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PRACTICE Bonding / Nomenclature Test

Total questions: 51

Worksheet time: 43mins

Name
Class
Date
1.

What is a valence electron?

a)

The sum of neutrons and protons.

b)

electrons in the outer shell

c)

A type of bond.

d)

A popular compound.

2.

Ionic bonds are between...

a)

Metal and Non-metal

b)

Non-metal and Non-metal

c)

Metal and Metal

d)

not possible

3.

How are ionic bonds formed?

a)

Metals transfer of electrons

b)

Sharing of electrons

c)

never heard of them

4.

Why do elements bond together?

a)

To be friends

b)

To create a new element

c)

To become stable

5.
Atoms that gain electrons become...
a)
negatively charged
b)
positively charged
c)
remain neutrally charged
d)
21
6.

Why do all bonds form?

a)

so the number of protons equals the number of electrons

b)

so an atom can become unstable

c)

to fill the outermost energy level

d)

so they feel better

7.

How many Aluminum atoms are in Al2O3?

a)

3

b)

5

c)

2

d)

1

8.
What are ionic bonds?
a)

Metals transfer electrons to the nonmetal

b)

Nonmetals share electrons

c)

metallic elements share all of the electrons

9.

Write the correct formula for Sodium Chloride.

a)

SC

b)

SCl

c)

NaCl

d)

NaCl2

10.
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.
11.
Covalent bonds are between...
a)
Metal and Non-metal
b)
Non-metal and Non-metal
c)
Metal and Metal
12.
What molecule could this be? 
a)
BF3
b)
CH4
c)
H2O
d)
CO2
13.
What molecule could this be? 
a)
H2O
b)
CCl4
c)
PCl5
d)
NaCl
14.

what is the name of CCl4?

a)

carbon tetrachloride

b)

monocarbon tetrachloride

c)

tetracarbon monochloride

d)

carbon chloride

15.

What is the name of the compound P2O5

a)

Pentaphosphorus dioxide

b)

Phoshphide dioxide

c)

Diphosphorus pentoxide

16.
Select the correct formula for sulfur hexachloride
a)
S2Cl6
b)
S6Cl
c)
SCl6
d)
SF6
17.
C3O8
a)
Tricarbon Octoxide
b)
Carbon Octoxide
c)
Carbon Oxide
d)
Carbon (VIII) Oxide
18.

H2O

a)

Dihydrogen Monoxide

b)

Hydrogen Oxide

c)

Hydrogen Monoxide

d)

Pure Water

19.
Name the following compound: SnO2
a)
tin(II) oxide
b)
tin(IV)oxide
c)
tin(II)oxygen 
d)
tin oxide
20.

Zn3P2

a)

Zinc Phosphide

b)

Zinc (III) Phosphide

c)

Trizinc Diphosphide

d)

Zinc Phosphate

21.
What is the formula for Potassium Fluoride? 
a)
KF
b)
K2F
c)
KF2
d)
none of the above
22.
What is the charge on the calcium ion?
a)
1+
b)
2+
c)
2-
d)
1-
23.
Name Al2S3
a)
Aluminum sulfide
b)
Dialuminum trisulfide
c)
ammonium sulfide
d)
aluminum (II) sulfice
24.

What is the formula for lead (II) carbonate?

a)

PbCO3

b)

Pb2CO3

c)

Pb(CO3)2

d)

Pb(CO)4

25.
What is the metallic ion in the compound CuCl?
a)
Cu1+
b)
Cu2+
c)
Cu1-
d)
Cu2-
26.

What is the formula for aluminum sulfite?

a)

Al3S2

b)

AlSO4

c)

Al3(SO4)2

d)

Al2(SO3)3

27.

What is the formula for tin (II) chromate

a)

Sn2(CrO4)4

b)

Sn(CrO4)2

c)

Sn4(CrO4)2

d)

SnCrO4

28.
What is the formula for barium hydride?
a)
BaOH2
b)
Ba(OH)2
c)
BaH2
d)
BaOH
29.
Name the compound HCl
a)
hydrogen chlorite
b)
hypochlorous acid
c)
hydrogen chlorate
d)
hydrochloric acid
30.
What element do all acids contain?
a)
H
b)
O
c)
C
d)
He
31.
carbonic acid
a)
H2CO3
b)
H2CrO4
c)
H2C2O4
d)
HCO3
32.
chlorous acid
a)
HClO3
b)
HClO2
c)
HClO
d)
HCl
33.
H2SO3
a)
sulfuric acid
b)
hydrosulfuric acid
c)
sulfurous acid
d)
persulfuric acid
34.
What is the formula for phosphorous acid?
a)
H3PO4
b)
H2PO4
c)
H3P
d)
H3PO3
35.
What is the formula for perchloric acid?
a)
H3ClO3
b)
H3ClO4
c)
HClO3
d)
HClO4
36.

Name the following ionic compound: CaSO4*6H2O

a)

calcium sulfate hexahydrate

b)

calcium tetrasulfate hexahydrate

c)

calcium sulfate heptahydrate

d)

carbon sulfuroxide hexahydrate

37.

Na2CO3 · 10H2O is known as

a)

sodium carbonate hydroxide

b)

sodium carbonate hydrate

c)

sodium carbonate decahydrate

d)

None of the above

38.

The proper name for this compound, CuSO4 * 5H2O is ....

a)

copper sulfate pentahydrate

b)

copper sulfur tetroxide penthydrate

c)

copper I sulfate pentahydrate

d)

copper II sulfate pentahydrate

39.

What is the correct chemical formula for barium hydroxide octahydrate?

a)

Ba(OH)2 . 8H2O

b)

Ba(OH)2 . H2O

c)

8Ba(OH)2 . H2O

d)

Ba . 8(OH)2

40.

Which of the following is NOT formed by a covalent bond?

a)

K2O

b)

H2O

c)

I2

d)

CO2

41.
What is the electrical charge of a cation?
a)
positive charge
b)
no charge
c)
negative charge
d)
none of these
42.
What is the electrical charge of a anion?
a)
positive charge
b)
no charge
c)
negative charge
d)
none of these
43.
Question Image

Match the following to form true statements:

a)

When solid, ionic compounds

1.

cannot conduct electricity

b)

When melted ionic compounds

2.

can conduct electricity

c)

Ionic compounds have

3.

high melting and high boiling points

d)

There are many strong bonds

4.

between ions in an ionic compound.

e)

Elements in group 1 of the periodic table form ions

5.

with a charge of 1+

44.

In an ionic bond, electrons are ​ (a)   from the ​ (b)   to the ​ (c)   . Ionic bonds are ​ (d)   because of the big difference in electronegativity.

Choose from the below words
transferred
metal
nonmetal
strong
weak
semimetal
shared
45.

If an atom gains an electron, it becomes a(n) ​ (a)   which is ​ (b)   charged. If an atom loses an electron, it becomes a(n) ​ (c)   which is ​ (d)   charged.

Choose from the below words
anion
negatively
cation
positively
neutrally
46.

What property is describing an ionic compound?

a)

shares electrons

b)

high melting point

c)

weak bonds

d)

made up of nonmetals.

47.

If a substance has a low melting point, it most likely has what type of bond?

a)

ionic

b)

covalent

c)

metallic

48.
When dissolved in water, the solution is a good conductor of electricity.
a)
ionic compounds
b)
covalent compounds
49.

Generally low melting and boiling points

a)

Ionic compounds

b)

Covalent compounds

50.

Generally high melting & boiling points

a)

Ionic compounds

b)

Covalent compounds

51.

Poor electrical conductivity

a)

Ionic compounds

b)

Covalent compounds

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