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Honors Quiz Covalents (No Network)

Total questions: 34

Worksheet time: 3hrs 50mins

Name
Class
Date
1.

What is the chemical formula for dinitrogen heptachloride?

a)

N2Cl7

b)

2N7Cl

c)

2NCl7

d)

N2Cl5

2.

Which of these is NOT an exception to the octet rule when drawing Lewis dot structures?

a)

stable with less than 8 electrons

b)

odd number of electrons

c)

expanded octet

d)

double octet

3.

Which of these is NOT a polar molecule?

a)
b)
c)
d)
4.

Which of the following is the weakest bond?

a)

Single

b)

Double

c)

Ionic

d)

Triple

5.
Carbon atom undergo
a)
sp hybridization
b)
sp2 hybridization
c)
sp3 hybridization
d)
dsp3 hybridization
6.
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
7.

Which of the following is the correct LD Diagram for Hydrogen Cyanide, HCN?

a)

A

b)

B

c)

C

d)

D

8.
What is the measure of a tetrahedral bond angle?
a)
90 Degrees
b)
109.5 Degrees
c)
120 Degrees
d)
180 Degrees
9.
Which of the following shapes has unshared pairs of electrons on the central atom? 
a)
Linear
b)
Bent
c)
Trigonal Planar
d)
Tetrahedral
10.
What is the MOLECULAR geometry of the central oxygen?
a)
Linear
b)
Trigonal Planar
c)
Bent
d)
Tetrahedral
11.

Which of the following has T-shape molecular geometry?

a)
b)
c)
d)
12.

XeF4 is a square planar. It has

a)

4 bonding pairs

b)

6 bonding pairs

c)

4 bonding pairs with 2 lone pairs

d)

5 bonding pairs with 1 lone pair

13.

What is the hybridization of Xe in XeF4

a)

sp

b)

sp3d

c)

sp

d)

sp3d2

14.

A double bond consists of...

a)

 1σ & 1π1\sigma\ \&\ 1\pi  bonds

b)

 1π & 2σ1\pi\ \&\ 2\sigma  bonds

c)

 2π2\pi  bonds

d)

 2σ2\sigma  bonds

15.

How many pi bonds are in the following molecule?

a)

0

b)

5

c)

2

d)

3

16.

Give the formula: tetraphosphorus nonasulfide

a)

P4S9

b)

P9S4

c)

P2S3

d)

P4NS

17.

When dissolved in water, the solution is a poor conductor of electricity.

a)

ionic compounds

b)

covalent compounds

18.

A single covalent bond is made up of _____ electrons.

a)

one

b)

two

c)

three

d)

four

19.
CO, carbon monoxide, obeys the octet rule using a coordinate covalent bond. What is a coordinate covalent bond?
a)
both bonding electrons come from one atom
b)
a very strong bond.
c)
one electron serves as its own pair
d)
CO is an exception to the octet rule
20.
Forms when one atom donates a pair of electrons to be shared with an atom or ion that needs two electrons to becomes stable.
a)
covalent bond 
b)
sigma bond
c)
polar covalent bond
d)
coordinate covalent bond
21.

In the nitrite ion (NO2-), __________.

a)

both bonds are single bonds

b)

both bonds are double bonds

c)

both bonds are the same because of resonance

d)

there are 20 valence electrons

e)

there is one single and one double bond

22.

A valid Lewis structure of _______ cannot be drawn without violating the octet rule.

a)

NF3

b)

IF3

c)

PF3

d)

SbF3

e)

SO42-

23.

Which atom can accommodate an octet of electrons, but doesn't necessarily have to accommodate an octet?

a)

N

b)

C

c)

H

d)

O

e)

B

24.

As the number of covalent bonds between two atoms increases, the distance between the atoms ______ and the strength of the bond between them ______.

a)

increases, increases

b)

decreases, decreases

c)

increases, decreases

d)

decreases, increases

e)

is unpredictable

25.

The Lewis structure of the CO32- ion is

a)
b)
c)
d)
e)
26.
Consider the molecule below.  Determine the molecular geometry at each of the 2 labeled carbons.
a)
C1 = tetrahedral, C2 = linear
b)
C1 = trigonal planar, C2 = bent
c)
C1 = bent, C2 = trigonal planar
d)
C1 = trigonal planar, C2 = tetrahedral
27.
This molecule has______bond and is a _________molecule.
a)
non-polar; non-polar
b)
polar, polar
c)
polar,
non-polar
d)
non-polar; polar
28.
After drawing in your bonds, what do you do if you don't have enough electrons to get each atom to its octet?
a)
Place dots until everything has eight
b)
Place dots only around the terminal atoms
c)
Add a multiple bond
d)
Have eight only around the central atom
29.

WHat is the shape of this molecule?

a)

Bent

b)

Linear

c)

Tetrahedral

d)

Pyramidal

e)

Trigonal Planar

30.

Molecules:

a)

have covalent bonds and are always polar

b)

have covalent bonds and are always non-polar

c)

have covalent bonds and can be polar or non-polar

d)

have ionic bonds and are always polar

31.

Why do simple molecular substances have low melting and boiling points?

a)

The intermolecular forces between simple molecules are weak.

b)

The covalent bonds holding the atoms together in a simple molecule are strong.

c)

A large number of covalent bonds hold the atoms together in simple molecules.

32.

What is the difference between a polar covalent bond and a nonpolar covalent bond?

a)

The difference between a polar covalent bond and a nonpolar covalent bond is the unequal sharing of electrons and the resulting charge separation in a polar covalent bond.

b)

A nonpolar covalent bond occurs when electrons are completely transferred from one atom to another.

c)

A polar covalent bond involves the sharing of electrons between two atoms of the same element.

d)

A polar covalent bond is stronger than a nonpolar covalent bond.

33.
Molten compound conducts electricity.
a)
ionic compound
b)
covalent compound
34.
forms ions in solution
a)
ionic compounds
b)
covalent compounds

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