Jessica RaybeChemistry Final E.C.

Per. 212/20/11

1. A piece of metal with a mass of 117g is placed in a 100mL graduated cylinder. The water level rises from 15mL to 28mL. What is the density of the metal?

a. 7.0g/mLb. 11.0g/mLc. 3.0g/mLd. 9.0g/mL

2. What is the volume of a sample that has a mass of 16g and a density of 4g/mL?a. 8mLb. 4mLc. 2mLd. 5mL

Complete the Graph

Prefix Symbol Factor Scientific NotationGiga

Mk 10³

Deci 1/101/100 10⁻²

Milli 10⁻³Micro

n 10⁻⁹p 1/1000000000000

3. Express the following quantities in scientific notationa. 0.00000529kg ___________________________________b. 0.0032kg __________________________________c. 4300000m _______________________________d. 664000000000m _________________________________e. 706000m ___________________________________f. 0.00000572kg ________________________________

4. Solve the following addition and subtraction problems. Express your answers in scientific notation.

a. 5×10⁻⁵m + 3×10⁻⁵m ________________________________b. 9×10²m - 4×10²m ____________________________

5. Solve the following multiplication and division problems. Express your answers in scientific notation.

a. (4×10⁶cm) / (2×10⁴cm) __________________________________b. (3×10²cm) × (3×10⁻³cm) _________________________________c. (2×10⁻³cm)× (3×10²cm) _____________________________________d. (9×10⁵cm) / (3×10⁻³cm) ______________________________________

6. Convert 350s to msa. 0.035msb. 0.35msc. 350000msd. 35000ms

7. Convert 5400dm to ma. 0.54mb. 540mc. 54000md. 54m

8. Convert 27kg to mga. 0.27mgb. 270mgc. 27000mgd. 0.027mg

9. The density of silver is 20.9g/mL. What is gold’s density in decigrams per liter?a. 20900dg/Lb. 209000dg/Lc. 2090dg/Ld. 0.209dg/L

True or false

10. ______ Accuracy refers to how close a series of measurements are to one another. Precision refers to how close a measured value is to an accepted value.

11. ______ The formula for percent error is Accepted value × 100 Error

12. ______ Non-zero numbers are always significant.13. ______All final zeros to the right of the decimal place are not significant.14. ______ Counting numbers and defined constants have an infinite number of significant figures15. ______ When rounding, if the digit to the immediate right of the last significant figure is less

than five, do not change the last significant figure.16. ______ If the digit to the immediate right of the last significant figure is equal to five and is

following by a non-zero digit, do not round up.

17. ______ The slope of a graph isy2− y1x2−x1

= ΔxΔy

18. Which one of the these is not a substance?

a. Waterb. All of the abovec. Table Saltd. Seawater

19. Which one of the following are extensive properties?a. Massb. Lengthc. Volumed. All of the above

20. What is the difference between the states of matter?a. Solids have their own definite shape and volume, liquids flow and have constant volume and

take the shape of its container, gas flows to conform to the shap of its container and fills the entire volume of its container.

b. The particles of matter in a solid are very tightly packed, the particles in a liquid are rigidly help in place, the particles of gases are very far apart.

c. Gases are not easily compressed, a liquids volume is constant, and the tight packing of particles in a solid makes it incompressible.

d. A solid cannot be pressed into a smaller volume, liquid particles are not able to move past each other, and in gases there is a significant amount of space between particles.

21. Which of the following is a physical change?a. Bendb. All of the abovec. Grindd. Crush

22. A student carefully placed 17.4g of sodium in a reactor supplied with an excess quantity of chlorine gas. When the reaction was complete, the student obtained 42.7g of sodium chloride. How many grams of chlorine gas reacted?

a. 22.3gb. 15.6gc. 25.3d. 21.7

23. Explain the difference between a heterogeneous mixture and a homogeneous mixture.

24. Which of the following is an example of a solution system?a. Gas-liquidb. Gas-gasc. Solid-solidd. All of the above

Complete Concept Map

25. A 76.0g sample of an unknown compound contains 12.2g of hydrogen. What is the percent by mass of hydrogen in the compound?

a. 15.9%b. 16.1%c. 18.7%d. 22.6%

True or False

26. _____ Democritus states that matter is composed of empty space through which atoms move.27. _____ Both Democritus and Dalton state that atoms cannot be created, divided into smaller

particles, or destroyed.28. _____ Dalton says that in chemical reactions, atoms are not separated, combined, or

rearranged.29. _____ Aristotle wrote on many subjects, including politics, ethics, nature, physics, and

astronomy.

30. Which of the following does not describe the nucleus?

a. Centrally located within the atom

b. Occupies a large spacec. Contains all of an atom’s positive charged. Virtually all of the atom’s mass

31. Describe the difference between a proton and a neutron.

Complete the Graph

Element Atomic Number Protons ElectronsN 7Sn 50Mg 12

32. An atom of an element contains 77 electrons. What element is it?a. Molybdenumb. Chromiumc. Irond. Iridium

33. Write the nuclear equation for Radium-226→Radon-222 + Alpha Particle ___________________________________

Complete the Chart

Radiation Type Symbol Mass (amu) ChargeAlpha HeBeta 1/1840

y 0

34. A longer wavelength creates ___________ frequency than a shorter wavelength.a. Lowerb. Higherc. The samed. None of the above

35. What is the speed of an electromagnetic wave that has a frequency of 7.4 × 10⁶Hz?a. 3.00 × 10⁸m/sb. 4.10 × 10⁷m/sc. 3.68 × 10⁷m/s

d. 2.34 × 10⁶m/s36. Plank’s constant has a value of

a. 6.02 × 10²³ J·sb. 4.637 × 10⁻²⁶ J·sc. 5.342 × 10³⁴ J·sd. 6.626 × 10⁻³⁴ J·s

37. What is the energy of the following types of radiation?a. 6.34 × 10²⁰ s⁻¹ ____________________________b. 9.34 × 10¹¹ Hz _____________________________c. 2.36 × 10¹⁸ s⁻¹ ____________________________

38. Draw the 1s orbital and py orbital.

39. Find the complete electron configuration and electron configuration using noble-gas notation for the following elements.a. Sodium ______________________ ________________________b. Silicon _______________________ _________________________c. Sulfur ________________________ _________________________

40. Metals are elements that are which of the following?a. Solid at room temperatureb. Malleable and ductilec. Good conductors of heat and electricityd. All of the above

41. S-block Elements consists of groups….a. 2A and 4Ab. 1A and 2Ac. 3A and 4Ad. 5A and 6A

42. Which is true about alkali metals?a. Extremely hardb. Bad conductors of heat and electricityc. Highly reactived. None of the above

43. Which is true about Beryllium?a. Lightest member of group 2Ab. None of the abovec. Chemical properties differ from aluminumd. Never combines with aluminum

44. Which is true about Calcium?a. Not essential for humansb. Not found in naturec. Never combines with carbond. Found in chalk, marble, and limestone

45. Nitrogen gas is….a. Colorlessb. Odorlessc. Relatively unreactived. All of the above

46. Chlorine…a. Reacts with nearly all of the elementsb. Is a deadly gasc. Has many uses, including some that can save livesd. All of the above

47. All of the following are true except…a. Most ionic compound are called saltsb. Ionic bond is the electrostatic force that holds oppositely charged particles together in an

ionic compoundc. Many ionic compounds are binaryd. If ionic bonds occur between a metal and a halogen, oxide forms

Write the correct formula for the ionic compound composed of the following pairs of ions.

48. Potassium and Chloride _____________________________49. Magnesium and Bromide ______________________________50. Barium and Nitride __________________________________

51. Name the following ionic compounds

a. ClO₄⁻ _______________________________b. ClO₃⁻ _______________________________c. ClO₂⁻ _______________________________d. ClO⁻ _______________________________

52. Explain the difference between endothermic and exothermic reactions.

Write Balanced Chemical Equations for each of the following

53. Hydrogen(g) + Chlorine (g) → Hydrogen Chloride _________________________________54. Bromine (g) + Nitrogen (g) → Bromine Nitride ___________________________________55. Cupric Chloride + Oxygen (g) → Cupric Chlorate __________________________________

State what kind of reaction it is and balance the reaction

56. _____________________________ Al(s) + CaCl₂ →57. _____________________________ C₆H₁₂ (l) + O₂ →58. _____________________________ KCl (s) + O₂ →59. _____________________________ Ni (s) + CuO (aq) →

SHOW ALL WORK!!!!

60. Determine the number of atoms in 2.70 mol Zn

61. How many molecules are in 12.6 mol H₂O?

62. Determine the mass in grams of each of the followinga. 3.24 mol Al

b. 47.2 mol Si

c. 2.766 mol Zn

63. Determine the number of moles in 25.3g Ag

64. How many atoms are in 53.4g Li

65. What is the mass in grams of 3.20 × 10²² atoms He?

66. Determine the number of moles of chloride ions in 3.20 mol ZnCl₂.

67. Calculate the number of moles of hydrogen atoms in 12.1 mol water.

68. Calculate the percent composition of sodium sulfate

69. 14.7g of Nitrogen, 4.06g of Hydrogen, and 34.6g of Chlorine gases react to produce solid ammonium chloride.a. Balanced Equation

b. What is/are the limiting reactant(s)?

c. Which reactant(s) are in excess and by how many grams?

d. How many grams of ammonium chloride are produced if the percent yield is 37.7%?

70. If 0.500L of a 0.300M solution of magnesium chlorate is reacted with 0.200L of a 0.250M solution of ammonium bromide, aqueous ammonium chlorate and solid magnesium bromide are formed. Calculate the mass in grams of the magnesium bromide produced.

71. How many grams of iron are formed when 83.7g of carbon monoxide react with excess ferric oxide to produce iron and carbon dioxide?

72. How many moles of nitrogen gas are needed to react with 4.63 moles of lithium to produce lithium nitrate?