which acid and base react to produce NaCl? HCl and NaOH (USRG:36,2,7)

975. True/False: HCl is a strong acid. True; HCl dissociates completely in aqueous solutions. (USRG:36,2,7)

976. True/False: NaOH is a weak base. False; NaOH dissociates completely in aqueous solutions. (USRG:36,2,7)

977. What is the pH level of KBr? 7 (USRG:36,2,7)

978. What acid and base react to produce KBr? HBr and KOH (USRG:36,2,7)

979. True/False: HBr is a strong acid. True; HBr dissociates completely in solutions. (USRG:36,2,7)

980. True/False: KOH is a weak base. False; KOH dissociates completely in solutions. (USRG:36,2,7)

981. What does a salt react with during hydrolysis? water (USIRG:26,1,1)

982. What is the pH range of a solution in which the anion undergoes hydrolysis?

>7 (USIRG:26,1,1)

983. What is the pH range of a solution in which the cation undergoes hydrolysis?

<7 (USIRG:26,1,1)

984. What type of salts do anions of weak acids generally form?

basic (USIRG:26,2,1)

985. What type of salts do cations of weak bases generally form?

acidic (USIRG:26,2,3)

986. What are the three most common salt‐forming cations? NH4+, CH3NH3+, Cu2+ (USIRG:26,2,3)

987. What are the four most common salt‐forming anions? F‐, HCO3‐, SO42‐, CH3COO‐ (USIRG:26,2,3)

988. What type of reactions are precipitate reactions? double replacement reactions (USRG:37,1,1)

989. What type of ions does not form a precipitate in a precipitate reaction?

spectator ions (USRG:37,1,1)

990. What do precipitates often resemble in solutions? clouds or crystals (USRG:37,1,1)

991. What is a net reaction? a chemical equation with omitted spectator ions (USRG:37,1,4)

992. What is another term for a net reaction? a net equation (USRG:37,1,4)

993. What rules predict the formation of a precipitate? solubility rules (USRG:37,1,4)

994. What happens when Na+ ions and Cl‐ ions are mixed in a solution?

The ions remain separate and no reaction occurs. (USRG:37,2,1)

995. What happens when Pb2+ and Cl‐ ions are mixed in a solution?

They form a precipitate. (USRG:37,2,2)

996. What molecule do Pb2+ and Cl‐ form? PbCl2 (USRG:37,2,2)

997. What is the chemical formula for lead chloride? PbCl2 (USRG:37,2,2)

998. What is the net reaction for a lead chloride precipitate? Pb2++2Cl‐→PbCl2 (USRG:37,2,2)

999. Why are precipitates not beneficial for plants? Plants can only absorb dissolved nutrients. (USIRG:12539)

1000. Why do farmers add acids or bases to their farmland? to dissolve nutrients (USIRG:12539)

1001. Why is soil usually acidic? Acid rain lowers the pH of soil. (USIRG:12539)


IV Reactions

1002. How do farmers combat the effects acid rain on their soil?

by adding bases to the soil (USIRG:12539)

1003. What is the most infamous metal contaminant? mercury (USIRG:27,2,2)

1004. How does mercury enter the environment? atmospherically from fossil fuel power plants and into lakes from electrolytic cells (USIRG:27,2,2)

1005. What are particulates? atmospheric particles (USIRG:28,1,1)

1006. How do environmentalists use precipitates to their advantage?

Solid substances are easier to bury or eliminate than are solutions. (USIRG:28,1,2)

1007. On what type of salt did early photographs predominantly rely for development?

silver halides (USIRG:28,2,1)

1008. What is a common abbreviation for oxidation‐reduction reactions?

redox reactions (USRG:38,1,1)

1009. What is the focus of redox reactions? an electron transfer from one atom to another (USRG:38,1,1)

1010. How many electrons does sodium have? 11 (USRG:38,1,1)

1011. How many valence electrons does sodium have? 1 (USRG:38,1,1)

1012. How many electrons does a sodium ion have? 10 (USRG:38,1,1)

1013. What happens when a sodium atom oxidizes? It loses an electron and becomes a sodium ion. (USRG:38,1,1)

1014. What is the loss of electrons termed? oxidation (USRG:38,1,1)

1015. What is the gain of electrons termed? reduction (USRG:38,1,1)

1016. How many electrons does silver have? 47 (USRG:38,1,1)

1017. How many electrons does a silver ion have? 46 (USRG:38,1,1)

1018. During what process does silver become a silver ion? oxidation (USRG:38,1,1)


Na + Ag+ → Na+ + Ag?

redox (USRG:38,1,1)

1020. What type of reactions run batteries? redox (USRG:38,1,2)

1021. What is an oxidation number? the number of electrons that must be added to an ion to produce a neutral atom (USRG:38,1,3)

1022. What is the oxidation number of

Ag in AgCl?

+1 (USRG:38,1,4)


Cl in AgCl?

‐1 (USRG:38,1,4)


Al in Al2O3?

+3 (USRG:38,1,4)


O in Al2O3?

‐2 (USRG:38,1,4)


Na in its natural state?

0 (USRG:38,2,1)


H in most compounds?

+1 (USRG:38,2,1)


IV Reactions


group I elements in most compounds?

+1 (USRG:38,2,1)


oxygen in most compounds?

‐2 (USRG:38,2,1)


neutral atoms in most compounds?

0 (USRG:38,2,1)

1031. What is the sum of oxidation states

in neutral molecules?

0 (USRG:38,2,1)


in polyatomic ions?

the charge of the ion (USRG:38,2,1)


in water?

0 (USRG:38,2,1)


in NH4+?

+1 (USRG:38,2,1)


in O2?

0 (USRG:38,2,1)

1036. What is the oxidation number

of K in KMnO4?

+1 (USRG:38,2,6)


of O in KMnO4?

‐2 (USRG:38,2,2)


of Mn in KMnO4?

+7 (USRG:38,2,2)

1039. True/False: Electrons are conserved in redox reactions. True; electrons are conserved in all non‐beta decay reactions. (USRG:39,1,1)

1040. What is equal to the number of electrons freed in a redox reaction?

the number of electrons used by another element (USRG:39,1,1)

1041. How are redox reactions simplified? They are split into half reactions. (USRG:39,1,2)

1042. What are the two half reactions in a redox reaction? the reduction half‐reaction and the oxidation half‐reaction (USRG:39,1,2)

1043. Why might a half reaction need to be multiplied by a constant?

so that the total number of electrons is conserved when the half reaction is added to another half reaction to form a

complete reaction (USRG:39,1,2)


Cu+2Ag → Cu+2+2Ag?

a redox reaction (USRG:39,1,3)

1045. What two half reactions form the reaction

Cu+2Ag+ → Cu+2+2Ag?

Cu → Cu2++2e‐

and

Ag++1e‐ → Ag (USRG:39,1,3)

1046. Which half reaction needs to be multiplied by a constant to balance the reaction

Cu+2Ag+ → Cu+2+2Ag?

Ag++1e‐ → Ag (USRG:39,1,3)


IV Reactions

1047. What process creates the lustrous parts of cars? chrome plating (USRG:39,1,6)

1048. According to the official curriculum, what is the most commonly used type of electroplating?

chrome plating (USRG:39,1,6)

1049. In what units are cell potentials measured? volts (USRG:39,1,7)

1050. What concept lies behind the energy in batteries? cell potential (USRG:39,1,7)

1051. What element is Cu? copper (USRG:39,1,3)

1052. What element is Ag? silver (USRG:39,1,3)

1053. What does a cell potential represent? the cellʹs ability to do work (USRG:39,1,7)

1054. What is the term for a positive ion in a redox reaction? cation (USRG:39,1,0)

1055. What is the term for the negative ion in a redox reaction?

anion (USRG:39,1,0)

1056. What has happened to a battery when its redox reaction is complete?

It has run down. (USRG:39,2,0)

1057. What is the potential energy of the half reaction

F2(g)+2e‐ → 2F‐ (aq)?

+2.87 V (USRG:39,2,diagram)


Cl2(g)+2e‐ → 2Cl‐(aq)?

+1.36V (USRG:39,2,diagram)


MnO2(s)+4H+(aq)+2e‐ → Mn2+(aq)+2H2O(l)?



NO3‐(aq)+4H+(aq)+3e‐ → NO(g)+2H2O(l)?



Ag+(aq)+e‐ → Ag(s)?



Fe3+(aq)+e‐ → Fe2+(aq)?



O2(g)+2H2O(l)+4e‐ → 4OH‐(aq)?



Cu2+(aq)+2e‐ → Cu(s)?



2H+(aq)+2e‐ → H2(g)?

0.0V (USRG:39,2,diagram)


N2(g)+5H+(aq)+4e‐ → N2H5+(aq)?

‐0.23V (USRG:39,2,diagram)


Fe2+(aq)+2e‐ → Fe(s)?



Zn2+(aq)+2e‐ → Zn(s)?


1069. Under what pressure is the value for the potential energy of a half reaction generally calculated?

1 atm (USRG:39,2,1)


IV Reactions

1070. With what type of solution is the value for the potential energy of a half reaction generally calculated?

a 1 molar solution of the ion in question (USRG:39,2,1)

1071. What happens to the potential of a half reaction when the direction of the reaction reverses?

It becomes equal in magnitude, but opposite in sign. (USRG:39,2,2)


2H2O(l)+2e‐ → H2(g)+2OH‐(aq)?



Na+(aq)+e‐ → Na(s)?



Li+(aq)+e‐ → Li(s)?


1075. What element is Li? lithium (USRG:55)

1076. What half reaction provides the standard from which the potential energies of all half reactions are measured?

2H+(aq)+2e‐ → H2(g) (USRG:39,2,1)

1077. Given the potential energies for two half reactions, how can a chemist calculate the voltage of a complete reaction?

by subtracting the potential energy of the oxidation half reaction from the potential energy of the reduction half

reaction (USRG:39,2,3)

1078. If the total voltage of a complete reaction is positive, in what direction will the reaction proceed?

In the same direction as it is written. (USRG:39,2,4)

1079. Where can one attach a voltmeter in a galvanic cell in order to measure the potential of a redox reaction?

between the two strips of metal immersed in their solution (USRG:40,1,diagram)

1080. In a galvanic cell, what is the term for the tube of solution that connects the two containers of aqueous solutions?

a salt bridge (USRG:40,1,diagram)

1081. True/False: The reaction

Cu+2Ag+ → Cu2++2Ag

is spontaneous.

True; this reaction will proceed as written. (USRG:40,1,1)

1082. Under what circumstances will a reaction occur spontaneously?

when its total potential is positive (USRG:40,1,1)

1083. What is the term for the electrode in a galvanic cell in which a reduction reaction takes place?

cathode (USRG:40,2,2)

1084. What is the term for the electrode in a galvanic cell in which an oxidation reaction takes place?

anode (USRG:40,2,2)

1085. In the reaction

Zn(s)+Cu2+(aq) → Zn2+(aq)+Cu(s),

what element is being oxidized?

zinc (USRG:40,1,diagram)

1086. What is the potential energy of the reaction

Cu+2Ag+ → Cu2++2Ag?

+0.46V (USRG:40,1,1)


Li+Fe3+ → Li++Fe2+?

+2.28V (USRG:40,2,2)


IV Reactions

1088. What solution is at the anode of a galvanic cell in which the reaction

Zn(s)+Cu2+ → Zn2+(aq)+Cu(s)?

aqueous Zn2+ (USRG:40,1,diagram)

1089. What anion is in the salt bridge of the galvanic cell depicted in the guide in which the reaction

Zn(s)+Cu2+(aq) → Zn2+(aq)+Cu(s)

is taking place?

SO42‐ (USRG:40,1,diagram)

1090. In what year was the earliest reliable battery created? 1836 (USRG:40,2,3)

1091. Who invented the first reliable battery? J. F. Daniell (USRG:40,2,3)

1092. What was the overall cell potential of the first reliable battery?

+1.10V (USRG:40,2,3)

1093. What redox reaction fueled the first reliable battery? Zn(s)+Cu2+(aq) → Zn2+(aq)+Cu(s) (USRG:40,2,3)

1094. What is the term given a cell in which a voltage is applied to make the reaction proceed in a non‐spontaneous direction?

an electrolytic cell (USRG:40,2,4)

1095. What is the term for the process in which an external voltage is applied to a redox reaction to make it proceed in a non‐spontaneous direction?

electrolysis (USRG:40,2,4)

1096. How large of an external voltage must be applied to an electrolytic cell to make it effective?

one larger in magnitude than the total potential of the redox reaction (USRG:40,2,4)

1097. What industry has developed around the concept of applying a voltage to a redox reaction in order to make it proceed in a non‐spontaneous reaction?

electroplating (USRG:40,2,4)

1098. What spontaneous reaction is commonly used for zinc plating in industry?

Zn → Zn2++2e‐ (USRG:40,2,4)

1099. What color finish results from electroplating silver with platinum?

silver gray (USIRG:28,2,2)

1100. What practical advantage accompanies coating silver with platinum?

The finish resists corrosion. (USIRG:28,2,2)

1101. What sort of instruments is often coated with platinum?

surgical instruments (USIRG:28,2,2)

1102. What practical advantages accompany plating a car with chromium?

The finish provides hardness, corrosion resistance, wear resistance, and a more attractive appearance. (USIRG:28,1,4)

1103. Aside from the automobile industry, what industry frequently plates its products with chromium?

the aerospace industry (USIRG:28,1,4)

1104. What element produces finishes that are often mistakenly called ʺwhite goldʺ?

palladium (USIRG:28,2,2)

1105. Of what nation was Michael Faraday? Britain (USIRG:28,2,3)

1106. For what practical reason is silver sometimes plated with rhodium?

It prevents tarnishing. (USIRG:28,2,2)

1107. What color finish is characteristic of rhodium? white (USIRG:28,2,2)


IV Reactions

1108. What is the electrical charge of one Faraday? the charge of one mole of electrons (USIRG:28,2,3)

1109. Why did Michael Faraday have a unit of electrical charge named after him?

He discovered the amount of electrons necessary to convert one mole of the silver ion Ag+ to one mole of silver.

(USIRG:28,2,3)

1110. What is the current standard unit for electrical charge? coulombs (USIRG:28,2,3)

1111. How many coulombs are in one Faraday? 96,500 (USIRG:28,2,3)

1112. Where does the aerospace industry tend to use gold plating?

on exposed parts of rockets and space shuttles (USIRG:28,1,5)

1113. For what purpose does the aerospace industry use gold plating?

It prevents the parts from reacting with chemicals on Earth and other planets. (USIRG:28,1,5)

1114. Why do gold plated rocket components tend to stay cooler?

gold reflects solar radiation (USIRG:28,1,5)

1115. Approximately how many kilograms of gold were used in the construction of the space shuttle Columbia?

41 (USIRG:28,1,5)

1116. How many times longer than regular automobile parts do chromium‐plated parts generally last?

10 (USIRG:28,1,5)

1117. What eight metals does the official curriculum mention as being frequently used in electroplating?

palladium, nickel, platinum, copper, silver, gold, rhodium, and chromium (USIRG:28,1,5)

1118. According to the official curriculum, what material has replaced many parts that used to be plated?

stainless steel (USIRG:28,2,2)

1119. How many Faradays are necessary to plate one mole of chromium?

3 (USIRG:28,2,3)

1120. What materials does a rhodium finish effectively resist? body oils (USIRG:28,2,2)

1121. On what objects are palladium finishes frequently used?

expensive watches (USIRG:28,2,2)

1122. In what year was Michael Faraday born? 1791 (USIRG:28,2,3)

1123. How many coulombs of charge are on one electron? 1.6∙10‐19 (http://www.windows.ucar.edu/tour/link=/physical_science/p

hysics/atom_particle/electron.html)

1124. How much energy is necessary to create 52 grams of chromium plate?

579 kilojoules (USIRG:28,2,3)

1125. What sort of cutlery was often plated with silver? iron cutlery (USIRG:28,2,2)

1126. What was a common problem with silver‐plated cutlery?

It required frequent polishing. (USIRG:28,2,2)

1127. What type of ions is in the solution through which a current is passed during the process of electroplating?

cations (USIRG:28,2,2)

1128. What were the two occupations of Michael Faraday? physicist and chemist (USIRG:28,2,3)

1129. In what year was Walther Nernst born? 1864 (USIRG:29,1,1)

1130. In what nation was Walther Nernst born? Prussia (http://nobelprize.org/nobel_prize/chemistry/laureates/1920/n

ernst‐bio.html)

1131. What is the most fundamental form of the Nernst equation?

E = E0 ‐ RTlnQ/(nF) (USIRG:29,1,2)


IV Reactions

1132. What does the symbol F represent in the Nernst equation?

the Faraday constant (USIRG:29,1,3)

1133. What is the most useful form of the Nernst equation? E = E0 ‐ (0.0592log Q)/n (USIRG:29,1,3)

1134. What does the symbol E0 represent in the Nernst equation?

the standard state potential of the galvanic cell at 298 K (USIRG:29,1,4)

1135. What is the purpose of the Nernst equation? to determine the potential of galvanic cells under nonstandard conditions (USIRG:29,1,2)

1136. What surrounding temperature is assumed in the most useful form of the Nernst equation?

298K (USIRG:29,1,3)

1137. In the most fundamental form of the Nernst equation, what does the symbol R represent?

the universal gas constant (http://www.statemaster.com/encyclopedia/Nernst‐equation)

1138. In the Nernst equation, what does the symbol n represent?

the number of moles of electrons transferred per unit reaction (USIRG:29,1,4)

1139. What does the symbol E represent in the Nernst equation?

the potential of the cell under certain nonstandard conditions (USIRG:29,1,4)

1140. In the Nernst equation, what does the symbol Q represent?

the ratio of product concentrations to reactant concentrations (USIRG:29,1,4)

1141. What are the units of n in the Nernst equation? moles per mole (USIRG:29,1,4)

1142. What temperature is assumed in the value of E0? 298K (USIRG:29,1,4)

1143. What is the value of n in the equation

Zn(s)+Cu2+(aq) → Zn2+(aq)+Cu(s)?

2 (USIRG:29,1,5)

1144. What is a concentration cell? a galvanic cell that has the same chemical in each compartment, but still has a voltage because of different

concentrations in each compartment (USIRG:29,2,1)



when the concentration of Zn2+(aq) is 0.50 M and the concentration of Cu2+(aq) is 0.10 M?

+1.08V (USIRG:29,2,1)



in standard concentrations at the temperature 873K?

+1.10V (USIRG:29,2,1)


Li+Fe3+ → Li++Fe2+

when the concentration of Fe3+ is 0.60 M and the concentration of Li+ is 1.30 M?

+2.26V (USIRG:29,2,1)


Li+Fe3+ → Li++Fe2+

in standard concentrations at the temperature 410K?

+2.28V (USIRG:29,2,1)

1149. What is stoichiometry? the practice of using a balanced equation to keep track of the amounts of chemical substances changing from one

compound to another in a reaction (USRG:41,1,2)

1150. What are the units used in a balanced equation? moles (USRG:41,1,3)


IV Reactions

1151. What is the balanced equation for hydrogen burning in air to produce water?

2H2+O2 → 2H2O (USRG:41,1,3)

1152. How many moles of water result from two moles of hydrogen burning in air?

2 (USRG:41,1,4)

1153. What is the molar mass of water? 18 grams/mole (USRG:41,2,4)

1154. How many moles of oxygen are necessary to produce one mole of water?

1/2 (USRG:41,1,4)

1155. How does stoichiometry resemble accounting? Accounting involves keeping track of dollars going in and out of a bank account in a manner similar to the way that

stoichiometry tracks compounds in a reaction. (USRG:41,1,2)

1156. What type of equations omits spectator ions? a net ionic equation (USRG:41,2,0)

1157. What is the formula for silver nitrate? AgNO3 (USRG:41,2,1)

1158. What is the formula for sodium sulfide? Na2S (USRG:41,2,1)

1159. What are the ionic products of aqueous MgCl2? Mg2+ and 2Cl‐ (USRG:41,2,0)

1160. What aqueous solution results from mixing a solution of sodium sulfide with a solution of silver nitrate?

sodium nitrate (USRG:41,2,1)

1161. What precipitate results from mixing a solution of sodium sulfide with a solution of silver nitrate?

silver sulfide (USRG:41,2,1)

1162. How many moles of precipitate result from mixing a solution of sodium sulfide with a solution of silver nitrate?

1 (USRG:41,2,1)

1163. How many moles of ions result from mixing a solution of sodium sulfide with a solution of silver nitrate?

4 (USRG:41,2,1)

1164. What are the spectator ions in the balanced equation

2AgNO3(aq)+Na2S(aq) → 2NaNO3(aq)+Ag2S(s)?

NO3‐ and Na+ (USRG:41,2,1)

1165. What is the net ionic equation for mixing a solution of sodium sulfide with a solution of silver nitrate?

2Ag++S2‐ → Ag2S(s) (USRG:41,2,1)

1166. What do chemists use to balance redox reactions? half‐reactions (USRG:41,2,2)

1167. What are empirical formulas? the lowest mole ratio of atoms in a molecule (USRG:41,2,3)

1168. What is the empirical formula for water? H2O (USRG:41,2,3)

1169. What is the empirical formula for acetylene? CH (USRG:41,2,3)

1170. What is the molecular formula for acetylene? C2H2 (USRG:41,2,3)

1171. True/False: CH is a stable molecule. False; CH is not a stable molecule. (USRG:41,2,3)

1172. With what units of measurement do balance chemical equations when they are trying to create measurable yields?

They use molar masses. (USRG:41,2,4)

1173. How many grams of water result from burning 4 grams of hydrogen in unlimited oxygen?

36 (USRG:41,2,4)

1174. What is a limiting reactant? a reactant that exists in limited amounts and thus controls the amount of products (USRG:41,2,5)


IV Reactions

1175. Under what circumstances is determining the limiting reactant important?

when exact stoichiometric amounts of reactants are absent (USRG:41,2,5)

1176. What is the molar mass of oxygen gas? 32 grams/mole (USRG:41,2,4)

1177. How many moles of hydrogen gas are in 12 grams of H2?

6 (USRG:42,1,1)

1178. What is the limiting reagent when 12 grams of H2 burns in 32 grams of O2?

oxygen (USRG:42,1,1)

1179. How many moles of excess reactant remain when 12 grams of H2 burns in 32 grams of O2?

4 (USRG:42,1,1)

1180. How many grams of product result from burning 12 grams of H2 in 32 grams of O2?

36 (USRG:42,1,1)

1181. What is the term for the speed at which a reaction takes place?

the reaction rate (USRG:42,1,4)

1182. What is happening when a reaction is at equilibrium? the rate of the forward reaction is the same as that of the reverse reaction (USRG:42,1,4)

1183. What symbol do chemists use to indicate a reaction can proceed in both the forward and the reverse direction?

a double headed arrow (USRG:42,1,4)

1184. True/False: Chemical reactions proceed in reverse as product is formed.

True; reactions proceed in both directions to achieve equilibrium. (USRG:42,1,2)

1185. How do chemists determine the equilibrium constant of a reaction?

They multiply the equilibrium concentrations of its products, then divide the product by the product of the equilibrium

concentrations of its reactants. (USRG:42,1,2)

1186. What expression do chemists use to calculate an equilibrium constant?

equilibrium constant expression (USRG:42,1,2)

1187. What symbol denotes the equilibrium constant of a reaction?

K (USRG:42,2,1)

1188. What is the equilibrium constant for the reaction

A+B → C+D?

[C][D]/[A][B] (USRG:42,2,1)

1189. What is the K expression for the reaction

A+B→2C?

[C]2/[A][B] (USRG:42,2,2)

1190. What symbol is used for the equilibrium expression of a reaction involving acids?

Ka (USRG:42,2,4)

1191. What symbol is used for the equilibrium expression of a reaction involving bases?

Kb (USRG:42,2,4)

1192. What symbol is used for the equilibrium expression of a reaction involving gases?

KP (USRG:42,2,4)

1193. What symbol is used for the equilibrium expression of a reaction that forms a precipitate?

KSP (USRG:42,2,4)

1194. What symbol is used for the equilibrium expression of a reaction that involves solutions and concentrations?

KC (USRG:42,2,4)

1195. What does the value of an equilibrium constant indicate?

how far the reaction will proceed in a certain direction (USRG:42,2,5)


IV Reactions


3Y+4X → Z?

[Z]/[Y]3[X]4 (USRG:42,2,3)


H → 6I+2J?

[I]6[J]2/[H] (USRG:42,2,3)

1198. What is the KC expression for the reaction

aA+bB → cC+dD,

with a, b, c, and d being constants?

[C]c[D]d/[A]a[B]b (USRG:42,2,3)

1199. What does an equilibrium constant greater than 1 indicate about a reaction?

At equilibrium, products will exceed reactants. (USRG:42,2,5)

1200. What does an equilibrium constant less than 1 indicate about a reaction?

At equilibrium, reactants will exceed products. (USRG:42,2,5 )

1201. What does the symbol [A] represent when calculating equilibrium expressions?

the concentration of substance A (USRG:42,2,6)

1202. What units do chemists use to measure concentrations when they calculate the equilibrium expression of a reaction?

moles per liter (molarity) (USRG:42,2,6)

1203. What happens to substances that are pure solids during calculations of an equilibrium expression for a reaction?

Pure solids are not factored into the expression. (USRG:42,2,6)

1204. What happens to substances that are pure liquids during calculations of equilibrium expression?

Pure liquids are not factored into the expression. (USRG:42,2,6)

1205. Why are pure solids and pure liquids treated differently than other substances in calculations of equilibrium expressions?

The concentrations of these substances themselves do not change. (USRG:42,2,6)

1206. When calculating the equilibrium expression for a gas, what does the symbol PC indicate?

the pressure of the gas C (USRG:43,1,1)

1207. In the equation used to convert from a KC value to a KP value, what does the symbol Δn represent?

the total change in the number of moles of gas in the reaction (total products ‐ total reactants) (USRG:43,1,2)

1208. What equation is used to convert from a KC value to a KP value?

KP = KC(RT)Δn (USRG:43,1,2)

1209. Under what circumstances will KC equal KP? when the number of moles of gas does not change during the reaction (USRG:43,1,2)

1210. What is the KP expression for the reaction

aA+bB → cC+dD,

with a, b, c, and d being constants?

PCcPDd/PAaPBb (USRG:43,1,2)

1211. What ion is always involved in acid reactions? H+ (USRG:43,1,3)

1212. What does a small Ka constant indicate about the strength of an acid?

The acid is weak. (USRG:43,1,3)

1213. What does a small Kb constant indicate about the strength of a base?

The base is weak. (USRG:43,1,3)

1214. What is the formula for acetic acid? HC2H3O2 (USRG:43,1,4)


IV Reactions

1215. What is the Ka expression for acetic acid in water? Ka= [H+][ C2H3O2‐ ]/[ HC2H3O2] (USRG:43,1,4)

1216. What is the value of the Ka constant for vinegar? 1.8 x 10‐5 (USRG:43,1,5)

1217. What equation is used to calculate the pH of a solution, given its concentration of H+ ions?

pH= ‐log[H+] (USRG:43,1,5)

1218. True/False: Acetic acid is a strong acid. False; acetic acid does not fully dissociate in solution. (USRG:43,1,5)

1219. What is the Kb expression for the reaction

NH3+H2O → NH4++OH‐?

[NH4+][ OH‐]/[ NH3] (USRG:43,1,5)

1220. What is NH3? ammonia (USRG:43,1,5)

1221. What is the Kb value for the reaction

NH3+H2O → NH4++OH‐?

1.8 x 10‐5 (USRG:43,1,5)

1222. What type of base is NH3? a weak base (USRG:43,1,5)

1223. What do the values of KSP constants indicate about reactions?

how much a solid will ionize in a solution (USRG:43,1,6)

1224. What is the KSP expression for the reaction

AgCl(s) → Ag+ (aq)+ Cl‐ (aq)?

[Ag+][Cl‐] (USRG:43,1,6)

1225. What is the value of the KSP constant for the reaction

AgCl(s) → Ag+ (aq)+ Cl‐ (aq)?

1 x 10‐10 (USRG:43,1,6)

1226. What compound is indicated by the formula AgCl(s)? silver chloride (USRG:43,1,6)

1227. True/False: Silver chloride is a soluble substance. False; silver chloride is practically insoluble. (USRG:43,2,0)

1228. What does a small KSP constant indicate about a substance?

The substance is insoluble. (USRG:43,2,0)

1229. What purpose can a KSP constant serve in a precipitation reaction?

It predicts how much precipitate will be formed. (USRG:43,2,1)

1230. With what subjects is the field of kinetics concerned? the rates of various reactions and what affects the rates of reactions (USRG:43,2,2)

1231. What type of equation is a rate law? an algebraic equation (USRG:43,2,2)

1232. What is necessary to determine a rate law? experimental evidence about a reaction (USRG:43,2,2)

1233. What information is indicated in a rate law? the way in which changing the concentration of a reaction will affect how fast the reaction will happen (USRG:43,2,2)

1234. True/False: All precipitation reactions have the same rate law.

False; no reactions have the same rate law. (USRG:43,2,2)

1235. How is the average rate of a reaction calculated? by measuring the change in the concentration of the reactants over a set unit of time (USRG:43,2,3)

1236. How is the instantaneous rate of a reaction calculated? by graphing the concentration of the reactant versus time and then taking the slope of lines tangent to the graph at certain

points (USRG:43,2,3)

1237. In what units is the rate of a reaction measured? moles per liter per second (USRG:43,2,3)


IV Reactions

1238. Under what circumstances will the average rate of a reaction differ from the instantaneous rate of a reaction?

when the instantaneous rate of a reaction is changing as the reaction progresses (USRG:43,2,3)

1239. What does the symbol Ea represent? the activation energy of a reaction (USRG:44,1,diagram)

1240. What does the symbol ΔG represent? the free energy change of a reaction (USRG:44,1,diagram)

1241. According to the official curriculum, what is the best model for chemical reactions?

the collision model (USRG:44,1,1)

1242. According to the official curriculum, what model is similar to the best model for chemical reactions?

the Kinetic Theory (USRG:44,1,1)

1243. What is the premise of the best model for chemical reactions?

molecules must collide in order to react (USRG:44,1,1)

1244. How does increasing the temperature of a reaction generally affect the rate of that reaction?

It increases the rate of the reaction. (USRG:44,1,1)

1245. How does increasing the surface area of an Alka‐Seltzer tablet affect the rate at which it reacts with the water around it?

It increases the rate at which it reacts with water. (USRG:44,1,2)

1246. How does increasing the concentration of a solution generally affect the rate of a reaction?

It increases the rate of the reaction. (USRG:44,1,3)

1247. According to the official curriculum, what is necessary for a reaction to occur?

reacting molecules must collide with a certain amount of energy (USRG:44,1,4)

1248. Why does increasing the surface area of a solid dissolving in water affect the rate at which that solid reacts with the water?

because the solid has more surface area that can collide with water molecules (USRG:44,1,2)

1249. To what does the term ʺactivation energyʺ refer? the energy necessary for collisions between molecules to result in a reaction (USRG:44,1,4)

1250. What is shown on a potential energy diagram? the specific energy of a collection of chemicals before and after a reaction (USRG:44,1,4)

1251. On a potential energy diagram, what is plotted on the horizontal axis?

the progress of the reaction (USRG:44,1,4)

1252. On a potential energy diagram, what is plotted on the vertical axis?

free energy (USRG:44,1,diagram)

1253. True/False: The products of a chemical reaction generally have about the same amount of free energy as the reactants.

False; all reactions involve energy changes. (USRG:44,1,diagram)

1254. What aspect of a reaction most affects the rate at which it will proceed?

the size of its activation energy (USRG:44,2,1)

1255. What is the relationship between the activation energy of a reaction and the rate of a reaction?

as the activation energy of a reaction increases, the rate at which it progresses decreases (USRG:44,2,1)

1256. What is a catalyst? a substance that provides a lower energy pathway for a given reaction (USRG:44,2,2)

1257. How does a catalyst change the rate at which a reaction proceeds?

It speeds up the progress of the reaction. (USRG:44,2,2)


IV Reactions

1258. True/False: A reaction that proceeds with the help of a catalyst must end with the same ratio of products and reactants as it would without a catalyst.

False; if a catalyst lowers the activation energy for a reaction in one direction, but not in another, the equilibrium ratio of

the reaction will be different. (USRG:44,2,2)

1259. What SI unit measures the catalytic activity of a catalyst?

the katal (USRG:44,2,3)

1260. What is the term for catalysts in the human body? enzymes (USRG:44,2,3)

1261. What does the field of thermochemistry concern? measuring energy changes in chemical reactions (USRG:44,2,4)

1262. What forms the basis of the study of thermodynamics? the ideas of energy and temperature in the Kinetic Molecular Theory (USRG:44,2,4)

1263. What can study of thermodynamics ultimately explain? whether a reaction will ultimately occur (USRG:44,2,4)

1264. In thermodynamics, what term is used for the reaction a chemist is studying?

the system (USRG:44,2,4)

1265. In thermodynamics, what term is used for the universe outside of the reaction a chemist is studying?

the surroundings (USRG:44,2,4)

1266. What must be understood in order for the laws of thermodynamics to make sense?

the movement of matter and energy between a system and its surroundings (USRG:44,2,4)

1267. What are endothermic reactions? reactions that have a net absorption of heat (USRG:45,1,1)

1268. What are exothermic reactions? reactions that have a net release of heat (USRG:45,1,1)

1269. How does a catalyst affect the degree to which a reaction is endothermic or exothermic?

It has no effect on the degree to which a reaction is endothermic or exothermic, because it does not change the

energy level of the products of a reaction. (USRG:45,1,1)

1270. How does the energy of the products of an exothermic reaction compare to the energy of its reactants?

It is lower. (USRG:45,1,1)

1271. How does the energy of the products of an endothermic reaction compare to the energy of its reactants?

It is higher. (USRG:45,1,1)

1272. What are state functions? properties of a system that are determined by where it is, not how it arrived there (USRG:45,1,2)

1273. What are three examples of state functions? volume, pressure, and energy (USRG:45,1,2)

1274. What symbol do chemists use to indicate the amount of change in a state function?

Δ, also known as ʺdeltaʺ (USRG:45,1,2)

1275. What does the symbol H represent? the enthalpy of a system (USRG:45,1,3)

1276. What sort of function is enthalpy? a state function (USRG:45,1,3)

1277. What is enthalpy? the energy content of a system measured by the heat given off or taken in by that system (USRG:45,1,3)

1278. To what parts of a reaction is enthalpy generally assigned?

individual chemical substances (USRG:45,1,3)

1279. What is the relationship between the amount of a substance undergoing a reaction and its enthalpy?

direct proportionality (USRG:45,1,3)

1280. In what units is enthalpy generally measured? kilojoules (USRG:45,1,3)


IV Reactions

1281. How much energy is given off as heat when one mole of coal becomes one mole of carbon dioxide?

393.5 kilojoules (USRG:45,1,4)

1282. What is the ʺheat of reactionʺ? the amount of energy released as heat during a chemical reaction (USRG:45,1,4)

1283. What symbol is used for a compoundʹs heat of formation?

ΔHformation (USRG:45,2,0)

1284. What is a compoundʹs heat of formation? the enthalpy change that occurs when one mole of a compound is formed from its elements in standard conditions

(USRG:45,2,0)

1285. What is calorimetry? the process by which enthalpy changes are measured (USRG:45,2,1)

1286. In calorimetry, against what standard is the change in temperature of a reacting mixture measured?

the change in temperature of the same mass of pure water as heat is added from a burner (USRG:45,2,1)

1287. How many joules of heat does it take to raise the temperature of one gram of water one degree Celsius?

4.18 (USRG:45,2,1)

1288. What is the definition of a calorie? the energy needed to raise one gram of water one degree Celsius (USRG:45,2,1)

1289. Who formulated Hessʹ Law? Germain Hess (USIRG:30,1,1)

1290. In what year was the creator of Hessʹ Law born? 1802 (USIRG:30,1,1)

1291. What is the premise of Hessʹ Law? the total heat created or absorbed in a chemical reaction is the same whether the reaction takes place in one step or in several

steps (USIRG:30,1,1)

1292. What is another name for Hessʹ Law? the law of constant heat summation (USIRG:30,1,1)

1293. What is the formula for carbon monoxide? CO (USIRG:30,1,2)

1294. What is the enthalpy of formation for carbon monoxide?

‐110 kJ/mol (USIRG:30,2,3)

1295. What is the reaction equation for the formation of carbon monoxide?

C(s)+ ½O2(g) → CO(g) (USIRG:30,2,0)

1296. What is the enthalpy of formation for carbon dioxide? ‐393 kJ/mol (USIRG:30,2,2)

1297. What is the reaction equation for the formation of carbon dioxide?

C(s)+O2 (g) → CO2(g) (USIRG:30,2,2)

1298. What does the negative enthalpy of formation for carbon monoxide indicate about the reaction?

It is exothermic. (USIRG:30,2,3)

1299. What is the enthalpy of oxidation for carbon monoxide becoming carbon dioxide?

‐283 kJ/mol (USIRG:30,2,2)

1300. Why do chemists subtract the enthalpy of oxidation for CO2 from the enthalpy of formation of CO2 to get the enthalpy of formation for CO?

To get from CO2 to CO, chemists must reverse the reaction in which CO is oxidized to form CO2, so that the product of this reaction is CO; since the reaction is reversed, its enthalpy is

subtracted from the enthalpy of formation for CO2. (USIRG:30,2,2)

1301. On what basic principle does Hessʹ law depend? the conservation of energy (USIRG:30,1,1)


IV Reactions

1302. How does Hessʹ Law allow chemists to find the enthalpy of formation for certain compounds without observing that reaction directly?

It allows them to calculate the enthalpy of formation for those compounds by calculating the enthalpy of a series of indirect

steps towards those compounds. (USIRG:30,1,1)

1303. In what nation was the formulator of Hessʹ Law born? Switzerland (http://www.cartage.org.lb/en/themes/ Biographies/MainBiographies/H/Hess/1.html)

1304. What is entropy? the energy associated with disorder (USRG:45,2,2)

1305. What is the symbol for entropy? S (USRG:45,2,2)

1306. With what is the second law of thermodynamics concerned?

the increasing entropy of the universe (USRG:45,2,2)

1307. Why did chemists conceive of the concept of entropy? because enthalpy alone could not account for all the physical and chemical changes of matter (USRG:45,2,2)

1308. What substances are more ordered than gases but less ordered than liquids?

solutions (USRG:45,2,3)

1309. What results from all natural processes? increased entropy (USRG:45,2,3)

1310. Why can some chemical reactions result in an increase in system order despite the second law of thermodynamics?

A decrease in order also takes place outside of the system. (USRG:45,2,3)

1311. What was J.W. Gibbsʹs nation of origin? the United States (USRG:45,2,4)

1312. What was the occupation of J.W. Gibbs? a chemist (USRG:45,2,4)

1313. What two factors determine whether a chemical reaction will occur?

its enthalpy and its entropy (USRG:45,2,4)

1314. True/False: Entropy is a state function. True; a change in entropy is denoted by the symbol ΔS. (USRG:45,2,4)

1315. Why is keeping track of the signs of ΔS and ΔH important when determining whether or not a reaction will occur?

Changes in enthalpy and entropy can be both positive and negative. (USRG:45,2,4)

1316. What sort of function is Gibbs Free Energy? a state function (USRG:45,2,4)

1317. What formula determines whether a reaction will take place spontaneously?

ΔG=ΔH ‐ TΔS (USRG:46,1,0)

1318. In the formula that determines whether a reaction will take place, what does T represent?

the temperature of the system in Kelvin (USRG:46,1,1)

1319. If both the entropy and the enthalpy of a reaction are positive, under what circumstances will it occur spontaneously?

high temperatures (USRG:46,0,diagram)

1320. If both the entropy and the enthalpy of a reaction are negative, under what circumstances will it occur spontaneously?

low temperatures (USRG:46,0,diagram)

1321. True/False: 2HgO(s) → O2(g)+2Hg(l)

occurs spontaneously at high temperatures.

True; for this reaction, both the entropy and enthalpy are positive. (USRG:46,0,diagram)

1322. True/False: NH3(g)+HCl(g) → NH4Cl(s)

occurs spontaneously at high temperatures.

False; this reaction occurs spontaneously at low temperatures. (USRG:46,0,diagram)


IV Reactions

1323. Under what circumstances will a reaction occur spontaneously if it has a negative entropy but a positive enthalpy?

It will not occur, but the reverse reaction will be spontaneous at all temperatures. (USRG:46,0,diagram)

1324. Under what circumstances will a reaction occur spontaneously if it has a negative enthalpy but a positive entropy?

all temperatures (USRG:46,0,diagram)

1325. Under what circumstances will the reaction

3O2 → 2O3 occur spontaneously?

none; but the reverse reaction is spontaneous at all temperatures (USRG:46,0,diagram)


2H2O2 → 2H2O+O2

occur spontaneously?

all temperatures (USRG:46,0,diagram)


O2(g)+2Hg(l) → 2HgO(s)


low temperatures (USRG:46,0,diagram)

1328. Under what circumstances will the spontaneity of a reaction depend on temperature?

when its enthalpy and entropy are of the same sign (USRG:46,0,diagram)

1329. In what direction will a reaction proceed if its change in free energy is negative, its equilibrium constant is less than one, and its cell potential is positive?

toward the products (USRG:46,1,diagram)

1330. In what state is a reaction that has an equilibrium constant of one and a cell potential and Gibbs Free Energy of zero?

equilibrium (USRG:46,1,diagram)

1331. In what direction will a reaction proceed if its change in free energy is positive, its equilibrium constant is greater than one, and its cell potential is negative?

toward the reactants (USRG:46,1,diagram)

1332. What happens to the cell potential of a reaction as it approaches equilibrium?

It approaches zero. (USRG:46,2,0)

1333. What happens to the ΔG of a reaction as it approaches equilibrium?

It approaches zero. (USRG:46,2,0)

1334. What equation allows chemists to calculate the free energy of a reaction from its equilibrium constant?

ΔG0= ‐RTlnK (USRG:46,2,2)

1335. What equation allows chemists to calculate the free energy of a reaction from its cell potential?

<delta>G0= ‐nFE0cell

(USRG:46,2,2)

1336. True/False: If the cell potential of a reaction is positive, its free energy will be positive?

False; its free energy will be negative. (USRG:46,2,2)

1337. If a reaction has an equilibrium constant greater than one, what sign will its free energy be?

negative (USRG:46,2,2)


NH4Cl(s) → NH3(g)+HCl(g)


high temperatures (USRG:46,0,diagram)

1339. Which state of matter is most affected by increases in the pressure of its surroundings?

gases (USIRG:21,2,3)



1340. What is the general industrial use of supercritical CO2? a solvent (USIRG:23,1,2)

1341. What is the pressure of waterʹs triple point? 0.00603 atm (USIRG:22,1,diagram)

1342. What is the temperature of waterʹs triple point? 0.0098 ?C (USIRG:22,1,diagram)

1343. What two examples of specific industrial uses for supercritical CO2 are mentioned in the official curriculum?

making new medications and removing grease stains from clothing (USIRG:23,1,2)

1344. What happens to industrial supercritical CO2 after it boils away?

It is captured and reused. (USIRG:23,2,1)

1345. Which hydroxide compounds are soluble? those that include a group I metal (USRG:30,1,3)

1346. Which oxide compounds are soluble? those that include a group I metal (USRG:30,1,3)

1347. What was François Raoultʹs nationality? French (USIRG:23,1,3)

1348. What three examples does the official curriculum give of colligative properties?

the boiling point, freezing point, and osmotic pressure of a solution (USIRG:23,1,2)

1349. What is the molar mass of glucose? 180.16 grams/mol (USRG:55)

1350. What is the chemical formula for calcium magnesium acetate?

CaMg(CH3COO)2 (USIRG:24,1,2)

1351. What organization published a guide to purifying seawater for human and agricultural use?

the California Coastal Commission (USIRG:24,2,1)

1352. What sort of impurities can be present in distilled water but not in water treated with reverse osmosis?

volatile contaminants (USIRG:25,2,0)

1353. How many hydroxide ions are attached to glucose? 5 (USRG:30,2,diagram)

1354. What is the basic shape of a glucose molecule? a ring (USRG:30,2,diagram)

1355. What unit for volume is used in the gas laws? the liter (USIRG:21,2,3)

1356. What are the products of carbon‐10 undergoing beta plus decay?

boron‐10, 1 neutrino, and 1 positron (USIRG:17,2,4)

1357. What is the ratio of protons to neutrons in boron‐10? 1:1 (USIRG:17,2,4)

1358. Who first demonstrated that bombarding nitrogen with alpha particles creates oxygen?

Ernest Rutherford (USIRG: 18,2,2)

1359. Which isotope of uranium is used to make fission bombs?

Uranium‐235 (http://www.eoearth.org/article/Uranium)

1360. What is the most common isotope of uranium? Uranium‐238 (http://www.eoearth.org/article/Uranium)

1361. Which two isotopes were used to create fission bombs during the Manhattan project?

Uranium‐235 and Plutonium‐239 (http://nuclearweaponarchive.org/Usa/Med/Med.html)

1362. How are fission reactions used to produce electricity? The reaction produces heat, which converts water to steam, which turns the turbines of a generator. (USIRG:19,1,0)

1363. What is the balanced equation for bombarding carbon‐12 with alpha particles to create nitrogen?

126C+42He → 147N+11H (USIRG:18,2,1)

1364. What is the molecular formula for ozone? O3 (USIRG:16,1,diagram)



1365. What is the balanced equation for the fusion of deuterium with tritium?

21H+31H → 42He+10n (USIRG:18,2,diagram)

1366. What is the balanced equation for the fission of uranium to create strontium and xenon?

23592U+ 10n → 13454Xe+10038Sr+10n+10n (USIRG:18,1,diagram)

1367. What is 1 atm in mmHg? 760 mmHg (http://www.thefreedictionary.com/mm+Hg)

1368. What is the vapor pressure of water at 20°C? 17.5 mmHg (USIRG:21,2,0)

1369. What is a colloquial name for buckminsterfullerene? bucky balls (USRG:49,1,7)

1370. What reactions allow scientists to test salts for acidity in water?

reactions between the water and the cation or anion of the salt (USIRG:26,1,2)

1371. What are the products of the anion in a salt reacting with water?

the hydroxide ion and the conjugate acid of the anion (USIRG:26,2,1)

1372. What is the chemical formula for the ion associated with basic solutions?

OH‐ (USIRG:26,2,1)

1373. What are the products of the cation in a salt reacting with water?

the hydronium ion and the conjugate base of the cation (USIRG:26,2,1)

1374. What sort of solution does sodium acetate form in water?

a basic solution (USIRG:26,2,1)

1375. What reaction takes place when sodium acetate is dissolved in water?

CH3COO‐(aq)+H2O(l) → CH3COOH(aq)+OH‐(aq) (USIRG:26,2,1)

1376. What is the conjugate acid of acetate? acetic acid (USIRG:26,2,1)

1377. Why does dissolving the anion of a weak acid in water form a basic solution?

The anion pulls a hydrogen nucleus from surrounding water molecules, forming the hydroxide ion.

(USIRG:26,2,1)

1378. What type of solution is formed by dissolving the anion of a strong acid in water?

a neutral solution (USIRG:26,2,5)

1379. What type of solution is formed by dissolving the cation of a strong base in water?

a neutral solution (USIRG:26,2,5)

1380. How does the acetate anion act as a base when dissolved in water?

It accepts a proton. (USIRG:26,2,0)

1381. What type of solution is the product of dissolving in water a salt composed by the anion of a weak acid and the cation of a strong base?

a basic solution (USIRG:26,2,3)

1382. What type of solution is formed by dissolving ammonium chloride in water?

an acidic solution (USIRG:26,2,3)

1383. What ions are spectators when ammonium chloride is dissolved in water?

chloride ions (USIRG:26,2,3)

1384. What type of solution is formed by dissolving the cation of a weak base in water?

an acidic solution (USIRG:26,2,3)

1385. What reaction takes place when ammonium cations are dissolved in water?

NH4+(aq)+ H2O(l) → NH3(aq)+ H3O+(aq) (USIRG:26,2,3)

1386. What is the chemical formula for the hydronium ion? H3O+ (USIRG:26,2,3)


IV Reactions

1387. What is the main source of the compounds that react with raindrops to make them more acidic?

burning fossil fuels to generate electricity (http://www.epa.gov/acidrain/what/index.html)

1388. How does the cation of ammonium chloride act as an acid when dissolved in water?

It donates a proton to the solution. (USIRG:26,2,3)

1389. Why does the conjugate base of NH4+ not make the solution basic when NH4+ is dissolved in water?

It is a weak base that does not ionize very much. (USIRG:26,2,3)

1390. What are six cations that do not form acidic or basic solutions when dissolved in water?

Na+ , K+ , Rb+ , Cs+ , Mg2+ , Ca2+ (USIRG:26,0,table)

1391. What are six anions that do not form acidic or basic solutions when dissolved in water?

Cl‐, Br‐, I‐, ClO4‐, BrO4‐, NO3‐ (USIRG:26,0,table)

1392. What are the main compounds that contribute to acid rain?

sulfur dioxide and nitrous oxides (http://www.epa.gov/acidrain/what/index.html)

1393. What is a chemical that mercury is used to produce? chlorine (USIRG:27,2,3)

1394. What is the process by which poisons such as mercury become concentrated in the bodies of animals higher in the food chain?

biomagnification (USIRG:27,2,diagram)

1395. What is the process by which mercury suspended in the water becomes part of the air?

volatilization (USIRG:27,2,diagram)

1396. What is the process by which excess silver was removed from a photographic image made using silver halide salts?

fixing (USIRG:28,2,1)

1397. With what molecule was excess silver complexed after it was used to create images in an early photography process?

sodium thiosulfate (USIRG:28,1,1)

1398. What item can be added to a solution of silver and sodium thiosulfate to form a metallic precipitate?

steel wool (USIRG:28,1,1)

1399. Where are the alkali metals located on the periodic table?

all the elements in group 1 on the periodic table except hydrogen

(http://www.chemicalelements.com/groups/alkali.html)

1400. Where are the alkaline earth metals located on the periodic table?

all the elements in group 2 on the periodic table (http://www.chemicalelements.com/groups/alkaline.html)

1401. What is the oxidation number of all the alkali metals? +1 (http://www.chemicalelements.com/groups/alkali.html)

1402. What is the oxidation number of all the alkaline earth metals?

+2 (http://www.chemicalelements.com/groups/alkaline.html)

1403. What factor determines the oxidation number of elements that are nonmetals and elements in groups 1 and 2 on the periodic table?

the number of electrons the element would need to gain or lose to have an outer shell that resembled that of a nearest

noble gas (http://www.alonsoformula.com/inorganic/numero_oxidacion

.htm)

1404. What is the most electronegative element on the periodic table?

fluorine (http://www.green‐planet‐solar‐energy.com/electronegativity‐values.htm)

1405. What groups on the periodic table compose the transition metals?

groups 3 to 12 (http://www.dayah.com/periodic/)



1406. What are the atomic numbers of the Lathanides? 57 to 71 (http://www.dayah.com/periodic/)

1407. What are the atomic numbers of the Actinides? 89 to 103 (http://www.dayah.com/periodic/)

1408. Where are the halogens located on the periodic table? all the elements in group 17 on the periodic table (http://www.dayah.com/periodic/)

1409. What group on the periodic table are the noble gases? group 18 (http://www.dayah.com/periodic/)

1410. What is the usual oxidation number of all the halogens?

‐1 (http://www.dayah.com/periodic/)

1411. What is an alternate term for the metals in the Lathanide and Actinide series?

the rare earth metals (http://www.dayah.com/periodic/)

1412. What elements compose the halogens? fluorine, chlorine, bromine, iodine, astatine (USRG:55)

1413. What elements compose the alkali metals? lithium, sodium, potassium, rubidium, cesium, francium (USRG:55)

1414. What elements compose the alkaline earth metals? beryllium, magnesium, calcium, strontium, barium, radium (USRG:55)

1415. Which of the alkali metals are liquids in standard conditions?

cesium and francium (http://www.dayah.com/periodic/)

1416. Which of the halogens is liquid in standard conditions? bromine (http://www.dayah.com/periodic/)

1417. Which of the halogens are gases in standard conditions?

fluorine and chlorine (http://www.dayah.com/periodic/)

1418. Which of the halogens are solid in standard conditions? iodine and astatine (http://www.dayah.com/periodic/)

1419. What elements are noble gases? helium, neon, argon, krypton, xenon, radon (http://www.dayah.com/periodic/)

1420. What is name of the most massive noble gas? radon (USRG:55)

1421. What is the atomic weight of the most massive noble gas?

222 amus (USRG:55)

1422. What is the least massive noble gas? helium (USRG:55)

1423. What is the atomic weight of the least massive noble gas?

4.003 amus (USRG:55)

1424. What is the name of the least massive transition metal? scandium (USRG:55)

1425. What is the atomic number of the least massive transition metal?

21 (USRG:55)

1426. What is the name of the most massive transition metal? roentgenium (USRG:55)

1427. What is the atomic number of the most massive transition metal?

111 (USRG:55)

1428. What is the name of the most massive alkali metal? francium (USRG:55)

1429. What element is Be? beryllium (USRG:55)

1430. What element is Mg? magnesium (USRG:55)

1431. What element is K? potassium (USRG:55)

1432. What element is Cs? cesium (USRG:55)

1433. What element is Rb? rubidium (USRG:55)



1434. What element is Fr? francium (USRG:55)

1435. What element is Sr? strontium (USRG:55)

1436. What element is Ba? barium (USRG:55)

1437. What element is Ra? radium (USRG:55)

1438. What element is Ca? calcium (USRG:55)

1439. What element is B? boron (USRG:55)

1440. What element has an atomic number that is one greater than that of iron?

cobalt (USRG:55)

1441. What element has an atomic number that is one greater than that of sodium?

magnesium (USRG:55)

1442. What element has an atomic number that is one less than that of iron?

manganese (USRG:55)

1443. What element is Cr? chromium (USRG:55)

1444. What element is Mn? manganese (USRG:55)

1445. What is the name of the atomically smallest alkali metal?

lithium (USRG:55)

1446. What is the atomic mass of the atomically largest alkali metal?

223 amus (USRG:55)

1447. What is the atomic mass of the atomically smallest metal?

6.941 amus (USRG:55)

1448. What is the name of the atomically largest alkaline earth metal?

radium (USRG:55)

1449. Why are some of the masses of the elements on the periodic table given in parentheses?

because these elements have no stable isotopes‐the number given is the number of the longest‐lasting isotope

(http://www.dayah.com/periodic/)

1450. What element is Sn? tin (USRG:55)

1451. What element is Cd? cadmium (USRG:55)

1452. What element is Br? bromine (USRG:55)

1453. What element is I? iodine (USRG:55)

1454. What element is Ne? neon (USRG:55)

1455. What element is Ar? argon (USRG:55)

1456. What element is Kr? krypton (USRG:55)

1457. What element is Xe? xenon (USRG:55)

1458. What element is Rn? radon (USRG:55)

1459. What element is Au? gold (USRG:55)

1460. What element is Hg? mercury (USRG:55)

1461. What element is Pd? palladium (USRG:55)

1462. What element is Pt? platinum (USRG:55)

1463. What element is Ni? nickel (USRG:55)



1464. What element is Ti? titanium (USRG:55)

1465. What element is Y? yttrium (USRG:55)

1466. What element is Zr? zirconium (USRG:55)

1467. What element is Mo? molybdenum (USRG:55)

1468. What element is Tc? technetium (USRG:55)

1469. What element is Ac? actinium (USRG:55)

1470. What element is Th? thorium (USRG:55)

1471. Which of the alkaline earth metals has no stable isotopes?

radium (USRG:55)

1472. What element is Pu? plutonium (USRG:55)

1473. What element is Am? americium (USRG:55)

1474. What is the atomic mass of iron? 55.85 amus (USRG:55)

1475. Which nine of the transition metals have no stable isotopes?

rutherfordium, dubnium, seaborgium, bohrium, hassium, technetium, meitnerium, darmstadtium, and roentgenium

(USRG:55)

1476. What is the atomic mass of nitrogen? 14.01 amus (USRG:55)

1477. What is the atomic mass of potassium? 39.10 amus (USRG:55)

1478. What is the atomic mass of calcium? 40.08 amus (USRG:55)

1479. What is the atomic mass of copper? 63.55 amus (USRG:55)

1480. What is the atomic number of zinc? 30 (USRG:55)

1481. What is the atomic number of bromine? 35 (USRG:55)

1482. What is the atomic number of iodine? 53 (USRG:55)

1483. What is the atomic number of fluorine? 9 (USRG:55)

1484. Which elements have atomic masses which are shown as whole numbers, not including the elements without stable isotopes?

oxygen and fluorine (USRG:55)

1485. What three groups on the periodic table belong to the subgroup 8B?

groups 8,9, and 10 (USRG:55)

1486. What is the atomic number of silicon? 14 (USRG:55)

1487. What element lies between uranium and plutonium on the periodic table?

neptunium (USRG:55)

1488. What is the atomic number of iron? 26 (USRG:55)

Documents

SCIENCE - Carl Schurz High School