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NAME ___________________________________________ DATE __________________________Physical Science: Semester 1 Exam Review

**There will be some things on the test that are not in this packet.**

CHAPTER 1: INTRODUCTION TO SCIENCE

1. The base units of measurement are _________________ (length), _______________ (mass), ___________________ (time), and ______________ (volume).

2. Write the symbol and meaning of each prefixa. kilo- ______________ ______________b. hecto- ______________ ______________c. deka- ______________ ______________d. Basee. deci- _____________ ______________f. centi- ______________ ______________g. milli- ______________ ______________

scientific theory science variable physicsmodel technology critical thinkingscientific law

chemistry

3. The branch of physical science that studies forces and energy ________________________

4. Observing, studying, and experimenting to find the nature of things ________________________

5. A representation used to study an object or event ________________________

6. The application of scientific knowledge for practical purposes ________________________

7. An explanation of how or why a natural process works ________________________

8. Description of a process in nature, can be tested by repeated experiments ___________________

9. A branch of physical science that studies matter and its changes________________________


10. Thinking logically to solve a problem ________________________

11. A factor that can change in an experiment ________________________

12. Write 56,780,000,000 in scientific notation ______________ x ______________

13. Write 0.00000064 in scientific notation ______________ x ______________

14. Write 8.3 x 10-8 in standard form ____________________________________

15. Write 3.2 x 104 in standard form____________________________________

16. Complete the following conversions4.8 g to kg ________ 3.03 mm to dam ________0.007 L to dL ________ 140,000 hm to mm ________

17. Identify the steps of the scientific method, in order.

________________________ ________________________________________________ ________________________________________________ ________________________________________________ ________________________


CHAPTER 2: CLASSIFYING MATTER

1. Matter is defined as: ______________________________________________________________

2. The study of matter is called: ______________________________________

3. List the 3 states of matter: __________________, __________________, __________________

4. Iron is an example of an ________________________, a substance that cannot be broken down into smaller means.

5. ____________________________ are substances made up of atoms of two or more different elements joined chemically, and cannot be physically separated

6. Benzene, C6H6 element compound7. Aluminum, Al element compound8. Acetylene, C2H2 element compound9. Zinc, Zn element compound


10. Compounds or elements that are mixed, but not chemically bonded are called ________________. Heterogeneous:

_______________________________________________________________ Homogeneous:

________________________________________________________________

Classify each of the following11. Banana split heterogeneous homogeneous

Chocolate syrup heterogeneous homogeneousPail of sand and water heterogeneous homogeneousMilk heterogeneous homogeneous

12. Mixtures can be separated by [physical / chemical] means Example: Separating sand and water with a filter13. Different substances in a mixture [keep / lose] their properties.

14. Matter has ___________________ and ____________________ properties Physical properties : properties such as ____________________ point and

_________________ pointDensity - The ratio of mass to volume of an object o D = ____ / ____ o V = ____ / ____

Chemical Properties : properties such as reactivity and ______________________15. Why is the physical property of density important and useful?

Calculate the following: An object has a mass of 23.6 grams and a volume of 2

mL: what is the density?

An object has a density of 3 g/mL and a mass of 21 g: what is its volume?


Matter can be changed both physically and chemically16. ________________________ - A change of matter from one state to another

without a chemical change Example: Dissolving sugar in water

17. Chemical - When one or more substances _________________ into an entirely new __________________ Example: Baking a loaf of bread

18. PHYSICAL / CHEMICAL: occur when one or more substances changes into an entirely new substances

19. PHYSICAL / CHEMICAL: occurs without changing the identity of the substance

20. Chemical changes CAN / CANNOT be reversed

21. List five potential signs of a chemical change

22. List four different examples of a chemical change (i.e. burning wood)

CH 3: STATES OF MATTER23. The three most familiar states of matter are: _________________,

______________, and ______________24. The most common state of matter is: _______________________________25. The state of matter is determined by how the ______________________________

move26. According to the kinetic theory of matter

_____________________________________________________________________________________________________________________________


Observations of particles in motion:1. ____________________________________________________________________________2. ____________________________________________________________________________

27. Draw the particles for each state of matter.

28. Phase changes occur by _________________ or ____________________ heat

29. For each phase change, determine whether energy is required or released

Liquid to Solid ______________________________Solid to Gas ______________________________Gas to Liquid ______________________________Solid to Liquid ______________________________Liquid to Gas ______________________________Gas to Solid ______________________________

30. When matter condenses, it changes from a ________________________ to a ______________. The particles will [speed up / slow down] and [spread out / clump together

31. Phase changes include: Sublimation: _____________ to _________

Melting: ____________ to _____________ Condensation: _________ to ___________

Vaporization: _____________ to ________ Freezing: ____________ to ____________

32. Complete the table below on states of matter.

Solid Liquid Gas


Shape(fixed or changes)

Volume(fixed or changes)

Particle

Behavior

33. What happens to particles if energy is removed? ______________________________________________________________________________________

34. If it is added? ______________________________________________________________________________________


CHAPTER 4: ATOMS35. Complete the table on atomic theory.

Scientist Theory Evidence/Experiment/Discovery

Democritus

Dalton

Thomson

Rutherford

Bohr

Schrodinger

Chadwick

36. Atoms are made of three main particles, ________________, _________________,

and _________________.37. Particle Charge Location in

Atom


38. Atoms have no overall charge because there are an [equal / unequal] number of charged and uncharged particles

39. Two isotopes of an element will have different numbers of _____________________

40. Explain the Law of Definite Proportions.

41. Explain the difference between the atomic number, mass number, and the atomic mass.

42. What two particles make up the mass of an atom?

43. How do you find the number of neutrons in an atom?

44. Complete the table.Element Atomic #

(same as protons)

Mass #(protons

+ neutrons)

Protons(same at atomic)

Neutrons(mass – protons)

Electrons(same as protons)

Calcium-42

20 22

Sulfur 32 16 16Argon 18 40 18Nickel 59


Rubidium-87

20

Barium 137Technetiu

m99

Silver-106Tin-___ 121

45. Why do most atoms have no charge even though they are made up of positively charged protons and negatively charged electrons?

46. What is an energy level?

47. Isotopes have the [ same / different ] chemical and physical properties of the element.

48. An isotope of an element has a mass of 89, and an atomic number of 56. Show this atom in isotope notation.

CHAPTER 5: THE PERIODIC TABLE49. An atom becomes an ion by _______________________ or ____________________

electrons


50. Atoms that give up electrons are specifically called _________________________, and atoms that gain electrons are specifically called ___________________________.

51. Elements on the [right / left ] of the periodic table are more likely to be cations, and elements on the [right / left] of the periodic table are more likely to be anions.

52. The periodic table has rows called _________________________ and columns called _____________________.

53. Elements are classified into three different groups: _____________________, _____________________, and _____________________

Metals Nonmetals Semiconductors

Prop

erti

esEx

ampl

es

54. These three groups are divided into _________________________55. Why is the periodic table a useful tool for scientists?


Family Group #

Valence Electron

s

Properties

Alkali

Alkaline-Earth

Transition

Noble Gases

Halogens

56. In addition to the noble gases and halogens, list the six other nonmetals: ______, ______, ______, ______, ______, and ______.

57. ____________________________ is in a class by itself

58. The electrons in the outermost shell are called ___________________ electrons. To be a stable atom, there should be _________ electrons in this shell.

59. Atoms that are in the same group will have the same number of _________________________ ______________________.

60. If there are not _______ electrons in an atom’s outermost shell, it will go through ___________________________, a process in which atoms gain or lose electrons.


61. The modern periodic table is arranged by _________________________ ________________.

62. The group number indicates how many __________________________ _____________________ are in each atom, and the period number indicates how many ___________________________ __________________ are in the atom.

63. Complete the table. In the symbol column, use isotope notation and charges as needed.

Element Atomic #

Mass # Neutrons

Protons Electrons

Symbol

Barium 137 54Cesium 78 Cs1+

Polonium 123 86Gallium 39 Ga3+

Bismuth 209 86Carbon 12 10Iodine 127 I1-

Silicon 14 Si4-

Lithium 2 2

64. Color and label the periodic table to represent the different families of elements.


Chapter 6: The Structure of

Matter

65. Describe an ionic bond:

66. Describe a covalent bond:

67. Label each picture as either an ionic bond or a covalent bond.

68. Elements are made of one single kind of ______________________Example - Oxygen

69. Compounds are made of _________ or more ________________________ that are chemically combinedExample – H2O, Water


70. The way a compound bonds determines many of its ______________________________

71. Atoms bond when their ________________________ ______________________ interact.

72. Atoms with their outermost orbitals full will be more [stable / unstable] than atoms with only [partially / completely] filled outer orbitals.

73. A single covalent bond shares [one / two] electrons and is represented by [one / two] single line(s)

74. What type of bond is formed between two metals? ________________________________

75. A metal and a nonmetal will create a(n) ____________________________ bond76. Two nonmetals will form a(n) ___________________________ bond

77. List the steps for naming an ionic compound

78. List the steps for naming a covalent compound

79. Compounds should have an overall charge of _______80. List the prefixes used in naming covalent compounds:

# of Atoms

Prefix


81. Name the following ionic compounds. Make note of transition metals!:Fel2: ____________________________________CrCl2: ___________________________________MgS: ____________________________________NaCl: ___________________________________

82. Name the following covalent compounds: SeO2: ___________________________________Snl4: ____________________________________As2O5: __________________________________P4S3: ___________________________________

Chapter 7: Chemical Reactions

83. ________________________ ________________________ occur when substances go through chemical ________________ to create new ___________________________

84. The reactants are placed on the [left / right] side of the arrow, and the _____________________ on the right

_________________ ____________________85. The arrow in a chemical equation means _____________________ or

___________________86. The total amount of energy in the reactants must

[be more / be equal to / be less] than the total amount of energy in the products.

87. In a chemical reaction, the ______________________ are simply __________________________ to create new _____________________________


88.EXOTHERMIC ENDOTHERMIC

Exothermic reactions: ________________________________________________________________________________________________________________________The amount of energy released as a product is __________________________ than the amount of energy ___________________________ to break the bonds

Endothermic reactions: ________________________________________________________________________________________________________________________More energy is needed to __________________ the bonds in the __________________ than is given off by forming bonds in the _________________________

89. A balanced equation follows the law _________________________________________________

90. In order to balance an equation, ________________________________ must be added in front of one or more of the _______________________________

91. Balance ____ H2O ____ H2 + ____ O2

____ H2 + ____ Cl2 ____ HCl


____ C2H6 + ____ O2 ____ CO2 + ____ H2O

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Salem Science - Homeysalemscience.weebly.com/uploads/2/2/6/7/22675926/... · Web view_____ are substances made up of atoms of two or more different elements joined chemically, and