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Chemical Bonding-HNRS

Total questions: 81

Worksheet time: 1hrs 18mins

Name
Class
Date
1.
Elements on the LEFT side of the periodic table will most likely form:
a)
Positive ions
b)
Negative ions
c)
Neutral Ions
d)
None of these
2.
An ionic bond forms when atoms ___________ electrons.
a)
gain
b)
share
c)
increase
d)
transfer
3.
Which type of bond has an equal sharing of electrons?
a)
Polar Covalent 
b)
Non Polar Covalent
c)
Ionic
d)
Metallic
4.
Which type of bond has an unequal sharing of electrons?
a)
Polar Covalent 
b)
Non Polar Covalent
c)
Ionic
d)
Metallic
5.
Chemical bonds form when atoms
a)
combined nuclei
b)
give up neutrons
c)
gain protons
d)
share or transfer electrons
6.
If an atom loses two electrons what charge will it have?
a)
+ 2
b)
 - 2
c)
+1
d)
-1
7.
If an atom gains one electron what charge will it have?
a)
-2
b)
-1
c)
+1
8.
What is the number of valence electrons for Oxygen?
a)
8
b)
6
c)
2
d)
1
9.
How many valence electrons in this structure?
a)
6
b)
5
c)
4
d)
7
10.

The following properties are all characteristics of ionic compounds EXCEPT

a)

high melting and boiling points

b)

soft

c)

crystal lattice structure

d)

conduct electricity when dissolved in water

11.
Which of the following is a property of an ionic compound?
a)
high melting point
b)
soft
c)
malleable
d)
liquid at room temperature
12.

What properties does an ionic compound have?

a)

A low boiling point and it conducts electricity when dissolved in water

b)

A high melting and it conducts electricity when liquid

c)

A high boiling point and it conducts electricity when solid

13.

Ionic compounds conduct electricity when dissolved in water. Which statement below best explains the property?

a)

Ions are free to move.

b)

Electrons are free to move.

c)

Bonds are strong.

d)

There are weak intermolecular forces of attraction.

14.

Which three of the following are features of ionic compounds? (click 3 boxes)

a)

They have bonds between metals and non-metals.

b)

They have bonds between two non-metals.

c)

They form simple molecular structures.

d)

They form giant ionic lattices.

e)

They involve the transfer of electrons.

15.

Why do ionic compounds have high melting and boiling points?

a)

Their ions are free to move.

b)

Their ions are held in fixed positions.

c)

They have many strong bonds.

d)

They have many weak bonds.

16.

True or false? Ionic compounds have high melting points.

a)

true

b)

false

17.

True or false? Ionic compounds conduct electricity when they are in their solid state.

a)

true

b)

false

18.

Why do ionic compounds NOT conduct electricity when they are in their solid state?

a)

Their ions are free to move.

b)

Their ions are held in fixed positions.

c)

Their electrons are free to move

d)

Their electrons are held in a fixed state

19.

Why do ionic compounds conduct electricity when they are molten or dissolved?

a)

Their ions are free to move.

b)

Their ions are held in fixed positions.

c)

Their electrons are free to move

d)

Their electrons are held in a fixed state

20.

Compounds composed of a ______________ and _____________ like the compound CaCl2 , are ionic compounds.

a)

metal ... metal

b)

nonmetal ... nonmetal

c)

metal ... nonmetal

21.

Which of the following describes covalent bonds?

a)

Bonds form because of opposite charges

b)

electrons are shared to fill outer electron shells

c)

Electrons are transferred between atoms

d)

Covalent bonds are magical

22.

Some are solids, some are liquids, and some are gases at room temperature.

a)

ionic compounds

b)

molecular compounds

23.

usually hard but brittle

a)

ionic compounds

b)

molecular compounds

24.

When dissolved in water, the solution does NOT conduct electricity.

a)

ionic compounds

b)

molecular compounds

25.
Which of the following is a molecular compound?
a)
CaO
b)
NaCl
c)
CaCl2
d)
CH4
26.
Formed when a non-metal shares electrons with another non-metal.
a)
ionic compound
b)
molecular compound
27.
 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
28.
What is the VSEPR theory used to predict?
a)
Bond Strength
b)
Polarity
c)
Molecular Shape
d)
Electronegativity
29.

What 3-D VSEPR shape does this molecule exhibit?

a)

linear

b)

tetrahedral

c)

trigonal pyramidal

d)

trigonal planar

30.

Which Lewis Dot Model drawing correctly shows an O2 molecule?

a)
b)
c)
d)
31.
What is the VSEPR shape of H2S?
a)
linear
b)
trigonal planar
c)
bent
d)
tetrahedral
32.
How many electrons are shared in a double bond?
a)
1
b)
2
c)
4
d)
6
33.

Which type of molecular shape is shown by this molecule?

a)

trigonal pyramidal

b)

tetrahedral

c)

bent

d)

trigonal planar

34.
Low melting point and low solubility in water are general properties of ______________________ compounds
a)
ionic
b)
covalent
c)
chemical
d)
glucose
35.

Which of these Lewis structures is incorrect?

a)
b)
c)
d)
36.

Which is the correct molecular structure for carbon dioxide?

a)
b)
c)
d)
37.
What is the ELECTRONIC geometry of the following?
a)
Linear
b)
Trigonal planar
c)
Tetrahedral
d)
Trigonal Bipyramidal
38.
What is the MOLECULAR geometry of the central oxygen?
a)
Linear
b)
Trigonal Planar
c)
Bent
d)
Tetrahedral
39.
Which of the following molecular shapes would have a bond angle of 180 Degrees?
a)
Bent
b)
Trigonal Planar
c)
Tetrahedral
d)
Linear
40.
Which shapes are altered by unshared pairs of electrons? 
a)
Bent and Pyramidal
b)
Trigonal Planar and Bent
c)
Tetrahedram and Bipyramidal
d)
Pyramidal and Linear
41.
What molecular shape is the structure shown here? (NH4+)
a)
linear
b)
trigonal planar
c)
tetrahedral
d)
trigonal pyramidal
42.
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
43.

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

a)

Evenly

b)

Unevenly

c)

Electrons are not shared

d)

None of the Above

44.

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

a)

Evenly

b)

Unevenly

c)

Electrons are not shared

d)

None of the Above

45.

In a polar covalent bond, the electrons gather around...

a)

The atom with the Greatest Electronegativity

b)

The atom with the Lowest Electronegativity

c)

Each atom Equally

d)

None of the Above

46.

The polarity of a bond is determined by...

a)

The sum of the electronegativities of the two atoms

b)

The difference in the electronegativities of the two atoms

c)

The charges of the atoms

d)

None of the Above

47.

Partial charges are present in which type of bond?

a)

Ionic

b)

Nonpolar Covalent

c)

Polar Covalent

d)

Both Polar Covalent and Ionic

48.

Molecules that contain whole number charges on atoms (+1,-3, etc.) must be...

a)

Polar Covalent

b)

Nonpolar Covalent

c)

Ionic

d)

Polar Covalent or Ionic

49.

A diatomic molecule like O2 is always _____ because electrons are shared _____

a)

nonpolar; unequally

b)

polar; equally

c)

nonpolar; equally

d)

polar; unequally

50.

Order the types of bonds based on the charge of their molecules. (lowest amount of charge to greatest)

a)

Polar Covalent --> Ionic --> Nonpolar Covalent

b)

Ionic --> Nonpolar Covalent --> Polar Covalent

c)

Ionic --> Polar Covalent --> Nonpolar Covalent

d)

Nonpolar Covalent --> Polar Covalent --> Ionic

51.

Is this molecule polar or non-polar?

a)

Polar

b)

Non-polar

52.

Is this molecule polar or non-polar?

a)

Non-polar

b)

Polar

53.

Is this molecule polar or non-polar?

a)

Non-polar

b)

Polar

54.

Is this molecule polar or non-polar?

a)

Polar

b)

Non-polar

55.
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
56.
This is an example of a __________ bond.
a)
non-polar covalent
b)
polar covalent
c)
ionic
d)
metallic
57.
Which formula represents a polar molecule?
a)
H2
b)
H2O
c)
CO2
d)
CCl4
58.
Will this molecule be polar or nonpolar? CCl4
a)
polar
b)
nonpolar
59.
Will this molecule be polar or nonpolar? H2S
a)
polar
b)
nonpolar
60.
According to the octet rule most elements need _______ valence electrons.
a)
2
b)
8
c)
6
d)
18
61.
Hydrogen needs _____ electrons in its valence shell to be stable.
a)
4
b)
6
c)
8
d)
2
62.
A Lewis structure can be used for showing an ionic bond but instead for dashes for the bonds positive and negative _____ are represented.
a)
atoms
b)
ions
c)
molecules
d)
electrons
63.
Each line in a Lewis Structure represents __________ electron(s).
a)
3
b)
2
c)
1
d)
4
64.
The theory that is used to predict the arrangement of atoms about a central atom is called?
a)
Valence shell repulsion
b)
Valence shell electron sharing
c)
Valence shell electron pair repulsion
d)
Valence electron shell repulsion pair
65.
 Lone electron pairs in a molecule...
a)
Never exist
b)
Are lost in space
c)
Creates an isotope
d)
Push the bonded atoms closer
66.

Is this the correct structure for CH2O?

a)

Yes

b)

No

67.
Which of the following is the correct Lewis structure for the compound PBr3?
a)
structure A
b)
structure B
c)
structure C
d)
structure D
68.

By replacing the element symbol, this could be a diagram of which element?

a)

Li

b)

Al

c)

C

d)

Be

69.

NH3 has how many lone pairs?

a)

0

b)

1

c)

2

d)

3

70.

CCl4 has how many double bonds?

a)

0

b)

1

c)

2

d)

3

71.

In HCN (Carbon is usually the central atom) what kind of bond is between the C and N

a)

Single

b)

Double

c)

Triple

72.
Hydrogen bonding occurs when hydrogen is bonded to N, O, or F.  Which of the following has hydrogen bonding?
a)
CBr4
b)
NO2
c)
H2S
d)
NH3
73.
Does H2O have hydrogen bonding?
a)
yes
b)
no
74.
Does HCl have hydrogen bonding?
a)
yes
b)
no
75.
Does CH4 have hydrogen bonding?
a)
yes
b)
no
76.
Does NH3 have hydrogen bonding?
a)
yes
b)
no
77.
Which is the second strongest intermolecular force, after hydrogen bonding?
a)
dipole-dipole attraction
b)
London forces
78.
All molecules have London forces between them, but dipole-dipole and hydrogen bonding are so much stronger that when they are present we can ignore London forces.  Which of these has ONLY London forces?
a)
I2
b)
NH3
c)
OCl2
d)
SH2
79.

________________________ have the strongest intermolecular forces of attraction.

a)

Dipole- Dipole

b)

Dispersion

c)

Hydrogen Bonds

80.
Which of the following statements correctly compares the behavior of a mixture of ethanol and water at STP?
a)
Water will evaporate first, because it has weaker intermolecular forces
b)
Ethanol will evaporate first, because it has weaker intermolecular forces
c)
Ethanol and water will evaporate simultaneously
d)
The aqueous solution will evaporate partially at a temperature between the boiling points of water and of ethanol
81.
Hydrogen bonds are a form of bonding.
a)
True 
b)
False

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