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Unit 6 Review

Total questions: 162

Worksheet time: 9hrs 45mins

Name
Class
Date
1.
What is the molar mass of C6H12O6?
a)

180.18 g/mol

b)

180.12 g/mol

c)

180.24 g/mol

d)

180.06 g/mol

2.
If you start with atoms of NaOH and are going to moles of NaOH, how many steps is it?
a)
1
b)
2
c)
3
d)
4
3.
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
4.
N2 +  3H2 → 2NH3 
How many moles of hydrogen are needed to react with 2 moles of nitrogen?
a)

6 mol H

b)

2 mol H

c)

3 mol H

d)

1 mol H

5.
2H2   +   O2  →  2H2O
How many moles of water can be produced if 8 moles H2 are used?
a)
4 moles
b)
8 moles
c)
16 moles
d)
2 moles
6.
2 NaClO3 (s) --> 2NaCl (s) +3 O2 (g)  
12.00 moles of NaClO3 will produce how many grams of O2?
a)
256 g of O2
b)
576 g of O2
c)
288 g O2
7.
B2H6 + 3O2 -->2 HBO2 + 2 H2O
 What mass of O2 will be needed to burn 36.1 g of B2H6?
a)
13.8 g O2
b)
3.86 mol of O2
c)
124 g O2
8.
4 Al + 3 O2 –> 2 Al2O3  How much aluminum would be needed to completely react with 45 grams of O2?
a)
1.05 moles
b)
3.75 moles
c)
1.875 grams
d)
1.875 moles
9.
2Al + 3H2SO4 -> Al2(SO4)3 + 3H2
How many grams of aluminum sulfate would be formed if 250g H2SO4 completely reacted with aluminum?
a)
0.85 g
b)
290 g
c)
450 g
d)
870 g
10.
Mg(s) + 2 HCl(aq)  -->  MgCl₂(aq)   + H₂(g)
How many moles of HCl are consumed in the production of 7.5 moles of MgCl₂?
a)
3.8 moles
b)
15 moles
c)
7.5 moles
d)
23 moles
11.
Balance the following reaction :
 
CaC₂(s)   +   H₂O(l)   -->   C₂H₂(g)   +   Ca(OH)₂(aq)
a)
1,2,2,2
b)
1,2,1,1
c)
2,1,1,1
d)
2,1,2,1
12.
 CaC₂(s) + 2H₂O(l)   -->   C₂H₂(g)   + Ca(OH)₂(aq)
how many grams of Ca(OH)₂ would be formed with 3.20 moles of CaC₂?
a)
119 g
b)
21.2 g
c)
114 g
d)
237 g
13.
Use the following equation:
NaIO3(aq) + 6HI(aq) --> 3I2(s) + NaI(aq) + 3H2O(l)
How many moles of iodine can be made from 6.55 moles of NaIO3?
a)
4.55 moles I2
b)
23.18 moles I2
c)
19.65 moles I2
d)
34.99 moles I2
14.
Using the following equation:
4NH3(g) + 5O2(g) --> 4NO(g) + 6H2O(l)
How many grams of oxygen gas are needed to react with 56.8 grams of ammonia?
a)
45.08 g O2
b)
133.33 g O2
c)
260.77 g O2
d)
75.92 g O2
15.
N2 +  3H2 → 2NH3 
How many moles of hydrogen are needed to react with 2 moles of nitrogen?
a)
6
b)
2
c)
3
d)
1
16.
2H2   +   O2  →  2H2O
How many moles of water can be produced if 8 moles H2 are used?
a)
4 moles
b)
8 moles
c)
16 moles
d)
2 moles
17.
For the Balanced Reaction: 3 Mg + 1 Fe2O3 → 3 MgO + 2 Fe; What is the Ratio of moles of MgO to moles Fe?
a)
3mol Mg / 2 mol Fe
b)
2 mol Mg/ 3 mol Fe
c)
1 mol Fe/ 2 mol Fe
d)
3 mol MgO / 2 mol Fe
18.
Cl2 + 2KBr → Br2 + 2KCl
How many grams of potassium chloride (KCl) can be produced from 356 g of potassium bromide (KBr)?
a)
749 g
b)
223 g
c)
479 g
d)
814 g
19.
CH4 + 2 O2 → CO2 + 2 H2O
How many moles of carbon dioxide are produced from the combustion of 110 g of CH4?
a)
13.7 mol
b)
2.75 mol
c)
6.11 mol
d)
6.85 mol
20.
B2H6 + 3O2 -->2 HBO2 + 2 H2O
 What mass of O2 will be needed to burn 36.1 g of B2H6?
a)
13.8 g O2
b)
3.86 mol of O2
c)
125.2 g O2
21.
Balance the following reaction :
 
CaC₂(s)   +   H₂O(l)   -->   C₂H₂(g)   +   Ca(OH)₂(aq)
a)
1,2,2,2
b)
1,2,1,1
c)
2,1,1,1
d)
2,1,2,1
22.
Using the following equation:
Fe2O3(s) + 3H2(g) → 2Fe(s) + 3H2O(l)
How many moles of iron can be made from 3 moles of Fe2O3?
a)
6 moles Fe
b)
4 moles Fe
c)
2 moles Fe
d)
1 moles Fe
23.
2Al + 3H2SO4 -> Al2(SO4)3 + 3H2
How many grams of aluminum sulfate would be formed if 250g H2SO4 completely reacted with aluminum?
a)
0.85 g
b)
290 g
c)
450 g
d)
870 g
24.
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
25.
2 KClO3 → 2 KCl + 3 O2
How many moles of oxygen are produced when 6.7 moles of KClO3 decompose completely?
a)
6.7 mol
b)
1.0 mol
c)
10.1 mol
d)
4.5 mol
26.
2Na + 2H2O → 2NaOH+ H2
How many grams of hydrogen are produced if 120 g of Na are available?
a)
5.2 g
b)
2.6 g
c)
690 g
d)
45 g
27.
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
28.
2 CO (g) + O2(g) → 2 CO2 (g)
In the formation of CO2 from CO and oxygen, how many Liters of CO2 are produced by the reaction of 8 mols of O2 with an excess of carbon monoxide?
a)
0.178 L
b)
358.4 Liters
c)
704 grams
d)
0.36 grams
29.
 SiO2 + 3C → SiC + 2CO
I need to add 8 moles of Carbon to the reaction. How many grams of Carbon should I weigh?
a)
96 g
b)
0.67 g
c)
2.67 g
d)
48 g
30.
Cl2 + 2 KBr → Br2 + 2 KCl
How many grams of potassium chloride can be produced from 356 g of chlorine and 356 g of potassium bromide?
a)
749 g
b)
223 g
c)
479 g
d)
814 g
31.
A chemist interested in the efficiency of a chemical reaction would calculate the
a)
mole ratio
b)
rate of reaction
c)
percent yield
d)
energy released
32.
What is a Excess Reagent?
a)
amount you end with
b)
what you run out of first
c)
what you have left over
d)
what you start with
33.
CH4 + 2 O2 → CO2 + 2 H2O
How many moles of carbon dioxide are produced from the combustion of 110 g of CH4?
a)
13.7 mol
b)
2.75 mol
c)
6.11 mol
d)
6.85 mol
34.
Fe (s) + S (l) --> FeS (s)  

In the experiment above, 7.62 g of Fe are allowed to react with 8.67 g of S.
How much FeS is formed?
a)
14.8 g
b)
12.2 g
c)
13.7 g
d)
19.9 g
35.
Identify the limiting reagent when 6.00 g HCl combines with 5.00 g Mg to form MgCl2.
 
Mg +  2HCl --> MgCl2  +  H2   
 
a)
Mg
b)
H2
c)
MgCl2
d)
HCl
36.
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
37.
1. What is a limiting reagent?
a)
any reactant used up first in a reaction.
b)
any reactant left over at the end of a reaction.
c)
the maximum amount of product formed from a given amount of reactant.
d)
the purity of the reactant.
38.
1 Cheese + 2 Bread --> 1 Grilled cheese
How many grilled cheeses can you make with 26 slices of bread and 14 pieces of cheese?
a)
14
b)
13
c)
26
d)
7
39.

The reactant that is not completely used up in a chemical reaction is called the __________ .

a)

spectator reagent

b)

limiting reagent

c)

excess reagent

d)

catalyst

40.
When 12 moles of O2 reacts with 6 moles of C10H8, what is the limiting reactant?  
1 C10H8 + 12 O2 --> 10 CO2 + 4 H2O
a)
Oxygen
b)
C10H8
c)
Water
d)
Carbon Dioxide
41.
Use the equation 2 Al + 3 Cl2 ---> 2 AlCl3.  If 2 moles of aluminum and 2 moles of chlorine are reacted, identify the limiting reactant.
a)
AlCl3
b)
Cl2
c)
Al
d)
None
42.
Identify the limiting reagent when 6.00 moles HCl combines with 5.00 moles Mg to form MgCl2.
 
1 Mg +  2 HCl --> 1 MgCl2  +  1 H2   
 
a)
Mg
b)
H2
c)
MgCl2
d)
HCl
43.

Which reactant is the limiting reagent and why?

2H2(g) + O2(g) → 2H2O(l)

a)

Hydrogen is the limiting reagent because two moles of hydrogen is required for every one mole of oxygen to produce two water.

b)

Oxygen is the limiting reagent because two moles of hydrogen is required for every one mole of oxygen to produce two water.

44.

4NH3 + 5O2 --> 4NO + 6H2O


How many Liters of NO are formed if 6.30g of ammonia react with 1.80g of oxygen?

a)

1.5 L

b)

2.02 L

c)

1.01 L

d)

8.30 L

45.

6Na + Fe2O3 --> 3Na2O + 2Fe


If you are provided 200g of sodium and 250 grams of iron(III) oxide, how much of excess reagent is left?

a)

232 g

b)

18 g

c)

250 g

46.
2Na + 2H2O → 2NaOH+ H2
How many grams of hydrogen are produced if 120 g of Na are available?
a)
5.2 g
b)
2.6 g
c)
690 g
d)
45 g
47.

Determine the number of oxygen atoms in Al(OH)3

a)

1

b)

2

c)

3

d)

4

48.

C3H5(NO3)3 Identify the correct number of atoms

a)

C = 3, H = 5, N = 3, O = 9

b)

C = 3, H = 5, N = 1, O = 9

c)

C = 9, H = 15, N = 3, O = 9

d)

C = 9, H = 15, N = 1, O = 3

49.

Calculate the molar mass of CuBr2

a)

143.45 g/mol

b)

223.35 g/mol

c)

287.30 g/mol

d)

307.90 g/mol

50.

What is the percent by mass of Cu in CuBr2?

a)

50%

b)

71.6%

c)

28.4%

d)

44.3%

51.

What is the percent by mass of Br in CuBr2?

a)

50%

b)

71.6%

c)

28.4%

d)

44.3%

52.

What is the percent by mass of Na in NaOH?

a)

40%

b)

2.5%

c)

22.9%

d)

57.5%

53.

What is the percent by mass of H in NaOH?

a)

40%

b)

2.5%

c)

22.9%

d)

57.5%

54.

What is the percent by mass of O in NaOH?

a)

40%

b)

2.5%

c)

22.9%

d)

57.5%

55.

How many H atoms are in (NH4)3PO4?

a)

4

b)

7

c)

12

d)

15

56.

How many N atoms are in (NH4)3PO4?

a)

4

b)

3

c)

1

d)

7

57.

How many P atoms are in (NH4)3PO4?

a)

4

b)

3

c)

1

d)

7

58.

What is the percent by mass of H in (NH4)3PO4?

a)

1%

b)

8%

c)

12%

d)

21%

59.

What is the percent by mass of N in (NH4)3PO4?

a)

28%

b)

8%

c)

12%

d)

21%

60.

What is the percent by mass of O in (NH4)3PO4?

a)

8%

b)

43%

c)

12%

d)

21%

61.
How many liters would you need to make a 1 M solution if you have 6 mol of Sodium Hydroxide? 
a)
2
b)
3
c)
4
d)
6 
62.
What is the molarity of 4 g of NaCl (MM=58.45) in 3,800 mL of solution?
a)
0.018 M
b)
0.0011 M
c)
1.052 M
d)
0.062 M
63.
How many grams of solute are dissolved in 125.0 mL of 5.00 M NaCl (MM = 58.45)?
a)
0.625 g NaCl
b)
625 g NaCl
c)
36.5 g NaCl
d)
0.04 mol NaCl
64.
Find the molarity of 186.55 g of sucrose, C12H22O11 (MM = 342) in 250 mL of water.
a)
2.18 M
b)
0.746 M
c)
1.18 M
d)
0.545 M
65.
How many moles of NaCl are present in a solution with a molarity of 8.59 M and a volume of 125 mL?
a)
1074 mol
b)
0.069 mol
c)
1.07 mol
d)
62.7 mol
66.
Which sweet tea would you expect to taste the sweetest?
a)
1M
b)
3M
c)
3.1M
d)
2.5M
67.
True or False? The higher the concentration of a solution the less solutes it has in it.
a)
True
b)
False
68.
How many grams of AgNO3 (MM = 169.87) are needed to prepare 0.125M solution in 250 mL of water? 
a)
.03g
b)
0.5g
c)
5.3g
d)
84.9g
69.
Which of the following has the most NaCl (MM = 58.44)?
a)
100 mL of a 1.8 M solution
b)
50 mL of a 4.1 M solution
c)
9.35 grams
d)
1 mole
70.
What is the molarity of a solution made by diluting 26.5 mL of 6.00M HNO3 to a volume of 250 mL?
a)
15.9 M
b)
0.636 M
c)
0.642 M
d)
1.59 M
71.
How many mL of 10.8M HCl are required to make 100.0 mL of 3.00M acid?
a)
27.8 mL
b)
27.78 mL
c)
2.8 mL
d)
278 mL
72.
Calculate the molarity of the following solution:  1.0 mole of KCl in 750.0 mL of solution.
a)
0.750 M
b)
99 M
c)
1.3 M
d)
2.0 M
73.
What volume of 1.50 M KBr can be made from 15.6 mL of concentrated KBr with a molarity of 9.65 M?
a)
150. mL
b)
151 mL
c)
1.00 L
d)
100. mL
74.
What is the molarity of a solution made by adding 1.565 moles of PbNO3 to 500 mL?
a)
300. M
b)
31.3 M
c)
3.13 M
d)
1.56 M
75.
How many moles are needed to make 2.5 L of a 3.8 M solution? 
a)
9.5 mol
b)
0.66 mol
c)
1.5 mol
d)
15 mol
76.
A compound consists of 72.2% magnesium(Mg) and 27.8% nitrogen(N) by mass. What is the empirical formula?
a)
Mg4N3
b)
MgN2
c)
Mg3N2 
d)
MgN
77.
Which of the following is considered an empirical formula?
a)
CH3COOH
b)
C6H12O6
c)
H2O
78.
You are given the following percentages: 40.05% S and 59.95% O. Find the empirical formula for these elements.
a)
SO
b)
SO2
c)
SO3
d)
SO4
79.

How many molecules are in 2.5 mol of NaCl?

a)

1.5 x 1024 molecules

b)

1.5 molecules

c)

4.15 molecules

d)

1.5 x 1023 molecules

80.
Which pair has the same empirical formula?
a)
NaCrO4 and Na2Cr2O7
b)
C2H4O2 and C6H12O6
c)
C3H6O3 and C2H6O2
d)
CH4 and C2H6
81.
A compound consists of 72.2% magnesium(Mg) and 27.8% nitrogen(N) by mass. What is the empirical formula?
a)
Mg4N3
b)
MgN2
c)
Mg3N2 
d)
MgN
82.
A formula with the lowest whole # ratio of elements in a compound is called
a)
Molecular Formula
b)
Chemical Formula
c)
Empirical Formula 
d)
Distance Formula
83.
Glycerol has a molar mass of 92.09g/mol. Its percent composition is: 39.12% C, 8.75% H, and 51.12% O. What is the molecular formula for glycerol?
a)
C2H3O2
b)
CH2O
c)
C2H4O2
d)
C3H8O3
84.

2.40 g of an explosive, J, contains 0.473 g of nitrogen. J also contains 33.8% carbon and 1.41% hydrogen by mass. The remainder of J is oxygen.


What is the empirical formula of J?

a)

C4HNO2

b)

CH2N2O

c)

C2HNO2

d)

CHNO

85.

2.40 g of an explosive, J, contains 0.473 g of nitrogen. J also contains 33.8% carbon and 1.41% hydrogen by mass. The remainder of J is oxygen.


What is the empirical formula of J?

a)

C4HNO2

b)

CH2N2O

c)

C2HNO2

d)

CHNO

86.
What is the percent by mass of magnesium in MgO?
a)
20%
b)
40%
c)
50%
d)
60%
87.
What is the percent composition by mass of sulfur in the compound MgSO4 (gram formula mass = 120 g/mol)?
a)
20%
b)
27%
c)
46%
d)
53%
88.
What is the empirical formula if you have 88.80% copper and 11.20% oxygen?
a)
Cu3O8
b)
CuO4
c)
Cu2O
d)
Cu4O10
89.
What is the empirical formula if you have 36.84% nitrogen and 63.16% oxygen?
a)
NO
b)
N2O3
c)
N2O4
d)
N2O5
90.
What is the molecular formula if the empirical formula is CH2O and the molecular molar mass is 180.18?
a)
CH2O
b)
C2H4O2
c)
C4H8O4
d)
C6H12O6
91.
What is the molecular formula for a compound with the empirical formula: K2SO4 and a molecular mass of 696g.
a)
K2SO4 
b)
K8SO16
c)
K8S4O8 
d)
K8S4O16 
92.
EF = CF2 
Molecular formula mass = 192
MF =
a)
C4F8
b)
C4F
c)
CF8
d)
C2F4
93.
?
a)
CH4N20
b)
CH4N0
c)
CHN20
d)
C2H4N208
94.
When calculating the EF the mole ratio is given as follows:
H1O3.5
What will the EF be?
a)
H1O3.5
b)
HO3.5
c)
HO4
d)
H2O7
95.
20% Ca, 80 Br. EF=
a)
CaBr
b)
CaBr2
c)
Ca2Br
d)
Ca2Br2
96.
a)

C4H6O1

b)

C2H3O5

c)

C10H15O1

d)

C20H30O5

97.
a)
25.6 %
b)
43.6 %
c)
56. 8 %
d)
71.3 %
98.
Which of the following represents an empirical formula?
a)
H2O2
b)
HC2O4
c)
H2O6
d)
H12O48
99.
In the equation 2 Al2O3 --> 4 Al + 3 O2, what is the mole ratio of aluminum to oxygen?
a)
10:6 
b)
3:4
c)
4:3
d)
2:3
100.
What can be determined from a balanced chemical equation?
a)
Mole ratio of any two substances in the reaction
b)
Energy released in the reaction.
c)
Electron configuration of all elements in the reaction. 
d)
Mechanism involved in the reaction. 
101.
Given the reaction: 4Al + 3O2 --> 2Al2O3
How many moles of Aluminum oxide do you have if you have 2 moles of Al?
a)
3 mole
b)
2 mole
c)
1 mole
d)
0.5 mole
102.
N2 +  3H2 → 2NH3 
What is the mole ratio between Nitrogen and Ammonium in the above reaction?
a)
1 moles NH3 / 2 moles N2 
b)
2 moles NH3 / 1 moles N2 
c)
2 moles N2 / 3 moles NH3 
d)
1 moles N2 / 3 moles NH3 
103.
2Na + S -->Na2S
What is the total number of moles of S that reacts when 4.0 moles of Na were completely consumed?
a)
1
b)
2
c)
0.5
d)
4
104.
4NH3 + 5O2-->4NO + 6H2O
What is the total number of moles of H2O produced when 12 mole of NH3 is completely consumed?
a)
15
b)
18
c)
20
d)
24
105.
6CO2 + 6H2O --> C6H12O6 + 6O2 
What is the total number of moles of water needed to make 2.5 moles of C6H12O6?
a)
2.5
b)
6
c)
12
d)
15
106.
6CO2 + 6H2O --> C6H12O6 + 6O2 
What is the total number of moles of CO2 needed to make 2 moles of C6H12O6?
a)
2.5
b)
6
c)
12
d)
15
107.
6CO2 + 6H2O --> C6H12O6 + 6O2 
What is the total number of moles of water needed to make 2.5 moles of C6H12O6?
a)
2.5
b)
6
c)
12
d)
15
108.
What number should be in front of N2 in this chemical equation?
___N2+___F2 --> ___ NF3
a)
1
b)
2
c)
3
d)
4
109.
3 Mg + 1 Fe2O3 → 3 MgO + 2 Fe
What is the Ratio of moles of Mg to moles Fe?
a)
3mol Mg / 2 mol Fe
b)
2 mol Mg/ 3 mol Fe
c)
1 mol Fe/ 2 mol Fe
d)
3 mol MgO / 2 mol Fe
110.
H2+Cl2-->2HCl
How many moles of Cl2 are needed to react with 3 moles of H2?
a)
5
b)
2
c)
3
d)
6
111.
6CO2 + 6H2O --> C6H12O6 + 6O2 
What is the total number of moles of CO2 needed to make 2 moles of C6H12O6?
a)
2.5
b)
6
c)
12
d)
15
112.
H2+Cl2-->2HCl
What is the total number of moles of HCl produced when 3 moles of H2 is completely consumed?
a)
5
b)
2
c)
3
d)
6
113.
2Na + S -->Na2S
What is the total number of moles of Na2S produced when 8.0 moles of Na were completely consumed?
a)
1
b)
2
c)
0.5
d)
4
114.

100 cm = 1 m.

What conversion factor would be used to convert 120 centimeters into meters?

a)

120 cm1 m\frac{120\ cm}{1\ m}  

b)

1 m120 cm\frac{1\ m}{120\ cm}  

c)

 100 cm1 m\ \frac{100\ cm}{1\ m}  

d)

100 m1 cm\frac{100\ m}{1\ cm}  

e)

1 m100 cm\frac{1\ m}{100\ cm}  

115.

1 kg = (a)   g

116.

1 hL = (a)   L

117.

1 dam = (a)   m

118.

1 dg = (a)   g

119.

1 cm = (a)   m

120.

1 mm = (a)   m

121.

The prefix "kilo" means...

a)

Thousand times bigger than the base

b)

Thousand times smaller than the base

122.

The prefix "milli" means...

a)

Thousand times bigger than the base

b)

Thousand times smaller than the base

123.

The prefix "centi" means...

a)

Hundred times bigger than the base

b)

Hundred times smaller than the base

124.

The prefix "hecta" means...

a)

Hundred times bigger than the base

b)

Hundred times smaller than the base

125.

The prefix "deca" means...

a)

Ten times bigger than the base

b)

Ten times smaller than the base

126.

The prefix "deci" means...

a)

Ten times bigger than the base

b)

Ten times smaller than the base

127.

Check all of the following that are base units:

a)

g

b)

L

c)

km

d)

s

e)

mg

128.
Blue Color: Chemical or Physical Property
a)
Chemical Property
b)
Physical Property
129.
Density: Chemical or Physical Property
a)
Chemical Property
b)
Physical Property
130.
Flammability (burns): Chemical or Physical Property
a)
Chemical Property
b)
Physical Property
131.
Solubility (dissolves): Chemical or Physical Property
a)
Chemical Property
b)
Physical Property
132.
Reacts with Acid: Chemical or Physical Property
a)
Chemical Property
b)
Physical Property
133.
Brittleness: Chemical or Physical Property
a)
Chemical Property
b)
Physical Property
134.
Sour Taste: Chemical or Physical Property
a)
Chemical Property
b)
Physical Property
135.
Melting Point: Chemical or Physical Property
a)
Chemical Property
b)
Physical Property
136.
Reacts with Water: Chemical or Physical Property
a)
Chemical Property
b)
Physical Property
137.
Hardness: Chemical or Physical Property
a)
Chemical Property
b)
Physical Property
138.
Boiling Point: Chemical or Physical Property
a)
Chemical Property
b)
Physical Property
139.
Luster: Chemical or Physical Property
a)
Chemical Property
b)
Physical Property
140.
Odor: Chemical or Physical Property
a)
Chemical Property
b)
Physical Property
141.
Reacts with Air: Chemical or Physical Property
a)
Chemical Property
b)
Physical Property
142.
What is the correct formula for the compound, lithium oxide?
a)
LiO
b)
Li2O
c)
LiO2
d)
Li2O2
143.
What is the formula for manganese(III) oxide?
a)
MgO
b)
Mg2O3
c)
MnO
d)
Mn2O3
144.
From the following ionic compounds, choose the name-formula pair that is not correctly matched.
a)
sodium sulfide  Na2S
b)
ammonium nitrate 
NH4NO3
c)
sodium sulfate 
Na2SO3
d)
calcium oxide  CaO
145.

Name the following ionic compound: MgSO4

a)

magnesium sulfoxide

b)

magnesium sulfide

c)

magnesium sulfate

d)

magnesium oxide

146.
Name the following ionic compound: Cr(NO2)3
a)
chromium nitrite
b)
chromium nitride
c)
chromium III nitride
d)
chromium III nitrite
147.
The chemical formula of Iron (III)bromide is
a)
FeBr
b)
Fe(III)Br
c)
FeBr₃
d)
Fe₂Br₃
148.
How do the following two elements bond together?
Na1+  F1-         
a)
NaF
b)
NaF3
c)
Na3F
d)
Na1F2
149.
How do the following two elements bond together?
Cr3+  O2-         
a)
CrO
b)
Cr3O2
c)
Cr2O3
d)
CrO3
150.
How do the following two elements bond together?
K1+  S2- 
a)
KS
b)
K8S
c)
K6S3
d)
K2S
151.
How do the following two elements bond together?
Al3+  O2-         
a)
AlO
b)
Al2O3
c)
Al3O6
d)
Al3O2
152.
Cu +2  and  OH -
a)
CuOH2
b)
Cu2OH
c)
Cu(OH)2
d)
correct answer is not given
153.
When adding a subscript to a polyatomic ion, you should...
a)
multiply any subscripts on the polyatomic ion by the subscript you are adding
b)

put parentheses (brackets) around the polyatomic ion before adding a subscript

c)
write the new subscript next to any subscripts on the polyatomic ion
d)
put the polyatomic ion in square brackets before adding the subscript
154.

Which elements usually form cations?

a)

non-metals

b)

metals

c)

any elements

d)

noble gases

155.
Anions are _______ that form ____________ ions and __________ electrons.
a)
nonmetals, positive, lose
b)
nonmetals, negative, gain
c)
metals, positive, gain
d)
metals, positive, lose
156.
Anions are _______ that form ____________ ions and __________ electrons.
a)
nonmetals, positive, lose
b)
nonmetals, negative, gain
c)
metals, positive, gain
d)
metals, positive, lose
157.
What is the charge of an atom that has gained one electron?
a)
-1
b)
-2
c)
+1
d)
+2
158.

The element Ca will form a cation. What would be the noble gas that this cation would have the same electron configuration as ?

a)

Ne

b)

Ar

c)

He

d)

Xe

159.

When iodine forms an iodide ion, into which orbital would the electron be going?

a)

5s

b)

4s

c)

5p

d)

3d

e)

It wont gain an electron, it would lose one.

160.

Which electron configuration belongs to a Chloride (Cl-) ion?

a)

1s2 2s2 2p6 3s2 3p5

b)

1s2 2s2 2p6 3s2 3p6

c)

1s2 2s2 2p6 3s2 3p7

d)

1s2 2s2 2p6 3p7

161.
What electron configuration matches an oxygen ion?
a)
1s22s22p63s2, 3p64s23d104p5
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p64s23d1
162.

An aluminium ion would have which electron configuration?

a)

1s2 2s2 2p6 3s2

b)

1s2 2s2 2p6 3s2 3p1

c)

1s2 2s2 2p6 3s2 3p6

d)

1s2 2s2 2p6

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