Download 8th Grade: First Semester Final Review

8th Grade: First Semester Final Review
Multiple Choice
Identify the choice that best completes the statement or answers the question.
1. Some substances are chemically combined in
12. A compound made from two elements will have
specific combinations. These are _____.
_____.
a. compounds
a. all the properties of both elements
b. heterogeneous mixtures
b. different properties than either element
2. Which item is a form of matter?
a. sound
b. air
13. Which one is NOT a solution?
a. fruit salad
b. brass
3. Which item is a substance?
a. trail mix
b. table salt
14. A neutral, or uncharged, atom definitely has the
same number of _____.
a. electrons and neutrons
b. protons and electrons
4. Which item is NOT a type of matter?
a. mixture
b. force
5. Which combination can be used to classify all the
matter on Earth?
a. solvents and solutes
b. substances and mixtures
6. An element’s atomic number tells how many are in
the nucleus of an atom of that element.
a. electrons
b. protons
7. In an atom, electrons _____.
a. stay in a region called the electron cloud
b. orbit the nucleus like planets around the Sun
8. A solvent and one or more solutes make up a
_____.
a. heterogeneous mixture
b. homogeneous mixture
9. How are protons and neutrons alike?
a. Both are charged particles.
b. Both are in the nucleus.
10. The electrons closest to an atom’s nucleus have less
than those further away.
a. energy
b. charge
11. Elements and compounds are _____.
a. mixtures
b. substances
15. Which statement can be used to describe a
heterogeneous mixture but NOT a solution?
a. It contains a solvent and solute.
b. Its individual parts can be seen.
16. Trail mix and salt water could be classified as
_____.
a. mixtures
b. compounds
17. Two atoms of the same element cannot have
different numbers of _____.
a. electrons.
b. protons
18. Which is NOT one of the main factors that
determine the state of matter?
a. particle motion
b. particle size
19. In which state of matter do molecules interact to
create surface tension?
a. liquid
b. solid
20. What happens when the motion of particles slows?
a. The particles move closer together.
b. The particles move further apart.
21. Which phrase best describes the particles in a solid?
a. vibrating in place
b. very far apart
22. What causes surface tension?
a. crystalline arrangement of particles
b. attractive forces between particles
23. Which grouping lists the states of matter in order of
increasing distance between particles?
a. solid, gas, liquid
b. solid, liquid, gas
24. Evaporation and boiling are two kinds of _____.
a. vaporization
b. sublimation
25. Deposition is a change from a _____.
a. gas to a solid
b. liquid to a gas
26. Vaporization that occurs within a liquid is _____.
a. boiling
b. evaporation
27. Deposition could be best described as the opposite
of _____.
a. condensation
b. sublimation
28. What happens when temperature increases on a gas
in a container that has a fixed volume?
a. Pressure increases
b. Volume increases
29. What relationship is described by Boyle’s law?
a. pressure and volume of gases at constant
temperature
b. pressure and temperature of gases at constant
volume
b. the thermal energy of the particles of a
substance
34. _____ has particles with the greatest average
kinetic energy.
a. Hot water
b. Room-temperature water
35. During which change of state does the thermal
energy of a substance increase?
a. sublimation
b. condensation
36. Which factor would increase the temperature of a
substance?
a. decreasing the number of particles
b. adding thermal energy
37. Which statement describes the relationship between
temperature and particle motion?
a. Temperature increases as particle motion
increases.
b. Temperature decreases as particle motion
increases.
38. How are the elements arranged on the periodic
table?
a. in rows and columns according to their
properties
b. in rows and columns alphabetically
39. Where are metalloids on the periodic table?
a. between metals and nonmetals
b. in two rows at the bottom
30. What relationship is described by Charles’s law?
a. pressure and temperature of gases at constant
volume
b. volume and temperature of gases at constant
pressure
40. The first periodic table arranged elements in order
of _____.
a. increasing atomic number
b. increasing atomic mass
31. Which factor measures the total potential and
kinetic energy of a substance?
a. thermal energy
b. pressure
41. On most periodic tables, an element’s key includes
the element’s chemical symbol, atomic number,
and _____.
a. atomic mass
b. density
32. Which change of state involves adding thermal
energy to a substance?
a. condensation
b. melting
42. All of the elements in groups 1–12, except for
hydrogen, are _____.
a. metals
b. metalloids
33. What does temperature measure?
a. the average kinetic energy of the particles of a
substance
43. Which group contains only metals?
a. sodium, gold, lithium
b. copper, oxygen, sulfur
44. The ability of a metal to be pulled into thin wires is
called _____.
a. luster
b. ductility
45. Gold can be hammered into thin sheets because of
_____.
a. density
b. malleability
46. All metals are good _____ of thermal energy and
electricity.
a. insulators
b. conductors
a. ductility
b. hardness
55. Which property do all metalloids share?
a. semiconductivity
b. high luster
56. Which part of an atom participates in chemical
bonding?
a. electron
b. neutron
57. An electron dot diagram shows _____.
a. the strength of electron energy fields
b. the number of valence electrons
47. The _____ are elements that have no metallic
properties.
a. metalloids
b. nonmetals
58. Except for helium atoms, atoms tend to gain, lose,
or share valence electrons until they have _____
valence electrons.
a. four
b. eight
48. One physical property of nonmetals is that they are
good _____.
a. conductors
b. insulators
59. In the chemical formula H2O, how many atoms of
oxygen are represented?
a. one
b. three
49. Which groups on the periodic table contain metals,
nonmetals, and metalloids?
a. 12 and 13
b. 14 and 15
60. A double covalent bond is created when _____.
a. two atoms share bonds with four other atoms
b. two atoms share two pairs of valence electrons
50. A metalloid has physical and chemical properties of
_____.
a. metals and noble gases
b. metals and nonmetals
51. Elements on the periodic table are arranged in rows
and columns according to their _____.
a. properties
b. weight
52. Where are metals located on the periodic table?
a. in the middle
b. on the left side
53. Which property increases and then decreases across
a period of the periodic table?
a. melting point
b. conductivity
54. All metals share properties that include luster,
conductivity, malleability, and _____.
61. Which activity makes an atom more stable when it
is forming an ionic bond?
a. losing an electron
b. gaining or losing an electron
62. Which type of bond joins nonmetal atoms to
nonmetal atoms?
a. covalent
b. ionic
63. Which type of covalent bond is the strongest?
a. triple covalent bond
b. double covalent bond
64. Which group of elements is the most stable?
a. nonmetals
b. noble gases
65. Which best describes a valence electron?
a. an inner electron that participates in chemical
bonding
b. an outermost electron that participates in
chemical bonding
66. Which equation is balanced?
a. 2Na + Cl2 → 2NaCl
b. CH4 + 2O2 → CO2 + H2O
67. Which equation is balanced?
a. 2Na + Cl2 → 2NaCl
b. CH4 + 2O2 → CO2 + H2O
Matching
Match each term with the correct definitions below. Not all terms are used.
a. electron
e. ion
b. nucleus
f. isotope
c. neutron
g. proton
d. electron cloud
1. The part of an atom that contains most of its mass
4. an atom that has a positive or negative charge
2. particle in the nucleus of an atom that has a positive
charge
3. particle of an atom that has a negative charge
5. uncharged particle in the nucleus of an atom
6. one of two or more atoms of an element that have
different numbers of neutrons
Match each term with the correct definitions below. Not all terms are used.
a. vaporization
e. deposition
b. thermal energy
f. kinetic energy
c. condensation
g. sublimation
d. temperature
h. potential energy
7. the energy an object has due to its motion
10. change from a liquid to a gas
8. measure of the average kinetic energy of all
particles in an object
11. change from a gas to a liquid
12. change directly from a solid to a gas
9. the total potential and kinetic energy of an object
Match the term with the correct definitions below. Not all terms will be used.
a. kinetic molecular theory
e. viscosity
b. vapor
f. Charles’s law
c. Boyle’s law
g. surface tension
d. pressure
h. temperature
13. describes particles and their interactions in all states
16. describes the relationship between the volume and
of matter
pressure of a gas at constant temperature
14. the gaseous state of a substance that is normally a
solid or liquid at room temperature
15. a liquid’s resistance to flow
17. describes the relationship between the temperature
and volume of a gas at constant pressure
18. uneven forces acting on the particles at the surface
of a liquid
Choose the letter of the term that matches it correctly. Each term is used only once.
a. Henry Moseley
d. Dimitri Mendeleev
b. nonmetals
e. period
c. group
19. arranged the elements according to increasing
22. located on the right side of the periodic table
atomic mass
23. arranged the elements according to increasing
20. a row on the periodic table
atomic number
21. a column on the periodic table
Choose the letter of the term that matches it correctly. Each term is used only once.
a. alkali metals
b. alkaline earth metals
c. transition elements
24. soft and silvery metals such as magnesium
d. lanthanide series elements
e. actinide series elements
27. Properties make them good building materials.
25. used to make strong magnets
28. Plutonium is one of these elements.
26. react quickly with other elements such as oxygen
Choose the letter of the term that matches it correctly. Each term is used only once.
a. halogen
d. oxygen and nitrogen
b. noble gases
e. carbon
c. metalloids
29. do not form natural compounds
32. nonmetals in your body
30. nonmetal from group 14
33. semiconductors
31. reacts with a metal to form a salt
Choose the letter of the term that matches it correctly. Not all terms are used.
a. metallic bond
e. polar molecule
b. electron dot diagram
f. ion
c. ionic bond
g. chemical bond
d. valence electron
34. a bond between positively and negatively charged
37. an atom that is no longer electrically neutral
atoms
38. has a slight positive end and a slight negative end
35. a force that holds atoms together
because of unequal sharing of electrons
36. a chemical bond formed when positively charged
atoms share their electrons
39. the part of an atom that participates in chemical
bonding
Match each term with the correct definitions below. Not all terms are used.
a. precipitate
d. product
b. chemical reaction
e. reactant
c. conservation
f. coefficient
40. a starting substance in a chemical reaction
42. a number placed in front of an element symbol or
chemical formula in an equation
41. a substance produced in a chemical reaction
43. a process in which atoms of one or more substances
rearrange to form one or more new substances
Short Answer
1. Identify one way that homogeneous mixtures and
heterogeneous mixtures are different.
3. List and describe three different methods that can
be used to separate the components of a mixture.
2. Describe an atom’s electron cloud using your own
words.
4. A neutral iron atom has an atomic number of 26.
How many electrons does this atom have? Explain
the reasoning you used to arrive at your answer.
9. Examine the element key below and explain what it
tells you about the element. Based on this key, what
can you predict about the atomic mass and atomic
number of the element to its right on the periodic
table?
5. Identify the relationship described in Charles’s law
and describe how it is different from Boyle’s law.
6. State two ways the particles in an ice cube change
when the ice cube melts.
7. Explain why an inflated balloon will pop if you
squeeze it hard enough. Relate this to Boyle’s law.
10. List the three types of atomic bonds and describe
the types of atoms—metal or nonmetal—that form
each type of bond.
11. What are the columns called on the periodic table?
12. Create an electron dot diagram for an atom of
oxygen, atomic number 8, group 16.
8. Differentiate between Mendeleev’s periodic table
and the later version developed by Moseley.
8th Grade: First Semester Final Review
Answer Section
MULTIPLE CHOICE
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A
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B
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B
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A
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B
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A
A
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B
B
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B
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B
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B
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B
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A
MATCHING
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B
G
A
E
C
F
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D
B
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A
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C
17. F
18. G
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E
C
B
A
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27.
28.
B
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E
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B
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A
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C
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C
G
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E
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43.
E
D
F
B
SHORT ANSWER
1. Sample answer: The individual components of a heterogeneous mixture can be seen; the individual components of
a homogeneous mixture cannot be seen. The individual components of a homogeneous mixture are evenly mixed;
the individual components of a heterogeneous mixture are not evenly mixed.
2. Sample answer: An electron cloud is the space around an atom’s nucleus in which the electrons move.
3. Sample answer: One way I could separate a mixture is by using a strainer to separate components of different sizes.
Another method I could use is evaporation, which could be used to separate a liquid and a substance dissolved in it.
I could also use a magnet to separate the components if one component is magnetic but the others are not.
4. Sample answer: The atomic number of 26 tells me that this atom has 26 protons. The atom is neutral, which means
it has no charge, so the number of electrons must equal the number of protons. Therefore, this atom must have 26
electrons.
5. Charles’s law describes the behavior of a gas when temperature and volume change and pressure is constant.
Boyle’s law describes the behavior of a gas when pressure and volume change and temperature is constant.
6. Possible answer: When an ice cube melts, the particles move further apart and the speed at which the particles
move increases.
7. Possible answer: An inflated balloon will pop if it is squeezed hard enough because squeezing reduces the volume
of the balloon. When the volume is reduced, pressure increases. When the particles inside exert enough pressure on
the walls of the balloon, the balloon will pop. This relates to Boyle’s law, which states that the pressure of a gas
increases if the volume decreases.
8. Mendeleev’s periodic table arranged elements according to increasing atomic mass. Moseley’s version, which we
use today, arranges the elements according to increasing atomic number.
9. The key indicates that the element abbreviation is Se, for selenium. Selenium is a solid at room temperature, has
the atomic number 34, and has a mass of 78.96. The element to the right will have the atomic number of 35, and
the mass will be higher than the mass of selenium.
10. Covalent—nonmetal atoms to nonmetal atoms; Ionic—nonmetal ions to metal ions; Metallic—metal atoms to
metal atoms
11. The columns are groups.
12. Because oxygen has an atomic number of eight, you know it has eight electrons. It is in group 16, so you know it
has six valence electrons. Student drawings should resemble this: