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Exam 6 - Bonding and Solutions

Total questions: 150

Worksheet time: 4hrs 48mins

Name
Class
Date
1.

A bond between a metal and a nonmetal is called a(n)

a)

covalent bond

b)

ionic bond

c)

metallic bond

d)

transfer bond

2.

A bond between a nonmetal and a nonmetal is called a(n)

a)

covalent bond

b)

ionic bond

c)

metallic bond

d)

transfer bond

3.

What type of bond involves the sharing of electrons between atoms?

a)

covalent bond

b)

ionic bond

c)

metallic bond

d)

transfer bond

4.

Identify the following compound as ionic or covalent: MgO

a)

ionic

b)

covalent

5.

Identify the following compound as ionic or covalent: SO2

a)

ionic

b)

covalent

6.
The 3 States of Matter are  __________, ___________, and ___________. 
a)
Volume, Density, and Mass
b)
Solid, Liquid, and Gas
c)
Gas, Liquid, and Volume
d)
Heat, Cold, and Magnetism
7.

What is a mixture?

a)

A combination of two or more substances that can't be easily separated.

b)

A combination of two or more substances that can be easily separated.

8.

Which is an example of a solution?

a)

Salt and Sugar

b)

Salt Water

c)

Jelly beans

d)

Concrete

9.

What can you do to separate salt from water?

a)

Add aditional water.

b)

Take some water out.

c)

Let it stand in the sun for a while.

d)

Decrease the temperature of the water.

10.
Are the atoms more stable when they are bonded together or when they are apart? 
a)
Bonded Together
b)
Apart
11.
Ionic Bonding involves...
a)
The transfer of protons
b)
The transfer of nuetrons 
c)
The transfer of electrons
d)
None Of the above
12.
What type of bond is present when electrons are freely shared between metal atoms?
a)
Metallic
b)
Ionic
c)
Covalent
d)
Hippie
13.
A substance which has a high melting point, conducts electricity when dissolved in water, and has a crystalline structure probably has what type of bond?
a)
Ionic
b)
Metallic
c)
Covalent
d)
Crystalline
14.
What type of bond occurs when two or more elements share electrons?
a)
Ionic
b)
Covalent
c)
Metallic
d)
Caring
15.
What type of bond occurs between a positive and a negative ion?
a)
Ionic bond
b)
covalent bond
c)
metallic bond
d)
p-n bond
16.
Which statement best describes the energy change as bonds are formed and broken in this reaction?
      H2 + Cl2  ➔  2HCl
a)
The forming of the H-Cl bond releases energy
b)
The forming of the H-Cl bond absorbs energy
c)
The breaking of the H-H bond releases energy
d)
The breaking of the Cl-Cl bond releases energy
17.
A solid substance is an excellent conductor of electricity. The chemical bonds in this substance are most likely?
a)
ionic, because the valence electrons are shared between atoms
b)
covalent, because the valence electrons are mobile
c)
metallic, because the valence electrons are stationary
d)
metallic, because the valence electrons are mobile
18.
An atom that gains an electron in an ionic bond becomes a/an _______________ charged ion.
a)
Negatively
b)
Positively
19.
Is the molecule H2O polar or non-polar?
a)
polar
b)
non-polar
20.
Exothermic reactions...
a)
Absorb energy
b)
Release energy
c)
Release Color
d)
Absorb Color
21.
Is photosynthesis an exothermic or endothermic reaction?
a)
Endothermic
b)
Exothermic
c)
Neither
22.
In an exothermic reaction, heat is ...
a)
taken in
b)
given out
23.
Is the combustion of gasoline endothermic or exothermic?
a)
Endothermic
b)
Exothermic
24.
If a reaction is exothermic
a)
It takes more energy to break the bonds of the reactants than is released when the bonds in the products are formed
b)
More energy is released when the bonds in the products are formed than is used to break the bonds in the reactants
c)
The same amount of energy is used to break the bonds of the reactants as is released when the bonds in the products are formed
d)
The temperature goes down
25.
If a reaction is endothermic,
a)
The temperature increases
b)
It takes more energy to break the bonds of the reactants than is released when the bonds in the products are formed
c)
More energy is released when the bonds in the products are formed than is used to break the bonds in the reactants
d)
The same amount of energy is used to break the bonds of the reactants as is released when the bonds in the products are formed
26.
Intermolecular force present in HCl?
a)
dipole dipole
b)
dispersion
c)
H-bond
d)
ionic
27.
Intermolecular force present in Cl2?
a)
dipole dipole
b)
H-bond
c)
dispersion
d)
metallic
28.
Type of intermolecular force present in HF.
a)
dipole dipole
b)
dispersion
c)
H-bond
d)
ionic
29.
Type of intermolecular force present in I2, Br2, and Cl2.
a)
dipole dipole
b)
H-bond
c)
dispersion
d)
metallic
30.
Intermolecular forces are the forces
a)
within molecules
b)
between molecules
31.
Which of the following has the highest boiling point?
a)
H2
b)
NH3
c)
N2
d)
O2
32.
Which of the following has the lowest boiling point?
a)
CaCl2
b)
PH3
c)
Cl2
d)
N2
33.
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.
34.
Which of these has the strongest London forces?
a)
F2
b)
Br2
c)
Cl2
d)
I2
35.
Which is not a kind of intermolecular force?
a)
Hydrogen bonding
b)
Covalent bond
c)
London Forces
d)
Dipole-dipole attraction
36.
What type of intermolecular force is the strongest?
a)
Hydrogen bonding
b)
Dipole-dipole attractions
c)
London forces
37.
What type of interaction does this represent?
a)
non-polar covalent
b)
dipole
c)
dipole-dipole
d)
none that I know of
38.
Which type of force is this?
a)
Intramolecular
b)
Intermolecular
c)
Hydrogen
d)
Chlorine
39.
What type of bond forms between two or more atoms that are charged (+/-)?
a)
Covalent bond
b)
Incomplete bond
c)
Ionic bond
d)
Metallic bond
40.
Which of the following is an example of an IONIC COMPOUND?
a)
NaCl
b)
H2O
c)
CO2
d)
NO
41.
Which of the following is an example of a COVALENT COMPOUND?
a)
H2S
b)
KI
c)
CaCl2
d)
MgO
42.
Name that Ion
Li+
a)
copper (III)
b)
lithium
c)
ladmium
d)
iodine
43.
Which category of elements have the property of being malleable and ductile?
a)
gases
b)
metals
c)
metalloids
d)
nonmetals
44.
Alloys include a "sea" of free moving _______. 
a)
electrons
b)
atoms 
c)
molecules 
d)
protons 
45.

What occurs when potassium reacts with chlorine to form potassium chloride?

a)

Electrons are shared and the bonding is ionic.

b)

Electrons are shared and the bonding is covalent.

c)

Electrons are transferred and the bonding is ionic.

d)

Electrons are transferred and the bonding is covalent.

46.

What is the net charge of an ion that has 8 protons, 9 neutrons, and 10 electrons?

a)

1+

b)

2+

c)

1-

d)

2-

47.

The equation in the image represents the formation of a

a)

fluorine atom, which is smaller in radius than a fluoride ion

b)

fluorine atom, which is larger is radius than a fluoride ion

c)

fluoride ion, which is larger in radius than a fluorine atom

d)

fluoride ion, which is smaller in radius than a fluorine atom

48.

Two grams of potassium chloride are completely dissolved in a sample of water in a beaker. This solution is classified as

a)

an element

b)

a compound

c)

a homogeneous mixture

d)

a heterogeneous mixture

49.

Which compound has the strongest hydrogen bonding between its molecules?

a)

HBr

b)

HCl

c)

HF

d)

HI

50.

What is the number of moles of C that must completely react to produce 2.0 moles of C2H6?

a)

3.0 mol

b)

4.0 mol

51.

The Lewis structure of the CO32- ion is

a)
b)
c)
d)
e)
52.

Which formula represents a polar molecule?

a)

Cl2

b)

CH4

c)

HCl

d)

CO2

53.

Which compound has both ionic and covalent bonds?

a)

CH4

b)

CO

c)

CaCl2

d)

MgSO4

54.

Classify the following molecule.

a)

polar

b)

nonpolar

55.

Classify the following molecule.

a)

polar

b)

nonpolar

56.

Classify the following molecule.

a)

polar

b)

nonpolar

57.

Is the following molecule polar or nonpolar?

a)

polar

b)

nonpolar

58.

Is the following molecule polar or nonpolar?

a)

polar

b)

nonpolar

59.

Is the following molecule polar or nonpolar?

a)

polar

b)

nonpolar

60.

Is the following molecule polar or nonpolar?

a)

polar

b)

nonpolar

61.

Is the following molecule polar or nonpolar?

a)

polar

b)

nonpolar

62.

Why is the molecule polar?

a)

There is a nonbonding pair on the central atom.

b)

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

c)

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

63.
HCl
a)
Polar 
b)
Nonpolar 
64.
F2
a)
Polar 
b)
Nonpolar 
65.
H2O
a)
Polar 
b)
Nonpolar 
66.

Why is the molecule polar?

a)

There are nonbonding pairs on the central atom.

b)

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

c)

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

67.

Classify the following molecule.

a)

polar

b)

nonpolar

68.

Why is the molecule nonpolar?

a)

There are nonbonding pairs on the central atom.

b)

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

c)

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

69.

Why is the molecule polar?

a)

There is a nonbonding pair on the central atom.

b)

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

c)

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

70.

Why is the molecule polar?

a)

There are nonbonding pairs on the central atom.

b)

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

c)

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

71.

Why is the molecule nonpolar?

a)

There are nonbonding pairs on the central atom.

b)

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

c)

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

72.

How many bonding pairs and lone pairs for a pyramidal molecule?

a)

2 bonding pairs 2 lone pairs

b)

2 bonding pairs 0 lone pairs

c)

3 bonding pairs 1 lone pairs

d)

4 bonding pairs 2 lone pairs

73.

What is the bond angle of an ammonium ion

a)

107.0

b)

104.5

c)

109.5

d)

120.0

74.
Which of the following molecular shapes would have a bond angle of 180 Degrees?
a)
Bent
b)
Trigonal Planar
c)
Tetrahedral
d)
Linear
75.

What would be the bond angle between atoms in this molecule?

a)

109.5

b)

120

c)

180

d)

90

76.

What shape would a molecule have if it has 2 bonded pairs and 1 lone pair around its central atom? (It may help if you sketch this out)

a)

Linear

b)

Trigonal planar

c)

Tetrahedral

d)

Bent

77.

What is the name of this molecule's shape?

a)

Bent

b)

Linear

c)

Tetrahedral

d)

Trigonal pyramidal

78.

What 3-D shape would this molecule have: H2S ?

a)

bent

b)

tetrahedral

c)

linear

d)

trigonal pyramidal

79.

What 3-D shape would this molecule have?

a)

Trigonal planar

b)

Pyramidal

c)

Tetrahedral

d)

Bent

80.

What 3-D shape would this molecule have?

a)

tetrahedral

b)

trigonal planar

c)

trigonal pyramid

d)

bent

81.

Which Lewis Dot Model drawing correctly shows an O2 molecule?

a)
b)
c)
d)
82.

Which best describes a triple bond?

a)

3 shared pairs of electrons

b)

3 shared electrons

c)

a central electron with 3 atoms bonded around it

83.

What shape would a molecule have if it has 4 bonded pairs around its central atom? (It may help if you sketch this out)

a)

Linear

b)

Trigonal planar

c)

Tetrahedral

d)

Bent

84.

How many valence electrons should Lithium have in its Lewis dot model?

a)

1

b)

2

c)

3

d)

4

85.

This is a correct dot diagram for carbon (C)

a)

true

b)

false

86.

Which of these is incorrect?

a)
b)
87.

Which is the correct molecular structure for carbon dioxide?

a)
b)
c)
d)
88.

How many total valence electrons are participating in bonding in the molecule above?

a)

8

b)

4

c)

2

d)

3

89.

CO2 has how many lone pairs?

a)

0

b)

1

c)

2

d)

3

e)

4

90.
This is the correct dot diagram for sodium (Na)
a)
true
b)
false
91.
Which of the following is the correct Lewis dot structure for the molecule fluorine (F2)?
a)
A
b)
B
c)
C
d)
D
92.

CCl4 has how many double bonds?

a)

0

b)

1

c)

2

d)

3

93.

What is a cation?

a)

a metal with a negative (-) charge that gains electrons

b)

a non-metal with a negative (-) charge that loses electrons

c)

a metal with a positive (+) charge that loses electrons

d)

a non-metal with a positive (+) charge that loses electrons

94.

What is a anion?

a)

a metal with a negative (-) charge that loses electrons

b)

a non-metal with a negative (-) charge that gains electrons

c)

a metal with a positive (+) charge that gains electrons

d)

a non-metal with a positive (+) charge that loses electrons

95.
has the same composition throughout and does not vary from sample to sample
a)
pure substance
b)
compound
c)
solvent
d)
solution
96.
substance that dissolves
a)
solvent
b)
solution
c)
solute
d)
unsaturated
97.
contains less solute than a saturated solution
a)
unsaturated solution
b)
saturated solution
c)
supersaturated solution
98.
contains the maximum amount of dissolved solute
a)
unsaturated solution
b)
supersaturated solution
c)
saturated solution
99.
mixture in which the composition is not uniform throughout
a)
homogeneous mixture
b)
heterogeneous mixture
100.
amount of solute that can dissolve in a given amount of solvent at a given temperature
a)
saturated solution
b)
solubility
c)
pure substance
d)
colloid
101.
substance that dissolves the solute
a)
solution
b)
solvent
c)
saturation
102.
substance consisting of atoms or ions of two or more different elements joined by a chemical bond
a)
element
b)
mixture
c)
compound
103.
mixture of two or more substances; dissolved particles are spread evenly throughout the mixture
a)
solvent
b)
solute
c)
mixture
d)
solution
104.
a solute whose water solution conducts electricity is called a(n)
a)
nonconductor
b)
electrolyte
c)
nonelectrolyte
d)
aqueous solution
105.
__________ are made up of solutes and solvents.
a)
Solutions
b)
Suspension
c)
Colloid
106.
If an electrical current can run through a solution, it is said to contain
a)
magic
b)
nonelectrolytes
c)
electricity
d)
electrolytes
107.
Which of the following is an electrolyte?
a)
sodium chloride
b)
sugar
c)
water
108.

True or false:

Dissolved particles will pass through a piece of filter paper.

a)

True

b)

False

109.

Solutions that conduct a current are called ____________ and are made from ___________ compounds.

a)

electrolytes; ionic

b)

nonelectrolytes; ionic

c)

electrolytes; molecular

d)

electrolytes; covalent

110.
Oil molecules are nonpolar. What kind of solvent is required to remove an oil stain?
a)
saturated
b)
unsaturated
c)
polar
d)
nonpolar
111.

You and your friend have a contest to see who can make sweet iced tea the fastest. Which of the following would NOT help you win?

a)

Cooling the water

b)

Using smaller sugar crystals

c)

Heating the water

d)

Stirring quickly

112.
what is the molarity of a solution that contains 125 g NaCl in 4.00 L of solution?
a)
0.535 M NaCl
b)
2.14 M NaCl
c)
8.56 M NaCl
d)
31.3 M NaCl
113.
What is the most common solvent in everyday life?
a)
Ethanol
b)
Tuluene
c)
Water
d)
Oils
114.

How much KNO3 solute is saturated at 40 degrees?

a)

75

b)

55

c)

65

d)

85

115.

At what temperature can you fully dissolve 140g of NaNO3?

a)

62

b)

73

c)

81

d)

You cannot determine this

116.

At what temperature can you fully dissolve 60g of KNO3?

a)

27

b)

30

c)

37

d)

You cannot determine this

117.

What type of a solution is 100g KNO3 at 40ºC in 100g H2O?

a)

Saturated

b)

Unsaturated

c)

Supersaturated

118.

What type of a solution is 55g KCl at 70ºC in 100g H2O?

a)

Saturated

b)

Unsaturated

c)

Supersaturated

119.
How does a solution become supersaturated?
a)
dissolve lots of solvent in it.
b)
dissolve a little solute in it. 
c)
dissolve more solute than you should be able to. 
d)
dissolve a super amount of solvent in it. 
120.

Define the term soluble.

a)

Can dissolve in water

b)

Cannot dissolve in water

c)

Partially dissolves in water

121.

Define the term insoluble.

a)

Can dissolve in water.

b)

Cannot dissolve in water.

c)

Partially dissolves in water.

122.
At standard pressure, which substance becomes less soluble in water as temperature increases from 10oC to 80oC?
a)
HCl
b)
KCl
c)
NaCl
d)
NH4Cl
123.

Which substance is least soluble at 0 ºC?

a)

KI

b)

KNO3

c)

KClO3

d)

Ce2(SO4)3

124.

Which solution is more concentrated?

Solution 1:

500 mL of water

100 g of salt


Solution 2:

500 mL of water

90 g of salt

a)

Solution 1

b)

Solution 2

c)

They have the same concentration

d)

I have no idea

125.
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 
126.
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
127.
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
128.
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
129.
True or False? The higher the concentration of a solution the less solutes it has in it.
a)
True
b)
False
130.
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
131.
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
132.
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
133.
Determine the molarity of 2.25 mole of sulfuric acid, H2SO4, dissolved in 725 mL of solution.
a)
322.2 M
b)
3.1 M
c)
0.32 M
d)
2.25 M
134.
Molarity is measured in
a)
moles per kg
b)
mols per L
c)
moles per kJ
d)
moles per mL
135.
What is the concentration, in percent by mass, of 0.62 g of solute in 45.0 g of solution?
a)
0.014 %
b)
1.4 %
c)
0.13%
136.
What is the concentration, in percent by volume, of 15.3 mL of solute in 2.65 L of solution?
a)
0.58%
b)
0.0058%
c)
5.8%
137.
What mass of solute is needed to make 75.0 g of a 3.4% solution?
a)
2.55 g
b)
22 g
c)
0.05 g
138.

What is the concentration of a solution in parts per million if 0.02 grams of NaCl is dissolved in 1000 grams of water?

a)

2 ppm

b)

20 ppm

c)

200 pm

d)

0.2 ppm

139.

Which unit can be used to express the concentration of a solution?

a)

mols/L

b)

m/s

c)

g/mol

d)

amu

140.

Which unit can be used to express the concentration of a solution?

a)

L/s

b)

J/g

c)

ppm

d)

kPa

141.

Which salt below has the largest effect on freezing point?

a)

C2H4O2

b)

H2S

c)

LiBr

d)

CaF2

142.

Using the graph above, which compound would dissolve the fastest at 20° C, KCl, NaCl, KNO3, or KClO3?

a)

KCl

b)

NaCl

c)

KNO3

d)

KClO3

143.
The freezing point of a solution is ____ the freezing point of the pure solvent.
a)
the same as
b)
lower than
c)
higher than
d)
no relation to
144.
The boiling point of a solution is ______ the boiling point of the pure solvent.
a)
higher than
b)
the same as
c)
lower than
d)
higher or lower than
145.
A beaker contains a mixture of a sand and small pebbles. What kind of mixture is this?
a)
Homogeneous  
b)
Solution
c)
Heterogeneous  
d)
Compound    
146.
A solution has 10 moles of ammonia in 2L of solution. What is the molarity? 
a)
5.0 M
b)
20 M
c)
0.5 M
d)
0.2 M
147.
Zinc Carbonate (ZnCO3)
a)
Soluble 
b)
Insoluble 
148.
Potassium hydroxide (KOH)
a)
Soluble 
b)
Insoluble
149.
Zinc Hydroxide (Zn(OH)2)
a)
Soluble 
b)
Insoluble
150.
Sodium acetate (NaC2H3O2)
a)
soluble
b)
insoluble

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147 questions

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146 questions

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145 questions

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Worksheet

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