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Test 6 Review

Total questions: 71

Worksheet time: 2hrs 22mins

Name
Class
Date
1.

Arrange the following species in order of increasing size:

N versus N3-

a)

N > N3-

b)

N < N3-

c)

N = N3-

2.
Which of the following ions has the largest ionic radius?
a)
Na+
b)
Al3+
c)
S2-
d)
Cl-
3.
The Na+ ion is isoelectronic with...
Ne
Al3+
N3-
a)
Ne only
b)
Ne & Al3+
c)
Ne, Al3+ & N3-
d)
None of the above
4.

Which of these has the greatest ionic radius?

a)

potassium

b)

aluminum

c)

carbon

d)

oxygen

5.
Which of the following is the least electronegative element?
a)
oxygen
b)
potassium
c)
fluorine
d)
nitrogen
6.
What elements have zero electronegativity?
a)
metals
b)
nonmetals
c)
metalloids
d)
noble gases
7.
What do we call a covalent bond where electrons are shared UNEVENLY or UNEQUALLY?
a)
Ionic
b)
Polar Covalent
c)
Nonpolar Covalent
d)
Van der Waals Force
8.
What type of bond is shown in this image?
a)
Ionic
b)
Polar Covalent
c)
Nonpolar Covalent
d)
Van der Waals Force
9.
Diatomic elements are defined as IDENTICAL elements that bond with each other (i.e. Oxygen with Oxygen).  What type of bond should they form?
a)
Ionic
b)
Polar Covalent
c)
Nonpolar Covalent
d)
Van der Waals force
10.
Beryllium will ____ valence electrons when forming an ionic bond.
a)
lose 4
b)
gain 4
c)
lose 2
d)
gain 2
11.
Predict the bond that will form between Sr and S.
a)
Ionic
b)
Covalent
12.
How many electrons does oxygen (O) need to gain to become stable?
a)
1
b)
2
c)
3
d)
4
13.
What is it called when atoms share two pairs of electrons?
a)
A double bond
b)
A single bond
c)
A triple bond
d)
A quadruple bond
14.

A molecular geometry with 2 lone pairs and 2 bonding pairs is

a)

Tetrahedral

b)

Trigonal pyramidal

c)

Bent

d)

Linear

15.

The bond angle of trigonal planar is

a)

90 degrees

b)

120 degrees

c)

Less than 120 degrees

d)

Less than 90 degrees

16.

HCN is a linear molecular geometry. What is the polarity of HCN molecule?

a)

Polar molecule

b)

Non-polar molecule

17.
 A lone pair is defined as
a)
A pair of bonding electrons
b)
One non-bonding electron
c)
A pair of non-bonding electrons
d)
A pair of electrons on the central atom
18.
How many lone pairs of electrons are on the P atom in PF3?
a)
1
b)
2
c)
3
d)
0
19.
Who could this molecule be?
a)
CH4
b)
CO2
c)
PCl5
d)
BF3
20.
According to VSEPR, molecules adjust their shapes to keep which of the following as far away as possible?
a)
Pairs of valence electrons
b)
Inner shell electrons
c)
Mobile Electrons
d)
Electrons closest to the nucleus
21.
VSEPR stands for ________ theory.
a)
Valence Structure of Electron Pyramids and Regression
b)
Varied Structures of Electrons Paired and Replaced
c)
Varied Shell Energy of Protons and Radiation
d)
Valence Shell Electron Pair Repulsion
22.

3 atoms bonded and 0 lone pairs

a)

linear

b)

trigonal planar

c)

bent

d)

tetrahedral

e)

trigonal pyramidal

23.

3 atoms bonded and 1 lone pairs

a)

true linear

b)

trigonal planar

c)

bent

d)

tetrahedral

e)

trigonal pyramidal

24.

2 atoms bonded and 2 lone pairs

a)

linear

b)

trigonal planar

c)

bent

d)

tetrahedral

e)

trigonal pyramidal

25.

Use the electron dot formula of sulfur difluoride to predict its molecular shape

a)

Bent

b)

linear

c)

trigonal planar

d)

terahedral

26.
HCl
a)
Polar 
b)
Nonpolar 
27.
N2
a)
Polar 
b)
Nonpolar 
28.
F2
a)
Polar 
b)
Nonpolar 
29.
H2O
a)
Polar 
b)
Nonpolar 
30.
NF3
a)
Polar 
b)
Nonpolar 
31.
Which of the following molecules, based on the elements present, would be most polar?
a)
HF
b)
H2
c)
HCl
d)
HBr
32.
A molecule containing polar covalent bonds is always polar.
a)
True
b)
False
33.

Hydrogen bonding occurs between adjacent molecules that contain hydrogen atoms bonded to N, O, or F. Which of the following molecules could experience hydrogen bonding interactions?

a)

CBr4

b)

NO2

c)

H2S

d)

NH3

34.

Can adjacent H2S molecules have hydrogen bonding interactions?

a)

yes

b)

no

35.

Can adjacent HF molecules have hydrogen bonding interactions?

a)

yes

b)

no

36.

Can adjacent HCl molecules have hydrogen bonding interactions?

a)

yes

b)

no

37.
A substance capable of hydrogen bonding has a ___________ boiling point than a similar substance that doesn't hydrogen bond.
a)
higher
b)
lower
38.

In general, substances with stronger intermolecular forces have ___________ boiling points than those with weaker intermolecular forces

a)

higher

b)

lower

39.

Is this molecule polar or non-polar?

a)

Polar

b)

Non-polar

40.

Which of these is most electronegative?

a)

aluminum

b)

oxygen

c)

sulfur

d)

neon

41.

Is this molecule polar or non-polar?

a)

Non-polar

b)

Polar

42.
In a polar covalent bond, electrons are shared ___________.
a)
equally
b)
unequally
c)
between non-metals with similar electronegativities
d)
between a metal and a non-metal
43.
What geometry will this molecular structure have?: H2S
a)
bent
b)
tetrahedral
c)
linear
d)
trigonal pyramidal
44.
What geometry will this molecular structure have?: PH3
a)
bent
b)
tetrahedral
c)
linear
d)
trigonal pyramidal
45.
Will this molecule be polar or nonpolar? CH4
a)
polar
b)
nonpolar
46.
How many electrons are shared between two atoms that are triple bonded?
a)
6
b)
2
c)
4
d)
8
47.

Which type of IMF is responsible for the attraction pictured above?

a)

Dipole-Dipole Interaction

b)

Ion-Dipole Interaction

c)

Hydrogen Bonds

d)

Covalent Bond

e)

Ionic Bond

48.

Which type of IMF is responsible for the attraction pictured above?

a)

Dipole-Dipole Interaction

b)

Ion-Dipole Interaction

c)

Hydrogen Bonds

d)

Covalent Bond

e)

Ionic Bond

49.

Which type of IMF is responsible for the attraction pictured above?

a)

Dipole-Dipole Interaction

b)

Ion-Dipole Interaction

c)

Hydrogen Bonds

d)

Covalent Bond

e)

Ionic Bond

50.

Which type of IMF is responsible for the attraction pictured above?

a)

Dipole-Dipole Interaction

b)

Ion-Dipole Interaction

c)

Hydrogen Bonds

d)

Covalent Bond

e)

Ionic Bond

51.

Intermolecular forces are attractions between ______.

a)

Cations and anions

b)

Atoms within a molecule

c)

Neighboring molecules

d)

Protons and electrons

52.

Intermolecular forces are responsible for which of the following properties?

a)

State of matter

b)

Color

c)

Odor

d)

Conductivity

53.
How many carbon atoms are in propane
a)
1
b)
2
c)
3
d)
4
54.
Name this alkane
a)
Methane
b)
Ethane
c)
Propane
d)
Butane
55.

Which of the following has the highest boiling point?

a)

heptane

b)

pentane

c)

nonane

56.
As you move down the first group, reactivity _________.
a)
Increases
b)
Decreases
c)
Stays the same
d)
They are all inert
57.
Which two groups on the Periodic Table are the MOST reactive?
a)
Group 1 and Group 17
b)
Group 2 and Group 16
c)
Group 13 and Group 15
d)
Group 17 and Group 18
58.
What is the shape and polarity of CO2?
a)
linear and polar
b)
linear and nonpolar
c)
bent and polar
d)
bent and nonpolar
59.
What is the polarity of BeH2?
a)
polar
b)
nonpolar
60.
Which of these is not an intermolecular force?
a)
covalent bonding
b)
hydrogen bonding
c)
London dispersion forces
d)
dipole-dipole forces
61.

Which is the strongest intermolecular force below?

a)

Ionic

b)

Dispersion

c)

Hydrogen bonding

d)

dipole-dipole

62.

Which of the following does NOT contain hydrogen bonding?

a)

NH3

b)

H2O

c)

CH4

d)

HOF

63.
Which IMF is the predominant IMF for non-polar molecules?
a)
London Dispersion Forces
b)
Dipole Dipole
c)
Hydrogen Bonding
d)
Both Dipole Dipole and Hydrogen Bonding
64.

Which of these has the strongest Dispersion forces?

a)

F2

b)

Br2

c)

I2

d)

Cl2

65.

What type of intermolecular force is present in a sample of Cl2?

a)

Dipole-Dipole

b)

Hydrogen bonds

c)

Dispersion forces

d)

Metallic

66.

What is the strongest intermolecular force present in a sample of HCl?

a)

Dipole-Dipole

b)

Dispersion forces

c)

Hydrogen bonds

d)

Ionic

67.

What is the strongest type of intermolecular force present in a sample of HF?

a)

Dipole-Dipole

b)

Dispersion forces

c)

Hydrogen bonds

d)

ionic

68.

What type of intermolecular force is present in I2, Br2, and Cl2?

a)

Dipole-Dipole

b)

Hydrogen bonds

c)

Dispersion forces

d)

Metallic

69.
In general, substances with stronger intermolecular forces have ___________  boiling points than those with weaker intermolecular forces
a)
higher
b)
lower
70.

Rank these in order of DECREASING strength:

Dispersion forces

hydrogen bond

dipole-dipole attraction

a)

dipole-dipole>hydrogen bond>Dispersion forces

b)

Dispersion forces>dipole-dipole>hydrogen bond

c)

hydrogen bond>dipole-dipole>Dispersion forces

d)

hydrogen bond>dipole-dipole>Dispersion forces

71.

What intermolecular force is present in CHF3?

a)

Hydrogen bonds

b)

Dipole-Dipole

c)

Dispersion forces

d)

ionic

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