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Final Exam Review Part 2H

Total questions: 112

Worksheet time: 3hrs 13mins

Name
Class
Date
1.
What elements generally make an ionic bond?
a)
metal and nonmetal
b)
2 nonmetals
c)
metal
d)
none of the above
2.
What elements generally make a covalent bond?
a)
metal and nonmetal
b)
2 nonmetals
c)
metal
d)
none of the above
3.
The number of _____ is most important in determining how an atoms will bond. 
a)
Neutrons
b)
Protons
c)
Valence Electrons
d)
Electron sin the innermost shell
4.
What type of bond is illustrated above?
a)
Metallic
b)
Ionic
c)
Covalent
d)
Wiggly
5.
A substance which has a high melting point, conducts electricity when dissolved in water, and has a crystalline structure probably has what type of bond?
a)
Ionic
b)
Metallic
c)
Covalent
d)
Crystalline
6.

A mixture of two or elements at least one of which is a metal is called

a)

an ion

b)

an alloy

c)

steel

d)

a crystal

7.

A solid substance is an excellent conductor of electricity in both solid and molten states and is malleable and ductile. The chemical bonds in this substance are most likely?

a)
ionic, because the valence electrons are shared between atoms
b)
covalent, because the valence electrons are mobile
c)
metallic, because the valence electrons are stationary
d)
metallic, because the valence electrons are mobile
8.

Bonds formed by transferring electrons from one atom to another are

a)

ionic

b)

metallic

c)

non polar covalent

d)

covalent

9.

Bonds formed by sharing electrons between atoms are

a)

ionic

b)

metallic

c)

covalent

d)

dipole-dipole

10.

A compound that is a poor conductor and has low melting and boiling points is most likely

a)

ionic

b)

metallic

c)

covalent

11.
Which is the name of the kind of solid substance formed in this figure?  
a)
aqueous 
b)
precipitate
c)
acid
d)
synthesis 
12.

Describes the number of molecules or moles in a compound and is used to balance a chemical reaction. 

a)
coefficient 
b)
subscript
c)
superscript
d)
SI unit
13.
What are the correct coefficients when this equation is balanced?
KClO3  --> KCl  +  O2
a)
2,2,2
b)
2,2,3
c)
1,2,3
d)
3,3,3
14.
Potassium iodide is a catalyst in a chemical reaction where would this be placed when writing the chemical reaction? 
a)
product side
b)
reactant side
c)
above the arrow
d)
left out 
15.

If an element is diatomic it should have a subscript of___

a)

1, always

b)

2, only when it is an element

c)

it shouldn't have a subscript, it should have a coefficent

d)

2, when bonded in a compound

16.

The symbol for a substance dissolved in water is ______

a)

(s)

b)

(l)

c)

(aq)

d)

(g)

17.

Predict the products of this synthesis reaction: H2 + Cl2 →

a)

HCl

b)

H2Cl2

c)

H2Cl

d)

HCl2

18.

What type of reaction is this?

2 C6H14 + 19 O2 → 12 CO2 + 14 H2O

a)

Single Replacement

b)

Double Replacement

c)

Combustion

d)

Decomposition

19.

Predict the products for the decomposition of aluminum oxide, Al2O3 →

a)

Al + O2

b)

O + Al2

c)

Al2 + O3

d)

Al + O

20.

What type of reaction is shown below?

Zn + 2HCl --> ZnCl2 + H2

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

21.
Which of the following is not evidence of a chemical reaction?
a)
Formation of a precipitate
b)
Production of gas
c)
Change in temperature
d)
Change in state of matter
22.
Mass cannot be ____ or _____.
a)
made, changed
b)
created, destroyed
c)
rearranged, unmade
d)
stagnant, unchanging
23.

Which of the following is an example of synthesis?

a)

Na + Br2 → NaBr

b)

KClO3 → KCl + O2

c)

HgO + Cl2 →HgCl + O2

d)

Cl2 + NaBr → NaCl + Br2

24.

What type of reaction is this?

NO2 → N2 + O2

a)

Synthesis

b)

Decomposition

c)

Single replacement

d)

Combustion

e)

Double replacement

25.

Which of the following chemical equations is an example of a double replacement reaction?

a)

2Al2O3 ⟶ 4Al + 3O2

b)

2C5H10 + 15O2 ⟶ 10CO2 + 10H2O

c)

2MgCl2 + Na2CO3 ⟶ 2 NaCl + MgCO3

d)

K2O + H2O ⟶ 2 KOH

26.

Unlike Ionic compounds, Covalent compounds require what when naming them?

a)

A roman numeral

b)

A charge

c)

A prefix

27.

When is the prefix mono not used?

a)

It is never used when naming covalent compounds

b)

It is never used on the second element

c)

It is never used when on the first element

28.

What is the name for NI3?

a)

Mononitrogen TretraIodide

b)

Nitrogen Triiodide

c)

Nitrogen (III) Triiodide

d)

Nitrogen Iodide

29.

What is the name for P2O5?

a)

Diphosphorous Pentaoxide

b)

Phosphorous Oxide

c)

Phosphorous (III) Oxide

d)

Diphosphide Oxide

30.

The name of FeCl₂ is

a)

iron chloride

b)

iron (II) chloride

c)

iron (I) chloride

d)

iron dichloride

31.

LiBr is called

a)

lithium bromine

b)

lithium (I) bromine

c)

lithium bromide

d)

lithuim (I) bromide

32.
How many particles are in a mole?
a)
602
b)
602 million
c)
602 moles
d)
6.02 x 1023
33.

Calculate the molar mass for Al(OH)3

a)

78.0 g/mol

b)

72 g/mol

c)

28 g/mol

d)

25 g/mol

34.
How many particles would be in 8.4 moles of Octane (C8H18)?
a)
5.77 x 1023
b)
5.04 x 1024
c)
5.77 x 1026
d)
5.04 x 1023
35.
What is the mass of 0.89 mol of CaCl2?
a)
111 grams
b)
0.008 grams
c)
98.9 grams
d)
none of the choices
36.

Convert 86.235 g of diphosphorus pentaoxide to moles.

a)

12240 moles

b)

1.8747 moles

c)

.608 moles

d)

.60755 moles

37.

How many molecules are there in 5.5 moles potassium chloride?

a)

4.08 x 10-24

b)

3.31 x 1024

c)

33.11

d)

0.98

38.

What is the percent by mass of fluorine in CaF2 (molar mass = 78 g/mol)?

a)
24%
b)
49%
c)
51%
d)
65%
39.

What is the percent by mass of calcium in CaF2 (molar mass = 78 g/mol)?

a)
24%
b)
49%
c)
51%
d)
65%
40.
If a chemist calculates the maximum amount of product that could be obtained in a chemical reaction, he or she is calculating the
a)
theoretical yield
b)
mole ratio
c)
actual yield
d)
percentage yield
41.
What is the measured amount of a product obtained from a chemical reaction?
a)
mole ratio
b)
theoretical yield
c)
percentage yield
d)
actual yield
42.
Mole ratios are obtained from the
a)
balanced chemical equation
b)
periodic table
c)
molar mass
43.
What is the mole ratio of H2O to H3PO4 in the following chemical equation?   P4O10 + 6 H2O --> 4 H3PO4 
a)
6:4
b)
4:6
c)
1:3
d)
3:1
44.
When does a chemical reaction stop?
a)
When the lab is finished
b)
When the excess reactant is used up
c)
When the limiting reactant is used up
d)
Chemical reactions never stop
45.
Using the following equation:
Fe2O3(s) + 3H2(g) → 2Fe(s) + 3H2O(l)
How many moles of iron can be made from  6 moles H2? 
a)
4 moles Fe
b)
6 moles Fe
c)
9 moles Fe
d)
2 moles Fe
46.

Fe (s) + S (l) --> FeS (s)   In the reaction above, 6.78 g of FeS was measured to have been produced, but 7.84 g was calculated to be produced. What is the % yield of FeS (s)?

a)
14.8 g
b)
12.2 g
c)
13.7 g
d)
19.9 g
47.
At higher temperatures
a)

particles in an object move faster and have less KE

b)

particles in an object move faster and have more KE

c)

particles in an object move slower and have more KE

48.

What letter on the diagram represents a gas?

a)

A

b)

B

c)

C

d)

D

49.

What letter on the diagram represents the triple point?

a)

A

b)

B

c)

C

d)

D

50.

What line segment represents only the solid state? (Diagram F)

a)

A-B

b)

B-C

c)

C-D

d)

D-E

51.

Between which points is the temperature of the substance remaining constant? (Diagram F)

a)

A-B only.

b)

A-B, C-D, E-F

c)

B-C only.

d)

B-C, D-E

52.

A substance's heating curve is shown in the graph. What is its boiling point? (Diagram B)

a)

100 C

b)

60 C

c)

80 C

d)

20 C

53.

Is the substance gaining or losing energy? (Diagram D)

a)

Gaining

b)

Losing

54.

What will occur when the substance changes from 1 atm to 30 at a constant temperature of -15oC? (Diagram A)

a)

condensation

b)

deposition

c)

melting

d)

sublimation

55.

**An ice cube feels cold when we hold it. Which of the following best explains why?

a)

Heat moves from our hands into the ice cube.

b)

Cold moves from our hands into the ice cube.

c)

Heat moves from the ice cube into our hands.

d)

Cold moves from the ice cube into our hands.

56.

What is the normal boiling point of this substance? (Diagram C)

a)

150 °C

b)

100 °C

c)

-50 °C

d)

0 °C

57.
All changes in the state of matter of a substance requires
a)
vibration
b)
water
c)
permission
d)
energy
58.
In which segment is the kinetic energy remaining constant?
a)
A-B
b)
B-C
c)
C-D
d)
E-F
59.

Where on the graph are phase changes taking place?

a)

1

b)

2

c)

3

d)

4

e)

5

60.
Which of the following pairs of substances may best be separated through distillation
a)
 sand and soil
b)
water and soil
c)
salt and sand
d)
 water and alcohol
61.

This diagram represents...

a)

An element

b)

A molecule

c)

A compound

d)

A mixture of elements and compounds

62.
What type of mixture is this?
a)
heterogeneous 
b)
homogeneous
63.
Sand floating in water, but most of the sand is settled at the bottom this an example of which type of mixture?
a)
A solution
b)
A colloid
c)
A suspension
d)
A compound
64.
A solution that is considered dilute would be....
a)
Dark in color
b)
Have a strong scent
c)
Have a large amount of solute
d)
Have a small amount of solute
65.

In a solution the substance that dissolves in the solvent.

a)

Solute

b)

Suspension

c)

Colloid

d)

Solvent

66.

In a solution the substance which the solute dissolves

a)

solvent

b)

suspension

c)

colloid

d)

solution

67.
____ is another name for a homogeneous mixture. 
a)
Solution
b)
Suspension
c)
Substance
d)
Liquid 
68.

A mixture with more solute dissolved in the solvent than is usually soluble is called:

a)

concentrated

b)

supersaturated

c)

saturated

d)

unsaturated

69.

Which of the following is NOT a unit used to express concentration?

a)

Molality

b)

Molarity

c)

Mass percent

d)

Density

70.
How many grams of K2Cr2O7, are soluble in 100 g of water at 95 ºC?
a)
83 grams
b)
75 grams
c)
40 grams
d)
12 grams
71.
Which substance is MOST soluble at 0 ºC?
a)
KI
b)
NaNO3
c)
NaCl
d)
Ce2(SO4)3
72.
When 50 grams of KCl is dissolved in 100 grams of water at 50 ºC, the solution can be correctly described as:
a)
supersaturated
b)
unsaturated
c)
saturated
73.
When materials combine to form a mixture, they
a)
A. keep their original properties.
b)
B. react to form a new substance with new properties.
c)
C. combine in a specific ratio.
d)
D. always change their physical state.
74.

Solubility refers to the ____ of solute that can dissolve in a certain volume or mass of solvent, at a certain temperature.

a)

Mean

b)

Range

c)

Amount

d)

Mode

75.
An unsaturated solution is one that....
a)
contains the maximum amount of dissolved solute.
b)
contains less solute than a saturated solution.
c)
contains more solute than a saturated solution.
d)
is the amount of a substance required to form a saturated solution.
76.
An electrolyte is...
a)
The rapid, random movement of particles in colloidal dispersion.
b)
A substance that dissolves in water and conducts electric current.
c)
A substance that dissolves in water and does not conduct electric current.
d)
The solution process when water is the solvent.
77.
What is the molarity of a 2 liter solution containing 5 moles of NaCl?
a)
2.5
b)
0.4
c)
2.5 moles/liter
d)
10 moles/liter
78.
Which of the following would dissolve the slowest?
a)
a sugar cube in hot water
b)
a sugar cube in cool water
c)
powdered sugar in cool water
d)
powdered sugar in hot water
79.

Which of the following factors affects the solubility of solutes?

a)

temperature

b)

polarity of solute and solvent

c)

stirring

d)

both a and b

80.

What is the correct order for obtaining salt from a mixture of sand and salt?

a)

Dissolving in water - filtration – evaporation

b)

Evaporation - filtration - dissolving in water

c)

Filtration - dissolving in water - evaporation

d)

Dissolving in water – evaporation - filtration

81.

Which mixture can be separated using a filtration method?

a)

oil and water

b)

sand and iron powder

c)

sand and water

d)

water and ethanol

82.

Dyes in water soluble markers may be separated by means of..

a)

crystallization

b)

sublimation

c)

chromatography

d)

sedimentation

83.

When KCl (potassium chloride) is dissolved in water, how many particles are in solution for each unit?

a)

1

b)

2

c)

3

d)

4

e)

6

84.

Which techniques could increase or speed up the rate of dissolving?

a)
Allowing the mixture to settle
b)
Stirring the mixture
c)

stirring and heating the mixture

d)
Adding more water
85.
Colligative properties depend on the _________ of the solute but not the __________ of the solute.
a)
 concentration; identity
b)
identity; concentration
c)
reactivity; nature
d)
nature; reactivity
86.

When CaBr2 is dissolved in water, how many particles will be in solution for each unit?

a)

1

b)

2

c)

3

d)

4

e)

5

87.

At the same concentration, which salt will have the largest effect on the freezing point?

a)

C2H4O2

b)

H2S

c)

LiBr

d)

CaF2

88.
Colligative properties depend on the _____ of solute particles in solution.
a)
type
b)
number
c)
pH
d)
nature
89.
The freezing point of a solution is ____ the freezing point of the pure solvent.
a)
the same as
b)
lower than
c)
higher than
d)
no relation to
90.
The boiling point of a solution is ______ the boiling point of the pure solvent.
a)
higher than
b)
the same as
c)
lower than
d)
higher or lower than
91.

The van't Hoff factor measures the number of particles formed in solution. What is the van't Hoff factor for the compound Na2SO4?

a)

1

b)

3

c)

5

d)

7

92.

Electrolytes have a greater effect on colligative properties than nonelectrolytes do because electrolytes

a)

are volatile

b)

have higher boiling points

c)

produce fewer moles of solute particles per mole of solvent

d)

produce more moles of solute particles per mole of solvent

93.
Why are ions formed?
a)
To make our lives difficult
b)
Because atoms want 8 valence electrons
c)
Because atoms have the same number of protons and electrons
d)
Because atoms gained neutrons
94.
An atom becomes _________ when it gains electrons.
a)
Positive
b)
Negative
c)
Neutral
d)
Invinsible
95.
Group 17 always has ions with a charge of 
a)
+1
b)
+2
c)
-1
d)
-2
96.

Which group has a -3 charge?

a)

group 13

b)

group 3

c)

group 15

d)

group 14

97.
Cations are...
a)
Positive
b)
Negative
c)
Neutral
d)
Purring
98.
Anions are...
a)
Positive
b)
Negative
c)
Neutral
d)
Crying
99.
An atom becomes _______ when it loses electrons.
a)
Positive
b)
Negative
c)
Neutral
d)
Invinsible
100.

Elements in group 2 will form ions with what charge?

a)
-2
b)
-1
c)
+1
d)
+2
101.

What's the first thing you should do when you see a temperature in Celsius?

Ex: 48°C48\degree C  

a)

add 273

b)

subtract 273

c)

multiply 273

d)

divide 273

102.

When gas particles collide with the side of the container, it creates

a)

volume

b)

pressure

c)

temperature

d)

quantity

103.

Flask A has hydrogen gas and Flask B has oxygen gas. Both are kept at the same temperature and same pressure. What conclusion can you make?

a)

Flask A has more gas particles.

b)

Flask B has more gas particles.

c)

Flask A and B have equal particles.

d)

There's not enough information.

104.

What temperature scale must we use in the Gas Laws?

a)

Rankine

b)

Fahrenheit

c)

Kelvin

d)

Celsius

105.

How do we measure an increase in kinetic energy?

a)

volume

b)

temperature

c)

Liters

d)

none of the above

106.

A sample of He gas (2.35 mol) occupies 57.9 L at 300.0 K and 1.00 atm. The volume of this sample is ___L at 423 K and 1.00 atm.

a)

0.709 L

b)

57.9 L

c)

41.1 L

d)

81.6 L

e)

1.41 L

107.

A sample of a gas (5.0 mol) at 1.0 atm is expanded at constant temperature from 10.0 L to 15.0 L. The final pressure is ___ atm.

a)

1.5 atm

b)

15 atm

c)

0.67 atm

d)

3.3 atm

e)

7.5 atm

108.

A gas sample is held at constant pressure. The gas occupies 3.62 L of volume when the temperature is 21.6°C. Determine the temperature at which the volume of the gas is 3.42 L.

a)

312K

b)

278K

c)

20.4K

d)

295K

e)

552K

109.
Determine the number of moles in a container of gas at STP with a volume of 99.2 L. 
a)
2222.08 moles
b)
4.43 moles
c)
22.4 moles 
d)
76.8 moles
110.

What is the pressure exerted by 5.00 moles of nitrogen gas contained in a 30.0 Liter container at 25.0 °C?

a)

3670 atm

b)

0.245 atm

c)

4.08 atm

d)

605 atm

111.

A sample of a gas (5.0 mol) at 1.0 atm is expanded at constant temperature from 10.0 L to 15.0 L. The final pressure is ___ atm.

a)

1.5 atm

b)

15 atm

c)

0.67 atm

d)

3.3 atm

e)

7.5 atm

112.

A sample of He gas (2.35 mol) occupies 57.9 L at 300.0 K and 1.00 atm. The volume of this sample is ___L at 423 K and 1.00 atm.

a)

0.709 L

b)

57.9 L

c)

41.1 L

d)

81.6 L

e)

1.41 L

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