Name: ________________________ Class: ___________________ Date: __________
Physical Science Final Part 1
Multiple Choice
Identify the choice that best completes the statement or answers the question.
____
1. A horizontal row of the periodic table is usually referred to as a
a. family.
b. period.
c. group.
d. property.
____
2. A golf ball has more mass than a tennis ball because it
a. takes up more space.
b. contains more matter.
c. contains different kinds of matter.
d. has a definite composition.
____
3. An example of an extensive property of matter is
a. temperature.
b. pressure.
c. mass.
d. hardness.
____
4. Which of the following is a physical property?
a. explosive
b. combustible
c. melting point
d. ability to rust
____
5. Which of the following is a physical property of water?
a. It reacts with calcium metal to produce a basic solution.
b. It can be decomposed by electrolysis.
c. It is composed of hydrogen and oxygen.
d. It melts below room temperature.
____
6. How do vapors and gases differ?
a. Generally, a gas is in the solid state at room temperature and a vapor is in the gaseous
state at room temperature.
b. Generally, a gas is in the liquid state at room temperature and a vapor is in the solid state
at room temperature.
c. Generally, a gas is in the gaseous state at room temperature and a vapor is in either the
solid state or liquid state at room temperature.
d. The terms gas and vapor are always used interchangeably, there is no difference.
____
7. A substance that forms a vapor is generally in what physical state at room temperature?
a. solid
b. liquid
c. gas
d. liquid or solid
1
ID: A
Name: ________________________
ID: A
____
8. Which state of matter has a definite volume and takes the shape of its container?
a. solid
b. liquid only
c. gas only
d. both b and c
____
9. Which state of matter takes both the shape and volume of its container?
a. solid
b. liquid only
c. gas only
d. both b and c
____ 10. Which state of matter is characterized by having a definite shape and a definite volume?
a. gas
b. liquid only
c. solid only
d. both b and c
____ 11. Which state of matter expands when heated and is easy to compress?
a. gas
b. liquid only
c. solid only
d. both b and c
____ 12. Which of the following is a physical property of a substance in the liquid state?
a. definite volume
b. indefinite mass
c. not easily compressed
d. definite shape
____ 13. Which of the following is a physical change?
a. corrosion
b. explosion
c. evaporation
d. rotting of food
____ 14. Which of the following is a heterogeneous mixture?
a. air
b. salt water
c. steel
d. soil
____ 15. Which of the following is true about homogeneous mixtures?
a. They are known as solutions.
b. They consist of two or more phases.
c. They have compositions that never vary.
d. They are always liquids.
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Name: ________________________
ID: A
____ 16. Which of the following is a heterogeneous mixture?
a. vinegar in water
b. milk
c. oil and vinegar
d. air
____ 17. Which of the following is a homogeneous mixture?
a. salt water
b. beef stew
c. sand and water
d. soil
____ 18. Which of the following materials is a substance?
a. air
b. gasoline
c. stainless steel
d. silver
____ 19. What is one difference between a mixture and a compound?
a. A compound consists of more than one phase.
b. A compound can only be separated into its components by chemical means.
c. A mixture can only be separated into its components by chemical means.
d. A mixture must be uniform in composition.
____ 20. Which of the following represents a compound?
a. H
b. H-3
c. H2O
d. O-16
____ 21. The chemical formula of a compound indicates
a. the source of the elements in the compound.
b. how elements are joined in the compound.
c. the alchemy symbols for the elements in the compound.
d. the relative proportions of the elements in the compound.
____ 22. What do chemical symbols and formulas represent, respectively?
a. elements and compounds
b. atoms and mixtures
c. compounds and mixtures
d. elements and ions
____ 23. Which of the following is a chemical property?
a. color
b. hardness
c. freezing point
d. ability to react with oxygen
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Name: ________________________
ID: A
____ 24. In the chemical reaction in which sucrose is heated and decomposes to form carbon dioxide and water, which
of the following is a reactant?
a. sucrose
b. carbon dioxide
c. water
d. heat
____ 25. What must occur for a change to be a chemical reaction?
a. There must be a change in chemical properties.
b. There must be a change in physical properties.
c. The change must involve a change in mass.
d. The change must involve a change in volume.
____ 26. Which of the following is a chemical change?
a. grating cheese
b. melting cheese
c. fermenting of cheese
d. mixing two cheeses in a bowl
____ 27. Which of the following processes involves a change in physical properties?
a. rusting
b. fermenting
c. boiling
d. burning
____ 28. A chemical change occurs when a piece of wood
a. splits.
b. is painted.
c. decays.
d. is cut.
____ 29. When paper turns yellow-brown upon exposure to sunlight, what type of change is likely taking place?
a. a physical change
b. a chemical change
c. neither a physical change nor a chemical change
d. both a physical change and a chemical change
____ 30. What happens to matter during a chemical reaction?
a. Matter is neither destroyed or created.
b. Some matter is destroyed.
c. Some matter is created.
d. Some matter is destroyed and some is created.
____ 31. Which of the following is true for all chemical reactions?
a. The total mass of the reactants increases.
b. The total mass of the products is greater than the total mass of the reactants.
c. The total mass of the products is less than the total mass of the reactants.
d. The total mass of the reactants equals the total mass of the products.
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Name: ________________________
ID: A
____ 32. What is the SI unit of mass?
a. liter
b. joule
c. candela
d. kilogram
____ 33. What is the temperature of absolute zero measured in C?
a. –373C
b. –273C
c. –173C
d. –73C
Use the table to help you answer the question(s).
Prefix
mega (M)
kilo (k)
deci (d)
centi (c)
milli (m)
micro ()
nano (n)
pico (p)
Commonly Used Metric Prefixes
Meaning
1 million times larger than the unit it precedes
1000 times larger than the unit it precedes
10 times smaller than the unit it precedes
100 times smaller than the unit it precedes
1000 times smaller than the unit it precedes
1 million times smaller than the unit it precedes
1000 million times smaller than the unit it precedes
1 trillion times smaller than the unit it precedes
Factor
10 6
10 3
10 1
10 2
10 3
10 6
10 9
10 12
____ 34. Which of the following equalities is correct?
a. 100 cg = 10 g
b. 1000 mm = 100 m
c. 1000g = 1 kg
d. 10 kg = 1 g
____ 35. A cubic meter is about the same as the volume occupied by a ____.
a. kilogram of water
b. cup of milk
c. washing machine
d. basketball arena
____ 36. Who was the man who lived from 460 B.C.–370 B.C. and was among the first to suggest the idea of atoms?
a. Atomos
b. Dalton
c. Democritus
d. Thomson
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Name: ________________________
ID: A
____ 37. Dalton's atomic theory included which idea?
a. All atoms of all elements are the same size.
b. Atoms of different elements always combine in one-to-one ratios.
c. Atoms of the same element are always identical.
d. Individual atoms can be seen with a microscope.
____ 38. Evidence about Dalton’s atomic theory has shown that
a. all of Dalton's hypotheses were correct.
b. atoms of an element can have different numbers of protons.
c. atoms are divisible.
d. all atoms of an element are not identical but they must all have the same mass.
____ 39. Which of the following is true about subatomic particles?
a. Electrons are negatively charged and are the heaviest subatomic particle.
b. Protons are positively charged and the lightest subatomic particle.
c. Neutrons have no charge and are the lightest subatomic particle.
d. The mass of a neutron nearly equals the mass of a proton.
____ 40. Which hypothesis led to the discovery of the proton?
a. When a neutral hydrogen atom loses an electron, a positively-charged particle should
remain.
b. A proton should be 1840 times heavier than an electron.
c. Cathode rays should be attracted to a positively-charged plate.
d. The nucleus of an atom should contain neutrons.
____ 41. The nucleus of an atom is
a. the central core and is composed of protons and neutrons.
b. positively charged and has more protons than neutrons.
c. negatively charged and has a high density.
d. negatively charged and has a low density.
____ 42. Isotopes of the same element have different
a. numbers of neutrons.
b. numbers of protons.
c. numbers of electrons.
d. atomic numbers.
____ 43. In which of the following sets is the symbol of the element, the number of protons, and the number of
electrons given correctly?
a. In, 49 protons, 49 electrons
b. Zn, 30 protons, 60 electrons
c. Cs, 55 protons, 132.9 electrons
d. F, 19 protons, 19 electrons
____ 44. How many protons, electrons, and neutrons does an atom with atomic number 50 and mass number 125
contain?
a. 50 protons, 50 electrons, 75 neutrons
b. 75 electrons, 50 protons, 50 neutrons
c. 120 neutrons, 50 protons, 75 electrons
d. 70 neutrons, 75 protons, 50 electrons
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Name: ________________________
ID: A
____ 45. If E is the symbol for an element, which two of the following symbols represent isotopes of the same
element?
1. 20
E
2. 20
E
3. 219 E
4. 21
E
10
11
10
a.
b.
c.
d.
1 and 2
3 and 4
1 and 4
2 and 3
____ 46. How is the number of neutrons in the nucleus of an atom calculated?
a. Add the number of electrons and protons together.
b. Subtract the number of electrons from the number of protons.
c. Subtract the number of protons from the mass number.
d. Add the mass number to the number of electrons.
____ 47. In which of the following is the number of neutrons correctly represented?
a. 199 F has 0 neutrons.
b.
c.
d.
75
33
24
12
238
92
As has 108 neutrons.
Mg has 24 neutrons.
U has 146 neutrons.
____ 48. How do the isotopes hydrogen-1 and hydrogen-2 differ?
a. Hydrogen-2 has one more electron than hydrogen-1.
b. Hydrogen-2 has one neutron; hydrogen-1 has none.
c. Hydrogen-2 has two protons; hydrogen-1 has one.
d. Hydrogen-2 has one proton; hydrogen-1 has none.
____ 49. What unit is used to measure weighted average atomic mass?
a. amu
b. gram
c. angstrom
d. nanogram
____ 50. In Bohr's model of the atom, where are the electrons and protons located?
a. The electrons move around the protons, which are at the center of the atom.
b. The electrons and protons move throughout the atom.
c. The electrons occupy fixed positions around the protons, which are at the center of the
atom.
d. The electrons and protons are located throughout the atom, but they are not free to move.
____ 51. The principal quantum number indicates what property of an electron?
a. position
b. speed
c. energy level
d. electron cloud shape
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Name: ________________________
ID: A
____ 52. When an electron moves from a lower to a higher energy level, the electron
a. always doubles its energy.
b. absorbs a continuously variable amount of energy.
c. absorbs a quantum of energy.
d. moves closer to the nucleus.
____ 53. Which color of visible light has the shortest wavelength?
a. yellow
b. green
c. blue
d. violet
____ 54. Which of the following elements is in the same period as phosphorus?
a. carbon
b. magnesium
c. nitrogen
d. oxygen
____ 55. In which of the following sets is the symbol of the element, the number of protons, and the number of
electrons given correctly?
a. In, 49 protons, 49 electrons
b. Zn, 30 protons, 60 electrons
c. Cs, 55 protons, 132.9 electrons
d. F, 19 protons, 19 electrons
____ 56. The atomic number of an element is the total number of which particles in the nucleus?
a. neutrons
b. protons
c. electrons
d. protons and electrons
____ 57. What is the charge of a cation?
a. a positive charge
b. no charge
c. a negative charge
d. The charge depends on the size of the nucleus.
____ 58. Which of the following statements is true about ions?
a. Cations form when an atom gains electrons.
b. Cations form when an atom loses electrons.
c. Anions form when an atom gains protons.
d. Anions form when an atom loses protons.
____ 59. In which of the following sets are the charges given correctly for all the ions? NOTE - Does the elements
want to gain or lose electrons? What will happen to the charge?
a. Na  , Mg  , Al 
b. K  , Sr 2  , O 2 
c. Rb  , Ba 2  , P 3 
d. N  , O 2  , F 3 
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Name: ________________________
ID: A
____ 60. Chemical reactions
a. occur only in living organisms.
b. create and destroy atoms.
c. only occur outside living organisms.
d. produce new substances.
____ 61. Chemical equations
a. describe chemical reactions.
b. show how to write chemical formulas.
c. give directions for naming chemical compounds.
d. describe only biological changes.
____ 62. A catalyst is
a. the product of a combustion reaction.
b. not used up in a reaction.
c. one of the reactants in single-replacement reactions.
d. a solid product of a reaction.
____ 63. What are the coefficients that will balance the skeleton equation below?
N 2 + H 2  NH 3
a.
b.
c.
d.
1, 1, 2
1, 3, 3
3, 1, 2
1, 3, 2
____ 64. When the equation Fe  Cl 2  FeCl 3 is balanced, what is the coefficient for Cl 2 ?
a.
b.
c.
d.
1
2
3
4
____ 65. When the following equation is balanced, what is the coefficient for HCl?
Mg(s)  HCl(aq)  MgCl 2 (aq)  H 2 (g)
a.
b.
c.
d.
6
3
1
2
____ 66. When the equation KClO 3 (s)  KCl(s) + O 2 (g) is balanced, the coefficient of KClO3 is
a.
b.
c.
d.
1.
2.
3.
4.
____ 67. In the kinetic theory, the particles in a gas
a. move independently of each other.
b. move slowly.
c. are relatively close together.
d. have attractive and repulsive forces.
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Name: ________________________
ID: A
____ 68. What instrument is normally used to measure atmospheric pressure?
a. thermometer
b. barometer
c. vacuum
d. manometer
____ 69. What is the SI unit of pressure?
a. candela
b. mole
c. pascal
d. newton
____ 70. What happens to the average kinetic energy of the particles in a sample of matter as the temperature of the
sample is increased?
a. The average kinetic energy decreases.
b. The average kinetic energy increases.
c. The average kinetic energy does not change.
d. The change in average kinetic energy cannot be determined.
____ 71. What is the key difference between a liquid and a gas?
a. intermolecular attractions
b. the ability to flow
c. average kinetic energy
d. the motion of their particles
____ 72. Which states of matter can flow?
a. gases only
b. liquids only
c. gases and liquids only
d. gases, liquids, and solids
____ 73. In a dynamic equilibrium between the liquid state and the gas state, what is true about the rate of
evaporation?
a. It is greater than the rate of condensation.
b. It is less than the rate of condensation.
c. It is equal to the rate of condensation.
d. The rate of evaporation cannot be determined.
____ 74. An increase in the temperature of a contained liquid
a. has no effect on the kinetic energy of the liquid.
b. causes the vapor pressure above the liquid to decrease.
c. causes fewer particles to escape from the surface of the liquid.
d. causes the vapor pressure above the liquid to increase.
____ 75. Which of the following best describes the motion of the particles in a piece of steel?
a. None are moving.
b. A few are moving.
c. All are moving.
d. Most are moving.
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Name: ________________________
ID: A
____ 76. Most solids
a. are dense and difficult to compress.
b. are able to flow.
c. are amorphous.
d. have a disorderly structure.
____ 77. Which of the following is an example of a phase?
a. pressure
b. water vapor
c. temperature
d. triple point
____ 78. Which of these changes would cause a decrease in the pressure of a contained gas?
a. The volume of the container is increased.
b. More of the gas is added to the container.
c. The temperature is increased.
d. The average kinetic energy of the gas in increased.
____ 79. If a balloon is heated, what happens to the volume of the air in the balloon if the pressure is constant?
a. It increases.
b. It stays the same.
c. It decreases.
d. The change cannot be predicted.
____ 80. If a balloon is heated, what happens to the pressure of the air inside the balloon if the volume remains
constant?
a. It increases.
b. It stays the same.
c. It decreases.
d. The change cannot be predicted.
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