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07 Ionic Bonding

Total questions: 50

Worksheet time: 46mins

Name
Class
Date
1.

How many valence electrons does Helium Have?

a)

1 Valence electron

b)

2 Valence electron

c)

3 Valence electron

d)

4 Valence electron

e)

5 Valence electron

2.

How many valence electrons does Nitrogen Have?

a)

1 Valence electron

b)

2 Valence electron

c)

3 Valence electron

d)

4 Valence electron

e)

5 Valence electron

3.

How many valence electrons does Magnesium Have?

a)

1 Valence electron

b)

2 Valence electron

c)

3 Valence electron

d)

4 Valence electron

e)

5 Valence electron

4.

How many valence electrons does Aluminum Have?

a)

1 Valence electron

b)

2 Valence electron

c)

3 Valence electron

d)

4 Valence electron

e)

5 Valence electron

5.

How many valence electrons does Silicon Have?

a)

1 Valence electron

b)

2 Valence electron

c)

3 Valence electron

d)

4 Valence electron

e)

5 Valence electron

6.

How many valence electrons does Lithium Have?

a)

1 Valence electron

b)

2 Valence electron

c)

3 Valence electron

d)

4 Valence electron

e)

5 Valence electron

7.

How many valence electrons does Neon Have?

a)

4 Valence electron

b)

5 Valence electron

c)

6 Valence electron

d)

7 Valence electron

e)

8 Valence electron

8.

The Lewis Dot structure for aluminum would have ______ electrons.

a)

13

b)

3

c)

8

d)

27

9.

Valence electrons are those that are

a)

closest to the nucleus.

b)

freely floating between atoms.

c)

in the outermost energy level of the atom.

d)

unable to become involved in chemical bonding.

10.

Which of the following is not a way that ions can form?

a)

gaining electrons

b)

gaining protons

c)

losing electrons

d)

All of the above are ways that ions can form.

11.

Oxygen has six valence electrons. When forming an ion, oxygen will

a)

lose six electrons and have a charge of +6.

b)

lose six electrons and have a charge of -6.

c)

gain two electrons and have a charge is +2.

d)

gain two electrons and have a charge of -2.

12.

Look at the periodic table. What should be the charge on the ion formed by calcium?

a)

+1

b)

+2

c)

-1

d)

-2

13.

Atoms that have gained electrons form

a)

cations.

b)

anions.

c)

negions.

d)

positrons.

14.

Most elements are most stable when their outermost energy levels contain ________ electrons.

a)

2

b)

6

c)

8

d)

18

15.

Look at the Periodic table. Which of the following elements would you expect to form an ion that has the same charge as the oxide ion?

a)

calcium

b)

boron

c)

sulfur

d)

chlorine

16.

Which of the following elements is an exception to the octet rule?

a)

helium

b)

oxygen

c)

chlorine

d)

magnesium

17.

Which of the following tend to gain electrons when forming ions?

a)

metalloids

b)

metals

c)

nonmetals

d)

cations

18.

Anions have

a)

gained electrons.

b)

lost electrons.

c)

gained protons.

d)

lost protons.

19.
Na +  and  S -2
a)
Na2S
b)
NaS2
c)
Na2S2
d)
NaS
20.
K +  and  N-3
a)
KN
b)
KN3
c)
K3N3
d)
K3N
21.
The chemical formula for an ionic compound of potassium and oxygen is
a)
KO.
b)
K2O.
c)
K2O2.
d)
KO2.
22.
How do the following two elements bond together?
Al3+  O2-         
a)
AlO
b)
Al2O3
c)
Al3O6
d)
Al3O2
23.
What would be the proper chemical formula for combining Al3+ and l- :
a)
Al l3
b)
Al3l
c)
Al l
d)
Al3 l3
24.
What formula results when Ca+2  and  Br- ions bond?
a)
Ca2Br2
b)
CaBr
c)
Ca(br)2
d)
CaBr2
25.
NH4 +  and  OH -
a)
NH(OH)4
b)
NH4OH
c)
OHNH4
d)
correct answer not given
26.
Cu +2  and  OH -
a)
CuOH2
b)
Cu2OH
c)
Cu(OH)2
d)
correct answer is not given
27.
Fe +2  and  SO4 -2
a)
FeSO4
b)
Fe4(SO4)2
c)
FeSO2
d)
correct answer is not given
28.
Cr +3  and  CO3 -2
a)
Cr3(CO3)2
b)
CrCO3
c)
Cr2CO33
d)
correct answer is not given
29.
NH4 +1  and  C2O4 -2
a)
NH4C2O4
b)
(NH4)2C2O4
c)
NH4(C2O4)2
d)
correct answer is not given
30.
Fe +2  and  SO4 -2
a)
Fe2(SO4)2
b)
FeSO4
c)
SO4Fe
d)
correct answer is not given
31.
NH4 +  and  NO2 -
a)
NH4NO2
b)
NHNO2
c)
NO2NH4
d)
correct answer is not given
32.
Ga +3  and  PO4 -3
a)
GaPO4
b)
Ga4PO
c)
PO4Ga
d)
correct answer is not given
33.
Name the following ionic compound: BeCl2
a)
beryllium chlorine
b)
beryllium II chloride
c)
beryllium chloride
d)
beryllium dichloride
34.

Name the following ionic compound: MgSO4

a)

magnesium (II) sulfide

b)

magnesium sulfide

c)

magnesium sulfate

d)

magnesium (II) sulfate

35.

Name the following ionic compound: LiNO3

a)

lithium nitrate

b)

lithium III nitrate

c)

lithium nitride

d)

lithium nitrogen oxide

36.

Name the following compound: FeCl3

a)

iron chloride

b)

iron III chloride

c)

iron II chloride

d)

iron III chlorate

37.
When naming ionic compounds with transition metals you need to include roman numerals to show the _____ of the metal..
a)
atomic number
b)
mass number
c)
charge
d)
ionization energy
38.

The formula for Magnesium phosphide is:

a)

Mg3(PO4)2

b)

MgP

c)

MgPO4

d)

Mg3P2

39.

What is the name of Ca(NO3)2

a)

calcium nitrite

b)

calcium II nitrate

c)

calcium nitrate

d)

calcium nitride

40.

Name the following ionic compound: Cr(NO3)3

a)

chromium III nitride

b)

chromium II nitride

c)

chromium II nitrate

d)

chromium III nitrate

41.

What is the correct chemical name for Cu2O ?

a)

Copper oxide

b)

Copper oxalate

c)

Copper (II) oxide

d)

Copper (I) oxide

42.
Which of the following is a property of an ionic compound?
a)
high melting point
b)
soft
c)
malleable
d)
liquid at room temperature
43.

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.

44.

Ionic compounds form giant ionic lattices. What forces hold the giant ionic lattices together?

a)

strong frictional forces between the surfaces of the atoms

b)

strong magnetic forces of attraction between the poles of ions

c)

strong electrostatic forces of attraction between oppositely charged ions

45.

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.

46.

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

a)

true

b)

false

47.

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

48.

What is a crystal?

a)

A pure material that can’t be changed.

b)

Material with a regular,repeating arrangement of atoms.

c)

A foggy like material.

49.
Breakage along smooth, flat planes
a)
fracture
b)
cleavage
c)
streak
d)
ore
50.

Which crystal structure does the picture show?

a)

BBC (British Broadcasting Company)

b)

BCC (Body Center Cubic)

c)

SC (Simple Cubic)

d)

FCC (Face-Centered Cubic)

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