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Covalent, VSEPR, Naming, Bonding Review

Total questions: 60

Worksheet time: 2hrs 7mins

Name
Class
Date
1.
Which of the following elements will NOT be surrounded by an octet of electrons in a correctly drawn Lewis structure?
a)

Hydrogen

b)

Carbon

c)

Oxygen

d)

Chlorine

2.
The seven elements that occur as diatomic elements are:
a)

Fe₂, Rn₂, O₂, He₂, Ne₂, C₂, Br₂

b)

H₂, N₂, O₂, F₂, Cl₂, Br₂, I₂

c)

H₂, N₂, O₂, He₂, Ne₂, Cl₂, Br₂

d)

H₂, N₂, O₂, He₂, Ne₂, C₂, Na₂

3.

In the correct Lewis structure for the methane (CH₄) molecule, how many lone pairs (non-bonding valence-electron pairs) surround the carbon?

a)

0

b)

2

c)

4

d)

8

4.
Which of the following is an acceptable Lewis Structure for the molecule CNCl?
a)

Option L

b)

Option O

c)

Option V

d)

Option E

5.
Which of the following is an acceptable Lewis Structure for the molecule N₂?
a)

Option L

b)

Option O

c)

Option V

d)

Option E

6.

This lewis structure is WRONG! What ie one error in this Lewis structure for ClO3-?

a)

There are too few valence electrons shown in the structure.

b)

There are too many total valence electrons shown in the structure.

c)

All 3 bonds between Cl and O should be double bonds.

d)

None of the oxygen atoms are connected to 8 valence electrons.

7.

This Lewis structure for CH3F is WRONG! What's is one thing that is wrong with it?

a)

The F atom should be the center of the molecule, because it’s less electronegative than C.

b)

  • The C atom are connected to less than 8 valence electrons, which would make this molecule unstable.

c)

The H atoms are connected to more than 2 valence electrons. They form bonds to connect to 2 valence electrons only.

d)

The C atom at the center needs to have at least 1 lone pair of electrons.

8.
Covalent bonds are formed through the ____ of valence electrons
a)
Transfer
b)
Sharing
c)
Donation
d)
Removal
9.
Which of the following diatomic molecules will form a double bond?
a)
H2
b)
O2
c)
N2
d)
F2
10.

Which of the following diatomic molecules will form a triple bond?

a)
H2
b)
O2
c)
N2
d)
F2
11.
What is the name of the covalent molecule C4H10?
a)
Tetracarbon Decahydroxide
b)
Tetracarbon Decahydride
c)
Carbon Hydroxide
d)
Tetracarbon Decahydrogen
12.
What is the formula of Tricarbon Octafluoride?
a)
C3F8
b)
CF
c)
F3C8
d)
3C8F
13.
What is the formula of Silicon Tetrachloride?
a)
SiCl
b)
SiCl3
c)
SiCl4
d)
1Si4Cl
14.
Choose the correct shape for this molecule:
a)
Trigonal planar
b)
Trigonal pyramidal
c)
Bent
d)
Tetrahedral
15.
Choose the correct shape for this molecule:
a)
linear
b)
Trigonal pyramidal
c)
Bent
d)
Tetrahedral
16.
Choose the correct shape for this molecule:
a)
linear
b)
Trigonal pyramidal
c)
Bent
d)
Trigonal planar
17.
Choose the correct shape for this molecule:
a)
Tetrahedral
b)
Trigonal pyramidal
c)
Bent
d)
Trigonal planar
18.
Choose the correct shape for this molecule:
a)
Bent
b)
Linear
c)
Tetrahedral
d)
Trigonal pyramidal
19.
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
20.

Polar covalent and nonpolar covalent compounds are almost always poor conductors of electricity.

a)

False

b)

True

21.

Molecular (covalent) compounds have high melting points

a)

True

b)

False

22.

Why do solid metals conduct electricity?

a)

Metals form strongly-bonded latices made from + and - ions.

b)

Metals have low electronegativity. The valence electrons are delocalised and able to flow.

c)

Metals have high electronegativity. The valence electrons are shared between two metal ions

23.

Iron and sulfur will form a ______ bond

a)

ionic

b)

covalent

c)

metalloid

24.

One atom transfers its valence electrons to a different atom, resulting in oppositely-charged ions that are attracted to each other. This type of bond is called:

a)

ionic

b)

metallic

c)

non polar covalent

d)

covalent

25.

Bonds formed by sharing valence electrons between atoms are:

a)

ionic

b)

metallic

c)

covalent

d)

best friend bonds

26.

A compound is made of two nonmetals. It is

a)

ionic

b)

metallic

c)

covalent

27.

A compound that is a poor conductor of electricity and has a low melting point is most likely

a)

ionic

b)

metallic

c)

covalent

28.

Which compound would be likely to have a very low melting point?

a)

potassium chloride (KCl)

b)

iron (II) oxide

(FeO)

c)

sulfur difluoride

(SF₂)

d)

Calcium

(Ca)

29.

Which solid pure substance would be a good conductor of electricity?

a)

sodium chloride (NaCl)

b)

copper (II) sulfate

(CuSO₄)

c)

glucose

(C₆H₁₂O₆)

d)

aluminum

(Al)

30.

Which compound would be a good conductor when dissolved in water?

a)

aluminum (Al)

b)

sulfur dioxide (SO₂)

c)

ammonia (NH₃)

d)

sodium bromide (NaBr)

31.

Why don't noble gases form bonds?

a)

Noble gases do form bonds

b)

They all have a full octet

c)

They only bond with each other

32.

Predict the type of bond between helium and fluorine.

a)

ionic

b)

covalent

c)

metallic

d)

no bond

33.

Identify the following compound as ionic, metallic or covalent: MgO

a)

ionic

b)

covalent

c)

metallic

34.

Identify the following compound as ionic or covalent: Na2SO4

a)

ionic

b)

covalent

35.
A substance which has a high melting point, conducts electricity when dissolved in water, and has a crystalline structure probably has what type of bond?
a)
Ionic
b)
Metallic
c)
Covalent
d)
Crystalline
36.
A solid substance is an excellent conductor of electricity. The chemical bonds in this substance are most likely?
a)
ionic, because the valence electrons are shared between atoms
b)
covalent, because the valence electrons are mobile
c)
metallic, because the valence electrons are stationary
d)
metallic, because the valence electrons are mobile
37.
N2O5?
a)
Nitrogen oxide
b)
Dinitrogen pentaoxide
c)
Pentaoxide dinitrogen
d)
Nitrogen pentaoxide
38.
CCl4?
a)
Carbon tetrachloride
b)
Monocarbon tetrachloride
c)
Carbon hexachloride
d)
Monocarbon hexachloride
39.
Bromine monoflouride
a)
Br1F1
b)
BrF
c)
Br2F
d)
BrF2
40.

Name the compound H₂S.

a)

hydrogen sulfide

b)

dihydrogen sulfide

c)

dihydrogen monosulfide

d)

dihydrogen monosulfate

41.
What is the correct name for NO?
a)
Mononitrogen Monoxide
b)
Nitrogen Monoxide
c)
Mononitrogen Dioxide
d)
Nitrogen Oxide
42.

Classify the following molecule.

a)

polar

b)

nonpolar

43.

Classify the following molecule as polar or nonpolar: HCl

a)

Polar

b)

Nonpolar

44.

Classify the following molecule as polar or nonpolar: F2

a)

Polar

b)

Nonpolar

45.

Is the following molecule polar or nonpolar?

a)

polar

b)

nonpolar

46.

Electronegativity is a measurement of the ability of a nucleus to:

a)

attract bonding electrons

b)

attract other nuclei

c)

attract electrons in the non-valence energy levels

47.

Which of the following formulas represents a polar molecule?

a)

H2

b)

NI3

c)

CO2

d)

CCl4

48.
Which formula represents a nonpolar molecule?
a)
HBr
b)
H2S
c)
CBr4
d)
PCl3
49.

Classify the following molecule as polar or nonpolar: NCl3

a)

polar

b)

nonpolar

50.

Is the following molecule polar or nonpolar?

a)

polar

b)

nonpolar

51.

Is the following molecule polar or nonpolar?

a)

polar

b)

nonpolar

52.

Is the following molecule polar or nonpolar?

a)

polar

b)

nonpolar

53.
What geometry will this molecular structure have?: H2S
a)
bent
b)
tetrahedral
c)
linear
d)
trigonal pyramidal
54.
What is the correct formula for this molecule?
a)
NH
b)
N3H
c)
NH3
d)
NH4
55.

The total number of electrons to be counted for the Lewis structure of the PO43- polyatomic ion is:

a)

8

b)

26

c)

29

d)

32

56.

What molecular geometry would the compound PCl3 have?

a)

Trigonal planar

b)

Trigonal pyramidal

c)

Tetrahedral

d)

Linear

57.

Is this molecule polar or non-polar?

a)

Polar

b)

Non-polar

58.

Is this molecule polar or non-polar?

a)

Non-polar

b)

Polar

59.

What molecular geometry will this compound have? BCl3

a)

Trigonal planar

b)

Tetrahedral

c)

trigonal pyramidal

d)

bent

60.

What geometry will this molecularcompound have?: CCl4

a)
bent
b)
tetrahedral
c)
linear
d)
trigonal pyramidal

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