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HC04 Bonding

Total questions: 124

Worksheet time: 1hrs 22mins

Name
Class
Date
1.

A(n) (a)   is an atom or molecule that carries a charge

2.

This is an example of a(n) (a)  

3.

This is an example of a(n) (a)  

4.

Match the following

a)

a charged atom or molecule

1.

ion

b)

2.

a charged molecule

c)

3.

a charged atom

d)

an ion has lost or gained

4.

electrons

e)

has nothing to do with ions

5.

protons

5.

Will be attracted to...

Mark all that apply.

a)

oxide ion, a monatomic ion

b)

calcium ion, a monatomic ion

c)

hydroxide ion, a polyatomic ion

d)

ammonium ion, a polyatomic ion

6.

Match the ions that will be attracted to each other and the phrases that go together.

a)

1.

OH–

b)

2.

NH4+

c)

Opposite charges

3.

attract

d)

like charges

4.

repel

7.

Will be attracted to...

Mark all that apply.

a)

b)

c)

d)

8.

Match the following

a)

simplest form of matter

1.

element

b)

particle of an element

2.

atom

c)

particle of a covalent compound

3.

molecule

d)

two or more different elements bonded together

4.

compound

e)

anything that has mass and volume

5.

matter

9.

Which subatomic particles are the most involved in chemical bond and what happens to them determines the type of bond?

a)

valence electrons

b)

neutrons

c)

protons

d)

octet rule

e)

core electrons

10.

Which subatomic particles are at the outer portion of the atom?

a)

valence electrons

b)

neutrons

c)

protons

d)

octet rule

e)

core electrons

11.

Label the atom.

a)

neutron

b)

proton

c)

core electron

d)

Nucleus

e)

Valence electron

1
2
3
1)
2)
3)
12.

The rule that states atoms react to get a full valence shell is known as the (a)   rule.

13.

The outermost electrons are called the (a)   electrons.

14.

Ionic bonding involves the (a)   of electrons

15.

In an ionic bond oppositely charge (a)   are bonded to each other.

16.

Covalent bonding involves the (a)   of electrons

17.

Match the following

a)

ionic bonding

1.

transfer of electrons

b)

covalent bonding

2.

sharing of electrons

c)

oppositely charged ions bonded to each other

3.

ionic bonding

d)

atoms react to get a full outer shell

4.

octet rule

e)

outer most subatomic particles

5.

valance electrons

18.

The degree to which an atom will attract electrons in a chemical bond.

(a)  

19.

Which atom will attract electrons more in a chemical bond?

C or O

(a)  

20.

Which atom will attract electrons more in a chemical bond?

C or N

(a)  

21.

Which atom will attract electrons more in a chemical bond?

C or H

(a)  

22.

Which atom will attract electrons more in a chemical bond?

O or H

(a)  

23.

Which atom will attract electrons more in a chemical bond?

N or H

(a)  

24.

Which atom will attract electrons more in a chemical bond?

N or O

(a)  

25.

Which atom will attract electrons more in a chemical bond?

P or O

(a)  

26.

Which atom has the highest electronegativity of all the elements?



(a)  

27.

Attractions between molecules are called (a)   attractions.

28.

Match the following

a)

equal sharing of electrons

1.

nonpolar covalent bond

b)

unequal sharing of electrons

2.

polar covalent bond

c)

attractions between molecules

3.

intermolecular attraction

d)

very strong attraction between atoms

4.

chemical bond

e)

very strong attraction between oppositely charged ions

5.

ionic bond

29.

Organize these options into the right categories

Categorize the following

high ∆EN

low or no ∆EN

very high ∆EN

electrons unequally shared

electrons equally shared

electrons transferred

partial charges on the ends of the bonds

no charges on the ends

full charges

two different nonmetals

two of the same nonmetal atoms

usually a metal and a nonmetal

can cause molecules to have charges and stick to each other.

hydrogen bonding

attraction between molecules

polar covalent bone
nonpolar covalent bond
ionic bond
intermolecular attraction
30.

Match the following

a)

nonpolar covalent bond

1.

low or no electronegativity difference

b)

polar covalent bond

2.

high electronegativity difference

c)

ionic bond

3.

very high electronegativity difference

31.

Match the following

a)

nonpolar covalent bond

1.

two of the same nonmetals

b)

polar covalent bond

2.

two different nonmetals

c)

ionic bond

3.

metal and nonmetal

32.

Match the following

a)

nonpolar covalent bond

1.

no charges

b)

polar covalent bond

2.

partial charges

c)

ionic bond

3.

full charges

33.

How many covalent bonds can these elements typically form?

a)

H

1.

1

b)

O

2.

2

c)

N

3.

3

d)

C

4.

4

e)

Na

5.

0

34.

How many covalent bonds can

Hydrogen, H

form?

(a)  

35.

How many covalent bonds can

Oxygen, O

form?

(a)  

36.

How many covalent bonds can

Nitrogen, N

form?

(a)  

37.

How many covalent bonds can

Carbon, C

form?

(a)  

38.

How many covalent bonds can

chlorine, Cl

typically form?

(a)  

39.

How many covalent bonds can

Sulfur, S

typically form?

(a)  

40.

How many covalent bonds can

Phosphorous, P

typically form?

(a)  

41.

How many covalent bonds can

Silicon, Si

typically form?

(a)  

42.

How many covalent bonds are shown between the two carbon atoms?

(a)  

43.

How many covalent bonds are shown between the two carbon atoms?

(a)  

44.

How many covalent bonds are shown between the two carbon atoms?

(a)  

45.

How many covalent bonds are shown between the two chlorine atoms?

(a)  

46.

How many covalent bonds are shown between the two hydrogen atoms?

(a)  

47.

How many covalent bonds are shown between the two oxygen atoms?

(a)  

48.

How many covalent bonds are shown between the two nitrogen atoms?

(a)  

49.

Organize these options into the right categories based on the type of bond indicated by the green circle.

Categorize the following
polar covalent bond
nonpolar covalent bond
Ionic Bond
50.

What type of chemical bond is indicated by the green circle?

a)
Hydrogen bond
b)

polar covalent bond

c)

nonpolar covalent bond

d)
Ionic bond
51.

What type of chemical bond is indicated by the green circle?

a)
Hydrogen bond
b)

polar covalent bond

c)

nonpolar covalent bond

d)
Ionic bond
52.

What type of chemical bond is indicated by the green circle?

a)
Hydrogen bond
b)

polar covalent bond

c)

nonpolar covalent bond

d)
Ionic bond
53.

What type of chemical bond is indicated by the green circle?

a)
Hydrogen bond
b)

polar covalent bond

c)

nonpolar covalent bond

d)
Ionic bond
54.

What type of chemical bond is indicated by the green circle?

a)
Hydrogen bond
b)

polar covalent bond

c)

nonpolar covalent bond

d)
Ionic bond
55.

What type of chemical bond is indicated by the green circle?

a)
Hydrogen bond
b)

polar covalent bond

c)

nonpolar covalent bond

d)
Ionic bond
56.

The chemical bond indicated by the green circle will have

a)

no charges

b)

partial charges

c)

full charges

d)

no badges, we don't need no stinkin' badges.

57.

The chemical bond indicated by the green circle will have

a)

no charges

b)

partial charges

c)

full charges

d)

no badges, we don't need no stinkin' badges.

58.

The chemical bond indicated by the green circle will have

a)

no charges

b)

partial charges

c)

full charges

d)

no badges, we don't need no stinkin' badges.

59.

What type of chemical bond is indicated by the green circle?

a)
Hydrogen bond
b)

polar covalent bond

c)

nonpolar covalent bond

d)
Ionic bond
60.

What type of chemical bond is indicated by the green circle?

a)
Hydrogen bond
b)

polar covalent bond

c)

nonpolar covalent bond

d)
Ionic bond
61.

What type of chemical bond is indicated by the green circle?

a)
Hydrogen bond
b)

polar covalent bond

c)

nonpolar covalent bond

d)
Ionic bond
62.

What type of chemical bond is indicated by the green circle?

a)
Hydrogen bond
b)

polar covalent bond

c)

nonpolar covalent bond

d)
Ionic bond
63.

Label the ends of the C=O bond:

a)

Partially negative

b)

partially positive end

1
2
1)
2)
64.

Label the ends of the O–H bond:

a)

Partially negative end

b)

partially positive end

1
2
1)
2)
65.

Label the ends of the O–H bond:

a)

Partially negative end

b)

partially positive end

1
2
1)
2)
66.

Organize these options into the right categories

Categorize the following

has a molecular dipole

molecule has exposed partial charges

NO molecular dipole

NO partial charges

Polar Molecules
Nonpolar Molecules
67.

What type of molecule?

a)

polar molecule

b)

nonpolar molecule

c)

ionic molecule

68.

What type of molecule?

a)

polar molecule

b)

nonpolar molecule

c)

ionic molecule

69.

What type of molecule?

a)

polar molecule

b)

nonpolar molecule

c)

ionic molecule

70.

What type of molecule?

a)

polar molecule

b)

nonpolar molecule

c)

ionic molecule

71.

What type of molecule?

a)

polar molecule

b)

nonpolar molecule

c)

ionic molecule

72.

What type of molecule?

a)

polar molecule

b)

nonpolar molecule

c)

ionic molecule

73.

What type of molecule?

a)

polar molecule

b)

nonpolar molecule

c)

ionic molecule

74.

Which of these will dissolve in water and which in vegatable oil?

Categorize the following

polar molecules

nonpolar molecules

acetone, µ = 2.88 D

hexane, µ = 0.00 D

water
oil
75.

Which of these will probably dissolve in hexane?

a)

benzene, µ = 0.00D

b)

toluene, µ = 0.36 D

c)

Ethanol, EtOH µ = 1.69 D

d)

DMF, µ = 3.82 D

76.

Which of these will probably dissolve in methanol, MeOH?

a)

benzene, µ = 0.00D

b)

toluene, µ = 0.36 D

c)

Ethanol, EtOH µ = 1.69 D

d)

DMF, µ = 3.82 D

77.

"_____ _____ _____" means polar solvents dissolve polar compounds and nonpolar solvents dissolve nonpolar solvents.

(a)  

78.

Water and oil will NOT dissolve is each other. This is an example of "____ ____ ____"

(a)  

79.

Oil and water do NOT dissolve in each other because... and... Pick two.

a)

oil is polar

b)

oil is nonpolar

c)

water is polar

d)

water is nonpolar

80.

Methanol (MeOH) and ethanol (EtOH) will dissolve in each other because... and... Pick two.

a)

EtOH is nonpolar

b)

EtOH is polar

c)

MeOH is polar

d)

MeOH is nonpolar

81.

Hexane and benzene will dissolve in each other because... and... Pick two.

a)

hexane is nonpolar

b)

hexane is polar

c)

benzene is polar

d)

benzene is nonpolar

82.

Polar molecules will be dissolved by

a)

polar solvents

b)

nonpolar solvents

c)

molecular solvents

d)

ionic solvents

e)

chemical solvents

83.

Nonpolar molecules will be dissolved by

a)

polar solvents

b)

nonpolar solvents

c)

molecular solvents

d)

ionic solvents

e)

chemical solvents

84.

The number of bonds an element will form in a covalent compound will usually be equal to:

(Mark all that apply.)

a)

the number of valence electrons

b)

the number of single electrons in the Lewis structure of the element

c)

the number of electrons needed to fill its outer shell

d)

the "A" group number on the periodic table.

e)

the number of paired electrons in the Lewis structure of the element

85.

What kind of bond does this show?

a)

Ionic

b)

Covalent

86.

What kind of bonds are shown here?

a)

Covalent

b)

Ionic

87.

What type of bonding does this picture show?

a)

Ionic

b)

Covalent

88.
According to the octet rule most elements need _______ valence electrons.
a)
2
b)
8
c)
6
d)
18
89.

Which is the correct structure for NH3?

Pictures correspond with a-d.

a)

Option A.

b)

Option B.

c)

Option C.

d)

Option D.

90.
Which LD Diagram is correct for chloromethane (CH3Cl)
a)
A
b)
B
c)
C
d)
D
91.

What is the correct Lewis Dot Structure for NH3?

a)
b)
c)
d)
92.

When new chemical bonds form, energy ____________.

a)

is taken into the system.

b)

is released from the system.

c)

stays the same in the system.

93.

Does breaking bonds require energy, release energy, or not involve energy at all?

a)

requires energy to break

b)

releases energy when broken

c)

No energy involved

94.

X2 is H2, Y2 is N2, and Z2 is O2

According to this PE diagram, which element's bond length is longest?

a)

hydrogen

b)

oxygen

c)

nitrogen

95.

H2O has how many lone pairs in the molecule?

a)

0

b)

1

c)

2

d)

3

e)

4

96.

X2 is H2, Y2 is N2, and Z2 is O2

According to this PE diagram, which element requires the most energy to break the chemical bond?

a)

hydrogen

b)

oxygen

c)

nitrogen

97.

X2 is H2, Y2 is N2, and Z2 is O2

According to this PE diagram, which element has the weakest chemical bond?

a)

hydrogen

b)

oxygen

c)

nitrogen

98.

X2 is H2, Y2 is N2, and Z2 is O2

According to this PE diagram, which element's bond length is shortest?

a)

hydrogen

b)

oxygen

c)

nitrogen

99.

What type of bond is this?

a)

ionic

b)

covalent

100.

Using the PE diagram, what is the bond length of H2?

a)

74

b)

150

c)

45

d)

-432

e)

0

101.

Using this PE diagram, what is the bond energy for the H-H bond in H2?

a)

74

b)

150

c)

45

d)

-432

e)

0

102.

For this PE diagram, what are the units used for bond length?

a)

picometers

b)

angstrom, Å

c)

kilojoules

d)

kilojoules per mole

e)

electron volts

103.

For this PE diagram, what are the units used for bond enthalpy (bond energy)?

a)

picometers

b)

angstrom, Å

c)

kilojoules

d)

kilojoules per mole

e)

electron volts

104.

Bond enthalpy (bond energy) is

(Mark all that apply)

a)

amount of energy released when a bond is formed

b)

amount of energy needed to form a bond

c)

amount of energy needed to break a bond

d)

amount of energy released when a bond breaks

105.

Oxygen is in 6A, so how many bonds can it form based on electrons needed to fill its outer shell?

a)

1

b)

3

c)

4

d)

5

e)

2

106.

Hydrogen is in 1A, so how many bonds can it form based on electrons needed to fill its outer shell?

a)

1

b)

3

c)

4

d)

5

e)

2

107.

Nitrogen is in 5A, so how many bonds can it form based on electrons needed to fill its outer shell?

a)

1

b)

3

c)

4

d)

5

e)

2

108.

Which of the following is the correct Lewis structure for the compound PBr3?

a)

structure A

b)

structure B

c)

structure C

d)

structure D

109.

Which of these is the correct Lewis structure for SiBr4?

a)

A

b)

B

c)

C

d)

D

110.

Based on the position of the shared electrons, which element has a higher electronegativity?

a)

Element A

b)

Element B

c)

They have the same or similar electronegativity.

111.

What kind of bond is shown in the picture?

a)

nonpolar covalent bond

b)

polar covalent bond

c)

ionic bond

d)

hydrogen bond

e)

binary bond

112.

What kind of bond is shown in the picture?

a)

nonpolar covalent bond

b)

polar covalent bond

c)

ionic bond

d)

hydrogen bond

e)

binary bond

113.

What kind of bond is shown in the picture?

a)

nonpolar covalent bond

b)

polar covalent bond

c)

ionic bond

d)

hydrogen bond

e)

binary bond

114.

What kind of bond is shown in the picture?

a)

nonpolar covalent bond

b)

polar covalent bond

c)

ionic bond

d)

hydrogen bond

e)

binary bond

115.

What is the period and group trend for electronegativity? Mark one answer for each.

a)

increases across a period from left to right

b)

decreases across a period from left to right

c)

increases up a group

d)

increases down a group

116.

Which element has a higher electronegativity?

a)

carbon

b)

oxygen

117.

Which element has a higher electronegativity?

a)

sulfur

b)

oxygen

118.

Which element has a higher electronegativity?

a)

sulfur

b)

chlorine

119.

Which element has a higher electronegativity?

a)

bromine

b)

chlorine

120.

Using the model for the formation of Scandium Fluoride (an ionic compound), write the chemical formula.

a)

Sc3F

b)

Sc3F3

c)

Sc+3F-1

d)

ScF3

121.

Using the model, write the chemical formula for an ionic compound that has Mg and Cl.

a)

MgCl2

b)

Mg2Cl2

c)

Mg+2Cl-1

d)

Mg2Cl2

122.

Which shows the correct formation of chemical bonds between potassium, K and chlorine, Cl?

a)

b)

123.

Which shows the correct formation of chemical bonds between nitrogen, N and hydrogen, H?

a)

b)

124.

Which shows the correct formation of chemical bonds between aluminum, Al and oxygen, O?

a)

b)

c)

d)