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Worksheets

Chemical Bonding and IMF's mix etc

Total questions: 157

Worksheet time: 2hrs 33mins

Name
Class
Date
1.

Is the following compound ionic or covalent?

PBr5

a)

Ionic

b)

Covalent

2.

Is the following compound ionic or covalent?

A material with a high melting point

a)

Ionic

b)

Covalent

3.

Is the following compound ionic or covalent?

Some types of these Exist as a solid, liquid or gas at room temperature

a)

Ionic

b)

Covalent

4.

Is the following ionic or covalent?

Cl2

a)

Ionic

b)

Covalent

5.

Is the following compound ionic or covalent?

A material that forms a crystal lattice

a)

Ionic

b)

Covalent

6.

Is the following compound ionic or covalent?

A material that is hard and brittle

a)

Ionic

b)

Covalent

7.

The following properties are all characteristics of ionic compounds EXCEPT

a)

high melting and boiling points

b)

soft

c)

crystal lattice structure

d)

conduct electricity when dissolved in water

8.
Which of the following is a property of an ionic compound?
a)
high melting point
b)
soft
c)
malleable
d)
liquid at room temperature
9.

What type of forces hold on an ionic lattice together?

a)

Electrostatic attraction forces

b)

Covalent bond

c)

Metallic bond

d)

Van der Waals forces

10.

What properties does an ionic compound have?

a)

A low boiling point and it conducts electricity when dissolved in water

b)

A high melting and it conducts electricity when liquid

c)

A high boiling point and it conducts electricity when solid

11.

Ionic compounds conduct electricity when dissolved in water. Which statement below best explains why?

a)

Ions are now free to move.

b)

Electrons are now all unattached to atoms

c)

Bonds conduct electricity

d)

There are now weak intermolecular forces of attraction.

12.

Which three of the following are features of ionic compounds? (click 3 boxes)

a)

They have bonds between metals and non-metals.

b)

They have bonds between two non-metals.

c)

They form simple molecular structures.

d)

They form giant ionic lattices.

e)

They involve the transfer of electrons.

13.

True or false? Ionic compounds have low boiling points.

a)

true

b)

false

14.

True or false? Ionic compounds conduct electricity when they are in their liquid state but not as solids.

a)

true

b)

false

15.

Why do ionic compounds NOT conduct electricity when they are in their solid state?

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 now perfectly balanced and the charge is now zero

16.

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

17.

Is the following compound ionic or covalent?

LiBr

a)

Ionic

b)

Covalent

18.

Which of the following best describes the arrangement of electrons in a metal?

a)

All of the electrons are delocalized

b)

None of the electrons are delocalized

c)

the valence electrons are delocalized

19.
Which of the following is NOT a characteristic of most metals?
a)
Brittle
b)
Good conductor
c)
Ductile
d)
Malleable
20.

Which properties of metal makes it a good choice to make a cooking pot out of? Choose TWO

a)

it has luster - it is shiny

b)

it is a good conductor of heat

c)

it is ductile - able to be made into a wire

d)

it has a high melting point

21.

Malleability and ductility are characteristics of compounds with

a)

covalent bonds

b)

metallic bonds

c)

ionic bonds

d)

alloy bonds

22.

Alloys are

a)

mixtures of two or more metals with useful properties

b)

mixtures of two or more nonmetals with useful properties

c)

mixtures of metals and nonmetals with useful properties

23.

Why are metals good conductors?

a)

they have a communal mega orbital of shared electrons

b)

they have mobile atoms/ions

c)

they have crystal structures that can rearrange

d)

they have mobile protons

24.

Malleability means

a)

the ability to be drawn into a wire

b)

the electrons of metals are mobile

c)

the ability to be hammered into a shape

d)

the ability to be a conductor of electricity

25.

In metals, the valence electrons are

a)

attached to the most positive ions

b)

shared by all of the atoms

c)

are bonded to the least electronegative element

d)

shiny

26.

Metals are malleable and ductile because metallic bonds

a)

hold the layers of ions in rigid/fixed positions like in ionic compounds

b)

maximizes the repulsive force in a metal

c)

have a large communal orbital that can deform/change shape while still binding the positive ions in place

d)

are easily broken

27.

Metals are hard because metals have a

a)

sea of electrons that tightly hold the nuclei together

b)

they form triple bonds

c)

low melting point

d)

high luster

28.
There are more metals than non metals in the periodic table.
a)
True
b)
False
29.
At room temperature, most metals are
a)
liquid
b)
solid
c)
gas
d)
an alloy
30.
Which of these is NOT an alloy?
a)
bronze
b)
copper
c)
brass
d)
stainless steel
31.

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

a)

Malleability

b)

Ductility

c)

Conductivity

d)

Solubility

32.

Why do metals conduct electricity well

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

33.
A mixture of two or more metals is called:
a)
mixture
b)
solution
c)
compound
d)
alloy
34.

Which of the following is an alloy?

a)

stainless steel

b)

chromium

c)

nickel

d)

lead

35.

Which of these are considered properties of metals? (choose ALL that apply)

a)

brittleness

b)

low melting point

c)

luster (shininess)

d)

malleability

e)

ductility

36.

Which pair of characteristics is most closely associated with metallic solids?

I. low melting point

II. high malleability

III. low thermal conductivity

IV. high electrical conductivity

a)

I and II

b)

I and III

c)

II and III

d)

II and IV

e)

III and IV

37.

Intermolecular forces are attractions between ______.

a)

Cations and anions

b)

Atoms within a molecule

c)

Neighboring molecules

d)

Protons and electrons

38.

Intermolecular forces are responsible for which of the following properties?

a)

State of matter

b)

Color

c)

Odor

d)

Conductivity

39.
Will this molecule be polar or nonpolar? CCl4
a)
polar
b)
nonpolar
40.
Will this molecule be polar or nonpolar? PH3
a)
polar
b)
nonpolar
41.

For which of the following would hydrogen bonding occur between molecules?

a)
b)
c)
d)
42.
What explains the very high melting and boiling point of water
a)
Strong dipole-dipole bonds between water molecules
b)
Strong hydrogen bonds between water molecules
c)
Dispersion forces which are present in all molecules
d)
Asymmetrical shape of the polar bonds.
43.

Chemical bonding happens between _________________ of an element.

a)

atoms

b)

protons

c)

neutrons

d)

element

44.

Which substance would have the weakest intermolecular forces of attraction?

a)

CH4

b)

NaCl

c)

H2O

d)

MgF2

45.

The weaker the intermolecular forces of a substance the _____________ the boiling point

a)

higher

b)

lower

46.
Propane is a gas at STP, while bromine is a liquid at STP. Which statement correctly explains these observations?
a)
Bromine has weaker intermolecular forces than propane does
b)
Bromine has greater molecular polarity than propane does
c)
Bromine has weaker molecular polarity than propane does
d)
Bromine has stronger intermolecular forces than propane does
47.

Does NH3 or PH3 have a higher boiling point?

(Hint: identify the types of IMF's present for each)

a)

NH3 because it has the strongest IMF's

b)

PH3 because it has the strongest IMF's

c)

NH3 because it has the weakest IMF's

d)

PH3 because it has the weakest IMF's

48.

Which noble gas should have the highest boiling point? (Hint: Think about how size affects IMFs)

a)

He

b)

Ne

c)

Kr

d)

Xe

49.
Does CH4 have hydrogen bonding?
a)
yes
b)
no
50.

Which substance has the weakest intermolecular forces?

a)

Substance A, boiling point of 75 °C

b)

Substance B, boiling point of 105 °C

c)

Substance C, boiling point of 25 °C

d)

Substance d, boiling point of 45 °C

51.

In a sample of liquid water at room temperature there will be

a)

Only covalent bonds present

b)

Only hydrogen-bonding present

c)

Both covalent bonds and intermolecular hydrogen bonding

52.

If something is a solid at room temperature and conducts well but only if it is liquified, it is probably a

a)

ionic compound

b)

covalent compound

c)

metallic substance

53.

If something is a solid at room temperature, does not dissolve in water and is a poor conductor, it is probably a

a)

ionic compound

b)

covalent compound

c)

metallic substance

54.

If something is a gas at room temperature, it is most probably a

a)

ionic compound

b)

covalent compound

c)

metallic substance

55.

If something has a very high melting point but also conducts well as a solid it is probably

a)

ionic compound

b)

covalent compound

c)

metallic substance

56.

If something has a very high melting point and does not conduct well as a solid but does dissolve in water, it is probably

a)

ionic compound

b)

covalent compound

c)

metallic substance

57.

If something is solid at room temperature, dissolves easily into water but does not conduct electricity when dissolved, it is probably a

a)

ionic compound

b)

covalent compound

c)

metallic substance

58.

Which part of a water molecule will be attracted to the cations in an ionic compound?

a)

The hydrogen end

b)

The oxygen end

c)

both ends

59.

Which part of a water molecule will be attracted to a negative ion?

a)

The hydrogen end

b)

The oxygen end

c)

both ends

60.

What do you call the types of forces that cause molecules to attract and get larger when the molecules get larger?

a)

hydrogen bonding

b)

dipole-dipole forces

c)

London or Dispersion Forces

61.

Which has a higher electronegativity

a)

Carbon

b)

Nitrogen

c)

Fluorine

d)

Calcium

62.

What type of shape is H2O?

a)

Tetrahedral

b)

Bent triatomic

c)

Linear diatomic

d)

Linear triatomic

63.

Which has a lower electronegativity, Copper(Co) or Flourine(F)?

a)

Copper(Co)

b)

Fluorine(F)

64.

Fluorine has the highest electronegativity on the chart

a)

False

b)

True

65.

Is water(H2O) polar or nonpolar?

a)

Polar

b)

Nonpolar

66.

Is CO2 polar or nonpolar?

a)

Polar

b)

Nonpolar

67.

In a nonpolar covalent bond, electrons are evenly distributed between atoms

a)

true

b)

false

68.

Which of the following molecules are nonpolar?

a)

CO and CH4

b)

CO2 and CH4

c)

H2O and CO

d)

CO and CO2

69.

Which molecule has a polar covalent bond?

a)

H-F

b)

F-F

c)

K-F

d)

None of the above

70.

Which formula represents a polar molecule?

a)

H2

b)

H2O

c)

CO2

d)

CCl4

71.

What kind of compound is CO2?

a)

Ionic

b)

Polar molecule with polar bonds

c)

Non-polar molecule with polar bonds

d)

Polar molecule with nonpolar bonds

72.
How many Hydrogen atoms does a single water molecule have?
a)
1
b)
2
c)
3
d)
4
73.
Why does alcohol evaporate faster than water?
a)
It heats up quicker
b)
It has bigger molecules
c)
The molecules are not as attracted to each other
74.
Salt dissolves in water because
a)
The water molecules wiggle between the Na and Cl atoms
b)
Water gets warm and moves around too much
c)
The polar areas of water molecules stick to the Na and CL ions
75.

Predict the type of bond present is present between the following pairs of atoms

a)

Ionic

b)

Nonpolar

c)

Polar

76.

Predict the type of bond present is present between the following pairs of atoms

a)

Ionic

b)

Nonpolar

c)

Polar

77.

Predict the type of bond present is present between the following pairs of atoms (Magnesium and Oxygen)

a)

Ionic

b)

Polar

c)

Nonpolar

78.

The polarity of molecules is determined both by the polarity of bonds and molecular geometry.

a)

True

b)

False

79.

Water, with a bent molecular shape, is classified as a polar molecule.

a)

True

b)

False

80.

Which of the following molecules is tetrahedral?

a)

H2O

b)

SF6

c)

CH4

d)

BF3

81.

Atoms with high electronegativity have a greater tendency to attract electrons toward themselves.

a)

True

b)

False

82.

What is the polarity of methane, CH4?

a)

Polar

b)

Nonpolar

83.

What is the polarity of oxygen difluoride, OF2?

a)

Polar

b)

Nonpolar

84.
Choose the correct shape for this molecule:
a)
Bent
b)
Trigonal pyramidal
c)
Trigonal planar
d)
Linear
85.

Choose the correct shape for this molecule:

a)

Trigonal planar

b)

Linear

c)

Bent

d)

Tetrahedral

86.
Choose the correct shape for this molecule:
a)
linear
b)
Trigonal pyramidal
c)
Bent
d)
Tetrahedral
87.
Choose the correct shape for this molecule:
a)
linear
b)
Trigonal pyramidal
c)
Bent
d)
Tetrahedral
88.
Choose the correct shape for this molecule:
a)
Tetrahedral
b)
Trigonal pyramidal
c)
Bent
d)
Trigonal planar
89.

Which Lewis Dot Model drawing correctly shows an O2 molecule?

a)
b)
c)
d)
90.

To which term of reference does the following description refer to?

"an unequal distribution of an electrical charge"

a)

Polar

b)

Nonpolar

c)

Both

91.

The two (2) factors that determine if a molecule is Polar or Non-polar:

a)

The atoms's ionization energy

b)

the type of atoms in the molecule

c)

The atom's oxidation number

d)

the shape of the molecule

92.

Which consists of positive ions immersed in a 'sea' of mobile electrons?

a)

calcium

b)

sulfur

c)

nitrogen

d)

chlorine

93.

When a chemical bond is broken, energy is

a)

absorbed

b)

released

c)

neither absorbed or released

94.

Which of the following has the most stable electron configuration?

a)

Na

b)

Ca

c)

Cl

d)

Ne

95.

Which of the following has the most stable electron configuration?

a)

Na +1 ion

b)

Ca

c)

Cl

d)

F

96.

What type of bond exists in a molecule of hydrogen bromide?

a)

a polar covalent bond with an EN difference of zero

b)

a nonpolar covalent bond with an EN difference between 0.4 and 1.7

c)

a nonpolar covalent bond with an EN difference of zero

d)

a polar covalent bond with an EN difference between 0.4 and 1.7

97.

Which represents a compound that is formed primarily by sharing electrons?

a)

CaF2

b)

CF4

c)

CrF3

d)

KF

98.

Which molecule is nonpolar?

a)

CO2

b)

H2O

c)

NH3

d)

CO

99.

Consider the compound HF; the shared pair of electrons are

a)

more strongly attracted to hydrogen

b)

more strongly attracted to the atom with the lower electronegativity

c)

more strongly attracted to fluorine

d)

equally attracted to both atoms

100.

In a covalent bond the shared electrons are more strongly attracted to the atom with the

a)

higher electronegativity

b)

lower electronegativity

c)

higher electropositivity

101.

Which is true

a)

Bond types are either ionic or covalent and all can be clearly classified as on or the other

b)

Bond types are a spectrum and it is somewhat arbitrary where the cut-off for one type is

c)

Boding attractions do not exist between molecules only within them

102.

An element wit an electronegativity of 0.9 bonds with one having 3.1; which best describes the bond

a)

the bond is mostly covalent in character and formed between a metal and nonmetal

b)

the bond is mostly ionic in character and formed between a metal and nonmetal

c)

the bond is mostly covalent in character and formed between two nonmetals

d)

the bond is mostly ionic in character and formed between a two nonmetals

103.

When two atoms form a chemical bond by sharing electrons, the resulting molecule will

a)

always be polar

b)

always be nonpolar

c)

be either polar or non polar

d)

be neither polar nor nonpolar

104.

Which of the following has the least ionic character?

a)

KCl

b)

CaCl2

c)

AlCl3

d)

CCl4

105.

Which bond has the greatest ionic character?

a)

F to F

b)

Li to F

c)

H to F

d)

Br to F

106.

Which of the following contains a nonpolar covalent bond?

a)

NaCl

b)

Cl2

c)

H2O

d)

HCl

107.

Compared to a calcium atom, a calcium +2 ion has

a)

fewer protons

b)

more protons

c)

fewer electrons

d)

more electrons

108.

Which of the following has a triple covalent bond?

a)

N2

b)

H2

c)

F2

d)

Br2

109.

Which has the strongest hydrogen bonds?

a)

HCl

b)

HBr

c)

HF

d)

HI

110.

When dissolved in water the Na ions are attracted to

a)

other Na ions

b)

the oxygen side of a water molecule

c)

the hydrogen side of a water molecule

d)

neither side of a water molecule

111.

Which contains a double covalent bond?

a)

N2

b)

H2

c)

Cl2

d)

O2

112.

When combining with nonmetallic atoms, a metallic atom will usually

a)

gain electrons and form negative ions

b)

lose electrons and form positive ions

c)

gain electrons and form positive ions

d)

lose electrons and form negative ions

113.

At room temperature fluorine is a gas but iodine is a solid, because, compared to fluorine, iodine has

a)

weaker covalent bonds

b)

weaker intermolecular forces

c)

stronger intermolecular forces

d)

stronger covalent bonds

114.

Which is most likely an Ionic Compound?

a)

A

b)

B

c)

C

d)

D

115.

Which is most likely a Metallic Substance??

a)

A

b)

B

c)

C

d)

D

116.

Which will most likely form an ionic bond with Bromine?

a)

K

b)

O

c)

C

d)

S

117.

What happens when magnesium and oxygen come together to form magnesium oxide?

a)

Chemical bonds are broken and energy is absorbed

b)

New chemical bonds are created and energy is released

c)

New chemical bonds are created and energy is absorbed

118.

How can you use the periodic table to determine valence electrons

a)

You can use the period number on the left

b)

You can use the atomic mass in the box

c)

You can use the group number at the top

119.

How many valence electrons does S have?

a)

16

b)

6

c)

7

120.

Metals ________electrons to become ___________ and nonmetals _________ electrons to become ______________.

Hint: recall the names for postive and negative ions.

a)

accept, anion, donate, cation

b)

donate, cation, accept, anion

c)

Donate, anion, accept, cation

121.

Cations (select 2)

a)

negative charge

b)

accepted electrons

c)

usually metals

d)

donated electrons

e)

nonmetals

122.

Anions (select 3)

a)

have negative charge

b)

accepted electrons

c)

+2

d)

aluminum can form one

e)

usually

nonmetals

123.

Which group on the periodic table do not form ions because they are already stable?

a)

Transition metals

b)

Metalloids

c)

Noble Gases

d)

Halogens

124.

What is the chemical formula for Aluminum Phosphide?

a)

Al3P3

b)

AlP

c)

Al3P

d)

AlP3

125.
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
126.

Which of the following is true for ionic bonding & ionic compounds? Choose 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.

127.

Which types of atoms are hold on to their outer electrons most loosely?

a)

Metals

b)

Nonmetals

c)

Noble/Inert Gases

128.

Which types of atoms are hold on to their outer electrons most tightly?

a)

Metals

b)

Nonmetals

129.

Which types of atoms have the lowest energy electron configurations?

a)

Metals at the very left Group 1

b)

Nonmetals in Group 7

c)

Noble/Inert Gases

130.

Which of the following is the best representation of a molecule of fluorine (F2)?

a)

A

b)

B

c)

C

d)

D

131.
What is a diatomic element?
a)

a type of metal that exists in pairs

b)

an element made up of two different atoms bonded together

c)

an element whose atoms exist in pairs always

d)

an element whose atoms exist in pairs when the element is found by itself

132.
The number of bonds an element will form in a covalent compound will be equal to
a)
the number of valence electrons
b)

eight always

c)

the number of electrons needed to reach a noble gas-like configuration

d)

the number of bonds that is needed to form an octet always

133.

What is the formula for diphosphorus pentoxide?

a)

P2O5

b)

PO5

c)

P5O2

d)

P2O6

134.
What is the correct name for NO?
a)
Mononitrogen Monoxide
b)
Nitrogen Monoxide
c)
Mononitrogen Dioxide
d)
Nitrogen Oxide
135.

What is the reason why Noble gases are so stable?

a)

They have an even number of electrons

b)

They have no electrons

c)

They have the lowest energy electron configurations

d)

They bond with other atoms

136.

How can you fix this electron dot diagram?

a)

Erase the two extra electrons on Carbon

b)

Two more covalent bonds should be made to the oxygen on the left

c)

Share another pair of electrons between each oxygen and the central carbon

d)

1 more electrons should be added to each oxygen atom

137.

Which part of the atom is responsible for chemical bonding?

a)

Core Electrons

b)

Valence Electrons

c)

Protons

d)

Neutrons

138.

A group of covalently bonded atoms is called a _________________

a)

crystal

b)

molecule

c)

salt

d)

pod

139.

What holds the atoms together in a covalent bond?

a)

Spit

b)

Attractions between the opposite charges

c)

The shared electrons fly around both nuclei

d)

nothing

140.

This molecule has 3 bonds and 1 lone pair around the central atom. What shape is it?

a)

bent

b)

trigonal pyramidal

c)

tetrahedral

d)

linear

141.

Which is the 3D picture of this molecule?

a)
b)
c)
d)
142.

This molecule has 2 bonds and 2 lone pairs around the central atom. What shape is it?

a)

bent

b)

trigonal pyramidal

c)

tetrahedral

d)

linear

143.

Which is the 3D picture of this molecule?

a)
b)
c)
d)
144.

Which is the 3D picture of this molecule?

a)
b)
c)
d)
145.
Which has the greater EN: 
N or C?
a)
C
b)
N
146.
Which of the following is the least electronegative element?
a)
oxygen
b)
potassium
c)
fluorine
d)
nitrogen
147.

What type of bond is depicted in the image?

a)

Nonpolar Covalent

b)

Polar Covalent

c)

Ionic

148.

What is the electronegativity difference of the S-O bonds in 

SO2SO_2  ?

a)

0.5

b)

0.8

c)

2.5

d)

3.4

149.

NH3NH_3   is a covalent compound. Which atom, N or H, will electrons spend MORE time with?

a)

N

b)

H

c)

Neither

150.

A polar covalent bond should have an electronegativity difference ranges from _____?

a)

0-0.4

b)

0.5 to 1,7

c)

1.7 to 3.3

151.

'Partial'/not fully charged atoms are present in which type of bond?

a)

Ionic

b)

Nonpolar Covalent

c)

Polar Covalent

d)

Both Polar Covalent and Ionic

152.

A diatomic molecule like O2 is always _____ because electrons are shared _____

a)

nonpolar; unequally

b)

polar; equally

c)

nonpolar; equally

d)

polar; unequally

153.

Which of the following shows a trigonal pyramid shape?

a)
b)
c)
d)
154.

How many diatomic elements are there?

a)

3

b)

5

c)

6

d)

7

e)

8

155.

Which of the following is a diatomic element?

a)

Carbon

b)

Iodine

c)

Neon

d)

Magneium

156.

Which of the following is not a diatomic element?

a)

Fluorine

b)

Hydrogen

c)

Sulfur

d)

Bromine

e)

Nitrogen

157.

What did the covalent bond yell to the ionic bond? "Hey, didn't your dad ever teach you to

a)

steal

b)

share

c)

fight

d)

knit

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