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Chemistry 202 Semester 2 Exam Review

Total questions: 139

Worksheet time: 1hrs 10mins

Name
Class
Date
1.

What forms ionic bonds?

a)

metal and nonmetal

b)

even distribution of electrons in a bond between nonmetals

c)

uneven distribution of electrons between nonmetals

d)

metal and metal

2.

What forms polar covalent bonds?

a)

metal and nonmetal

b)

even distribution of electrons in a bond between nonmetals

c)

uneven distribution of electrons between nonmetals

d)

metal and metal

3.

What forms nonpolar covalent bonds?

a)

metal and nonmetal

b)

even distribution of electrons in a bond between nonmetals

c)

uneven distribution of electrons between nonmetals

d)

metal and metal

4.

What forms polar metalic bonds?

a)

metal and nonmetal

b)

even distribution of electrons in a bond between nonmetals

c)

uneven distribution of electrons between nonmetals

d)

metal and metal

5.

Which can dissolve in water? (Select all that apply)

a)

Ionic

b)

Nonpolar covalent

c)

Polar covalent

d)

Metalic

6.

Which has the highest melting/boiling points?

a)

Ionic

b)

Nonpolar covalent

c)

Polar covalent

d)

Metalic

7.

Which has the lowest melting/boiling points?

a)

Ionic

b)

Nonpolar covalent

c)

Polar covalent

d)

Metalic

8.

Which of the below has a pool of electrons?

a)

Ionic

b)

Nonpolar covalent

c)

Polar covalent

d)

Metalic

9.

How many valence electrons can there be in the valence shell (maximum #)?

a)

10

b)

12

c)

8

d)

14

10.

Which Lewis dot structure is this:

a)

Ionic

b)

Covalent

c)

Polyatomic

11.

Which Lewis dot structure is this:

a)

Ionic

b)

Covalent

c)

Polyatomic

12.

Which VSEPER shape is this:

a)

Tetrahydral

b)

Trigonal Pyramidal

c)

Bent

d)

Trigonal Planar

e)

Linear

13.

Which VSEPER shape is this (it has one lone pair):

a)

Tetrahydral

b)

Trigonal Pyramidal

c)

Bent

d)

Trigonal Planar

e)

Linear

14.

Which VSEPER shape is this (it has one lone pair):

a)

Tetrahydral

b)

Trigonal Pyramidal

c)

Bent

d)

Trigonal Planar

e)

Linear

15.

Which VSEPER shape is this (it has two lone pairs):

a)

Tetrahydral

b)

Trigonal Pyramidal

c)

Bent

d)

Trigonal Planar

e)

Linear

16.

Which VSEPER shape is this:

a)

Tetrahydral

b)

Trigonal Pyramidal

c)

Bent

d)

Trigonal Planar

e)

Linear

17.

Which VSEPER shape is this:

a)

Tetrahydral

b)

Trigonal Pyramidal

c)

Bent

d)

Trigonal Planar

e)

Linear

18.

Which VSEPER shape is 109.5 degrees?

a)

Tetrahydral

b)

Trigonal Pyramidal

c)

Bent

d)

Trigonal Planar

e)

Linear

19.

Which VSEPER shape is 106.5 degrees?

a)

Tetrahydral

b)

Trigonal Pyramidal

c)

Bent

d)

Trigonal Planar

e)

Linear

20.

Which VSEPER shape is 104.5 degrees?

a)

Tetrahydral

b)

Trigonal Pyramidal

c)

Bent

d)

Trigonal Planar

e)

Linear

21.

Which VSEPER shape is 120 degrees?

a)

Tetrahydral

b)

Trigonal Pyramidal

c)

Bent

d)

Trigonal Planar

e)

Linear

22.

Which VSEPER shape is 118.5 degrees?

a)

Tetrahydral

b)

Trigonal Pyramidal

c)

Bent

d)

Trigonal Planar

e)

Linear

23.

Which VSEPER shape is 180 degrees?

a)

Tetrahydral

b)

Trigonal Pyramidal

c)

Bent

d)

Trigonal Planar

e)

Linear

24.

As you go right across the periodic table, electronegativity gets:

a)

stronger

b)

weaker

c)

it stays the same

25.

As you go up the periodic table, electronegativity gets:

a)

stronger

b)

weaker

c)

it stays the same

26.

If the absolute value of the difference between two atom's electronegativity is greater than _______ but less than _______ it is polar covalent.

a)

.4

b)

2

c)

1

d)

3

27.

If the absolute value of the difference of two atom's electronegativity is less than __________, it is not polar

a)

.4

b)

2

c)

1

d)

3

28.

If the absolute value of the difference of two atom's electronegativity is greater than __________, it is ionic

a)

.4

b)

2

c)

1

d)

3

29.

If the polar bonds cancel out they are

a)

not polar

b)

still polar

30.

To determine whether a molecule is polar or not, it must be drawn in the proper

a)

lewis dot structure

b)

vsepr shape

31.

Intermolecular forces are

a)

between molecules

b)

inside one molecule

32.

Intramolecular forces are

a)

between molecules

b)

inside one molecule

33.

LDF, Dipole-Dipole, and hydrogen bonds are

a)

intermolecular forces

b)

intramolecular forces

34.

LDF:

a)

weakest force. temporarily attractive. all molecules interact with this force.

b)

attraction between positive and negative sides of two molecules.

c)

positive and negative ends of covalent molecules made of hydrogen bonding to N, O, or F

35.

Dipole-Dipole:

a)

weakest force. temporarily attractive. all molecules interact with this force.

b)

attraction between positive and negative sides of two molecules.

c)

positive and negative ends of covalent molecules made of hydrogen bonding to N, O, or F

36.

Hydrogen Bonds:

a)

weakest force. temporarily attractive. all molecules interact with this force.

b)

attraction between positive and negative sides of two molecules.

c)

positive and negative ends of covalent molecules made of hydrogen bonding to N, O, or F

37.

As the strength of intermolecular forces increase, the surface tension, viscosity, boiling point and melting points

a)

Increase

b)

Decrease

c)

Stay the same

38.

The resistance of a substance to spreading out is called the

a)

surface tension

b)

viscosity

c)

boiling points/melting points

39.

The resistance of a liquid to flow is called the

a)

surface tension

b)

viscosity

c)

boiling points/melting points

40.

Water has what molecular forces? (Select all that apply)

a)

London Dispersion Forces

b)

Dipole-Dipole

c)

Hydrogen

41.

Water having all three intermolecular forces means

a)

that it can become any shape and any state

b)

that it is forced to remain as a liquid

42.

Which items allow oil and water to mix by breaking the oil into smaller drops?

a)

Water

b)

Iron

c)

Soap

43.

Why does soap allow oil and water to mix?

a)

Soap is polar

b)

Soap is non-polar

c)

Soap has two different ends, one that loves water and one that hates it.

44.

Dissoving is called

a)

hydration

b)

dehydration

c)

sumblimination

d)

electrolytation

45.

To dissolve something there must be a _________ and a _________. (Select all that apply)

a)

Solute

b)

Solvent

c)

Electrolyte

d)

Non-electrolyte

46.

The substance that dissolves is

a)

a solvent

b)

a solute

47.

The substance that is dissolved is

a)

a solvent

b)

a solute

48.

As new intermolecular forces are formed between a solvent and solute, the solvent ________ the solute particles

a)

destroys

b)

carries off

c)

becomes

d)

ignores

49.

Free-floating ions in the solution allow electricity to be conduncted. What is this free-floating ion called?

a)

Electrolyte

b)

Non-electrolyte

c)

Ionic compound

50.

A solution in which no more solute can be dissolved

a)

saturated

b)

non-saturated

c)

super-saturated

51.

A solution in which more solute can be dissolved

a)

saturated

b)

unsaturated

c)

super-saturated

52.

A solution which has been heated up to dissolve more solute, then cooled down.

a)

saturated

b)

unsaturated

c)

super-saturated

53.

How does temperature affect solubility?

a)

Solubility increases with higher temperature

b)

Solubility stays the same with higher temperature

c)

Solubility decreases with higher temperature

54.

What is the formula for concentration?

a)

W/V x 100 = % (w/v)

b)

M = mols of solute/Liters of solvent

55.

What is the formula for molarity?

a)

W/V x 100 = % (w/v)

b)

M = mols of solute/Liters of solvent

56.

Fill in the blanks: If you know the ______, you also know the mass, which means you can convert the mass into ______ using the molecular mass. Then, use the mols solute to find morality.

a)

% w/v

b)

mols

c)

solute

d)

molarity

57.

Which is the proper way to find the concentration of ions?

a)

CaCl2 --> Ca+2 + 2 Cl-1

b)

NaCl --> 1NaCl+0

c)

FeCl2 --> Fe+1 + Cl2-2

58.

Which is the formula for finding pH?

a)

-log[H3O+1]

b)

10-pH

59.

Which is the formula for finding acidity?

a)

-log[H3O+1]

b)

10-pH

60.

The lower the pH, the _______ the acid.

a)

Stronger

b)

Weaker

61.

The higher the pH, the _______ the base.

a)

Stronger

b)

Weaker

62.

___ is the "neutral" number on the pH scale.

a)

8

b)

9

c)

7

d)

6

63.

Which reaction is used in solubility and precipitation reactions?

a)

single replacement

b)

double replacement

c)

decomposing

d)

combustion

64.

aq means

a)

dissolves in water

b)

solid

c)

gas

65.

s means

a)

dissolves in water

b)

solid

c)

gas

66.

If the attractions between the ions and the water is stronger than the attractions between ions, then the compound is

a)

soluble

b)

insoluble

67.

Ionic compounds are more stable with each other then they are when hydrated (in water), so they _____ separate into electrolytes and dissolve/

a)

do

b)

don't

68.

What is the mole ratio?

a)

the numbers infront of an element or compound in a chemical equation

b)

the mols of an element compared to the mols of another

c)

always 2:1

d)

it doesn't exist

69.

Balance the equation: __ H2 + __ O2 --> __ H2O

a)

2;1;2

b)

2;2;1

c)

1;2;2

d)

1;2;1

70.

If your stoichiometry problems starts with mols and you need to end in mols, you

a)

continue with the mol ratio

b)

continue with the mol ratio and then use the molar mass

c)

convert into mols and use the mole ratio

d)

convert into mols, use the mol ration, then use molar mass

71.

If your stoichiometry problems starts with mols and you need to end in grams, you

a)

continue with the mol ratio

b)

continue with the mol ratio and then use the molar mass

c)

convert into mols and use the mole ratio

d)

convert into mols, use the mol ration, then use molar mass

72.

If your stoichiometry problems starts with grams and you need to end in grams, you

a)

continue with the mol ratio

b)

continue with the mol ratio and then use the molar mass

c)

convert into mols and use the mole ratio

d)

convert into mols, use the mol ration, then use molar mass

73.

If your stoichiometry problems starts with grams and you need to end in mols, you

a)

continue with the mol ratio

b)

continue with the mol ratio and then use the molar mass

c)

convert into mols and use the mole ratio

d)

convert into mols, use the mol ration, then use molar mass

74.

What is STP? (select all that apply)

a)

Standard Temperature and Pressure

b)

22.4 L

75.

What is a limiting reactant?

a)

A reactant that keeps the reaction going even after it runs out

b)

A reactant that stops the reaction after it runs out

76.

How do you calculate which reactant is the limiting reactant?

a)

Finding out which has either the fewest mols/lowest mass

b)

Finding out what has the largest amount of mols/greater mass

77.

Use ______ to calculate the limiting reactant.

a)

Stoichiometry

b)

% w/v

c)

Molarity

78.

What is endothermic?

a)

a reaction that requires the absorption of heat

b)

a reaction that requires the release of heat

79.

What is exothermic?

a)

a reaction that requires the absorption of heat

b)

a reaction that requires the release of heat

80.

What is a system?

a)

molecules directly involved in the reation

b)

molecules not involved in the reation

81.

What are the surroundings?

a)

molecules directly involved in the reation

b)

everything not involved in the reation

82.

What is heat?

a)

the flow of energy from higher temp particles to lower temp particles

b)

the initial energy of the sample along with the pressure and volume

83.

What is enthalpy?

a)

the flow of energy from higher temp particles to lower temp particles

b)

the initial energy of the sample along with the pressure and volume

84.

which are units of energy?

a)

joules

b)

calories

c)

mols

d)

grams

85.

4.18 J = ______

a)

1 calorie

b)

4.18 cals

c)

1 mol

d)

4.18 mols

86.

Heat capacity is

a)

the amount of energy that can be absorbed before 1g of a substance's temperature has increased by 1 degree Celsius

b)

the use of energy changes in the surroundings to find energy changes in the system

87.

Calorimetry is

a)

the amount of energy that can be absorbed before 1g of a substance's temperature has increased by 1 degree Celsius

b)

the use of energy changes in the surroundings to find energy changes in the system

88.

Which is the equation for heat capacity?

a)

Change in Heat = m x Cp x (T2 - T1)

b)

Change in surroundings = -H of the system

89.

Which is the equation for calorimetry?

a)

Change in Heat = m x Cp x (T2 - T1)

b)

Change in surroundings = -H of the system

90.

Why doesn't the temperature change while things change their state of matter?

a)

There is no energy being used to change state, so nothing changes the temperature

b)

All of the energy is going into changing states by breaking IMF's

91.

What is Hfus (heat of fusion)?

a)

The energy that goes into melting 1g of something

b)

The energy that goes into boiling 1g of something

92.

What is Hvap (heat of vaportizatioin)?

a)

The energy that goes into melting 1g of something

b)

The energy that goes into boiling 1g of something

93.

Going from solid to liquid is

a)

+Hfus

b)

-Hfus

c)

+Hvap

d)

-Hvap

94.

Going from liquid to solid is

a)

+Hfus

b)

-Hfus

c)

+Hvap

d)

-Hvap

95.

Going from liquid to gas is

a)

+Hfus

b)

-Hfus

c)

+Hvap

d)

-Hvap

96.

Going from gas to liquid is

a)

+Hfus

b)

-Hfus

c)

+Hvap

d)

-Hvap

97.

A heating curve shows

a)

how temp changes as energy is added

b)

how temperature goes up

c)

how energy goes up

98.

Moving ______ the heating curve requires engery (exo.) and going __________ releases energy (endo.).

a)

up; down

b)

down; up

99.

Label A

a)

Solid only

b)

Liquid only

c)

Gas only

d)

Solid and liquid

e)

Liquid and gas

100.

Label B

a)

Solid only

b)

Liquid only

c)

Gas only

d)

Solid and liquid

e)

Liquid and gas

101.

Label C

a)

Solid only

b)

Liquid only

c)

Gas only

d)

Solid and liquid

e)

Liquid and gas

102.

Label D

a)

Solid only

b)

Liquid only

c)

Gas only

d)

Solid and liquid

e)

Liquid and gas

103.

Label E

a)

Solid only

b)

Liquid only

c)

Gas only

d)

Solid and liquid

e)

Liquid and gas

104.

What is enthalpy of of formation (Hf)?

a)

Net energy change during a chemical reaction

b)

Energy change when 1 mole of a compound is formed from elemental state

105.

What is enthalpy of Reaction (Hrxn)?

a)

Net energy change during a chemical reaction

b)

Energy change when 1 mole of a compound is formed from elemental state

106.

(The sum of Hf products) - (The sum of Hf reactants) is the formula for

a)

Enthalpy of reaction

b)

Enthalpy of formation

107.

Enthalpy of Reaction can be used in stoichiometry by

a)

using the mole ratio in the balanced chemical equation

b)

i don't know what to put here so go like look at the notes for 7.4 (it's on the back it makes more sense there)

108.

What is Hess's law?

a)

The sum of the energy changes during a series of reactions is equal to the sum of the reaction

b)

percentage by mass of an element in compound

c)

proportions of the elements present in a compound but not the actual numbers or arrangement of atoms

d)

number of atoms of each of the elements present in one molecule of a specific compound

109.

What is percent composition?

a)

The sum of the energy changes during a series of reactions is equal to the sum of the reaction

b)

percentage by mass of an element in compound

c)

proportions of the elements present in a compound but not the actual numbers or arrangement of atoms

d)

number of atoms of each of the elements present in one molecule of a specific compound

110.

What is an empirical formula?

a)

The sum of the energy changes during a series of reactions is equal to the sum of the reaction

b)

percentage by mass of an element in compound

c)

Chemical formula of a compound that is the lowest possible ration of atoms (not always real)

d)

number of atoms of each of the elements present in one molecule of a specific compound

111.

What is a molecular formula?

a)

The sum of the energy changes during a series of reactions is equal to the sum of the reaction

b)

percentage by mass of an element in compound

c)

proportions of the elements present in a compound but not the actual numbers or arrangement of atoms

d)

The actual ratio of atoms in a molecule (derived from the empirical formula)

112.

You're going to need to know how to do hess's law problems and it's a lot to make questions asking how to do it. What should you do (like, right now)?

a)

Review 7.5 (sounds like the better idea huh)

b)

I'm good (your loss bud)

113.

You're going to need to know how to do molecular and empirical formula problems and it's a lot to make questions asking how to do it. What should you do (like, right now)?

a)

Review Chapter 9.3 (sounds like the better idea huh)

b)

I'm good (your loss bud)

114.

What is an organic molecule?

a)

Contains carbon atoms bonded to other carbon atoms

b)

Molecules composed of carbon and hydrogen atoms only

c)

Hydrocarbons containing only single bonds

d)

Hydrocarbons containing a double bond

e)

Hydrocarbons containing a double bond

115.

What is a hydrocarbon?

a)

Contains carbon atoms bonded to other carbon atoms

b)

Molecules composed of carbon and hydrogen atoms only

c)

Hydrocarbons containing only single bonds

d)

Hydrocarbons containing a double bond

e)

Hydrocarbons containing a double bond

116.

What is a alkane?

a)

Contains carbon atoms bonded to other carbon atoms

b)

Molecules composed of carbon and hydrogen atoms only

c)

Hydrocarbons containing only single bonds

d)

Hydrocarbons containing a double bond

e)

Hydrocarbons containing a double bond

117.

What is a alkene?

a)

Contains carbon atoms bonded to other carbon atoms

b)

Molecules composed of carbon and hydrogen atoms only

c)

Hydrocarbons containing only single bonds

d)

Hydrocarbons containing a double bond

e)

Hydrocarbons containing a triple bond

118.

What is a alkyne?

a)

Contains carbon atoms bonded to other carbon atoms

b)

Molecules composed of carbon and hydrogen atoms only

c)

Hydrocarbons containing only single bonds

d)

Hydrocarbons containing a double bond

e)

Hydrocarbons containing a triple bond

119.

How do you label an alkane?

a)

By putting the proper prefix infront of -ane

b)

by putting the shortest distance from the double bond, the proper prefix, then -ene

c)

by putting the shortest distance from the double bond, the proper prefix, then -yne

120.

How do you label an alkene?

a)

By putting the proper prefix infront of -ane

b)

by putting the shortest distance from the double bond, the proper prefix, then -ene

c)

by putting the shortest distance from the double bond, the proper prefix, then -yne

121.

How do you label an alkyne?

a)

By putting the proper prefix infront of -ane

b)

by putting the shortest distance from the double bond, the proper prefix, then -ene

c)

by putting the shortest distance from the double bond, the proper prefix, then -yne

122.

Whatsuffix do you use to label hydrocarbon side branches?

a)

-ene

b)

-ane

c)

-yl

d)

-yne

123.

What is a halokane?

a)

hydrocarbons with one or more halogen

b)

contains and "OH" group

c)

contains an "O" between two carbon atoms

d)

a nitrogen with saturated carbons added

124.

What is a alchohol?

a)

hydrocarbons with one or more halogen

b)

contains and "OH" group

c)

contains an "O" between two carbon atoms

d)

a nitrogen with saturated carbons added

125.

What is a ether?

a)

hydrocarbons with one or more halogen

b)

contains and "OH" group

c)

contains an "O" between two carbon atoms

d)

a nitrogen with saturated carbons added

126.

What is a amine?

a)

hydrocarbons with one or more halogen

b)

contains and "OH" group

c)

contains an "O" between two carbon atoms

d)

a nitrogen with saturated carbons added

127.

What is a carboxylic acid?

a)

contains a carbonyl with an OH group

b)

contains a carbonyl with an oxygen atoms off of the carbon

c)

contains a carbonyl with 2 carbons bonded to the carbonyl

d)

contains a carbonyl-oxygen-carbonyl group

128.

What is a aldehyde?

a)

contains a carbonyl with an OH group

b)

contains a carbonyl with an oxygen atoms off of the carbon

c)

contains a carbonyl with 2 carbons bonded to the carbonyl

d)

contains a carbonyl-oxygen-carbonyl group

129.

What is a ketone?

a)

contains a carbonyl with an OH group

b)

contains a carbonyl with an oxygen atoms off of the carbon

c)

contains a carbonyl with 2 carbons bonded to the carbonyl

d)

contains a carbonyl-oxygen-carbonyl group

130.

What is a anhydryde?

a)

contains a carbonyl with an OH group

b)

contains a carbonyl with an oxygen atoms off of the carbon

c)

contains a carbonyl with 2 carbons bonded to the carbonyl

d)

contains a carbonyl-oxygen-carbonyl group

131.

You're going to need to know how to name the functional groups, what should you do (like, right now)?

a)

Review 11.2 (sounds good)

b)

Nothing, I'm good (your loss bud)

132.

Who found x-rays?

a)

Roentgen

b)

Becquerel

c)

Curries

133.

Who found that uranium gave off radiation?

a)

Roentgen

b)

Becquerel

c)

Curries

134.

Who found that some of thorium was radioactive?

a)

Roentgen

b)

Becquerel

c)

Curries

135.

What is nuclear radiation?

a)

he energy particles or rays that are given off from a radioactive element as it decays

b)

helium-4

c)

Wheren the mass number doesn't change but the atomic number increases by one

d)

Wheren the mass number doesn't change as well as the atomic number

e)

time for the mass of a sample to be cut in half

136.

What is an alpha particle?

a)

he energy particles or rays that are given off from a radioactive element as it decays

b)

helium-4

c)

Wheren the mass number doesn't change but the atomic number increases by one

d)

Wheren the mass number doesn't change as well as the atomic number

e)

time for the mass of a sample to be cut in half

137.

What is a beta particle?

a)

he energy particles or rays that are given off from a radioactive element as it decays

b)

helium-4

c)

Wheren the mass number doesn't change but the atomic number increases by one

d)

Wheren the mass number doesn't change as well as the atomic number

e)

time for the mass of a sample to be cut in half

138.

What is a gamma particle?

a)

he energy particles or rays that are given off from a radioactive element as it decays

b)

helium-4

c)

Wheren the mass number doesn't change but the atomic number increases by one

d)

Wheren the mass number doesn't change as well as the atomic number

e)

time for the mass of a sample to be cut in half

139.

What is a half-life?

a)

he energy particles or rays that are given off from a radioactive element as it decays

b)

helium-4

c)

Wheren the mass number doesn't change but the atomic number increases by one

d)

Wheren the mass number doesn't change as well as the atomic number

e)

time for the mass of a sample to be cut in half

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