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CHEMISTRY POST-TEST/FINAL EXAM REVIEW

Total questions: 75

Worksheet time: 59mins

Name
Class
Date
1.

Which of these measurements has been expressed to four significant figures?

a)

0.0420 cm

b)

4020 cm

c)

40200 cm

d)

0.04020 cm

2.

What is the density of silver if a sample has a mass of 46.16 g and occupies a volume of 4.40 mL?

a)

10.49 g/mL

b)

12.00 g/mL

c)

41.8 g/mL

d)

203 g/mL

3.

How many significant figures?

1000

a)

1

b)

2

c)

3

d)

4

4.

Which of these measurements has been expressed to two significant figures?

a)

0.040 cm

b)

4020 cm

c)

42.00 cm

d)

0.02 cm

5.

Which of these measurements has been expressed to three significant figures?

a)

0.040 cm

b)

4020 cm

c)

42.00 cm

d)

0.02 cm

6.
How many significant figure in 0.007?
a)
4
b)
3
c)
1
d)
0
e)

2

7.

Solve and give your answer with the correct number of significant figures
(12.470)(2.73)

a)

34.043

b)

34

c)

34.04

d)

34.0

8.

A 42.44 gram metal causes water to displace from 40.0 mL to 42.2 mL, what is the metal's density (D = m/v)?

a)

silver 10.49 g/cm³

b)

gold, 19.3 g/cm³

c)

aluminum, 2.70 g/cm³

d)

iron, 7.9 g/cm³

9.

A rock has a mass of 50.0 grams and a volume of 30.0 cm3. What is the density of the rock?

a)

0.6 g/cm3

b)

1500 g/cm3

c)

80 g/cm3

d)

1.67 g/cm3

10.

Which of these is not evidence of a chemical reaction?

a)

A gas is given off

b)

The material dissolves

c)

Heat is released

d)

A precipitate forms

11.

The mass of an atom is a result of the

a)

neutrons

b)

nuclear forces

c)

the number of protons and electrons

d)

the number of protons and neutrons

12.

Atoms have a neutral electric charge because they

a)

have an equal number of charged and noncharged particles

b)

have neutrons in their nuclei

c)

have an equal number of electrons and protons

d)

have an equal number of neutrons and protons

13.
The electron configuration of an atom is 1s22s22p6.  The number of electrons in the atom is 
a)
3
b)
6
c)
8
d)
10
14.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
15.

The electron configuration of sulfur is 1s² 2s² 2p⁶ 3s² 3p4. What is the electron configuration of chlorine?

a)

1s² 2s² 2p³

b)

1s² 2s² 2p⁶ 3s² 3p⁴

c)

1s² 2s² 2p⁶ 3s² 3p⁵

d)

1s² 2s² 2p⁶ 3s² 3p⁶

16.

The electron configuration of sulfur is 1s² 2s² 2p⁶ 3s² 3p4. How many valence electrons does sulfur have?

a)

1

b)

2

c)

4

d)

6

17.

The electron configuration of sulfur is 1s² 2s² 2p⁶ 3s² 3p4. What is its Noble gas configuration?

a)

[He]2s² 2p⁶ 3s² 3p4

b)

[He]3s²3p4

c)

[Ne]p4

d)

[Ne]3s²3p4

18.

How many electrons does an Iodine atom have?

a)

53

b)

126

c)

73

d)

179

19.

Iodine is in group 17. How many valence electrons does it have?

a)

7

b)

17

c)

53

d)

127

20.

Calculate the number of moles of a sample containing 7.00 g of silicon atoms (molar mass of Si = 28.0855 g/mol) is approximately

a)

0.125 mol

b)

0.249 mol

c)

8.02 mol

d)

98.3 mol

21.

The molar mass of H₂O is 18.02 g/mol. How many grams of H₂O are present in 0.40 mol?

a)

0.2 g

b)

7.2 g

c)

3.6 g

d)

90.1 g

22.

The electrons involved in the formation of a chemical bond are called

a)

ions

b)

d orbital electrons

c)

electron clouds

d)

valence electrons

23.

When an atom loses electrons it is called a(n) ______ and its charge is ______.

a)

positron, unbalanced

b)

cation, positive

c)

anion, negative

d)

neutrino, neutral

24.

When an atom gains electrons it is called a(n) ______ and its charge is ______.

a)

positron, unbalanced

b)

cation, positive

c)

anion, negative

d)

neutrino, neutral

25.

Metals tend to form a bond with nonmetals by

a)

losing valence electrons

b)

gaining valence electrons

c)

sharing valence electrons

d)

becoming anions

26.

Nonmetals tend to form a bond with nonmetals by

a)

losing valence electrons

b)

gaining valence electrons

c)

sharing valence electrons

d)

becoming anions

27.

What is the correct Lewis structure for fluorine, F2?

a)

F-F

b)

F=F

c)

F::F

d)

:F-F:

28.

LiBr is called

a)

lithium bromine

b)

lithium (I) bromine

c)

lithium bromide

d)

lithuim (I) bromide

29.

What is the formula for the compound formed by calcium ions and chloride ions?

a)

CaCl

b)

Ca2Cl

c)

CaCl2

d)

CaCl3

30.

Which is the correct name for the compound (NH4)2SO4?

a)

nitrogen tetrahydride sulfur tetraoxide

b)

diammonium sulfate

c)

ammonium sulfite

d)

ammonium sulfate

31.

In a polar molecule, there is

a)

a region of positive charge and a region of negative charge.

b)

equal sharing of valence electrons.

c)

a spectator ion.

d)

an equal exchange of ions.

32.

In a nonpolar molecule, there is

a)

a region of positive charge and a region of negative charge.

b)

equal sharing of valence electrons.

c)

a spectator ion.

d)

an equal exchange of ions.

33.
Molar mass is in units of ________.
a)
grams
b)
grams/mole
c)
mole
d)
moles/gram
34.
If an atom of Fluorine has an atomic mass of 19 amu, it has a Molar mass of ____
a)
19 lbs.
b)
19 kg
c)
How am I supposed to know?
d)
19 g/mol
35.

Which of the following combinations of symbol and explanation of symbol is correct when used in a chemical equation?

a)

(g), grams

b)

(l), liters

c)

(aq), dissolved in water

d)

(s), soluble in water

36.

The reaction represented by the equation Pb(NO3)2 + 2HCl → 2HNO3 + PbCl2 is a

a)

synthesis reaction.

b)

decomposition reaction.

c)

single-replacement reaction.

d)

double-replacement reaction.

37.

The reaction represented by the equation 2H2(g) + O2(g) → 2H2O(l) is a(n)

a)

synthesis reaction.

b)

decomposition reaction.

c)

single-replacement reaction.

d)

double-replacement reaction.

38.

The reaction represented by the equation 2Al(s) + 3CuCl2(aq) → 2AlCl3(s) + 3Cu(s) is a

a)

double-replacement reaction.

b)

synthesis reaction.

c)

decomposition reaction.

d)

single-replacement reaction.

39.

When the equation Fe + Cl2 → FeCl3 is balanced, what is the coefficient for Cl2?

a)

1

b)

2

c)

3

d)

4

40.

When the following equation is balanced, what is the coefficient for HCl?

Mg(s) + HCl(aq) → MgCl2(aq) + H2(g)

a)

2

b)

3

c)

6

d)

1

41.

Which equation is NOT balanced?

a)

4H2 + 2O2 → 4H2O

b)

H2 + O2 → H2O

c)

2H2 + O2 → 2H2O

42.

In the equation 2KClO3 → 2KCl + 3O2, which conversion factor would be used to determine how many moles of oxygen are produced when 2.75 mol of KClO3 decompose completely?

a)

2 mol KClO3

3 mol O2

b)

_3 mol O2_

2 mol KClO3

43.

In the equation 2KClO3 → 2KCl + 3O2, how many moles of oxygen are produced when 2.75 mol of KClO3 decompose completely?

a)

4.13 mol

b)

1.83 mol

c)

2.63 mol

d)

5.5 mol

44.

Which of the following controls the amount of product possible in a chemical reaction?

a)

composition reactant

b)

limiting reactant

c)

excess reactant

d)

mole ratio

45.

A sample of oxygen occupies 4.00 L when the pressure is 760.00 mm Hg. At constant temperature, what volume does the gas occupy when the pressure decreases to 665.00 mm Hg?

a)

2.29 L

b)

3.50 L

c)

7.00 L

d)

4.57 L

46.

The compound sodium chloride is placed in water and separates into ions. What are the correct names for these ions?

a)

The sodium ion is the cation and the chloride ion is the anion

b)

The sodium ion is the anion and the chloride ion is the cation

c)

They both form cations

d)

They both form anions

47.

What is the molarity of a solution that contains 5.53 moles KCl in 72.8 L solution?

a)

13.2 M

b)

0.0760 M

c)

0.760 M

d)

0.0194 M

48.

What is the molarity of a solution containing 7.00 moles of solute in 569 mL of solution?

M = mol/L

a)

1.23 M

b)

0.0123 M

c)

12.3 M

d)

0.123 M

49.

How many mL of a 4.0M NaCl solution are needed to make 100.0 mL of 2.0 M NaCl?

M1V1 = M2V2

a)

25 mL

b)

50 mL

c)

100 mL

d)

150 mL

50.

A cylinder of gas particles is shown in the diagram. Which of the following would result in an increase in the pressure of the gas below the piston?

a)

increasing the volume of the cylinder

b)

decreasing the volume of the container

c)

removing some of the gas from the cylinder

d)

decreasing the pressure of the gas outside the cylinder

51.

How many grams of potassium chloride will form a saturated solution at 50°C?

a)

40 g

b)

20 g

c)

80 g

d)

50 g

52.

How many grams of potassium chloride will precipitate out of solution when a saturated solution is cooled from 80°C to 50°C?

a)

70 g

b)

10 g

c)

20 g

d)

50 g

53.

How many grams of Si are there in 1.50 mol of Si if the molar mass of silicon is 28.0855 g/mol?

a)

0.0534 g

b)

84.2 g

c)

42.1 g

d)

5.34 g

54.

What is the mass of water produced from 0.25 mol of H₂O (molar mass = 18.02 g/mol)?

a)

4.5 g

b)

18 g

c)

3.6 g

d)

54 g

55.

What is the molarity of a solution if 3.0 moles of solute is dissolved in 679 mL solution?

a)

226 M

b)

2.04 M

c)

4.42 M

d)

0.00442 M

56.

What happens when the volume of the gas cylinder is decreased when temperature remains constant?

a)

The pressure inside the cylinder increases.

b)

The pressure inside the cylinder decreases.

c)

The pressure outside the cylinder increases.

d)

The pressure outside the cylinder decreases.

57.

Which of the following numbers has the least number of significant figures?

a)

0.0070

b)

700

c)

7.00

d)

0.070

58.

If you multiply 2.501 by 3.2, how many significant figures should the answer have?

a)

2

b)

3

c)

4

d)

5

59.

How many significant figures?

1001.00

a)

2

b)

4

c)

6

60.

How many significant figures?

0.001010

a)

1

b)

2

c)

3

d)

4

61.
What is the molar mass of Fe?
a)
26 g/mole
b)
55.85 g/mole
c)
56 g/mole
d)
6.02 x 1023 g/mole
62.

How is the percent composition of oxygen in carbon dioxide ( CO2CO_2 ) calculated?

a)

mass of Cmolar mass of CO2×100\frac{\text{mass of C}}{\text{molar mass of } CO_2} \times 100

b)

mass of O2molar mass of CO2×100\frac{\text{mass of O}_2}{\text{molar mass of } CO_2} \times 100

c)

molar mass of CO2mass of C×100\frac{\text{molar mass of } CO_2}{\text{mass of C}} \times 100

d)

mass of Omolar mass of CO2×100\frac{\text{mass of O}}{\text{molar mass of } CO_2} \times 100

63.

Which of the following would have the highest mass?

a)

1 mole of Li

b)

1 mole of Au

c)

1 mole of Si

d)

All have the same mass

e)

1 mole of O₂

64.
Based on the info below, solve for the molecular formula:
Empirical formula = NO
Molecular formula mass = 59.98g
a)
NO
b)
N2O3
c)
N2O2
d)
N4O4
65.
What is the molecular formula for a compound with the empirical formula: CaCl2  and a molecular mass of 330g.
a)
Ca2Cl4
b)
Ca3Cl6
c)
Ca3Cl9
d)
Ca3Cl5
66.

A compound's empirical formula is NO2 and its molar mass is 92.02 g/mol. What is its molecular formula?

a)

N 2_2 O 4_4

b)

NO 2_2

c)

N 2_2 O 6_6

d)

N 2_2 O 2_2

67.
What atom matches this electron configuration?
1s2 2s2 2p6 3s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
68.
How many valence electrons does phosphorus have?
a)
5
b)
2
c)
8
d)
15
69.

How many valence electrons are indicated in this electron configuration?

[Xe] 6s2 4f14 5d9

a)

9

b)

11

c)

14

d)

2

70.
What is this element? 
[Ar] 4s2
a)
Calcium
b)
Sodium
c)
Scandium
d)
Titanium
71.

The name of FeCl₂ is

a)

iron chloride

b)

iron (II) chloride

c)

iron (I) chloride

d)

iron dichloride

72.

Which of these combinations is an ionic compound made of?

a)

Metal and Metal

b)

Nonmetal and Nonmetal

c)

Metal and Nonmetal

d)

Cation and Cation

73.

The name of the compound Ca3(PO4)2

a)

calcium phosphate

b)

tricalcium diphosphate

c)

calcium phosphorus oxide

d)

calcium phosphide

74.

How many significant figures are in the following number?

34.900

(a)  

75.

Report your answer w/ the correct number of sig figs:


6.201 + 7.4 + 0.68 + 12.0 =

a)

26.281

b)

26.28

c)

26.2

d)

26.3

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