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2nd Semester Chemistry Final Exam

Total questions: 86

Worksheet time: 4hrs 42mins

Name
Class
Date
1.
Atoms form bonds:
a)
To become more stable
b)
To become neutral
c)
To be happy
d)
To gain potential energy
2.
What is the correct formula for calcium oxide?
a)
Ca2O2
b)
Ca2O
c)
CaO
d)
CaO2
3.
In covalent bonds, atoms...
a)
share a pair of electrons
b)
share an electron
c)
transfer electrons
d)
have an electron sea
4.
What is the name of the following compound: AlBr3?
a)
Aluminum bromine
b)
Aluminum bromate
c)
Aluminum bromide
d)
Aluminum (III) bromide
5.
Which type of atoms tend to form ionic bonds with each other?
a)
Metals only
b)
Metals and nonmetals
c)
Nonmetals only
d)
Noble Gases only
6.
Which of the following is not a property or characteristic of ionic bonds?
a)
High melting and boiling points
b)
Brittleness
c)
Non-Conductive in solid state
d)
Low melting points
7.
What's another name for an ionic compound?
a)
Salt
b)
Molecule
c)
Metal
8.
What is the name of the following polyatomic ion: OH-
a)
hydroxide
b)
peroxide
c)
chlorate
d)
water
9.
The roman number in "Copper (II) Sulfide" represents what?
a)
The charge of Copper
b)
The charge of Sulfur
c)
The number of Copper atoms in the formula
d)
The number of Sulfur in the formula
10.
What is the name of NH4+?
a)
Ammonium
b)
Ammonia
c)
Nitrate
d)
Nitrite
11.
What is the name of N3-?
a)
Nitride ion
b)
Nitrogen ion
c)
Nitride
d)
Nitrogen (III)
12.
Energy is ___________ when a bond is formed.
a)
Released
b)
Absorbed
13.
In an ionic bond, electrons are
a)
transferred
b)
shared
14.
Ionic compounds have what charge?
a)
Positive
b)
Negative
c)
Neutral
15.
What is the name of Al2O3?
a)
Aluminum oxide
b)
Aluminum (II) oxide
c)
Aluminum (III) oxide
d)
Aluminum peroxide
16.
What is the formula for Lead (IV) phosphate?
a)
Pb3PO
b)
Pb3(PO4)4
c)
Pb4(PO4)3
d)
Pb4P3O12
17.
The following describes which kind of bond:
-hard
-brittle
-solid
-high melting and boiling point
a)
Ionic
b)
Metallic
c)
Noble gas
d)
Halogen
18.
What is the molar mass of ammonium sulfate?
a)
132.14052 g/mol
b)
132.14052 amu
c)
114.10206 g/mol
d)
114.10206 amu
19.
How many grams are in 5.38 moles of Na2S?
a)
419.8850052 g
b)
420. g
c)
0.068934112 g
d)
0.0689 g
20.
What is the percentage of iron in Iron (III) Hydroxide?
a)
52.257% Fe
b)
90.784% Fe
c)
62.148% Fe
d)
76.656% Fe
21.
What is the empirical formula of a compound that contains 56.34% Copper and 43.66% Sulfide?
a)
Cu2S3
b)
CuS
c)
CuS1.5
d)
Cu3S2
22.
What is another name for a covalent compound?
a)
Molecule
b)
Salt
c)
Metallic bond
d)
Nonmetal
23.
What is the formula for nitrogen monoxide?
a)
NO
b)
N2O
c)
NO2
d)
Not enough information in name
24.
The empirical formula of a molecule is CH.  If its molar mass is 78.11364, what is its molecular formula?
a)
C6H6
b)
CH
c)
C4H4
d)
C8H8
25.
Which of the following is a property of something that is covalent bonded?
a)
Has low electrical conductivity
b)
Has high heat conductivity
c)
Malleable
d)
Ductile
26.
When atoms bond, they become
a)
more stable
b)
less stable
c)
molecules
d)
compounds
27.
Which type of covalent bond has an uneven distribution of electrons between atoms?
a)
Polar
b)
Nonpolar
c)
Ionic
d)
Hydrogen
28.
What is the name for P2O10 using the prefix?
a)
Diphosphorus decoxide
b)
Diphosphorus decaoxide
c)
Diphosphorus decaxide
d)
Phosphorus (II) oxide
29.
What is the name of the CH4 using the prefix system?
a)
carbon tetrahidride
b)
monocarbon tetrahidride
c)
carbon (IV) hydride
d)
carbide tetrahydrogen
30.
In an endothermic reaction, energy is _____________.  In an exothermic reaction energy is ____________.
a)
absorbed; released
b)
released; absorbed
c)
conserved; released
d)
released; conserved
31.
How do atoms reach stability with a covalent bond?
a)
Two atoms share 2 electrons
b)
An atom accepts an extra electron
32.

Identify the type of reaction of the following:

P4 + 3 O2 -> 2 P2O3

a)

Combustion

b)

Synthesis

c)

Double Replacement

d)

Single Replacement

33.
Exergonic reactions release energy.  Exothermic reactions specifically release which of the following?
a)
Heat
b)
Light
c)
Sound
34.
What is an example of an inhibitor?
a)
lemon juice on fruit (slow down browning)
b)
digestive enzymes (speed up digestion)
35.
What is the definition of a catalyst?
a)
Something that speeds up a rxn
b)
Something that slows a rxn
c)
Something that makes more products
d)
Something that makes more reactants
36.
The number in red is what?
2Mg + O2 -> 2MgO
a)
Subscript
b)
Coefficient
c)
Mole ratio
37.
True or false: Reactants are on the right side of the chemical equation
a)
False
b)
True
38.
What mass of water is required to absorb 170 KJ of thermal energy when the temperature increases from 23oC to 62oC?
a)
1.0x103 g
b)
1000 g
c)
1042 g
d)
1040 g
39.
How much thermal energy in kJ must be transferred as heat to 250 g of water to raise the temperature from 32oC to 100oC
a)
1.0x102 kJ
b)
100 kJ
c)
99.6 kJ
d)
99600 J
40.
The formula for oxygen gas is
a)
O
b)
O2
c)
O2 (g)
d)
2 O
41.

Write the balanced skeleton equation for the following:

aluminum bromide and chlorine gas react to form aluminum chloride and bromine gas.

a)

2 AlBr3 + 3 Cl2 -> 2 AlCl3 + 3 Br2

b)

AlBr3 + 3 Cl -> AlCl3 + 3 Br

c)

AlBr + Cl -> AlCl + Br

d)

2 AlBr + Cl2 -> 2 AlCl + Br2

42.

Which of the following are evidence of a chemical change?

a)

Solid forms

b)

Bubbles from heating

c)

Color change

d)

Light produced

e)

Temperature change

43.
What is the amount produced in a perfect reaction called?
a)
Theoretical yield
b)
Actual yield
c)
Percent Yield
d)
Stoichiometry
44.

What does percent yield compare?

a)

Percent Yield

b)

Actual Yield

c)

Theoretical Yield

d)

Concentration

45.
What is the amount produced from experimentation called?
a)
Actual Yield
b)
Theoretical Yield
c)
Percent Yield
46.
What's the percent yield of a reaction where through experimentation 34.2g of Rb are produced?  Theoretical yield is 39.7 g
a)
86.14609572%
b)
86.1%
c)
116%
d)
116.08187135%
47.
Using the pictured equation, how many moles of hydrogen can you make with 7.9 g Zn?
a)
.12 g
b)
.121 g
c)
520 g
d)
517 g
48.
Using the pictured equation, how many moles of ZnCl2 are in 13 moles of HCl?
a)
6.5
b)
26
49.
Using the pictured equation, how many grams of zinc chloride are produced from 7.89 moles of zinc?
a)
1075 g ZnCl2
b)
1080 g ZnCl2
c)
.05789 g ZnCl2
d)
.0579 g ZnCl2
50.
4.3 grams of sodium reacts with 2.6 grams of oxygen to produce 5.9 grams of sodium oxide.  What's the limiting reactant?
a)
Na
b)
NaO
c)
O2
51.
What is the mole ratio of Sulfur to Oxygen? (Hint: Balance the equation first!)
a)
1/8
b)
8/8
c)
1/1
d)
8/1
52.
What is the term for the compounds on the left side of the arrow?
a)
Products
b)
Reactants
53.
Which of the following is the reactant that you have enough of?
a)
Excess reactant
b)
Limiting reactant
c)
Stoichiometric reactant
d)
Theoretical reactant
54.
The amount of product formed depends on the excess reactant
a)
True
b)
False
55.
Which of the following is Charles Law?
a)
P1V1 = P2V2
b)
V1/T1=V2/T2
c)
V1T1=V2T2
d)
P1/V1=P2/V2
56.
Which of the following is Avogadro's Law?
a)
V1/n1=V2/n2
b)
P1/n1=P2/n2
c)
T1/n1=T2/n2
d)
R1/n1=R2/n2
57.
Which of the following is Dalton's Law of Partial Pressures?
a)
V1/P1=V2/P2
b)
­       Ptotal = P1 + P2 + P3 + P4 …
58.
Which of the following is not one of the 5 requirements that all ideal gases must obey?
a)
Volume is assumed to be zero
b)
Particles do not attact/repel each other
c)
Kinetic energy is indirectly related to temperature
d)
Particles are in constant, random motion
59.

What is the volume of 2 moles of gas at STP?

a)

22.4 L

b)

44.8 L

c)

40 L

d)

20 L

60.
What is the molar volume of an ideal gas at STP?
a)
1 mol = 22.4 L
b)
1 mol = 0.0821 L
c)
1 mol = 1 L
d)
1 mol = 273 L
61.
If I have 4 moles of a gas at a pressure of 5.6 atm and a volume of 12 liters, what is the temperature?
a)
204 K
b)
200 K
c)
2046 K
d)
2000 K
62.
What volume is occupied by 0.250 mol of CO2 gas at 25° C and 371 torr?
a)
12.5 L
b)
13 L
c)
.00805 L
d)
.0080 L
63.

Consider this reaction:

P4 + 6 H2 -> 4 PH3


What volume of Hydrogen gas at 27˚ C and 1.25 atm is required to react with 5.65 g of Phosphorous?

a)

5.39 L

b)

5.4 L

c)

21.6 L

d)

22 L

64.
A solution that has not reached limit of solute is
a)
Unsaturated
b)
Saturated
c)
Supersaturated
d)
Concentrated
65.
Something that is supersaturated:
a)
has more solute than it can hold at a certain temp
b)
has not reached its limit of solute
c)
can dissolve more solute
d)
can be dissolved
66.
The substance that is present in the largest amount (typically water) is
a)
Solute
b)
Solvent
c)
Solution
d)
Soluble
67.
Something that is soluble
a)
can be dissolved
b)
cannot be dissolved
68.
14.83 g of CuO is dissolved in 250. mL of solution.  What is the molarity of the solution?
a)
0.746 M
b)
0.7457 M
c)
0.75 M
d)
0.8 M
69.

If the mass percent of a NaCl solution was 38.5%, what mass of NaCl was added to make 300.g of NaCl solution?

a)

115 g

b)

116 g

c)

115.5 g

d)

120 g

70.

How many moles of HCl are needed to prepare 2.0 L of a .50 M HCl solution?

a)

1.0 mol

b)

1 mol

c)

0.2 mol

d)

0.25 mol

71.
What volume of 12 M NaOH must be used to prepare 0.50 L of .25 M NaOH
a)
0.010 M
b)
0.01 M
c)
96 mL
d)
96.4 mL
72.

Moles solute/Liters solution

a)

Molarity

b)

Mass Percent

c)

Molality

d)

Dilute

73.

Large amount of solute in a solvent

a)

Concentrated

b)

Dilute

c)

Saturated

d)

Supersaturated

74.
This is the part of a solution that dissolves
a)
Solute
b)
Solvent
c)
Solution
d)
Mixture 
75.
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
76.

Which of the following does not describe a base?

a)

Slippery

b)

Bitter

c)

Sour

d)

pH above 7

77.

What is the conjugate base of water?

a)

Hydroxide

b)

Hydronium

c)

A Proton

d)

An electron

78.

What type of solution tastes bitter?

a)

Acidic

b)

Basic

c)

Neutral

d)

Amphoteric

79.

What is the conjugate base of HCN?

a)

H2CN+

b)

H2CN-

c)

CN+

d)

CN-

80.

Which of the following is typically the type of solution in cleaning products?

a)

Acidic

b)

Basic

c)

Neutral

d)

Amphoteric

81.

H+ is also called:

a)

hydronium

b)

hydroxide

c)

a proton

d)

an electron

82.

What is the pH of a solution with a pOH of 5.89?

a)

8.11

b)

8

c)

4.11

d)

4

83.

What is the pOH of a solution with a hydroxide concentration of 3.5x10-8?

a)

7.5

b)

6.5

c)

1.0

d)

13

84.

What is the pH of a solution with a hydronium concentration of 2.12x10-2 M?

a)

1.67

b)

12.3

c)

1.00

d)

0

85.

What is the pH of a solution with a hydroxide concentration of 4.53x10-4 M?

a)

10.7

b)

3.34

c)

1.00

d)

13.0

86.

What is the concentration of hydronium for a solution with a pOH of 10.4?

a)

2.51x10-4 M

b)

3.60 M

c)

3.98x10-11 M

d)

10.4 M

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