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Final Exam Review

Total questions: 83

Worksheet time: 3hrs 53mins

Name
Class
Date
1.
What is the correct term for "bond that forms when electrons are shared equally"?
a)
ionic bond
b)
metallic bond
c)
nonpolar covalent bond
d)
polar covalent bond
2.
What is the correct term for "bond that forms between a metal and a nonmetal"?
a)
ionic bond
b)
metallic bond
c)
nonpolar covalent bond
d)
polar covalent bond
3.
What is the correct term for "atom with more protons than electrons"?
a)
positive ion (cation)
b)
negative ion (anion)
c)
neutral atom
d)
stable atom
4.
What is the correct term for "atom with more electrons than protons"?
a)
positive ion (cation)
b)
negative ion (anion)
c)
neutral atom
d)
stable atom
5.
Which of the following formulas represents the harmful gas, carbon monoxide?
a)
CO
b)
CO2
c)
NO
d)
SO2
6.
Which two elements would form an ionic bond?
a)
carbon and hydrogen
b)
oxygen and silicon
c)
cesium and iodine
d)
potassium and calcium
7.
The correct chemical formula for magnesium phosphide is
a)
MgP
b)
Mg₂P₃
c)
Mg₃P₂
d)
Mg₃(PO₄)₂
8.

Which equation is balanced?

a)

PbO2 + 2H2--> H2SO4

b)

SO2 + H20 --> H2SO4

c)

2Na + 2H2O --> 2NaOH + H2

d)

2Na + 2H2O --> 2NaOH + H

9.

3NH4NO3 + Na3PO4 --> (NH4)3PO4 + 3 NaNO3

Assuming we start with 30 g of NH4NO3 and 50 g of Na3PO4, identify the limiting reactant.

a)

ammonium phosphate

b)

sodium phosphate

c)

ammonium nitrate

d)

sodium nitrate

10.

3NH4NO3 + Na3PO4 --> (NH4)3PO4 + 3 NaNO3

Assuming we start with 30 g of NH4NO3 and 50 g of Na3PO4, What is the maximum amount of each product that can be formed?

a)

18.6 g of ammonium phosphate, 31.9 of sodium nitrate

b)

54 g of ammonium phosphate, 31.9 of sodium nitrate

c)

32.4 g of ammonium nitrate, 76 g of sodium phosphate

d)

21 g of ammonium nitrate, 34 g of sodium phosphate

11.

3CaCO3 + 2FePO4 --> Ca3(PO4)2 + Fe2(CO3)3

Assuming we start with 100 g of CaCO3 and 45 g of FePO4, How much of the excess reagent is left over after the reaction is complete?

a)

57.3 g of sodium phosphate

b)

54.0 g of calcium carbonate

c)

25 g of calcium carbonate

d)

16.9 g of iron(III) carbonate

12.
CH4  +  2O2  →  CO2  +  2H2O
24 grams of CH4 was added to the above reaction. Calculate the theoretical yield of CO2.
a)
66 grams
b)
132 grams
c)
33 grams
d)
8.72
13.

2Fe2O3 + C → Fe + 3CO2

You add 28 grams of carbon. You find the actual yield to be 181.2 grams of CO2. What is the percent yield of CO2?

a)

58.83%

b)

308%

c)

6435%

d)

15.5

14.
What is the molar mass of NaOH?
a)
40 g/mol
b)
38.989 g/mol
c)
23.998 g/mol
d)
57.004 g/mol
15.
How many molecules of sugar (C6H12O6) are in a mole?
a)
24 molecules
b)
180 molecules
c)
180 g
d)
6.02 x 1023 molecules
16.
You have 3.5 L of H2 (g) at STP. How many moles of gas are there?
a)
22.4 mol
b)
22.4 L
c)
0.16 mol
d)
0.16 L
17.

What is the percent composition by mass of magnesium in the compound MgSO4 (molar mass = 120 g/mol)?

a)
20%
b)
27%
c)
46%
d)
53%
18.
Calculate the volume that a 0.323-mol sample of a gas will occupy at 265 K and a pressure of 0.900 atm.
a)
7.18 L 
b)
7.81 L
c)
4.63 L
d)
4.36 L
19.
How many moles of propane gas are in a 7.0 L tank at 20°C and 5.45atm of pressure?
a)
0.629 mol
b)
1.59 mol
c)
23.2 mol
d)
917 mol
20.

If I initially have 4.0 L of a gas at a pressure of 1.1 atm, what will the volume be if I increase the pressure to 3.4 atm?

a)

1.29 L

b)

12.36 L

c)

1.29 atm

d)

12.36 atm

21.

A rigid plastic container holds 1.00 L methane gas at 0.9 atm pressure when the temperature is 22.0°C. How much more pressure will the gas exert if the temperature is raised to 44.6°C?

a)

0.97 atm

b)

1.82 atm

c)

0.97oC

d)

1.82oC

22.

Molarity is measured in _____.

a)

moles per g.

b)

mols per L.

c)

moles per mm.

d)

moles per mL.

23.

What is the molarity of a 0.5L sample of a solution that contains 60.0 g of sodium hydroxide (NaOH)

a)

0.8 M

b)

1.5M

c)

3.0M

d)

6.0M

24.
Which of the following substances is a heterogeneous substance?
a)
baby oil
b)
rocky road ice cream
c)
salt water
d)
milk
25.

Which of the following types of solutions has more room to dissolve solute?

a)

supersaturated

b)

saturated

c)

unsaturated

26.
What is a solvent?
a)
The substance that does the dissolving in a solution.
b)
The substance that is being dissolved in a solution.
c)
The mixing of different substances.
d)
The process in which neutral molecules lose or gain electrons
27.
The concentration of a mixture can be increased in which of the following ways?
a)
Heating the mixture
b)
Adding more water “solvent”
c)
Adding more powder “solute”
d)
Stirring the mixture
28.
Another name for a homogeneous mixture is 
a)
an element.
b)
a solution.
c)
a compound.
29.

If water is a polar molecule, then which of the following must be nonpolar

a)

sugar

b)

salt

c)

oil

d)

juice

30.

Electrolytes

a)

don't conduct electricity

b)

conduct electricity

31.

Which of the following will produce crystals if cooled or disturbed?

a)

unsaturated solution

b)

saturated solution

c)

supersaturated solution

d)

all of the above

32.

Since "like dissolves like", water and oil will not mix because

a)

both of them are polar

b)

both of them are nonpolar

c)

oil is polar and water is nonpolar

d)

oil is nonpolar and water is polar

33.
What is the correct name for NO?
a)
Mononitrogen Monoxide
b)
Nitrogen Monoxide
c)
Mononitrogen Dioxide
d)
Nitrogen Oxide
34.
What is Sulfur Trichloride?
a)
SCl3
b)
SiCl3
c)
SCl4
d)
Si3Cl
35.
What is the OFFICIAL name for H2O
a)
Hydrogen Oxide
b)
Oxygen Dinitride
c)
Agua
d)
Dihydrogen Monoxide
36.
Covalent bonds are between...
a)
Metal and Non-metal
b)
Non-metal and Non-metal
c)
Metal and Metal
37.

During an exothermic reaction, heat content in the surroundings increases because

a)

heat energy is destroyed during reactions

b)

the reaction absorbs heat energy

c)

the energy contained in the reactants is lower then the products

d)

the energy contained in the products is lower than the reactants

38.

A cast iron skillet is used to fry bacon. For optimal frying, the pan must be heated to about 178 oC from a room temperature of 22.0 oC. It is known that 1.58 x 105 J of heat energy are absorbed by the pan to reach the desired temperature and the specific heat of iron is 0.450 J/g oC. What must the mass of the skillet be?

a)

12.7 kg

b)

2.25 kg

c)

110 kg

d)

1.97 kg

39.
In an endothermic reaction the system is releasing energy.
a)
True
b)
False
40.
A reaction is performed in a beaker with a temperature probe recording the temperature changes of the reaction.  If the temperature began at 15.0 degrees Celsius and ended at 27.5 degrees Celsius.  If the reaction is our system, is the system endothermic or exothermic?
a)
Exothermic
b)
Endothermic
41.
For the formula:
 Q= m c ∆T
The  units for specific heat are:
a)
g /J C
b)
°C/g J
c)
kJ/g
d)
J/g°C
42.

If the specific heat of water is 4.18 J/g∙°C, how much heat is required to increase the temperature of 1.2 kg of water from 23 °C to 39 °C? (show your work)

a)

-80,256 J

b)

80.256 J

c)

80,256 J

d)

-80.256 J

43.
What is the specific heat of an unknown substance if 100.0 g of it at 200.0 °C reaches an equilibrium temperature of 27.1 °C when it comes in contact with a calorimeter of water.  The water weighs 75. g and had an initial temperature of 20.00 °C?  (Specific heat of water is 4.18 J/g°C) (show your work)
a)
0.111 J/g°C
b)
1.29 J/g°C
c)
0.129 J/g°C
d)
22225.85 J
44.
The SI unit of heat and energy is the __________.
a)
calorie
b)
heat
c)
joule
d)
watt
45.
When the rate of the forward reaction is equal to the rate of backward reaction, the system is said to be in
a)
Chemical Equilibrium
b)
Chemical Balance
c)
Chemical Constant
d)
Chemical Reaction
46.
For the reaction...
SO2 + O2 <=>  SO3
If the equilibrium position shifts to the right, the concentration of O2 will ___________.
a)
increase
b)
decrease
c)
remain the same
d)
double
47.
For the reaction...
SO2 + O2  <=>  SO3
If the concentration of SO2 is increased, the equilibrium position of the reaction will shift ___________.
a)
to the left
b)
to the right
c)
to the left and right 
d)
neither left nor right
48.

For the reaction...

N2 + O2 <=> 2NO + 182kJ (the 182 kJ means heat)

If the temperature is increased the equilibrium position will shift _______.

a)

to the left

b)

to the right

c)

to the left and right

d)

neither left nor right

49.

For the following reaction: H2(g) + Cl2 (g) ↔ 2HCl(g), calculate the concentration of HCl when Keq= 2.3x10-5, [H2]= 0.0056mol, [Cl2]= 0.0048mol.

a)

6.2 x 10-10 M

b)

2.5 x 10-5 M

c)

1.1 M

d)

1.2 M

50.

If K of a reaction is larger than one, the ________________ reaction was favored, if K is smaller than one, the ______________ reaction was favored.

a)

forward, reverse

b)

reverse, forward

c)

neither reaction was favored in either reaction at equilibrium

51.

What is the value of the Keq/Kc of the reaction "CO(g)+2H2(g)<---> CH3OH(g)" if the equilibrium concentrations of the reactants and product are: CO=0.17M, H2=0.34M, and CH3OH= 0.17M?

a)

0.085

b)

8.7

c)

0.12

d)

2.9

52.

What is the molarity of a 0.101 L solution containing 40.0 grams of NaCl? (molar mass of NaCl is 58.44)

a)

0.00678 M

b)

400 M

c)

6.78M

d)

0.396 M

53.
As you move down a group, atomic radius increases because - 
a)
you add more and more neutrons
b)
you add more and more protons
c)
you add more and more shells (energy levels)
d)
you add more atomic mass
54.
The atom with the largest atomic radius in Group 18 is - 
a)
Ar
b)
He
c)
Kr
d)
Rn
55.
The atom with the largest atomic radius in Period 4 (row 4) is - 
a)
K
b)
Kr
c)
Fe
d)
Fe
56.
Francium (Fr) has the lowest ionization energy in Group 1 because - 
a)
it has the smallest number of valence electrons
b)
it has the greatest atomic mass
c)
it has the greatest number of protons, so it attracts its electrons the strongest
d)
its 1 valence electron is very far from the nucleus, so little energy is needed to remove it
57.
As you move across the periodic table atoms tend to get smaller because, ______________.
a)
the atoms have more mass.
b)
the atoms have less mass
c)
the atoms have more protons.
d)
the atoms have less electrons.
58.
What is the name of family I
a)
Alkaline Earth Metals
b)
Boron Family
c)
Alkali Metals
d)
Halogen Family
59.
Families all have similar 
a)
Names
b)
atomic numbers
c)
atomic masses
d)
properties
60.
Which has the greater Electronegativity: 
N or C?
a)
C
b)
N
61.

What is a negatively-charged ion which forms when an atom gains electrons?

a)

cation

b)

anion

c)

electron

d)

ion

62.

Which of the following will have similar properties to 1s2 2s2 2p6 3s2 3p2?

a)

carbon

b)

calcium

c)

chlorine

d)

cesium

63.

Identify the Electron Configuration for Aluminum (Al)

a)

1s2 2s2 2p6 3s2 3p1

b)

1s2 2s2 2p6 3s2 3p3

c)

1s2 2s2 2p6 3s2 4p1

64.

What is the noble gas notation electron for Sulfur?

a)

[Ne] 3p4

b)

[He] 3s2 3p4

c)

[Ne] 3s2 3p4

d)

[Na] 3s2 3p4

65.

A student measures the pressure and volume of an empty water bottle to be 1.4 atm and 2.3 L. She then decreases the pressure to 0.65 atm. What is the new volume?

a)

2.1 L

b)

5.0 L

c)

8.2 L

d)

3.9 L

66.

What is the pressure of a car tire that had an initial pressure of 1.8 atm but was heated from 38°C to 123°C?

a)

0.9 atm

b)

2.1 atm

c)

1.6 atm

d)

3.4 atm

67.
What is 50 °C in Kelvin?
a)

223.15

b)

323.15

c)

100.15

d)

50.15

68.
Calculate the volume that a 0.323-mol sample of a gas will occupy at 265 K and a pressure of 0.900 atm.
a)
7.18 L 
b)
7.81 L
c)
4.63 L
d)
4.36 L
69.

What is the volume of 1 mole of gas at 298K at a pressure of 101,000Pa?

a)

24.5dm3

b)

24.5m3

c)

0.0245dm3

d)

0.0021m3

70.

What is the volume of 0.036 moles of gas at 450K at a pressure of 80,000Pa?

a)

1.7dm3

b)

0.0016m3

c)

0.117dm3

d)

0.017m3

71.

What is the volume of 5.5x10-3 moles of gas at 15oC at a pressure of 18KPa?

a)

0.72dm3

b)

38dm3

c)

0.04dm3

d)

0.0007m3

72.

  1. Which two variables of the electromagnetic spectrum have a direct relationship?
    (there may be more than one correct answer)

a)

Crests and trough

b)

Energy and frequency

c)

Wavelength and energy

d)

Frequency and wavelength

73.

Which of the following radiation has the lowest energy?

a)

Radio

b)

X-Rays

c)

Gamma Rays

d)

Visible

74.
Solve this problems using the equation: C = λ  x  ν
If an AM radio station broadcasts at 9.95 x 105 Hz, what is the wavelength of this radiation?
a)
6.59 x 10-28 m
b)
1.01 x 10-6 m
c)
3.32 x 10-3 m
d)
301 m
75.

Microwaves are used to cook food and transmit information. What is the wavelength of a microwave that has a frequency of 3.44 × 109 Hz?

For this problem, what formula do you use?

a)

c = λν

b)

E = hv

c)

λ = c/v

d)

v = c/λ

76.

Calculate the wavelength of the yellow light emitted by the street light, if the frequency of the radiation is 5.10x1014Hz.

a)

5.12 x 10-7m

b)

5.88 x 10-7 m

c)

4.20 x 1014m

d)

3.0 x 108m

77.
Kool-Aid - Powder, sugar, and water
Identify the solvent 
a)
water
b)
powder
c)
sugar
d)
powder and sugar
78.
Contains the maximum amount of dissolved solute
a)
unsaturated solution
b)
supersaturated solution
c)
saturated solution
79.
What mass of NaCl is needed to prepare 850 mls of 6.0 M NaCl solution?
a)
5.1 grams
b)
0.087 grams
c)
87 grams
d)
298 grams
80.
What is the molarity of  420 mls of a KCl solution that contains 16.0 grams of KCl
a)
625 M
b)
0.51 M
c)
3.19 M
d)
0.00563 M
81.

Water is polar, this means:

a)

both the H and O are negative

b)

the O is slightly negative and the H's are slightly positive

c)

water will dissolve oil

d)

hydrogen is slightly negative

82.

When a substance will not dissolve in water:

a)

soluble

b)

insoluble

c)

ionic

d)

moleculear

83.

A solution is:

a)

a homogenous mixture of two or more substances

b)

a pure substance

c)

a heterogenous mixture of only water

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