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Chemical Bonding

Total questions: 57

Worksheet time: 34mins

Name
Class
Date
1.

Nonmetals tend to

a)

gain electrons

b)

lose electrons

2.

Metals tend to

a)

gain electrons

b)

lose electrons

3.
If my charge becomes 2+ what does that say about me?
a)
I am stealing 2 electrons
b)
I am losing 2 electrons
c)
I am in period 2
d)
I have an atomic # of 2
4.
If I gain electrons I become
a)
Positive because I've added to my atom
b)
negative because I've added electrons
c)
same because i'm balanced
d)
equal because now I have electrons
5.
When metals bond with non-metals they form what type of bonds
a)
covalent
b)
ionic
c)
cooperative
d)
lewis
6.
How do the following two elements bond together?
Na1+  F1-         
a)
NaF
b)
NaF3
c)
Na3F
d)
Na1F2
7.
How do the following two elements bond together?
K1+  S2- 
a)
KS
b)
K8S
c)
K6S3
d)
K2S
8.

When a nonmetal gains electrons, it becomes this type of ion.

a)

Anion

b)

Cation

9.

When a metal loses electrons, it becomes this type of ion.

a)

anion

b)

cation

10.

Is this compound ionic or covalent?

a)

Ionic

b)

Covalent

11.

Is this compound ionic or covalent?

a)

ionic

b)

covalent

12.
How are ionic bonds formed?
a)
Transfer of electrons
b)
Sharing of electrons
13.
Nitrogen will form which of the following ions?
a)
N
b)
N-3
c)
N-5
d)
N+5
14.
Magnesium bromide is an ionic compound with the chemical formula MgBr₂.  What does the "2" tell you?
a)
There are 2 bromide ions for every magnesium ion
b)
Bromide has a 2- charge
c)
Bromide has a 2+ charge
d)
There are 2 magnesium ions to every bromide ion
15.
Which of the following is a property of an ionic compound?
a)
high melting point
b)
soft
c)
malleable
d)
liquid at room temperature
16.

What type of forces hold on an ionic lattice together?

a)

Electrostatic attraction forces

b)

Covalent bond

c)

Metallic bond

d)

Van der Waals forces

17.

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.

18.

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

a)

true

b)

false

19.

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

20.

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.

21.

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.

22.

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

23.
What part of an atom is involved in chemical bonding?
a)
protons
b)
neutrons
c)
electrons
d)
nucleus
24.
A ________ is a model of an atom in which each dot represents a valence electron.
a)
Valence electron
b)
Electron dot diagram/Lewis dot structure
c)
Lewis bond structure
25.
How many valence electrons does nitrogen have?
a)
3
b)

2

c)
5
d)
1
26.
Where are the non-metals located on the periodic table?
a)
All over
b)
On the left side of the "staircase"
c)
On the right side of the "staircase"
27.
Compounds made from only nonmetals are _________________ compounds.
a)
ionic
b)
covalent
c)
metallic
d)
chemical
28.
A covalent bond involves a __________ of electrons.
a)
sharing
b)
borrowing
c)
exchanging
d)
switching
29.
The chemical formula shows one carbon atom bonded to __________ oxygen atoms.
a)
one
b)
two
c)
three
d)
four
30.
 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
31.
What is the VSEPR theory used to predict?
a)
Bond Strength
b)
Polarity
c)
Molecular Shape
d)
Electronegativity
32.

What 3-D VSEPR shape does this molecule exhibit?

a)

linear

b)

tetrahedral

c)

trigonal pyramidal

d)

trigonal planar

33.

Which Lewis Dot Model drawing correctly shows an O2 molecule?

a)
b)
c)
d)
34.
What is the VSEPR shape of H2S?
a)
linear
b)
trigonal planar
c)
bent
d)
tetrahedral
35.
How many electrons are shared in a double bond?
a)
1
b)
2
c)
4
d)
6
36.

Which type of molecular shape is shown by this molecule?

a)

trigonal pyramidal

b)

tetrahedral

c)

bent

d)

trigonal planar

37.
Low melting point and low solubility in water are general properties of ______________________ compounds
a)
ionic
b)
covalent
c)
chemical
d)
glucose
38.

Which of these Lewis structures is incorrect?

a)
b)
c)
d)
39.

Which is the correct molecular structure for carbon dioxide?

a)
b)
c)
d)
40.
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
41.

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

a)

Evenly

b)

Unevenly

c)

Electrons are not shared

d)

None of the Above

42.

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

a)

Evenly

b)

Unevenly

c)

Electrons are not shared

d)

None of the Above

43.

The electrons in an ionic molecule are shared...

a)

Evenly

b)

Unevenly

c)

Electrons are not shared

d)

None of the Above

44.

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

45.

In a nonpolar 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.

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

a)

nonpolar; unequally

b)

polar; equally

c)

nonpolar; equally

d)

polar; unequally

48.

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

49.

When you have Br-Br, what is the polarity?

a)

Polar

b)

nonpolar

c)

Ionic

50.

When you have H-Cl, what is the polarity?

a)

nonpolar

b)

polar

c)

ionic

51.

When you have Li-O, what is the polarity?

a)

nonpolar

b)

polar

c)

ionic

52.

When you have Be-F, what is the polarity?

a)

nonpolar

b)

polar

c)

ionic

53.

When you have Si-O, what is the polarity?

a)

nonpolar

b)

polar

c)

ionic

54.

How would the melting point and boiling point for polar covalent bond?

a)

High

b)

Low

55.

How would the melting point and boiling point for nonpolar covalent bond?

a)

High

b)

Low

56.

What would solubility look like for polar covalent bond in water?

a)

soluable

b)

nonsoluable

57.

What would solubility look like for nonpolar covalent bond in water?

a)

soluable

b)

nonsoluable

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