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AP Chemistry Unit 2: IYKYK

Total questions: 57

Worksheet time: 58mins

Name
Class
Date
1.

Unit 2: A single bond is composed of

a)

1 sigma bond

b)

1 pi bond

c)

1 sigma and 1 pi bond

d)

no sigma or pi bonds

2.

Unit 2: A triple bond is composed of

a)

1 sigma bond

b)

1 pi bond

c)

2 pi bonds

d)

1 sigma and 2 pi bonds

3.

Unit 2: Lattice energy is the energy to break an ionic bond in a compound. Lattice energy increases as the ion’s charge increases. Lattice energy decreases as the radii of the ions increase.

a)

True

b)

False

4.

Unit 2: SiO2 (quartz) and diamonds are ____________________, and they have very high boiling/melting points.

a)

covalent network solids

b)

ionic solids

c)

molecular solids

d)

interstitial alloys

5.

Unit 2: ______________ alloys are made when a smaller atom fits into the gaps between larger atoms of a metallic crystal.

a)

Interstitial

b)

Substituitonal

6.

Unit 2: What type of alloy is made when the radii of the atoms are similar in size?

a)

interstitial

b)

substitutional

7.

Unit 2: In this molecule, Carbon has a formal charge of ____ and Nitrogen has a formal charge of _____.

a)

0, 0

b)

1, 0

c)

0, -1

d)

-1, 0

8.

Unit 2: What type of alloy is this?

a)

Interstitial

b)

Substitutional

9.

Unit 2: What is the total # of covalent bonds carbon can form when drawing a Lewis structure?

a)

12

b)

6

c)

4

d)

8

10.

Unit 2: What is the bond angle in BF3?

a)

90

b)

120

c)

109.5

d)

180

11.

Unit 2: What is the bond angle in H2O?

a)

120

b)

90

c)

180

d)

104.5

12.

Unit 2: Are asymmetrical molecules polar or nonpolar?

a)

Polar

b)

non-polar

c)

neither

13.

Unit 2: What is the bond angle in NH3

a)

120

b)

107.3

c)

180

d)

90

14.

Unit 2: What is the hybridization of carbon in CH4?

a)

sp3

b)

sp

c)

sp2

15.

Unit 2: What is the hybridization for carbon in CO2

a)

sp3

b)

sp

c)

sp2

16.

Unit 2: Count the number of sigma and pi bonds in this molecule:

a)

13 sigma, 1 pi

b)

14 sigma, 2 pi

c)

1 sigma, 14 pi

d)

2 sigma, 13 pi

17.

Unit 2: What is the hybridization for an oxygen in CO2

a)

sp3

b)

sp

c)

sp2

18.

Unit 2: Choose the correct shape for this molecule:

a)
Trigonal planar
b)
Trigonal pyramidal
c)
Tetrahedral
d)
Linear
19.

Unit 2: What is the total # of covalent bonds carbon has to make when drawing a Lewis structure?

a)

12

b)

6

c)

4

d)

8

20.

Unit 2: What is the the shape of this molecule according to VSPER theory?

a)
Linear
b)
Tetrahedral
c)
Trigonal Planar
d)
Trigonal pyramidal
21.

Unit 2: What compound could this be?

a)

CO2

b)

NH3

c)

H2S

d)

CH4

22.

Unit 2: Draw the Lewis Dot structure for PCl5 and determine the predicted molecular geometry

a)

octahedral

b)

trigonal pyramidal

c)

seesaw

d)

trigonal bipyramidal

23.

Unit 2: Choose the correct shape for this molecule:

a)
Trigonal planar
b)
Trigonal pyramidal
c)
Tetrahedral
d)
Linear
24.

Unit 2: Choose the correct shape for this molecule:

a)
Trigonal planar
b)
Trigonal pyramidal
c)
Tetrahedral
d)
Linear
25.

Unit 2: How many sigma and pi bonds does this have?

a)
1 sigma and 1 pi
b)
2 sigma and 1 pi
c)
1 sigma and 2 pi
d)
2 sigma and 2 pi
26.

Unit 2: How many sigma and pi bonds does this have? 

a)
3 sigma and 2 pi
b)
5 sigma and 5 pi
c)
5 sigma and 0 pi
d)
0 sigma and 5 pi
27.

Unit 2: Carbon atom undergo

a)
sp hybridization
b)
sp2 hybridization
c)
sp3 hybridization
d)
dsp3 hybridization
28.

Unit 2: What is the total # of covalent bonds carbon has to make when drawing a Lewis structure?

a)

12

b)

6

c)

4

d)

8

29.

Unit 2: What is the bond angle in BF3?

a)

90

b)

120

c)

109.5

d)

180

30.

Unit 2: What is the bond angle in H2O?

a)

120

b)

90

c)

180

d)

109.5

31.

Unit 2: Are asymmetrical molecules polar or nonpolar?

a)

Polar

b)

non-polar

c)

neither

32.

Unit 2: What is the bond angle in NH3

a)

120

b)

109.5

c)

180

d)

90

33.

Unit 2: What is an example of a covalent network solid?

a)

Salt

b)

Diamond

c)

Sugar

d)

Water

34.

Unit 2: What is the hybrid orbital used in CH4?

a)

sp3

b)

sp

c)

sp2

35.

Unit 2: What is the hybrid orbital used in CO2

a)

sp3

b)

sp

c)

sp2

36.

Unit 2: Count the number of sigma and pi bonds in this molecule:

a)

13 sigma, 1 pi

b)

14 sigma, 2 pi

c)

1 sigma, 14 pi

d)

2 sigma, 13 pi

37.

Unit 2: Why are asymmetrical molecules polar?

a)

Their dipoles do not cancel

b)

Their dipoles cancel

38.

Unit 2: What is the bond angle in SO2

a)

120

b)

90

c)

180

d)

109.5

39.

When two identical atoms, such as two oxygen atoms, bond, the resulting bond is​ (a)  

Choose from the below words
nonpolar covalent
polar covalent
ionic
metallic
40.

Click on the bond that shares the most electrons in this structure.

A
B
C
D
E
F
G
H
I
J
41.

Label the type of bonds seen in the structure to the right

a)

Double Bond

b)

Triple Bond

c)

Single bond

d)

Quadruple Bond

1
2
1)
2)
42.
Question Image
a)

Electronegativity difference is large enough to cause unequal sharing of electrons but not large enough to cause a transfer of electrons from one atom to another.

1.

C

b)

Compounds held together with these bonds are malleable with high thermal and electrical conductivity due to freely moving electrons

2.

A

c)

Bonded atoms share electrons without a dipole moment

3.

D

d)

Electronegativity difference between atoms is large enough to transfer electrons

4.

B

43.

Match the following

a)

One shared pair of electrons

1.

Single Bond

b)

Two shared pairs of electrons

2.

Double Bond

c)

Three shared pairs of electrons

3.

Triple Bond

44.

Match the types of elements with the correct bond formation.

a)

metal - nonmetal

1.

ionic bond

b)

metal - metal

2.

metallic bond

c)

nonmetal - nonmetal

3.

covalent bond

45.


Match the term and its diagram

a)
1.

Ionic bond

b)
2.

Covalent bond

c)
3.

Hydrogen bond

46.

​ ​ (a)   ​ compounds are usually the strongest.

Choose from the below words
Ionic
Covalent
47.

Match the following pictures to the types of bonds

a)

1.

metallic bond

b)

2.

hydrogen bond

c)

3.

ionic bond

d)

4.

covalent bond

e)

5.

polar bond

48.

A sea of electrons forms a ​ (a)  

Choose from the below words
metallic bond
ionic bond
covalent bond
49.

Match the following with their correct chemical bond type

a)

NaClNaCl

1.

Ionic

b)

H2OH_2O

2.

Covalent

c)

CoCo

3.

Metallic

50.
This is an example of a __________ bond.
a)
non-polar covalent
b)
polar covalent
c)
ionic
d)
metallic
51.
How many electrons are shared in a triple bond?
a)
6
b)
3
c)
6 pairs
d)
5
52.
What type of bond is this?
a)
ionic
b)
covalent
53.

The image above shows:

a)

covalent bonding

b)

ionic bonding

c)

metallic bonding

54.

Which best describes the bonding in the cyanide ion (CN-)?

a)

3 (sigma) bonds

b)

2 (sigma) bonds and I (pi) bond

c)

1 (sigma) bond and 2 (pi) bonds

d)

3 (pi) bonds

55.

Use your knowledge and electronegativity sheet to predict what the following compound is classified as.

a)

nonpolar covalent

b)

polar covalent

c)

ionic

d)

metallic

56.
What type of bond is illustrated above?
a)
Metallic
b)
Ionic
c)
Covalent
d)
Wiggly
57.

What is the name for the electrostatic force of attraction between the particles shown in the image?

a)

covalent bond

b)

dative covalent bond

c)

metallic bond

d)

ionic bond

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