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quizizz FINAL EXAM REVIEW

Total questions: 179

Worksheet time: 10hrs 36mins

Name
Class
Date
1.

How many significant figures are in the number 17.837

a)

2

b)

3

c)

4

d)

5

2.

How many significant figures are in the number 6004

a)

1

b)

2

c)

3

d)

4

3.

How many significant figures are in the number 2020

a)

1

b)

2

c)

3

d)

4

4.

How many significant figures are in the number 548.0

a)

1

b)

2

c)

3

d)

4

5.

How many significant figures are in the number 70.0

a)

1

b)

2

c)

3

d)

4

6.

How many significant figures are in the number 0.040

a)

1

b)

2

c)

3

d)

4

7.

How many significant figures are in the number 1000

a)

1

b)

2

c)

3

d)

4

8.

How would you write 4.3756 x 104 in standard form?

(a)  

9.

How would you write 0.0005 in scientific notation?

a)

50 x 10-5

b)

5 x 10-4

c)

5 x 103

d)

.5 x 103

10.

How would you write -5.6 x 10-3 in standard form?

(a)  

11.

How do you write 8.317 x 106 in standard form?

(a)  

12.

Which of the following numbers is written in scientific notation?

a)

20.35 x 104

b)

.2035 x 104

c)

2035 4

d)

2.035 x104

13.

Express the following in scientific notation:


.000457

a)

457 x 106

b)

457 x 10-6

c)

4.57 x104

d)

4.57 x 10-4

14.

Convert to scientific notation:


520,000,000

a)

52 x 107

b)

5.2 x 10-7

c)

5.2 x 108

d)

0.52 x 109

15.
This bullseye demonstrates...
a)
High Accuracy & High Precision
b)
High Accuracy & Low Precision
c)
Low Accuracy & High Precision
d)
Low Accuracy & Low Precision
16.
?
a)
High Accuracy & High Precision
b)
High Accuracy & Low Precision
c)
Low Accuracy & High Precision
d)
Low Accuracy & Low Precision
17.
Describe the accuracy and precision of the image
a)

Both accurate and precise

b)

Accurate but not precise

c)
not accurate and not precise
18.

Which student's data is the MOST PRECISE?

a)

Student A

b)

Student B

c)

Student C

19.

Which student's data is the MOST ACCURATE?

a)
Student A
b)
Student B
c)
Student C
20.

Does this image show results that are accurate and/or precise?

a)

Accurate, but not precise

b)

Precise, but not accurate

c)

Both precise and accurate

d)

Neither precise nor accurate

21.

Does this image show results that are accurate and/or precise?

a)

Accurate, but not precise

b)

Precise, but not accurate

c)

Both precise and accurate

d)

Neither precise nor accurate

22.
Zed went to the store and bought a bag of chips.  He estimated there would be 350 chips in the package, but realized there were only 210 chips in that package.  What was his percent error?
a)
35%
b)
67%
c)
85%
d)
92%
23.
Jessie estimates the weight of her cat to be 8 pounds.  The actual weight of the cat was 10 pounds.  Find the percent error.  
a)
15%
b)
20%
c)
25%
d)
30%
24.
Bob estimates that there will be 230 people who attend the concert.  There was an actual total of 300 people who attended.  Find the percent error.  
a)
23%
b)
33%
c)
27%
d)
37%
25.
An archaeologist estimated that a fossil was 520 years old. It was actually 500 years old. What was the percent error?
a)
4%
b)
20%
c)
3.8%
d)
none of these
26.
Griffin was buying a birthday card, he thinks the price is $4.50, but the actual price is $4. What is his percent of error?
a)
50%
b)
0.5%
c)
12.5%
d)
0.125%
27.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
28.
The electron configuration of an atom is 1s22s22p6.  The number of electrons in the atom is 
a)
3
b)
6
c)
8
d)
10
29.
This orbital diagram represents:  
a)
C
b)
B
c)
N
d)
O
30.
Which element is pictured?
a)
neon
b)
fluorine
c)
magnesium
d)
argon
31.
Which element is pictured?
a)
neon
b)
fluorine
c)
magnesium
d)
argon
32.
 The diagram above represents two electrons with 
a)
a. opposite spins.
b)
 b. the same spin.
c)
c. different energies.
d)
d. different energy levels.
33.
What is the correct noble-gas notation for the electron configuration of an atom of chlorine? 
a)
a. [Ar]3s2 3p5
b)
 b. [Ne]3s2 3p4
c)
 c. [Ar]3s2 3p4
d)
 d. [Ne]3s2 3p5
34.

Using noble-gas notation, calcium is represented by [Ar]4s2. How many electrons does calcium have?

a)

18

b)

20

c)

22

d)

24

35.

Which rule is being broken this orbital diagram?

a)

Aufbau Principle

b)

Pauli Exclusion Principle

c)

Hund's Rule

d)

The diagram is correct.

36.

This orbital diagram represents:

(a)  

37.
Which orbital shows a violation of the Pauli Exclusion Principle?
a)
A
b)
B
c)
C
d)
D
38.
Which orbital shows a violation of the Aufbau Principle?
a)
A
b)
B
c)
C
d)
D
39.
Electrons occupy orbitals of lowest energy first is part of what electron configuration rule?
a)
Hund’s Rule
b)
Aufbau Principle
c)
Pauli Exclusion Principle
40.
Each orbital will hold ____ electrons
a)
5
b)
4
c)
8
d)
2
41.
What electron configuration matches an oxygen atom?
a)
1s22s22p63s2, 3p64s23d104p5
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p64s23d1
42.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
43.
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
44.

What is the wavelength of a wave having a frequency of 3.76 x 10^14 s^-1?

a)

0.7978 x 10^-6

b)

7.98 x 10^-7 m

c)

1.25 x 10^6 m

d)

0.13 x 10^7

45.

What is the frequency of a 6.9 x 10^-13 m wave?

a)

2.07 x 10^19 Hz

b)

0.434 x 10^-5 Hz

c)

2.30 x 10^-21 Hz

d)

4.35 x 10^20 Hz

46.

What is the wavelength of a 2.99 Hz wave?

a)

1.00 x 10^8 m

b)

5.99 x 10^9 m

c)

9.97 x 10^8 m

d)

1.00 m

47.

What is the wavelength of a 1.28 x 10^17 Hz wave?

a)

4.27 x 10^8 m

b)

2.34 x 10^-9 m

c)

1.72 x 10^25 m

d)

0.47 x 10^9 m

48.

What is the frequency of a 7.43 x 10^-5 m wave?

a)

0.404 x 10^3 s^-1

b)

4.04 x 10^12 s^-1

c)

2.47 x 10^-13 s^-1

d)

4.43 x 10^3 s^-1

49.

What is the frequency of a 2.60 m wave?

a)

1.15 Hz

b)

4.00 x 10^-8 Hz

c)

8.67 x 10^-8 Hz

d)

1.15 x 10^8 Hz

50.

What is the wavelength of a wave having a frequency of 4.34 x 10^15 s^-1?

a)

6.91 x 10^-8

b)

1.45 x 10^23

c)

0.691 x 10^7

d)

1.34 x 10^-8

51.
What would be the proper chemical formula for combining Al3+ and Cl- :
a)
AlCl3
b)
Al3Cl
c)
AlCl
d)
Al3Cl3
52.
Name the following ionic compound: BeCl2
a)
beryllium chlorine
b)
beryllium II chloride
c)
beryllium chloride
d)
beryllium dichloride
53.
Name the following ionic compound: MgSO4
a)
magnesium sulfoxide
b)
magnesium sulfide
c)
magnesium sulfate
d)
magnesium oxide
54.
Name the following ionic compound: LiNO3
a)
lithium nitrate
b)
lithium III nitrate
c)
lithium nitride
d)
lithium oxide
55.
Name the following ionic compound: Cr(NO2)3
a)
chromium nitrite
b)
chromium nitride
c)
chromium III nitride
d)
chromium III nitrite
56.
Name the following compound: FeCl3
a)
iron chloride
b)
iron III chloride
c)
iron chlorate
d)
iron III chlorate
57.
What is the charge on the hydroxide ion?
a)
0
b)
-1
c)
-2
d)
-3
58.
copper(II) chloride
a)
CuCl2
b)
CuCl
c)
Cu2Cl
d)
Cu2Cl2
59.
Name the ionic compound SnSe2
a)
Tin diselenide
b)
Tin (IV) Selenide
c)
Tin selenide
d)
Tin (II) triselenide
60.
Cu2CO3
a)
copper carbonate
b)
copper II carbonate
c)
copper I carbonate
d)
copper carbon oxide
61.
NH4Cl
a)
ammonium chloride
b)
ammonium chlorine
c)
nitrogen hydrogen chloride
d)
nitrogen chloride
62.
An atom that gains or loses electrons is called a _______.
a)
atom
b)
ion
c)
oxidation
d)
metal
63.
magnesium carbonate
a)
Mg2C
b)
Mg2CO4
c)
Mg2(CO3)2
d)
MgCO3
64.
When naming an ion containing a transition metal what would be included in the name?
a)
roman numeral
b)
prefix
c)
suffix
d)
superscript
65.
MgF2
a)
magnesium fluoride
b)
manganese Phosphide
c)
magnesium(III) fluoride
d)
magnesium fluoride(II)
66.
Covalent compounds
a)
Share electrons
b)
transfer electrons
c)
contain a sea of electrons
d)
conduct electricity
67.
Phosphorous trichloride
a)
PCl3
b)
P3Cl
c)
P3Cl3
d)
PCL
68.
Bromine monoflouride
a)
Br1F1
b)
BrF
c)
Br2F
d)
BrF2
69.
Disulfur trioxide
a)
S3O2
b)
SO
c)
S2O3
d)
S2O
70.
P2O5
a)
Phosphorus Oxide
b)
Pentaphosphorus Dioxide
c)
Diphosphorous pentoxide
d)
Phosphoric Oxygen
71.
SeF4
a)
Tetraselenium fluoride
b)
Selenium Fluoride
c)
Selenium tetraflouride
d)
Selenium (IV) Fluoride
72.

Octanitrogen tetroxide

a)
N8O3
b)
N7O3
c)

N2O

d)
N8O4
73.

CS2

a)

monocarbon disulfide

b)

carbon bisulfide

c)

carbon disulfide

d)

carbon disulfer

e)

monocarbon sulfide

74.

SCl6

a)

sulfur hexachloride

b)

monosulfur hexachloride

c)

sulfide hexachloride

d)

sulfur heptachloride

e)

sulfur chloride

75.

P4H7

a)

tetraphosphorus heptahydrogide

b)

phosphorus heptahydride

c)

tetraphosphorus heptahydride

d)

tetraphosphorus hexahydride

e)

tetraphosphorus heptahydrogen

76.

P3N5

a)

phosphorus pentanitride

b)

triphosphorus pentanitrogen

c)

triphosphide pentanitrogen

d)

triphosphorus pentanitride

e)

phosphorus nitride

77.
The desire for an element to have 8 atoms around it is called 
a)
Octet Rule
b)
Resonance
c)
Ionization energy
d)
Electronegativity
78.
Which has the greater EN: 
N or C?
a)
C
b)
N
79.
Which has the greater EN: 
H or F?
a)
H
b)
F
80.
Put these in increasing order:
C, H, and O
a)
H < C < O
b)
H < O < C
c)
O < C < H
d)
C < H < O
81.
 Which of the following generally applies to the noble gases? 
a)
high ionization energy, low electronegativity, high reactivity
b)
high ionization energy, high electronegativity, high reactivity
c)
low ionization energy, low electronegativity, low reactivity
d)
high ionization energy, low electronegativity, low reactivity 
82.
Which of the following is the least electronegative element?
a)
oxygen
b)
potassium
c)
fluorine
d)
nitrogen
83.

Chemical bond formed from the electrostatic attraction between positive and negative ions

a)

covalent bond

b)

ionic bond

c)

metallic bond

84.

When 2 atoms share electrons

a)

Ionic bond

b)

covalent bond

c)

metallic bond

85.

Use VSEPR theory to predict the shape of the hydrogen chloride molecule, HCl.

a)

tetrahedral

b)

linear

c)

bent

d)

trigonal planar

86.

Use VSEPR theory to predict the shape of the chlorate ion, ClO3–.

a)

trigonal planar

b)

octahedral

c)

trigonal pyramidal

d)

bent

87.
Which of the following shapes has an unshared pairs of electrons on the central atom? 
a)
Bipyramidal
b)
Bent
c)
Trigonal Planar
d)
Tetrahedral
88.
What molecule could this be? 
a)
BF3
b)
CH4
c)
H2O
d)
CO2
89.
Who could this molecule be?
a)
CH4
b)
CO2
c)
PCl5
d)
BF3
90.
Who could this be? 
a)
CO2
b)
NH3
c)
H2S
d)
CH4
91.
Who could this be?
a)
H2O
b)
NH3
c)
CO2
d)
CH4
92.

What molecular geometry would PH3 have?

a)

Trigonal Pyramidal

b)

Trigonal Bipyramidal

c)

Bent

d)

Linear

93.

Classify the following molecule.

a)

polar

b)

nonpolar

94.

Classify the following molecule as polar or nonpolar: HF (hydrogen fluoride)

a)

Polar

b)

Nonpolar

95.

Classify the following molecule as polar or nonpolar: F2

a)

Polar

b)

Nonpolar

96.

Is the following molecule polar or nonpolar?

a)

polar

b)

nonpolar

97.

Which of the following formulas represents a polar molecule?

a)

H2

b)

NI3

c)

CO2

d)

CCl4

98.
Which formula represents a nonpolar molecule?
a)
HBr
b)
H2S
c)
CBr4
d)
PCl3
99.

Classify the following molecule.

a)

polar

b)

nonpolar

100.

Classify the following molecule.

a)

polar

b)

nonpolar

101.

Why is the molecule polar?

a)

There is a lone pair of electrons on the central atom.

b)

There are different types of elements bonded to the central atom.

c)

There are no lone pairs of electrons on the central atom and all of the atoms bonded to the central atom are the same.

102.
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
103.
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
104.
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
105.
Given the following: 42.07% Na, 18.89% P, and 39.04% O, determine the empirical formula.
a)
 NaPO2
b)
Na2PO3
c)
Na3PO4
d)
NaPO4
106.
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 
107.
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
108.
Whats the empirical formula of a molecule containing 18.7% of Lithium, 16.3% of Carbon and 65.0% of oxygen?
a)
CO2Li3
b)
Li2CO3
c)
Li3CO2
d)
LiCO5
109.
Given the following: 42.07% Na, 18.89% P, and 39.04% O, determine the empirical formula.
a)
NaPO2
b)
Na2PO3
c)
Na3PO4
d)
NaPO4
110.

Which type of reaction is:

H2 + O2 → H2O

a)

Synthesis

b)

Decomposition

c)

Single Displacement

d)

Double Displacement

111.

Which type of reaction is:

NiCl2 → Ni + Cl2

a)

Synthesis

b)

Decomposition

c)

Single Displacement

d)

Double Displacement

112.

Which type of reaction is:

MgI2 + Br2 → MgBr2 + I

a)

Synthesis

b)

Decomposition

c)

Single Displacement

d)

Double Displacement

113.

Which type of reaction is:

NaCl + AgNO3 → NaNO3 + AgCl

a)

Synthesis

b)

Decomposition

c)

Single Displacement

d)

Double Displacement

114.
Always starts with a Hydrocarbon that reacts with oxygen and produces carbon dioxide and water. 
a)
Decomposition
b)
Synthesis
c)
Combustion
d)
Single Replacement
115.
Ca(OH)2 is an example of a(n)
a)
Acid
b)
Base
c)
Neutral
116.
HBr is an example of a(n)
a)
Acid
b)
Base
c)
Neutral
117.

Identify the type of reaction:

Zn(OH)2 + HNO3 ---> H2O + Zn(NO3)2

a)

single replacement

b)

combustion

c)

acid-base neutralization

d)

synthesis

e)

decomposition

118.

What is the formula for phosphorous acid?

a)

H3PO4

b)

H2PO4

c)

H3P

d)

H3PO3

119.

What is the formula for nitric acid?

a)

HNO2

b)

HNO3

c)

HNO4

d)

H2NO3

120.

Name this acid with the formula HF

a)

hydrofluoric acid

b)

hypofluoric acid

c)

hydrogen fluorine acid

d)

fluoric acid

121.

What is the formula for hydrochloric acid?

a)

HCl

b)

HClO

c)

H3ClO3

d)

HClO3

122.

carbonic acid

a)

H2CO3

b)

H2CrO4

c)

H2C2O4

d)

HCO3

123.

Binary acids start with the prefix "____________"

a)

acid

b)

nitric

c)

hydraulic

d)

hydro

124.

When naming binary acids, the ending always changes to:

a)

-ate

b)

-ite

c)

-ic

d)

-ous

125.

When naming oxyacids, change "-ite" to:

a)

-ate

b)

-ic

c)

-ous

d)

-ite

126.

Name this acid: H2SO4

a)

hydrogen sulfate

b)

hydrosulfuric acid

c)

sulfuric acid

d)

sulfurous acid

127.

Name the acid that uses an acetate ion: HC2H3O2

a)

Acetic acid

b)

Acetous acid

c)

Hydrogen Acetate acid

d)

Hydrogen Acetatic acid

128.

Name this acid: HNO2

a)

hydronitrous acid

b)

hydrogen nitrogen oxygen

c)

nitrous acid

d)

hyponitrous acid

129.

Translate the word equation below:

Nitrogen reacts with Hydrogen to form Ammonia (NH3).

a)

N  → H + NH3N\ \ \rightarrow\ H\ +\ NH_3

b)

N2 + H2 → NH3N_2\ +\ H_2\ \rightarrow\ NH_3

c)

N + H → NH3N\ +\ H\ \rightarrow\ NH_3

d)

N2 → H2 + NH3N_2\ \rightarrow\ H_2\ +\ NH_3

130.

Translate the word equation below.

Hydrogen and Carbon Dioxide react to form Carbonic Acid (H2CO3).

a)

H + CO2 → H2CO3H\ +\ CO_2\ \rightarrow\ H_2CO_3

b)

H → CO2 + H2CO3H\ \rightarrow\ CO_2\ +\ H_2CO_{3_{ }}

c)

H2 + CO2 → H2CO3H_2\ +\ CO_2\ \rightarrow\ H_2CO_3

d)

H2 → CO2 + H2CO3H_2\ \rightarrow\ CO_2\ +\ H_2CO_3

131.

Translate the word equation below.

Carbon Dioxide and Hydrogen react to form Methane (CH4) and Water

a)

CO2 + H2O → CH4 +H2 CO_{2_{\ }}+\ H_2O\ \rightarrow\ CH_4\ +H_2\

b)

CO2 → H2 + CH4 + H2OCO_2\ \rightarrow\ H_2\ +\ CH_4\ +\ H_2O

c)

CO2  + H2 + CH4  → H2OCO_2\ \ +\ H_2\ +\ CH_4\ \ \rightarrow\ H_2O

d)

CO2  + H2 → CH4 + H2OCO_2\ \ +\ H_2\ \rightarrow\ CH_4\ +\ H_2O

132.

Which is the correct chemical equation for the following: Solid Zn reacts with silver (I) chloride to produce Zinc (II) chloride and silver metal

a)

Zn + AgCl → ZnCl2 + Ag

b)

ZnCl2 + Ag → Zn + AgCl

c)

ZnCl2 + Ag2 → Zn + AgCl

d)

Zn2Cl + Ag → Zn + AgCl

133.

Which is the correct chemical equation for the following: Barium Chloride combined with sodium sulfide yields barium sulfide and sodium chloride

a)

BaCl + NaS → BaS+ NaCl

b)

BaCl2 + Na2S → BaS+ NaCl

c)

BaS+ NaCl → BaCl + NaS

d)

BaCl2 + Na2S → BaS+ NaCl2

134.
Which is NOT a diatomic molecule?
a)
Fluorine
b)
Nitrogen
c)
Boron
d)
Bromine
135.

Magnesium can be burned in oxygen to produce solid magnesium oxide.

a)

Mg(s) + O2(g)→ MgO(s)

b)

Mg(s) + O(g) → MgO(s)

c)

Mg(s) + CO2(g) → MgO(s) + C(s)

d)

Mg(s) + O2(g) → Mg2O2(s)

136.
Iron reacts with sulfur to produce iron(II) sulfide powder.
a)
2Fe(s) + S(s) → Fe2S(s)
b)
Fe(s) + S(s) → FeS(s)
c)
Fe(s) + S(g) → FeS(s)
d)
4Fe(s) + S2(g) → 2Fe2S
137.
___C3H8 +___O2 --> ___CO2 + ___H2O
a)
1,5,3,4
b)
2,10,6,8
c)
already balanced
d)
1,5,5,4
138.
__Al + __Fe3N2 -->__AlN + __Fe
a)
already balanced
b)
4,2,4,6
c)
2,1,2,3
d)
1,2,1,3
139.
__Na + __Cl2 --> __NaCl
a)
1,1,2
b)
2,1,2
c)
2,1,1
d)
already balanced
140.
__C6H12O6 + __O2 --> __H2O + __CO2
a)
1,6,6,6
b)
already balanced
c)
1,6,1,6
d)
2,12,12,12
141.
__H2O + __CO2 --> __C7H8 + __O2
a)
4,7,1,9
b)
4,7,1,7
c)
2,3,1,3
d)
already balanced
142.
__(NH4)3PO4 + __Pb(NO3)4 --> __Pb3(PO4)4 + __NH4NO3
a)
2,1,1,6
b)
1,2,2,3
c)
4,3,1,12
d)
4,2,1,12
143.
__BF3 + __Li2SO3 --> __B2(SO3)3 + __LiF
a)
2,3,1,3
b)
2,3,1,6
c)
4,4,2,12
d)
3,3,1,9
144.
10. __C7H17  + __O2 --> __CO2 + __H2O
a)
1,2,7,9
b)
2,14,7,17
c)
3,28,14,17
d)
4,45,28,34
145.
What explains the very high melting and boiling point of water
a)
Strong dipole-dipole bonds between water molecules
b)
Strong hydrogen bonds between water molecules
c)
Dispersion forces which are present in all molecules
d)
Asymmetrical shape of the polar bonds.
146.
Does HCl have hydrogen bonding?
a)
yes
b)
no
147.
Does CH4 have hydrogen bonding?
a)
yes
b)
no
148.
All molecules have London forces between them, but dipole-dipole and hydrogen bonding are so much stronger that when they are present we can ignore London forces.  Which of these has ONLY London forces?
a)
I2
b)
NH3
c)
OCl2
d)
SH2
149.

Which substance would have the weakest intermolecular forces of attraction?

a)

CH4

b)

NaCl

c)

H2O

d)

MgF2

150.

Intermolecular forces for: NH3

a)

Dispersion Force

b)

Dipole dipole

c)

Hydrogen bonding

151.
Intermolecular force present in HCl?
a)
dipole dipole
b)
dispersion
c)
H-bond
d)
ionic
152.

Intermolecular forces for: CO2

a)

Dispersion Force

b)

Dipole dipole

c)

Hydrogen bonding

153.
Rank these in order of strength:
covalent bond
London forces
hydrogen bond
dipole-dipole attraction
a)
dipole-dipole>covalent bond>hydrogen bond>London
b)
London>dipole-diple>hydrogen bond>covalent bond
c)
covalent bond>hydrogen bond>dipole-dipole>London
d)
hydrogen bond>dipole-dipole>London>covalent bond
154.
How will the following molecule bond with itself?
a)
Dispersion
b)
Dipole
c)
Hydrogen bond
155.

Type of intermolecular force present in I2, Br2, and Cl2.

a)

dipole dipole

b)

H-bond

c)

London dispersion

d)

metallic

156.

Water has an unusually high boiling point for a molecular compound because it has

a)

hydrogen bonding

b)

ion-ion attractions

c)

a high density

d)

a large gram formula mass

157.

How many step will it take for me to go from moles given to moles unknown?

a)

1

b)

2

c)

3

d)

4

158.
2NaClO3 (s) → 2NaCl (s) + 3O2 (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
159.
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
160.
Fe2O3 + 3H2 → 2Fe + 3H2O
About how many grams of H2O will be produced from 150 grams of Fe2O3? 
a)
50 grams H2O
b)
60 grams H2O
c)
5000 grams H2O
d)
6000 grams H2O
161.
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
162.
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
163.
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
164.
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
165.
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
166.
The limiting reactant
a)
slows the reaction down
b)
is used up first
c)
is the reactant that is left over
d)
controls the speed of the reaction
167.
What is the limiting reactant if 10 moles of NH3  react  with 30.0 moles of NO?
4NH3+6NO --> 5N2 + 6H2O
a)
NH3
b)
NO
c)
N2
d)
water
168.
When 12 moles of O2 reacts with 1.1 mole of C10H8 what is the limiting reactant?  C10H8 + 12 O2 --> 10 CO2 + 4 H2O
a)
Oxygen
b)
C10H8
c)
Water
d)
Carbon Dioxide
169.
P4 + 3O2 --> P4O6 
What is the limiting reactant is 12 moles of P4 react with 15 moles of O2?
a)
P4
b)
O2
c)
P4O6 
d)
none of the above
170.

P4 + 3O2 --> P4O6

How many moles of P4O6 can be made if 3 moles of P4 react with 6 moles of O2?

a)

1 mole

b)

2 moles

c)

4 moles

d)

0 moles

171.

Use the equation 2 Al + 3 Cl2 ---> 2 AlCl3. If 2 moles of aluminum and 3 moles of chlorine are reacted, how much AlCl3 can be made?

a)

1 mole

b)

2 moles

c)

4 moles

d)

0 moles

172.

Using the following equation:

Fe2O3(s) + 3H2(g) → 2Fe(s) + 3H2O(l)

How many moles of iron can be made from 6 moles H2 and excess Fe2O3?

a)

4 moles Fe

b)

6 moles Fe

c)

9 moles Fe

d)

2 moles Fe

173.
How many grams of FeS are formed from 7.62g of Fe reacted with excess S?
a)
3.82g
b)
7.62g
c)
12.2g
d)
11.4g 
174.
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

175.

When reacting Na with Cl2, we calculated that the theoretical yield should be 13 grams. Our actual yield was 12.5 grams. What is the percent yield?

a)

90.4%

b)

104%

c)

96.15%

d)

1.04%

176.

2Fe2O3 + 3C → 4Fe + 3CO2

You add 28 grams of carbon. You find the actual yield to be 81.2 grams of CO2. What is the percent yield of CO2? (Hint: calculate theoretical yield of CO2 first)

a)

58.83%

b)

308%

c)

6435%

d)

79.14%

177.
Theoretical yield = 73g
Actual yield = 62g
Calculate the percent yield.
a)
1.16%
b)
116%
c)
85%
d)
76%
178.
P4 + 6Cl2 --> 4PCl3 
The reaction of 75.0g P4 with excess chlorine gas produces 110g PCl3 in lab. Find the theoretical yield and calculate percent yield for the reaction. 
a)
78%
b)
64%
c)
27%
d)
33%
179.

11.

LiOH + KCl → LiCl + KOH


b) I actually produced 6 grams of lithium chloride and I began this reaction with 20.0 grams of lithium hydroxide. What is my percent yield?

a)

16.9%

b)

5.91%

c)

1.88%

d)

12.3%

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