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Unit 4 TEST REVIEW- Bonding S23

Total questions: 84

Worksheet time: 3hrs 48mins

Name
Class
Date
1.
Which of the following has a full valence shell?
a)
Oxygen
b)
Neon
c)
Barium
d)
Carbon
2.
An ionic bond forms when atoms ___________ electrons.
a)
gain
b)
share
c)
increase
d)
transfer
3.
Which type of bond has an equal sharing of electrons?
a)
Polar Covalent 
b)
Non Polar Covalent
c)
Ionic
d)
Metallic
4.
Which type of bond has an unequal sharing of electrons?
a)
Polar Covalent 
b)
Non Polar Covalent
c)
Ionic
d)
Metallic
5.
Which type of bond has a transfer of an electron from on atom to another?
a)
Polar Covalent 
b)
Non Polar Covalent
c)
Ionic
d)
Metallic
6.
If an atom loses two electrons what charge will it have?
a)
+ 2
b)
 - 2
c)
+1
d)
-1
7.

Which of the following is the correct name for the compound PbO?

a)

lead oxide

b)

lead monoxide

c)

lead (I) oxide

d)

lead (II) oxide

8.

Which of the following is the correct chemical formula of calcium nitrate?

a)

CaNO3

b)

Ca(NO3)2

c)

CaN

d)

Ca3N2

9.

What is the correct IUPAC name for the compound P2O5?

*IUPAC stands for International Union of Pure and Applied Chemistry and it is the naming system that we use in class.

a)

phosphorus pentoxide

b)

diphosphorus pentoxide

c)

phosphorus oxide

d)

potassium oxide

10.

Metals are good conductors of electricity because when the metal atoms bond the valence electrons are

a)

highly mobile

b)

transferred

c)

shared equally

d)

shared unequally

11.

Which of the following compounds contains both ionic and covalent bonds?

a)

NaCl

b)

PCl3

c)

NaClO4

d)

CaBr2

12.

How many pairs of electrons are shared between the nitrogen atoms in a molecule of nitrogen?

a)

2

b)

3

c)

4

d)

6

13.

Which of the following forms a nonpolar covalent bond?

a)

Br2

b)

HBr

c)

NaBr

d)

PBr3

14.

Which of the following is the most polar?

a)

HF

b)

HCl

c)

HBr

d)

HI

15.

Which of the following is a polar molecule?

a)

O2

b)

CO2

c)

NH3

d)

CH4

16.

Predict the bond that is formed between Phosophorus and Chlorine?

a)

Ionic

b)

Covalent

c)

Metallic

d)

H-bond

17.

Which of the pair of elements form an ionic bond?

a)

Magnesium and Oxygen

b)

Magnesium and Sodium

c)

Iron and Zinc

d)

Nitrogen and Hydrogen

18.

How many valence electrons are shown in the diagram?

a)

16

b)

7

c)

6

d)

2

19.

TRUE OR FALSE: Ionic compounds have high boiling points because they consist of a strong ionic bond.

a)

TRUE

b)

FALSE

20.
Which of these is NOT an alloy?
a)
bronze
b)
copper
c)
brass
d)
stainless steel
21.
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.
22.
The ability of a material to be shaped in all directions without cracking or breaking.
a)
hardness
b)
ductility
c)
malleability
d)
conductivity
23.

Which of the following is true for ionic bonding & ionic compounds? Check all that apply!!

a)

They must be made of ions with like charges.

b)

The negative ion must be written first.

c)

Compounds must have an overall charge of zero.

d)

They are made of metals and nonmetals.

e)

The positive ion must be written first.

24.

Which of the following elements does NOT form an ion with a charge of 2+?

a)

Beryllium

b)

Strontium

c)

Magnesium

d)

Fluorine

25.

When Alkali metals (Group 1) form ions, they ____.

a)

lose 1 proton

b)

gain 1 proton

c)

lose 1 electron

d)

gain 1 electron

26.

How does fluorine (F) obey the octet rule when reacting to form compounds?

a)

It doesn’t change its number of electrons - it has a full octet!

b)

Fluorine does not obey the octet rule.

c)

It gains an electron.

d)

It gives up an electron.

27.

Which of the following shows correctly an ion pair and the ionic compound the two ions form?

a)

Sn4+ and N3- form Sn4N3

b)

Cu2+ and O2- form Cu2O2

c)

Cr3+ and I- form CrI

d)

Cr2+ and I- form CrI2

28.

What is the chemical formula of sodium nitride?

a)

NaN

b)

Na2N

c)

Na3N

d)

NaNO3

29.

Select the correct formula for boron trichloride.

a)

B2Cl

b)

B3Cl

c)

BCl3

d)

BCl2

30.
What is the correct chemical name for the ionic compound: Fe3N2
a)
Iron nitride
b)
Iron (III) nitride
c)
Iron (II) nitride
d)
TriIron dinitride
31.
What is the correct chemical name for the ionic compound: CuS
a)
copper sulfide
b)
copper (I) sulfide
c)
copper (II) sulfide
d)
copper monosulfide
32.
What is the correct chemical name for the molecular compound:  CS2
a)
Carbon Sulfide
b)
Carbon diSulfide
c)
diCarbide diSulfide
d)
Carbon (II) Sulfide
33.
Given the picture, what type of bond is  holding the atoms together in this molecule?
a)
polar covalent bond
b)
nonpolar covalent bond
c)
ionic bond
d)
metallic bond
34.
What geometry will this molecular structure have?: H2S
a)
bent
b)
tetrahedral
c)
linear
d)
trigonal pyramidal
35.
This is a correct dot diagram for oxygen (O)
a)
true
b)
false
36.
Choose the correct shape for this molecule:
a)
Trigonal planar
b)
Trigonal pyramidal
c)
Tetrahedral
d)
Linear
37.
Choose the correct shape for this molecule:
a)
Bent
b)
Trigonal pyramidal
c)
Trigonal planar
d)
Linear
38.
Choose the correct shape for this molecule:
a)
Trigonal planar
b)
Trigonal pyramidal
c)
Bent
d)
Tetrahedral
39.
Choose the correct shape for this molecule:
a)
Tetrahedral
b)
Trigonal pyramidal
c)
Bent
d)
Trigonal planar
40.
 A lone pair is defined as
a)
A pair of bonding electrons
b)
One non-bonding electron
c)
A pair of non-bonding electrons
d)
A pair of electrons on the central atom
41.
What is the VSEPR theory used to predict?
a)
Bond Strength
b)
Polarity
c)
Molecular Shape
d)
Electronegativity
42.
According to VSEPR, molecules adjust their shapes to keep which of the following as far away as possible?
a)
Pairs of valence electrons
b)
Inner shell electrons
c)
Mobile Electrons
d)
Electrons closest to the nucleus
43.
Choose the correct shape for this molecule:
a)
linear
b)
Trigonal pyramidal
c)
Bent
d)
Tetrahedral
44.
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
45.
P2O5
a)
Phosphorus Oxide
b)
Pentaphosphorus Dioxide
c)
Diphosphorous pentoxide
d)
Phosphoric Oxygen
46.

The geometry of a molecule with 4 bonded pairs of electrons and 0 lone pairs of electrons, AB4

a)

Tetrahedral

b)

Trigonal Planar

c)

Bent

d)

Trigonal Pyramidal

e)

Linear

47.

What is the molecular geometry of CO2?

a)

Bent

b)

Trigonal planar

c)

Trigonal pyramidal

d)

Linear

48.
Choose the correct shape for this molecule:
a)
linear
b)
Trigonal pyramidal
c)
Bent
d)
Trigonal planar
49.

Describe the shape of the molecule.

a)

linear

b)

bent

c)

trigonal pyramidal

d)

tetrahedral

50.

Ionic bonds are the _____ between positive and negative ions.

a)

covalent bonds

b)

metallic bonds

c)

polar bonds

d)

electrostatic attraction

51.

Ionic compounds have ____ melting points and _____ boiling points because _____ ionic bonds must be broken in order to break the lattice.

a)

low, low, weak

b)

low, high, weak

c)

low, high, strong

d)

high, high, strong

52.

Ionic compounds always conduct electricity - whether they are in the solid, liquid or gas form.

a)

True- they can conduct electricity in any form!

b)

False- they can only conduct electricity when dissolved in water or in melted (liquid) form

c)

False- they can only conduct electricity in solid form

53.

Ionic compounds conduct electricity only when molten or in a solution because...

a)

electrons are free to move

b)

water is free to move

c)

molecules are free to move

d)

ions are free to move

54.
Name the following ionic compound: MgSO4
a)
magnesium sulfoxide
b)
magnesium sulfide
c)
magnesium sulfate
d)
magnesium oxide
55.
The proper formula for magnesium hydroxide:
a)
MgOH
b)
Mg2OH
c)
Mg(OH)2
d)
Mg2OH2
56.

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

57.
What is the formula for copper(I) sulfate?
a)
CuSO3
b)
CuSO4
c)
Cu2SO3
d)
Cu2SO4
58.
What is the name of Al(NO3)3?
a)
Aluminum trinitrate
b)
Monoaluminum nitrate
c)
Aluminum (III) nitrate
d)
Aluminum Nitrate
59.
Name the following ionic compound: Cr(NO2)3
a)
chromium nitrite
b)
chromium nitride
c)
chromium III nitride
d)
chromium III nitrite
60.
If copper (II) and phosphate bond together, the resulting chemical formula would be:
a)
Cu2(PO4)3
b)
CuPO4
c)
Cu3(PO4)2
d)
Cu3PO4
61.
Name the Compound:
SnO2
a)
tin(II) oxide
b)
tin(IV)oxide
c)
tin(II)oxegen 
d)
tin oxide
62.
Name this formula: 
FeSO4
a)
Iron (I) Sulfate
b)
Iron (II) Sulfate
c)
Iron Sulfate
d)
Iron Sulfide
63.

Is the following compound ionic or covalent?

LiBr

a)

Ionic

b)

Covalent

64.

Is the following compound ionic or covalent?

Exists as a solid, liquid or gas

a)

Ionic

b)

Covalent

65.

Is the following compound ionic or covalent?

A material that has a low boiling point

a)

Ionic

b)

Covalent

66.

Is the following compound ionic or covalent?

A material that forms a crystal lattice

a)

Ionic

b)

Covalent

67.

Is the following compound ionic or covalent?

A material that is hard and brittle

a)

Ionic

b)

Covalent

68.

Is the following compound ionic or covalent?

A material that SHARES electrons

a)

Ionic

b)

Covalent

69.
A ________ is a model of an atom in which each dot represents a valence electron.
a)
Valence electron
b)
Electron dot diagram/Lewis dot structure
c)
Lewis bond structure
70.
Low melting point and low solubility in water are general properties of ______________________ compounds
a)
ionic
b)
covalent
c)
chemical
d)
glucose
71.

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).

72.

Which element is most likely to form 4 bonds?

a)

Carbon

b)

Fluorine

c)

Sulfur

d)

Nitrogen

73.

The following properties are all characteristics of ionic compounds EXCEPT

a)

solid at room temperature

b)

soft

c)

crystal lattice structure

d)

conduct electricity when dissolved in water

74.

Which types of elements become cations?

a)

non-metals

b)

metals

c)

metalloids

75.

Ionic bonds could be best described as:

a)

A bond formed when 2 atoms share electrons

b)

A firm handshake

c)

An electrostatic attraction between oppositely charged ions

d)

An electrostatic attraction between anions

76.

Have very strong intermolecular forces

a)

ionic compounds

b)

covalent compounds

77.

Why do atoms form bonds?

a)

to increase their potential energy AND decrease stability by filling up their valence shell

b)

to lower their potential energy AND increase stability by filling up their valence shell

c)

to increase their atomic number

78.

Metals have positive ions in a ‘sea of electrons’. Which metal atom provides the most electrons for the sea?

a)

Aluminium

b)

Sodium

c)

Calcium

d)

Magnesium

79.

Copper is a metallic element.

Which statements about copper are correct? Choose all that apply!

a)

Copper is malleable because layers of ions are in fixed positions and cannot move.

b)

The structure of copper consists of negative ions in a lattice.

c)

Copper conducts electricity because electrons can move through the metal.

d)

Electrons hold copper ions together in a lattice by electrostatic attraction.

80.
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.
81.
Why do metals have high melting points?
a)
They don't
b)
The negatively charged electrons act as a glue to hold the positively charged ions together.
c)
All the electrons become delocalised
82.

Why does the melting point of metals increase across period 3, from Sodium (Na) to Aluminium (AI)?

a)

Size of atoms gets smaller

b)

Attraction force between nuclei and free electron increases

c)

Increased space between the valence electrons in the "sea"

d)

Increased number of valence electrons contributed to the "sea"

83.

Metallic bonds form because metals

a)

"want" to give up valence electrons

b)

always share valence electrons

c)

have many valence electrons

d)

always gain valence electrons

84.

What is the ability of a substance to be pulled into a wire?

a)

Malleability

b)

Ductility

c)

Conductivity

d)

Solubility

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