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Chemistry Phase Review

Total questions: 104

Worksheet time: 58mins

Name
Class
Date
1.

The scientist credited with identifying the modern atomic structure is

a)

Bohr

b)

Aristotle

c)

Dalton

d)

Rutherford

2.

Electrons are found rotating around the nucleus in

a)

A predictable elliptical orbit

b)

an electron cloud

c)

a circular rotation

d)

the ground state

3.

What sub atomic particle(s) make up the atomic mass of an atom?

a)

Protons & electrons

b)

Neutrons & electrons

c)

Protons & neutrons

d)

Protons

4.

Almost all the mass of an atom is located in its

a)

protons

b)

electrons

c)

electron cloud

d)

nucleus

5.

An electron is a particle with

a)

A negative charge, found in the nucleus

b)

A positive charge, found in the nucleus

c)

No charge, found outside the nucleus

d)

A negative charge, found outside the nucleus

6.

Which particle is the least massive?

a)

proton

b)

electron

c)

neutron

d)

quark

7.

All atoms of an element have the same

a)

mass number

b)

number of isotopes

c)

atomic number

d)

number of neutrons

8.

The number of neutrons in an atom equals the

a)

Mass number minus atomic number

b)

Atomic number plus number of electrons

c)

Mass number plus atomic number

d)

Atomic number minus mass number

9.

The atomic number of sulfur is 16. How many electrons are there in an atom of sulfur-34?

a)

16

b)

34

c)

18

d)

5

10.

Electrons in the first energy level of an atom

a)

Have no energy

b)

Have the lowest possible energy

c)

Have the highest possible energy

d)

Are in an excited state

e)

Are in an unstable state

11.

What is the mass number of oxygen-18?

a)

8

b)

10

c)

16

d)

18

12.

An electron configuration describes

a)

Regions of space around the nucleus of an atom

b)

Possible energies that an electron can have

c)

The arrangement of electrons in an atom

d)

The emission of light from an excited atom

e)

The number of possible orbitals in an atom

13.

When valence electrons are lost, the atom becomes

a)

Neutral

b)

Positive

c)

Negative

14.

When valence electrons are gained, the atom becomes

a)

Neutral

b)

Positive

c)

Negative

15.

When an atom gains an electron, it is referred to as

a)

Ionization

b)

Reduction

c)

Oxidation

d)

Neutralization

16.

When an atom loses an electron, it is referred to as

a)

Ionization

b)

Reduction

c)

Oxidation

d)

Neutralization

17.

The energy applied to an outer electron to remove it from its atom

a)

Valence Energy

b)

Ionization Energy

c)

Electron Configuration

d)

Ions

18.

Determine the number of protons in the fluorine atom 19 9 F.

a)

19

b)

9

c)

10

d)

28

19.

What is the oxidation number for Oxygen?

a)

+1

b)

+2

c)

-2

d)

-1

20.

What is the arrow pointing to?

a)

atomic number

b)

atomic name

c)

atomic mass

d)

atomic symbol

21.

Which illustration appropriately depicts the correct Lewis Dot Structure for Florine?

a)

Lewis Dot Structure - A

b)

Lewis Dot Structure - B

c)

Lewis Dot Structure - C

d)

Lewis Dot Structure - D

22.

Atoms with different numbers of neutrons are:

a)

Quarks

b)

Compounds

c)

Molecules

d)

Isotopes

23.

The Lewis dot diagram for an unidentified element is shown below.

Which element could X represent?

a)

Chlorine

b)

Silicon

c)

Nitrogen

d)

Oxygen

24.

What are the elements that flow horizontally across the periodic table?

a)

Periods or Rows

b)

Groups or Families

25.

What are the elements that flow vertically up and down the periodic table?

a)

Periods or Rows

b)

Groups or Families

26.

When an atom loses an electron, it forms a(n)

a)

Anion

b)

Cation

c)

Polyatomic ion

d)

Neutral ion

27.

The elements on the right side of the periodic table are

a)

metals

b)

non-metals

c)

metalloids

28.

A chemical bond that forms when atoms share electrons is always a(n)

a)

Polar bond

b)

Ionic bond

c)

Metallic bond

d)

Covalent bond

29.

When two fluorine atoms share a pair of electrons, the bond that forms is a(n)

a)

Polar bond

b)

Ionic bond

c)

Metallic bond

d)

Non-Polar bond

30.

The compound with the formula SiCl4 is

a)

Silicon chloride

b)

Silicon chlorine

c)

Silicon(I) chloride

d)

Silicon tetrachloride

31.

When the highest occupied energy level is filled with electrons.

a)

Stable electron configuration

b)

valence electrons

c)

polarity

d)

ionization

32.

Which type of solid is likely to be the best conductor of electric current?

a)

Ionic compound

b)

Covalent compound

c)

Metal element

d)

Nonmetal element

33.

What happens to the charge on atoms when they form a polar covalent bond?

a)

the electrons are shared equally by each molecule

b)

the protons and electrons are shared equally by each molecule

c)

the attraction between the shared electrons causes the ends of the molecule to be positive

d)

the attraction between the shared electrons causes one end of the molecule to be positive and the other end to be negative

34.

Why is a rock salt crystal likely to shatter when struck?

a)

When ions with the same charge are pushed closer together, they repel one another

b)

The electrons are removed from the element

c)

The protons are removed from the element

d)

When ions with opposite charges are pulled farther from each other, the crystal shatters

35.

What is the formula for Copper(II) nitrate?

(Note: Remember the Criss-Cross Method)

a)

CuNO3

b)

Cu2(NO3)2

c)

Cu(NO3)2

d)

Cu2NO3

36.

The type of bond where electrons are permanently transferred between atoms.

a)

Covalent bond

b)

Ionic bond

c)

Metallic bond

d)

Polar bond

37.

Which accurately reflects the stages of the scientific method

a)

(1) Hypothesis (2) Observation (3) Experiment (4) Analysis (5) Conclusion

b)

(1) Observation (2) Hypothesis (3) Experiment (4) Analysis (5) Conclusion

c)

(1) Experiment (2) Hypothesis (3) gather data (4) Analyze data (5) disseminate data

d)

(1) Observation (2) Hypothesis (3) Experiment (4) Gather data (5) Analysis (6)

Conclusion

38.

What does the law of conservation of mass state?

a)

Mass cannot be destroyed, but changed to a different form

b)

Mass cannot be created nor destroyed, unless in a chemical reaction

c)

Mass cannot be created

d)

Mass cannot be created, only destroyed

39.

A chemical equation is the representation of:

a)

a chemical reaction by which reactants and products are expressed as ionic and covalent bonds

b)

a chemical reaction by which reactants and products are expressed only as coefficients

c)

a chemical reaction by which reactants and products are expressed as formulas

d)

a chemical ratio of cations and anions

40.

In the equation below, Sodium and Water are:


Na + H2O ----> NaOH + H

a)

Reactants

b)

Products

c)

Substrates

d)

Substances

41.

In the equation below, NaOH and H are the:


Na + H2O ----> NaOH + H

a)

Reactants

b)

Products

c)

Substrates

d)

Substances

42.

_________ reactions take the general form A + B → AB:


Example: 2Na + Cl → 2NaCl

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

43.

_________ reactions take the general form AB → A + B:


Example: 2NaCl → 2Na + Cl2

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

44.

_________ reactions take the general form A + BX → AX + B

Example: 2MgBr + Cl2 → 2MgCl + Br2

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

45.

_________ reactions take the general form AX + BY → AY + BX


Example: MgO + CaS → MgS + CaO

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

46.

The rate at which reactants change into products over time is known as:

a)

Reaction Rates

b)

Reaction Frequency

c)

Chemical Rates

d)

Chemical Reactions

47.

Using the Criss-Cross method, what is the product of the following reactants:


Ca2+ + O2-

a)

CaO

b)

CaO4

c)

CaO2

d)

Ca2O

48.

Using the Criss-Cross method, what is the product of the following reactants:


K+ + ClO4-

a)

KClO3-

b)

KClO2-

c)

KClO

d)

KClO4

49.

Using the Criss-Cross method, what is the product of the following reactants


Cr3+ + O2-

a)

Cr3O2

b)

Cr2O3

c)

Cr6O6

d)

Cr2O6

50.

Identify the balanced equation from the following:

K(s) + Br (l) → KBr(l)

s - solid

l - liquid

aq - aqeous

a)

3K(s) + 3Br (l) → 6KBr(s)

b)

2K(s) + Br(l) → 2KBr(s)

c)

K(s) + Br2 (l) → 2KBr(s)

d)

2K(s) + Br2(l) → 2KBr(s)

51.

Identify the balanced equation from the following:


N2(g) + H2(g) → 2NH3(aq)


s - solid

l - liquid

aq - aqeous

a)

N2(g) + 3H2(g) → 2NH3(g)

b)

N2(g) + 6H2(g) → 2NH(g)

c)

8N(g) + 12H(g) → 8NH3(g)

d)

2N(g) + 3H2(g) → 2NH(g)

52.

Identify the balanced equation from the following:


2Na(s) + Cl2(S) → 4NaCl(s)


s - solid

l - liquid

aq - aqeous

a)

2Na(s) + 2Cl2(g) → 4NaCl(s)

b)

4Na(s) + Cl2(g) → 4NaCl(s)

c)

4Na(s) + 2Cl2(g) → 4NaCl(s)

d)

4Na(s) + 2Cl(g) → 4NaCl(s)

53.

Which of the following are diatomic molecules?

a)

NaCl and MgBr

b)

CO2 and O2

c)

O2 and N2

d)

Ar2 and KCl2

54.

Identify the following:

Aluminum oxide plus potassium chloride yields aluminum chloride plus potassium oxide

a)

AlO4 + KCl2 → AlCl2 + KO

b)

2AlO + 2KCl → 2AlCl + 2KO

c)

AlO4 (s) + KCl2 (s) → AlCl2 (s) + KO2(s)

d)

2AlO2 (s) + 2KCl2(s) → 2AlCl2 (s) + KO2 (s)

55.

The following is a _________________ reaction:


2Na(s) + Cl (g) → 2NaCl(s)

a)

Single Replacement

b)

Double Replacement

c)

Synthesis

d)

Decomposition

56.

The following is a _________________ reaction:


KCl(aq) + AgNO3 (aq) → AgCl(s) + KNO3 (aq)

a)

Single Replacement

b)

Double Replacement

c)

Synthesis

d)

Decomposition

57.

The following is a _________________ reaction:


2H2O(l) → 2H2(g) + O2(g)

a)

Single Replacement

b)

Double Replacement

c)

Synthesis

d)

Decomposition

58.

The following is a _________________ reaction:


H2CO3(aq) → H2O(l) + CO2(g)

Note: the products are water and carbon dioxide

a)

Single Replacement

b)

Double Replacement

c)

Synthesis

d)

Combustion

59.

The parts of a solution are

a)

salt and vapor

b)

solvent and solid

c)

solute and water

d)

solute and solvent

60.

In a solution, the solute is the substance that

a)

Dissolves in the solvent

b)

Is in the greatest quantity

c)

Is the liquid

d)

Is the solid

61.

Ionic compounds produce ions in solution by

a)

dissociation

b)

dispersion

c)

evaporation

d)

condensation

62.

During the formation of a solution – energy is either released or absorbed

a)

Heat of Fusion

b)

Heat of Solution

c)

Sublimation

d)

Neutralization

63.

The process in which an ionic compound separates into ions as it dissolves.


Example: NaCl is broken down in a water solution.

a)

Dissociation

b)

Dispersion

c)

Ionization

64.

The process in which an ionic compound separates into ions as it dissolves.


Example: NaCl is broken down in a water solution.

a)

Dissociation

b)

Dispersion

c)

Ionization

65.

The process (chemical change) in which neutral molecules gain or loose electrons

a)

Dissociation

b)

Dispersion

c)

Ionization

66.

Which of the following is NOT characteristic of an acid?

a)

Tastes sour

b)

Reacts with metals

c)

Turns litmus paper blue

d)

Produces H2O (hydronium) ions in solution

67.

The maximum amount of a solute that dissolves in a given amount of solvent at a constant temperature.

a)

saturated

b)

supersaturated

c)

unsaturated

68.

A solution that has less than the maximum amount of solute that can be dissolved

a)

saturated

b)

supersaturated

c)

unsaturated

69.

A solution that contains more solute than it can handle – at a given temperature

a)

saturated

b)

supersaturated

c)

unsaturated

70.

A solution of sodium hydroxide (NaOH) in water is most likely to have a pH close to


Note: do not disregrard the hydroxide ion.

a)

12

b)

7

c)

5

d)

3

71.

Which pH indicates a solution of an acid?

a)

3

b)

7

c)

9

d)

14

e)

19

72.

Which pH indicates a solution of an base?

a)

3

b)

7

c)

9

d)

14

e)

19

73.

Acids produce the following ions:

a)

H3O+

b)

H2O

c)

OH-

d)

ClO4-

74.

Bases produce the following ions:

a)

H3O+

b)

H2O

c)

OH-

d)

ClO4-

75.

The picture depicts the detection of _________________.

a)

Acid

b)

Base

76.

The picture depicts the detection of _________________.

a)

Acid

b)

Base

77.

According to the pH scale given, baking soda (registers as a 9) is considered:

a)

a strong acid

b)

a strong base

c)

a weak acid

d)

a weak base

78.

Proton donors are

a)

acids

b)

bases

79.

Proton acceptors are

a)

acids

b)

bases

80.

What is the SI unit for mass?

a)

grams

b)

meters

c)

liters

d)

pounds

81.

A process where energy leaves the system - such as freezing or an explosion

a)

exothermic reaction

b)

endothermic reaction

82.

A process where energy enters the system - such as baking a cake or cooking an egg.

a)

Exothermic

b)

Endothermic

83.

A physical change whereby an object phase changes from a solid to a gas - without transitioning through the liquid phase.

a)

sublimation

b)

vaporization

c)

evaporation

d)

boiling

84.

Which of the substances is not an element?

a)

hydrogen

b)

aluminum

c)

water

d)

argon

85.

When a homemade oil-and-vinegar salad dressing is left standing, it separates into layers. The salad dressing is a

a)

solution

b)

suspension

c)

colloid

d)

compound

86.

The Manipulated variable is:

a)

The variable that responds to the experiment

b)

The "independent variable" or variable that can be changed in an experiment

c)

The variable that never changes

d)

The variable that changes in response to other variables

87.

What phase of matter is the arrow pointing to?

a)

solid

b)

liquid

c)

gas

d)

plasma

88.

4.29 cm2 x 3.24 cm2 = ______. What is the solution in scientific notation?

a)

13.9 cm2

b)

13.8996 cm2

c)

14 cm2

d)

13.89 cm2

89.

in What phase is the "x"?

a)

solid

b)

liquid

c)

gas

90.

Identify the phase of matter.

a)

solid

b)

liquid

c)

gas

d)

plasma

91.

Identify the phase of matter.

a)

solid

b)

liquid

c)

gas

d)

plasma

92.

Identify the phase of matter.

a)

solid

b)

liquid

c)

gas

d)

plasma

93.
The beta particle can initially be stopped by
a)
a thin sheet of paper
b)
a thin sheet of metal (i.e. aluminum)
c)
a quarter inch of lead
d)
1.5 inches of concrete
94.
The alpha particle can initially be stopped by
a)
a thin sheet of paper
b)
a thin sheet of metal (i.e. aluminum)
c)
a quarter inch of lead
d)
1.5 inches of concrete
95.
Gamma rays can initially be stopped by
a)
a thin sheet of paper
b)
a thin sheet of metal (i.e. aluminum)
c)
a quarter inch of lead
d)
a liquid substance
96.

The image is a representation of a _________; it has the same make up as a __________.

a)

alpha particle; helium nucleus

b)

beta particle; helium nucleus

c)

gamma particle; carbon nucleus

d)

hydrogen nucleus; alpha particle

97.
What type of reaction is represented by the following?
9140Zr → 9141Nb + -01e
a)
alpha decay
b)
beta decay
c)
gamma decay 
d)
delta decay
98.
What type of reaction is represented by the following?
24395Am→ 23993Np + 42He
a)
alpha decay
b)
beta decay
c)
gamma decay 
d)
delta decay
99.
Fill in the mission requirements.
21084Po → 20682Pb + _____
a)
-01e
b)
42He
c)
H3O+
d)
OH-
100.
Fill in the mission requirements.
146C → 147N + _____
a)
-01e
b)
42He
c)
H3O+
d)
OH-
101.

The type of reaction that occurs in the sun

a)

fission

b)

fusion

c)

neutralization

d)

ionization

102.

The reaction depicted is

a)

nuclear fusion

b)

nuclear fission

103.

The reaction depicted is

a)

nuclear fusion

b)

nuclear fission

104.

nuclear power plants are based on the principles of

a)

nuclear fission

b)

nuclear fusion

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