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Bonding and Formulas Test

Total questions: 80

Worksheet time: 3hrs 48mins

Name
Class
Date
1.
ammonium phosphate
a)
(NH4)3PO4
b)
NPO4
c)
NH4PO4
d)
NH4(PO4)3
2.
zinc fluoride
a)
ZnF2
b)
ZnF
c)
Zn2F
d)
Zn2F4
3.
sliver phosphide
a)
Ag3P
b)
Ag3PO4
c)
Ag3PO3
d)
AgP
4.
aluminum sulfite
a)
Al2(SO3)3
b)
Al2(SO4)3
c)
AlSO3
d)
Al3(SO3)2
5.
Ca(CN)2
a)
Calcium Cyanide
b)
Calcium Dicyanide
c)
Calcium Dicarbon Dinitrogen
d)
Calcium Thiocyanate
6.
Sr(OH)2
a)
Strontium Hydroxide
b)
Strontium Hydride
c)
Strontium Dihydroxide
d)
Strontium Dioxygen Dihydride
7.
Na2S
a)
Sodium Sulfide
b)
Sodium Sulfate
c)
Sodium Sulfite
d)
Disodium Sulfide
8.
What is the formula for copper(I) sulfate?
a)
CuSO3
b)
CuSO4
c)
Cu2SO3
d)
Cu2SO4
9.
What is the formula for magnesium chloride?
a)
MgCl
b)
Mg2Cl
c)
MgCl2
d)
Mg(ClO3)2
10.
Name this compound: 
NaBr
a)
Bromide sodide
b)
Sodium bromide
c)
Sodium bromate
d)
Sodium bromite
11.
Write the formula for copper(I) phosphide
a)
Cu3P
b)
CuP
c)
Cu1P
d)
CuP3
12.
Name this compound: 
NH4F
a)
Ammonia fluoride
b)
Ammonium fluorite
c)
Ammonia fluorate
d)
Ammonium fluoride
13.
Name this compound:
NiPO4
a)
Nickel (I) phosphate
b)
Nickel (II) phosphate
c)
Nickel (IV) phosphate
d)
Nickel (III) phosphate
14.
Write the formula for vanadium (IV) carbonate
a)
V(CO3)2
b)
V4C
c)
V(CO3)4
d)
V4(CO3)
15.
Name the following ionic compound: BeCl2
a)
beryllium chlorine
b)
beryllium II chloride
c)
beryllium chloride
d)
beryllium dichloride
16.
What is the formula for manganese(III) oxide?
a)
MgO
b)
Mg2O3
c)
MnO
d)
Mn2O3
17.
From the following ionic compounds, choose the name-formula pair that is not correctly matched.
a)
sodium sulfide  Na2S
b)
ammonium nitrate 
NH4NO3
c)
sodium sulfate 
Na2SO3
d)
calcium oxide  CaO
18.

Name the following ionic compound: MgSO4

a)

magnesium sulfoxide

b)

magnesium sulfide

c)

magnesium sulfate

d)

magnesium oxide

19.
Name the following ionic compound: Cr(NO2)3
a)
chromium nitrite
b)
chromium nitride
c)
chromium III nitride
d)
chromium III nitrite
20.

Which of the following combinations would need roman numerals in the name?

a)

potassium + fluorine

b)

beryllium + oxygen

c)

boron + iodine

d)

nickel + oxygen

21.
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
22.
The name of the compound Ca3(PO4)2
a)
calcium phosphate
b)
tricalcium diphosphate
c)
calcium phosphorus oxide
d)
calcium phosphide
23.
The chemical formula of Iron (III)bromide is
a)
FeBr
b)
Fe(III)Br
c)
FeBr₃
d)
Fe₂Br₃
24.
When adding a subscript to a polyatomic ion, you should...
a)
multiply any subscripts on the polyatomic ion by the subscript you are adding
b)
put parentheses around the polyatomic ion before adding a subscript
c)
write the new subscript next to any subscripts on the polyatomic ion
d)
put the polyatomic ion in square brackets before adding the subscript
25.
The purpose of bonding for most elements is to achieve greater stability and to have a complete ______ of electrons in the outermost energy level.
a)
pair
b)
nucleus
c)
octet
d)
molecule
26.
How many valence electrons are in an atom of phosphorus (P)?
a)
5
b)
4
c)
3
d)
2
27.
How many valence electrons are in an ion of arsenide, As3-?
a)
5
b)
18
c)
8
d)
2
28.
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.
29.
Ionic compounds are formed when one or more valence electrons are transferred from _____
a)
a nonmetal atom to a metal atom
b)
a nonmetal atom to a nonmetal atom
c)
a metal atom to a nonmetal atom
d)
a metal atom to a metal atom
30.

Why don't noble gases form bonds?

a)

Noble gases do form bonds

b)

They all have a full octet

c)

They only bond with each other

31.

In ionic bonds, metals tend to

a)

share valence electrons

b)

gain valence electrons

c)

lose valence electrons

d)

keep their electrons

32.

Which of the following is TRUE about ionic compounds?

a)

They have low melting and boiling points.

b)

They can conduct electricity in the solid state.

c)

They are stronger than covalent bonds.

d)

They are usually formed from 2 metals.

33.

Which of the following is NOT TRUE about covalent compounds?

a)

They have low melting and boiling points.

b)

They are formed from 2 nonmetals.

c)

They can conduct electricity when dissolved in water (aqueous).

34.

Which element is most likely to form 4 bonds?

a)

Carbon

b)

Fluorine

c)

Sulfur

d)

Nitrogen

35.
Phosphorous trichloride
a)
PCl3
b)
P3Cl
c)
P3Cl3
d)
PCL
36.
Bromine monoflouride
a)
Br1F1
b)
BrF
c)
Br2F
d)
BrF2
37.
Disulfur trioxide
a)
S3O2
b)
SO
c)
S2O3
d)
S2O
38.
P2O5
a)
Phosphorus Oxide
b)
Pentaphosphorus Dioxide
c)
Diphosphorous pentoxide
d)
Phosphoric Oxygen
39.
PBr5
a)
Phosphorus Bromide
b)
Phosphorus Pentabromide
c)
Pentaphosphorus bromide
d)
Phosphorus Bromine
40.
Name the following compound:
  BF3
a)
boron fluoride
b)
boron difluoride
c)
monoboron trifluoride
d)
boron trifluoride
41.
As4O10
a)
arsenic oxide
b)
quadarsenic decoxide
c)
tetraarsenic decoxide
d)
arsenic decoxide
42.
Hydrogen needs _____ electrons in its valence shell to be stable.
a)
4
b)
6
c)
8
d)
2
43.
How many electrons should Oxygen have around its Lewis dot model?
a)
5
b)
6
c)
7
d)
8
44.
Three pairs of electrons are shared in a
a)
Single bond
b)
Double bond
c)
Triple bond
45.
Which of the following is the correct Lewis dot structure for the molecule fluorine (F2)?
a)
A
b)
B
c)
C
d)
D
46.
Which of the following is the correct Lewis structure for the compound PBr3?
a)
structure A
b)
structure B
c)
structure C
d)
structure D
47.
Which of the following is an acceptable Lewis structure for CH3Cl?
a)
Option A
b)
Option B
c)
Option C
d)
Option D
48.

Which covalent structure is CO2?

a)

b)

c)

d)

e)

None of these

49.

Which covalent structure represents BH3?

a)

b)

c)

d)

All of them

50.

In HCN (Carbon is usually the central atom) what kind of bond is between the C and N

a)

Single

b)

Double

c)

Triple

51.

CHCl3 has how many double bonds?

a)

0

b)

1

c)

2

d)

3

52.

CH2O has which of the following?

a)

Multiple double bonds

b)

Multiple single bonds

c)

One double bond

d)

One single bond

e)

A lone pair

53.

Carbonate (CO32-) has how many double bonds?

a)

0

b)

1

c)

2

d)

3

54.
What is the basis of a metallic bond?
a)
the attraction of neutral metal atoms.
b)
the attraction between protons and neutrons.
c)
the attraction between positive metal ions and interlocking electrons.
d)
the attraction between positive metal ions and free floating electrons.
55.
Electrons that are free to move in metals
a)
delocalized electrons
b)
oxidation number
c)
chemical bond
d)
salts
56.
Why do metals conduct
a)
They are shiny
b)
The electrons are held tightly within the lattice
c)
The electrons are delocalised and able to move
d)
The electrons are shared between two metal ions
57.
A mixture of two or more metals is called:
a)
mixture
b)
solution
c)
compound
d)
alloy
58.

Why are metals malleable?

a)

They are shiny

b)

The electrons are held tightly within the lattice structure making it strong

c)

The electrons are delocalized and able to move between the atoms

d)

The electrons are shared between two metal ions and this holds the atoms together

59.
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
60.

How are compounds with metallic bonds similar to ionic compounds?

a)

Both tend to have double and triple bonds.

b)

Both tend to have low boiling point

c)

Both tend to have poor conductivity.

d)

Both tend to have high melting points.

61.
Metals like to ________ electrons.
a)
Gain
b)
Lose
c)
Anhilate
d)
Juggle
62.

Why do metallic compounds conduct electricity as solids?

a)

core electrons are mobile, allowing electricity to flow through the metal

b)

valence electrons are mobile, allowing electricity to flow through the metal

c)

protons are mobile, allowing electricity to flow through the metal

d)

the metal cations are mobile, allowing electricity to flow through the metal

63.
True or false:
Ionic compounds have high melting points.
a)
true
b)
false
64.
The melting point of sugar is__________________ the melting point of table salt.
a)
greater than
b)
less than
c)
equal to
65.
Properties of metals are related to the behavior of their _____________________.
a)
valence electrons
b)
protons
c)
atomic number
d)
neutrons
66.

What kind of element has high ionization energy?

a)

metal

b)

nonmetal

c)

noble gas

d)

metalloid

67.
What is a repeating three-dimensional pattern that forms when ions bond called?
a)
Crystal Lattice
b)
Crystal Lettuce 
c)
Crystal Configuration
d)
Quartz
68.

Which type of compound usually has lower conductivity, boiling point, and melting point?

a)

Ionic

b)

Covalent

c)

Metallic

69.

Which type of compound is less flammable and melts at really high temperatures?

a)

Ionic

b)

Covalent

70.

When electrons in a Lewis structure are not within bonds, what are they called?

a)

Secluded electrons

b)

Lone pairs

c)

Lone electrons

d)

Atoms

71.

Which of these represents a formula unit because the atoms form ionic bonds?

a)

I2

b)

AlCl3

c)

NH3

d)

CO

72.

Which of these represents a molecule and not a formula unit?

a)

NaCl

b)

MgBr2

c)

CaO

d)

NH3

73.
A substance that does not conduct electricity as a solid but does conduct electricity when melted is most likely classified as
a)
a nonmetal 
b)
an ionic compound
c)
a molecular compound 
d)
a metal
74.

steps (in order) for going from formula to name in an ionic compound are:

a)

write cation first, write anion, find elements on periodic table replace ending with -ide

b)

find elements, write name of cation first, write name of anion and replace ending with -ide.

c)

find elements, write name of anion first, write name of cation and replace ending with -ide.

d)

write name of anion first, write name of cation and replace ending with -ide, find elements on periodic table.

75.

Why are there two sodiums (Na), in the formation of this ionic compound?

a)

There always has to be 2 metals

b)

The overall charge needs to add up to 4

c)

The overall charge has to be 0

d)

It needs to have more metal atoms than nonmetal

76.

Using the model for the formation of Scandium Fluoride (an ionic compound), write the chemical formula.

a)

Sc3F

b)

Sc3F3

c)

Sc+3F-1

d)

ScF3

77.
Atoms create bonds to _______ their potential energy, therefore becoming _______ stable.
a)
lower ; less
b)
lower ; more
c)
increase ; less
d)
increase ; more
78.

Shortest bond length

a)

Single bond

b)

Double bond

c)

Triple bond

79.

Longest bond length

a)

Single bond

b)

Double bond

c)

Triple bond

80.

Requires the most energy to break

a)

Single bond

b)

Double bond

c)

Triple bond

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