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Chemistry Unit 2 AP

Total questions: 82

Worksheet time: 2hrs 42mins

Name
Class
Date
1.

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

a)

interstitial

b)

substitutional

2.

Which atom has the negative dipole in this molecule?

a)

Hydrogen

b)

Fluorine

c)

Neither

3.

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

4.

As the electronegativity difference between 2 atoms increases, the polarity of the bond ____________________

a)

increases

b)

decreases

5.

What type of bond forms between hydrogen and chlorine?

a)

polar covalent

b)

non-polar covalent

c)

ionic

d)

hydrogen bond

6.

What type of alloy is this?

a)

Interstitial

b)

Substitutional

7.

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

a)

12

b)

6

c)

4

d)

8

8.

What is the bond angle in BF3?

a)

90

b)

120

c)

109.5

d)

180

9.

What is the bond angle in H2O?

a)

120

b)

90

c)

180

d)

104.5

10.

What is the bond angle in NH3

a)

120

b)

107.3

c)

180

d)

90

11.

What is the hybridization of carbon in CH4?

a)

sp3

b)

sp

c)

sp2

12.

What is the hybridization for carbon in CO2

a)

sp3

b)

sp

c)

sp2

13.

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

14.

What is the hybridization for an oxygen in CO2

a)

sp3

b)

sp

c)

sp2

15.
Choose the correct shape for this molecule:
a)
Trigonal planar
b)
Trigonal pyramidal
c)
Tetrahedral
d)
Linear
16.

What type of bonding is represented by the model above?

a)

Covalent

b)

Ionic

c)

Metallic

17.

Based on atom type, what type of bond occurs in Ca ?

a)

Ionic

b)

Covalent

c)

Metallic

18.

What type of bonding is represented by the model above?

a)

Covalent

b)

Ionic

c)

Metallic

19.

Using electronegativity values, what type of bond is C–O?

a)

Non-polar covalent

b)

Polar covalent

c)

Ionic

d)

Metallic

20.

Which bond type has electrons that are shared equally?

a)

Metallic

b)

Non-polar covalent

c)

Polar covalent

d)

Ionic

21.

What type of bonding is represented by the model above?

a)

Covalent

b)

Ionic

c)

Metallic

22.

Based on atom type, what type of bond occurs between Si and O ?

a)

Ionic

b)

Covalent

c)

Metallic

23.

As two oppositely charged particles approach each other, what happens to the electrical force between them?

a)

The attractive force increases

b)

The magnitude of the electric force decreases

c)

The repulsive force increases

d)

The magnitude of their charges increases

24.
When distance increases, electrostatic force ____________; we call this relationship ____________ proportional
a)
decreases;directly
b)
decreases;inversely
c)
increases;inversely
d)
increases;directly
25.

As the value of r increases, what happens to the value of F?

a)

F increases

b)

F decreases

c)

F never changes, q does

d)

Cannot know from the information

26.

What does q measure?

a)

the distance between the two charged objects

b)

the amount of charge carried by the object

c)

the amount of force between two charged objects

27.

What correctly describes the interaction between two atoms at point C on the curve above ?

a)

two atoms are far away; weakly interacting

b)

two atoms are close; strongly interacting

c)

two atoms are very close; strongly interacting

d)

two atoms are far away; strongly interacting

28.

What correctly describes the interaction between two atoms at point A on the curve above ?

a)

two atoms are far away; weakly interacting

b)

two atoms are close; strongly interacting

c)

two atoms are very close; strongly interacting

d)

two atoms are far away; strongly interacting

29.

What correctly describes the potential energy at point A on the curve above ?

a)

relatively low

b)

relatively high

30.

What correctly describes the potential energy at point C on the curve above ?

a)

relatively low

b)

relatively high

31.

At what point on the curve are the attractive force equal to the repulsive forces ?

a)

A

b)

B

c)

C

d)

All of the above

32.

At what point on the curve are the repulsive forces the larger than attractive forces ?

a)

A

b)

B

c)

C

d)

All of the above

33.

What is the correct unit for potential energy ?

a)

Newton (N)

b)

electron

c)

Joule (J)

d)

Nanometer (nm)

34.

Which of the following noble gas elements will have the strongest interaction with a second atom of itself ?

a)

He

b)

Ne

c)

Ar

d)

Kr

35.

Which of the following elements will have the smallest distance between atoms when two atoms interact ?

a)

nitrogen

b)

oxygen

c)

fluorine

d)

chlorine

36.

Which pair of atoms will have a weaker interaction compared to the Cl-Cl interaction ?

a)

Br-Br

b)

I-I

c)

F-F

37.

What atom pair will have a larger potential energy "dip" compared to the O-O interaction ?

a)

F-F

b)

N-N

c)

H-H

38.

Why is the Xe-Xe interaction stronger than the Ne-Ne interaction ?

a)

Xe can form a diatomic molecule while Ne can not

b)

Ne can form a diatomic molecule while Ne ca not

c)

Xe has more charged particles than Ne

d)

Ne has more more charged particles than Xe

39.

Why is the Kr-Kr interaction weaker than the Br-Br interaction ?

a)

Kr can form a diatomic molecule while Br can not

b)

Br can form a diatomic molecule while Kr can not

c)

Kr has more charged particles than Br

d)

Br has more charged particles than Kr

40.

If curve A is for the Ne-Ne interaction, what interaction can curve B be for ?

a)

Br-Br

b)

He-He

c)

H-H

d)

Ar-Ar

41.
Which type of bonding allows for the conduction of electricity in the solid state?
a)
Metallic
b)
Ionic
c)
Network Covalent
d)
Molecular Covalent
42.

What type of alloy is shown in the diagram?

a)

Substitutional alloy

b)

Interstitial alloy

c)

Covalent alloy

d)

Ionic alloy

43.

What type of alloy is shown in the diagram?

a)

pure substance

b)

metal

c)

substitutional alloy

d)

interstitial alloy

44.

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

a)

8

b)

4

c)

2

d)

3

45.
Which of the following is the correct Lewis structure for CH2O?
a)
Option A
b)
Option B
c)
Option C
d)
Option D
46.

Why is this Lewis Structure incorrect? Select all that appy.

a)

There should be a single bond between H and C.

b)

There should be a triple bond between C and N.

c)

Carbon has too many bonds around it.

d)

Hydrogen needs more electrons.

47.

Why is this Lewis Structure incorrect? Choose all that apply.

a)

There are too many bonds around Si.

b)

There should only be single bonds in this Lewis Structure.

c)

The Structure is missing a triple bond.

d)

Chlorine only has 6 electrons surrounding it.

48.

Which image could be a representation of NH3?

a)

A

b)

B

c)

C

49.
For carbonate ions, how many resonance structures can be drawn ?
a)
2
b)
3
c)
4
d)
5
50.

What is the formal charge on the oxygen atom at the top of this Lewis dot structure?

a)

0

b)

-1

c)

+1

d)

-3

51.

What is the formal charge on the phosphorus atom in this Lewis dot structure?

a)

0

b)

-1

c)

+1

d)

-3

52.

What is the formal charge on the oxygen atom at the top of this Lewis dot structure?

a)

0

b)

+1

c)

-1

d)

-2

53.

What is the picture showing?

a)

All of the resonance structures for carbonate.

b)

The formal charge on each atom in carbonate.

c)

The electronegativity for carbonate.

d)

The ionization energy for carbonate.

54.
How many resonance structures for NO3- ion?
a)
1
b)
2
c)
3
d)
4
55.
How many resonance structure for SO2 ?
a)
1
b)
2
c)
3
d)
4
56.

Compounds that are composed of the same number and type of atoms but have them arranged in different ways are ___________.

a)

isomers

b)

isotopes

c)

polymers

d)

alkanes

57.
Are the following molecules isomers?
a)
Yes
b)
No
58.
Are the following molecules isomers?
a)
Yes
b)
No
59.

Are CH3OCH3 and CH3CH2OH isomers?

a)

yes

b)

no

60.

Which bond is the strongest?

a)

single

b)

double

c)

triple

61.

Which bond is the weakest?

a)

single

b)

double

c)

triple

62.

Which bond is the shortest?

a)

single

b)

double

c)

triple

63.

Which bond is the longest?

a)

single

b)

double

c)

triple

64.

5, 4, 1

a)

seesaw

b)

T-shaped

c)

square pyramid

d)

square planar

65.

5, 3, 2

a)

seesaw

b)

T-shaped

c)

square pyramid

d)

square planar

66.

6, 5, 1

a)

seesaw

b)

T-shaped

c)

square pyramid

d)

square planar

67.

6, 4, 2

a)

seesaw

b)

T-shaped

c)

square pyramid

d)

square planar

68.

In the resonance form of ozone shown, the formal charge on the central oxygen atom is _______.

a)

0

b)

+1

c)

-1

d)

+2

e)

-2

69.

The Lewis structure of the CO32- ion is

a)
b)
c)
d)
e)
70.

The electrons in a polar covalent molecule are shared...

a)

Evenly

b)

Unevenly

c)

Electrons are not shared

d)

None of the Above

71.

The electrons in a nonpolar covalent molecule are shared...

a)

Evenly

b)

Unevenly

c)

Electrons are not shared

d)

None of the Above

72.

Which diagram shows the bond with the correct dipole arrows and partial charge

a)

b)

c)

73.
In this Lewis structure, the symbol above F means...
a)
electrons are being transferred to Fluorine
b)
electrons are less attracted to F than H
c)
electrons are more attracted to F than H
d)
Fluorine has formed a cation
74.

The direction of the dipole arrow in this image tells us that

a)

H is the more electronegative atom in the bond

b)

Cl is the more electronegative atom in the bond

c)

H is the more polar atom in the bond

d)

Cl is the more polar atom in the bond

75.

Classify the following molecule.

a)

polar

b)

nonpolar

76.

Is the following molecule polar or nonpolar?

a)

polar

b)

nonpolar

77.

Is the following molecule polar or nonpolar?

a)

polar because there are different types of elements bonded to the central atom

b)

nonpolar because the central atom has no lone pairs of electrons

c)

polar because the central atom has a lone pair of electrons

d)

nonpolar because there are no lone pairs on the central atom and the atoms bonded to the central atom are all the same

78.

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.

79.

Draw SF6. What is the molecular geometry?

a)

octahedral

b)

trigonal bipyramid

c)

tetrahedral

d)

trigonal planar

80.

Draw PCl5. What is the molecular geometry?

a)

octahedral

b)

trigonal bipyramid

c)

tetrahedral

d)

trigonal planar

81.

Draw CCl4. What is the molecular geometry?

a)

octahedral

b)

trigonal bipyramid

c)

tetrahedral

d)

trigonal planar

82.

Draw BCl3. What is the molecular geometry?

a)

octahedral

b)

trigonal bipyramid

c)

tetrahedral

d)

trigonal planar

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