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Bonding Review

Total questions: 40

Worksheet time: 39mins

Name
Class
Date
1.
Are the atoms more stable when they are bonded together or when they are apart? 
a)
Bonded Together
b)
Apart
2.
Ionic Bonding involves...
a)
The transfer of protons
b)
The transfer of nuetrons 
c)
The transfer of electrons
d)
None Of the above
3.
What do atoms that form positive ions tend to do?
a)
Tend to lose electrons 
b)
Tend to lose protons
c)
Tend to gain electrons
d)
Tend to gain protons
4.
What usually forms the positive ion?
a)
Metal
b)
Non Metals
c)
None
5.

What happens when the sodium atom loses an electron?

a)

It becomes negatively charged

b)

It becomes positively charged

c)

none

6.
What usually forms the negative ion?
a)
nonmetals
b)
metal
c)
none
7.
Covalent compounds
a)
Share electrons
b)
transfer electrons
c)
contain a sea of electrons
d)
conduct electricity
8.
What two types of atoms make a covalent bond?
a)
2 Nonmetals
b)
1 Nonmetal and 1 Metal
c)
2 Metals
d)
2 Noble Gases
9.
What happens when an atom loses an electron?
a)
Neutral (no charge)
b)
Positive charge
c)
Negative charge
10.
What happens when an atom gain an electron?
a)
Neutral(no charge)
b)
Positive charge
c)
Negative charge
11.
What charges attract?
a)
Opposite
b)
Same
12.
What charges repel?
a)
Same
b)
Opposite
13.
What elements generally make an ionic bond?
a)
metal and nonmetal
b)
2 or more nonmetals
c)
metal
d)
none of the above
14.
What elements generally make a covalent bond?
a)
metal and nonmetal
b)
2 or more nonmetals
c)
metal
d)
none of the above
15.
Predict the bond that will form between Be and F.
a)
Ionic
b)
Covalent
16.
Predict the bond that will form between Se and Cl.
a)
Ionic
b)
Covalent
17.
Predict the bond that will form between Sr and S.
a)
Ionic
b)
Covalent
18.
What is a valence electron?
a)
an electron that is found in the outermost shell of an atom. 
b)
an electron found in the innermost shell of an atom.
c)
an electron found in the middle shell.
19.
What is the number of valence electrons for Oxygen?
a)
8
b)
6
c)
2
d)
1
20.
What is the number of valence electrons for Beryillum?
a)
1
b)
4
c)
2
d)
7
21.
What is the number of valence electrons for Silicon?
a)
1
b)
2
c)
6
d)
4
22.
What is the number of valence electrons for Neon?
a)
6
b)
7
c)
8
d)
9
23.
How many valence electrons in this structure?
a)
6
b)
5
c)
4
d)
7
24.
Is Hydrogen considered a metal or a non-metal?
a)
Metal
b)
Non-metal
25.

What type of bond is formed between two nitrogen atoms? Nitrogen's EN = 3.0

a)

ionic

b)

polar covalent

c)

nonpolar covalent

26.

What type of bond is formed between carbon and nitrogen? carbon's EN = 2.5, nitrogen's EN = 3.0

a)

ionic

b)

polar covalent

c)

nonpolar covalent

27.

What type of bond is formed between potassium and fluorine? potassium's EN = 0.8, fluorine's EN = 4.0

a)

ionic

b)

polar covalent

c)

nonpolar covalent

28.

What type of bond is formed between zinc and oxygen? zinc's EN = 1.6, oxygen's EN = 3.5

a)

ionic

b)

polar covalent

c)

nonpolar covalent

29.

What type of bond is formed between silicon and carbon? silicon's EN = 1.8, carbon's EN = 2.5

a)

ionic

b)

polar covalent

c)

nonpolar covalent

30.
What type of bond is illustrated above?
a)
Metallic
b)
Ionic
c)
Covalent
d)
Wiggly
31.
Which statement best describes the energy change as bonds are formed and broken in this reaction?
      H2 + Cl2  ➔  2HCl
a)
The forming of the H-Cl bond releases energy
b)
The forming of the H-Cl bond absorbs energy
c)
The breaking of the H-H bond releases energy
d)
The breaking of the Cl-Cl bond releases energy
32.
What explains the very high melting and boiling point of water
a)
Strong dipole-dipole bonds between water molecules
b)
Strong hydrogen bonds between water molecules
c)
Dispersion forces which are present in all molecules
d)
Asymmetrical shape of the polar bonds.
33.
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
34.
Does HCl have hydrogen bonding?
a)
yes
b)
no
35.
Intermolecular force present in HCl?
a)
dipole dipole
b)
dispersion
c)
H-bond
d)
ionic
36.
Type of intermolecular force present in I2, Br2, and Cl2.
a)
dipole dipole
b)
H-bond
c)
dispersion
d)
metallic
37.
Which of the following has the highest boiling point?
a)
H2
b)
NH3
c)
N2
d)
O2
38.
What explains the very high melting and boiling point of water
a)
Strong dipole-dipole bonds between water molecules
b)
Strong hydrogen bonds between water molecules
c)
Dispersion forces which are present in all molecules
d)
Asymmetrical shape of the polar bonds.
39.
Type of intermolecular force present in HF.
a)
dipole dipole
b)
dispersion
c)
H-bond
d)
ionic
40.

Use your electronegativity chart to determine if the type of bond the following elements would form.

C- H

a)

Ionic

b)

non-polar covalent

c)

polar covalent

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