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Bonding Review

Total questions: 60

Worksheet time: 1hrs 4mins

Name
Class
Date
1.
Why do atoms share electrons?
a)
To attain the electron configuration of a noble gas.
b)
To become ions and take a charge
c)
to increase the mass
d)
it's a nice thing to do.
2.
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
3.

How many electrons are shared in a single covalent bond?

a)

2 pairs

b)

4

c)

2

d)

1

4.
How do covalent bonds form?
a)
Donating & receiving valence e- between atoms.
b)
Opposite slight charges attract each other between compounds.
c)
Scientists are still not sure how they form.
d)
Sharing valence e- between atoms.
5.

Which of the following is a covalent bonding?

a)

MgS

b)

NaCl

c)

CH4

d)

LiBr

6.
What is a double bond?
a)
a bond between two atoms
b)
one pair of electrons shared between two atoms
c)
two pairs of electrons shared between two atoms
d)
James Bond's brother
7.
What is the charge on a chloride ion?
a)
-1
b)
1
c)
+2
d)
+1
8.
How many valence electrons does calcium have?
a)
2
b)
4
c)
6
d)
7
9.
A(n) _________ is an ion with a positive (+) charge.
a)
anion
b)
cation
c)
ion
d)
solute
10.
When an atom loses an electron, it becomes a:
a)
positive ion
b)
negative ion
c)
neutral ion
d)
neutral atom
11.
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
12.
Which of the following is a characteristic property of ionic compounds?
a)
They form hard, brittle crystals with characteristic shapes
b)
They have low melting points
c)
They have low boiling points
d)
They contain no charged particles
13.
A charged particle that has gained at least one electron is called a(n) _____.
a)
Anion
b)
Cation
c)
Anonion
d)
chemistry cat
14.

this type of structure is a solid at room temp

a)

covalent

b)

ionic

c)

both

d)

neither

15.

this type of bond creates a crystalline structure

a)

ionic

b)

covalent

c)

both

16.

this type of bond shares electrons unequally

a)

polar

b)

nonpolar

c)

ionic

d)

all

17.

How do 2 metals bond?

a)

sharing electrons

b)

giving electrons

c)

sea of electrons

d)

all of the above

18.

What is an alloy?

a)

metal + nonmetal bonded together homogenously

b)

2 nonmetals bonded together heterogenously

c)

combination of metals bonded together homogenously

d)

combination of metals bonded together heterogenously

19.
What are ionic bonds?
a)
valence electrons transferred between atoms
b)
Inner most electrons transferred between atoms
20.
When the number of electrons equals the number of protons the atom has what charge?
a)
sponge bob
b)
positive charge
c)
negative charge
d)
neutral charge
21.
An atom that has gained or lost electrons is called ...
a)
a winner
b)
an isotope
c)
an ion
d)
a loser
22.
which types of elements become cations?
a)
nonmetals
b)
all metals
c)
only transition metals
d)
some metals and some metalloids
23.

Most elements are trying to get how many electrons in their outer shell?

a)

2

b)

8

c)

16

d)

32

24.
The following statements are true for ionic bonding EXCEPT
a)
bonding between metal and non metal
b)
electrostatic forces between opposite charges
c)
transferring of electrons
d)
sharing of electrons
25.

How many valence electrons does lithium have?

a)

1

b)

3

c)

6.9

d)

7

26.
Where are metals located on the periodic table?
a)
Blue
b)
Green
c)
Red
27.
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
28.
Which formula represents an covalent compound?
a)
CO2
b)
Ag
c)
FeCl3
d)
Cs3P
29.

What is a polyatomic ion?

a)

A covalent molecule with a charge.

b)

An ionic molecule with a charge.

c)

A molecule made of multiple atoms with no charge.

d)

A neutral Lewis Structure.

30.

Which of the following represents the strongest polar covalent bond?

a)

H-N

b)

H-S

c)

H-O

d)

H-Br

31.
Fe(CO3)2
a)
Iron (IV) Carbonate
b)
Iron (II) Carbonate
c)
Iron Carbonate
d)
Iron (III) Carbonate
32.
Which of these combinations is an ionic compound made of?
a)
Metal and Metal
b)
Nonmetal and Nonmetal
c)
Metal and Nonmetal
d)
Cation and Cation
33.
What is the formula for copper(I) sulfate?
a)
Cu(SO3)
b)
Cu(SO4)
c)
Cu2(SO3)
d)
Cu2(SO4)
34.
Bromine monoflouride
a)
BaF
b)
BrF
c)
Br2F
d)
BrF2
35.
Name this compound: 
KF
a)
Potassium fluoride
b)
Potassium fluorite
c)
Fluorine potasside 
d)
Potassium fluorate
36.
What is the formula for sodium nitrate?
a)
Na3(NO)
b)
Na(NO)
c)
Na3(NO3)
d)
Na(NO3)
37.
What is the formula for magnesium chloride?
a)
MgCl
b)
Mg2Cl
c)
MgCl2
d)
Mg(ClO3)2
38.
All compounds made up of two elements must end with...
a)
-ide
b)
-ate
c)
-ite
39.
N2O5
a)
Dinitrogen pentoxide
b)
Nitrogen Oxide
c)
Nitric oxide
40.
Name this formula: 
KNO3
a)
Potassium Nitrogen Oxide
b)
Potassium Nitride
c)
Potassium Nitrate
d)
Potassium (I) Nitrite
41.
K +  and  N-3
a)
KN
b)
KN3
c)
K3N3
d)
K3N
42.
What does the prefix Mono mean?
a)
4
b)
6
c)
3
d)
1
43.
Naming a compound of two non-metals requires us to use..
a)
Prefixes
b)
Roman Numerals
c)
Nothing, just name it
44.
Phosphorous trichloride
a)
PCl3
b)
P3Cl
c)
P3Cl3
d)
PCL
45.

Nitrogen contains _____ valence electrons.

a)

7

b)

6

c)

5

d)

4

46.

Put these in increasing order of electronegativity: F, N, B

a)
B < N < F
b)
B < F < N
c)
N < F < B
d)
F < N < B
47.
Electronegativity is...
a)
how good an atom is at attracting electrons
b)
the ability of an atom to lose electrons
c)
the energy required to remove an electron from a specific atom
d)
how easy it is to make friends. 
48.

Why does electronegativity decrease as you go down a group?

a)

As you go down a group, the outer electrons are further away from the nucleus

b)

As you go down a group, the nucleus is less able to attract electrons in a bond

c)

Both of these

d)

None of these

49.

What does electronegativity do as you go across a period?

a)

decrease

b)

no pattern

c)

stay the same

d)

increase

50.

Electronegativity _________ as you go down a group.

a)

Increases

b)

Decreases

c)

Stays the same

51.

The name of FeCl₂ is

a)

iron chloride

b)

iron (II) chloride

c)

iron (I) chloride

d)

iron dichloride

52.

LiBr is called

a)

lithium bromine

b)

lithium (I) bromine

c)

lithium bromide

d)

lithuim (I) bromide

53.

Name the following ionic compound: Cs2S

a)

cesium sulfide

b)

cesium sulfate

c)

cesium II sulfate

d)

cesium II sulfide

54.

What is the name of the compound Na2(SO4)?

a)

Sodium sulfate

b)

Sodium sulfide

c)

Sodium sulfite

d)

Sodium sulfuroxide

55.

When naming a compound, which of these is written first?

a)

Metal

b)

Nonmetal

c)

Anion

d)

Cation

56.

What is the name of the following compound: CuBr2

a)

copper bromine

b)

copper bromide

c)

copper (I) bromide

d)

copper (II) bromide

57.

Which is the correct formula for the compound: Calcium Oxide

a)

CaO

b)

CaO2

c)

Ca2O

58.
Which of these compounds is ionic? 
a)
Carbon dioxide
b)
Dinitrogen Trioxide
c)
Silicon tetrachloride
d)
Lithium bromide
59.
The chemical formula for an ionic compound of potassium and oxygen is
a)
KO.
b)
K2O.
c)
K2O2.
d)
KO2.
60.

What is the ionic charge of Sulfur (S)?

a)

+2

b)

-2

c)

+1

d)

-1

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