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Unit 6 Bonding Review

Total questions: 58

Worksheet time: 1hrs 17mins

Name
Class
Date
1.
A charged particle that has gained or lost electrons is called a _____.
a)
molecule
b)
ion
c)
isotope
d)
element
2.
A cation is a ____ ion.
a)
negative
b)
positive
c)
neutral
d)
ficticious
3.
A anion will be a ____ ion.
a)
negative
b)
positive
c)
neutral
d)
ficticious
4.

Nitrogen, N, will form which of the following ions?

a)

N

b)

N-3

c)

N-5

d)

N+5

5.

Beryllium, Be, will ____ valence electrons when forming an ionic bond.

a)

lose 4

b)

gain 4

c)

lose 2

d)

gain 2

6.
In the compound aluminum oxide, which is the cation?
a)
Al+3
b)
Al
c)
O-2
d)
O
7.
Ionic bonds form between metals and ____.
a)
metalloids
b)
metals
c)
nonmetals
8.

Ionic bonds happen because of the ____ of valence electrons.

a)

sharing

b)

transfer

c)

keeping

d)

covering

9.

Boron, B, will ____ valence electrons when forming an ionic bond.

a)

lose three

b)

gain three

c)

lose 5

d)

gain 5

10.

Sulfur, S, will ____ valence electrons when forming an ionic bond.

a)

gain 1

b)

lose 1

c)

gain 2

d)

lose 2

11.
How many electrons are needed in the outer energy levels of an atom to be stable?
a)
2
b)
4
c)
6
d)
8
12.
Which of the following would produce an anion?
a)
Ca
b)
Al
c)
K
d)
F
13.

The name of FeCl₂ is

a)

iron chloride

b)

iron (II) chloride

c)

iron (I) chloride

d)

iron dichloride

14.

LiBr is called

a)

lithium bromine

b)

lithium (I) bromine

c)

lithium bromide

d)

lithuim (I) bromide

15.

Name the ionic compound SnSe2

a)

Tin diselenide

b)

Tin (IV) Selenide

c)

Tin selenide

d)

Tin (II) triselenide

16.

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

a)

potassium + fluorine

b)

beryllium + oxygen

c)

boron + iodine

d)

gold + oxygen

17.

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

18.

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

a)

Metal

b)

Nonmetal

c)

Anion

d)

Cation

19.

When naming a compound, what must the last part be?

a)

the element with "ide" at the end

b)

the element with the ending "ite"

c)

the name of the element

d)

the element with "ide" at the end, unless its a polyatomic ion

20.

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

a)

Sodium sulfate

b)

Sodium sulfide

c)

Sodium sulfite

d)

Sodium sulfuroxide

21.

What is the name of the compound Sc(OH)3?

a)

Scandium (III) hydroxide

b)

Scandium (I) hydroxide

c)

Scandium (II) hydroxide

d)

Scandium hydroxide

22.

The name of the compound Ca3(PO4)2

a)

calcium phosphate

b)

tricalcium diphosphate

c)

calcium phosphorus oxide

d)

calcium phosphide

23.

Magnesium Nitrate

a)

MgNO3

b)

Mg(NO3)

c)

Mg(NO3)2

d)

(MgNO3)2

24.

Zinc Oxide

a)

ZnO2

b)

Zn2O

c)

Zn4O

d)

ZnO

25.

Name the ionic formula of PbO

a)

Lead(II) oxide

b)

Lead(IV) oxide

c)

Lead oxide (II)

d)

Lead Oxide (IV)

26.

Name the ionic formula of AgNO3

a)

Silver nitrite

b)

Silver Chloride

c)

Silver nitrate

d)

silver sulphate

27.

Name the ionic formula of FeSO4

a)

Iron (II) sulphate

b)

Iron sulphate(II)

c)

Iron Sulphate (IV)

d)

Iron(III)Sulphate (V)

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.
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
30.
What is the correct name for C4H6?
a)
Carbon Hexahydride
b)
Pentacarbon Pentahydride
c)
Hexacarbon Tetrahydride
d)
Tetracarbon Hexahydride
31.
What is the correct name for NO?
a)
Mononitrogen Monoxide
b)
Nitrogen Monoxide
c)
Mononitrogen Dioxide
d)
Nitrogen Oxide
32.
What is the formula for Tricarbon Octahydride?
a)
Ca3O
b)
C2H8
c)
C3H8
d)
Ca3H8
33.
What is Sulfur Trichloride?
a)
SCl3
b)
SiCl3
c)
SCl4
d)
Si3Cl
34.
Phosphorous trichloride
a)
PCl3
b)
P3Cl
c)
P3Cl3
d)
PCL
35.
In general, this type of bond will form a compound with a high melting point.
a)
Ionic
b)
Covalent
36.
When dissolved in water, the solution is a good conductor of electricity.
a)
ionic compounds
b)
covalent compounds
37.
When dissolved in water, the solution does NOT conduct electricity.
a)
ionic compounds
b)
covalent compounds
38.

True or false? Ionic compounds have low boiling points.

a)

true

b)

false

39.

At room temperature, are ionic compounds solids, liquids or gases? Justify your answer.( click 2 boxes)

a)

solids

b)

liquids

c)

gases

d)

Room temperature is lower than the melting points of ionic compounds.

e)

Room temperature is higher than the boiling points of ionic compounds.

40.
Intermolecular forces are the forces
a)
within molecules
b)
between molecules
41.

Intramolecular forces are the forces

a)

within molecules

b)

between molecules

42.

Intermolecular forces are the forces

a)

within molecules

b)

between molecules

43.

High viscosity can be described as...

a)

a liquid that flows quickly

b)

a liquid that flows slowly

44.

Which statement explains why Br2 is a liquid at room temp and I2 is a solid at room temp?

a)

Molecules of Br2 are polar, and molecules of I2 are nonpolar

b)

Molecules of Br2 are nonpolar, and molecules of I2 are polar

c)

Molecules of Br2 have stronger intermolecular forces than molecules of I2.

d)

Molecules of I2 have stronger intermolecular forces than molecules of Br2.

45.
Which of these typically increases when intermolecular forces increase?
a)
Boiling Point
b)
Melting Point
c)
Viscosity
d)
All of these
46.

Classify the following molecule.

a)

polar

b)

nonpolar

47.

Classify the following molecule.

a)

polar

b)

nonpolar

48.

Is the following molecule polar or nonpolar?

a)

polar

b)

nonpolar

49.

Is the following molecule polar or nonpolar?

a)

polar

b)

nonpolar

50.

Is the following molecule polar or nonpolar?

a)

polar

b)

nonpolar

51.

Is the following molecule polar or nonpolar?

a)

polar

b)

nonpolar

52.
F2
a)
Polar 
b)
Nonpolar 
53.
H2O
a)
Polar 
b)
Nonpolar 
54.

If an element is diatomic it should have a subscript of___

a)

1, always

b)

2, only when it is an element

c)

it shouldn't have a subscript, it should have a coefficent

d)

2, when bonded in a compound

55.

Predict the products of this synthesis reaction: H2 + Cl2 →

a)

HCl

b)

H2Cl2

c)

H2Cl

d)

HCl2

56.

Predict the products for the this Single Replacement reaction:

K + HCl →

a)

KCl + H2

b)

KHCl

c)

KH + Cl2

d)

HCl + K2

57.

Predict the products for the this Double Replacement reaction:

AgNO3 + KCl →

a)

AgCl + KNO3

b)

AgK + ClNO3

c)

KAg + NO3Cl

d)

AgCl + 3 KNO

58.

Complete the balanced equation for this Double Replacement reaction.

3 NaOH + Fe(NO3)3 →

a)

NaFe + OH(NO3)3

b)

NaNO3 + Fe(OH)3

c)

3 NaNO3 + Fe(OH)3

d)

3 NaFe + 3 (OH)NO3

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