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BONDING QUIZ

Total questions: 159

Worksheet time: 2hrs 58mins

Name
Class
Date
1.
Nitrogen will form which of the following ions?
a)
N
b)
N-3
c)
N-5
d)
N+5
2.
Beryllium will ____ valence electrons when forming an ionic bond.
a)
lose 4
b)
gain 4
c)
lose 2
d)
gain 2
3.
In the chemical formula for an ionic compound, which item is written first?
a)
positive ion
b)
negative ion
c)
subscript
d)
the female
4.
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
5.
Which is the correct name for CaBr2?
a)
Calcium Bromine
b)
Bromine Calcium
c)
Calcium Bromide
d)
Carbon and Bromine
6.

Which is the correct formula for aluminum sulfide?

a)

AlS

b)

Al3S2

c)

S3Al2

d)

Al2S3

7.

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

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.

8.

The formula for beryllium phosphide will contain (a)   phosphide ions.

9.

Oxygen has (a)   valence electrons.

10.
What is the formula for aluminum fluoride?
a)
AlF
b)
Al2F3
c)
AlF3
d)
Al3F2
11.
Metals tend to 
a)
gain electrons
b)
lose electrons
12.
What is the correct formula for the compound, lithium oxide?
a)
LiO
b)
Li2O
c)
LiO2
d)
Li2O2
13.

What is the charge of ion "X" in the formula XF3?

a)

+3

b)

-3

c)

+1

d)

-1

14.

What is the charge of ion "X" in CaX?

a)

+1

b)

-1

c)

+2

d)

-2

15.

Which of the following pairs of elements will NOT form an ionic compound?

a)

sodium and fluorine

b)

phosphorous and aluminum

c)

potassium and magnesium

d)

strontium and oxygen

16.

Which of the following could NOT form an ionic compound? Check all that apply.

a)

Li+ and Cl-

b)

F- and O2-

c)

Ba2+ and Ag+

d)

Mg2+ and S2-

17.

Which of the following could form an ionic compound? Check all that apply.

a)

Na+ and F-

b)

S2- and O2-

c)

Ca2+ and Fe3+

d)

Mg2+ and Cl-

18.

In an ionic bond, the ions are held together because...

a)

the positive nucleus of each ion attracts the other ion's negatively charged electrons

b)

the ions have opposite charges

c)

as the electron moved from one atom to another it pulled the atom along with it

d)

electrons are being shared

19.

Which element(s) will lose valence electrons to form an ion? Check all that apply.

a)

Phosphorus

b)

Iron

c)

Barium

d)

Neon

20.

Which element(s) will form negative ions? Check all that apply.

a)

Potassium

b)

Sulfur

c)

Iodine

d)

Magnesium

21.

Which of the following pairs of elements could NOT react to form an ionic compound?

a)

Carbon and Oxygen

b)

Potassium and Fluorine

c)

Silver and Oxygen

d)

Aluminum and Chlorine

22.

Calcium Fluoride has a chemical formula of CaF2. What does the chemical formula tell you?

a)

There are 2 Calcium ions for every 1 Fluoride ion in the crystal

b)

There is 1 Calcium ion for every 2 Fluoride ions in the crystal

23.

The following ionic crystal has 6 Fe ions (red) and 9 O ions (blue). What is the formula for this ionic crystal?

a)

FeO

b)

Fe2O3

c)

Fe3O2

d)

Fe6O9

24.

The following ionic crystal has 4 Sr ions (red) and 8 Br ions (blue). What is the formula for this ionic crystal?

a)

SrBr

b)

SrBr2

c)

Sr2Br

d)

Sr4Br8

25.

The following ionic crystal has 4 Al ions (red) and 6 O ions (blue). What is the formula for this ionic crystal?

a)

Al3O2

b)

Al4O5

c)

Al4O6

d)

Al2O3

26.

How many electrons do atoms want to have in their valence shell? Hint: Octet rule!

(a)  

27.

Ionic bonds form between...

a)

nonmetals and nonmetals

b)

metals and nonmetals

c)

metals and metals

d)

noble gases

28.

In an ionic bond, the atom with ___ electronegativity will take an electron from the other atom.

a)

higher

b)

lower

c)

equal

d)

it cannot be predicted

29.

In ionic bonds, electrons tend to be transferred...

a)

from halogens to alkali metals

b)

from nonmetals to metals

c)

from metals to nonmetals

d)

they are shared equally

30.

Calcium will give up ____ electrons to have a full valence shell and form a cation with +___ charge.

(a)  

31.

An example of an ionic compound is...

a)

Ethanol (C2H5OH)

b)

Potassium iodide (KI)

c)

Magnesium metal (Mg)

d)

Hydrogen gas (H2)

32.

What is FALSE about ionic compounds?

a)

They usually dissolve easily in water

b)

They conduct electricity

c)

They tend to have solid, crystalline shapes

d)

They have a low melting point

33.

In a covalent bond...

a)

A metal bonds with a metal

b)

One electron is shared

c)

A pair of electrons are shared

d)

Atoms try to get 6 valence electrons total

34.

A covalent bond that is polar...

a)

Has an uneven share of electrons

b)

Electrons are shared equally

c)

The bond is magnetic

d)

H2 is an example

35.

What is TRUE about covalent compounds?

a)

They dissolve easily in water

b)

They have low melting and boiling points

c)

They are poor conductors of electricity

d)

Metals bond to nonmetals

36.

What is false about metallic bonds?

a)

There is a sea of electrons

b)

Metals are still forming cations

c)

They help give metals their properties

d)

They are between nonmetals and metals

37.

When two atoms bond, if there is a LARGE difference in electronegativity, they will form...

a)

A covalent bond

b)

An ionic bond

c)

A metallic bond

d)

A double bond

38.

When two atoms bond, if there is a very SMALL difference in electronegativity, they will form...

a)

A nonpolar covalent bond

b)

A polar covalent bond

c)

An ionic bond

39.

In a nonpolar covalent bond...

a)

The electronegativity difference is less than 0.3 between the atoms

b)

H2 (two hydrogens bonded) is an example

c)

There is an equal share of electrons

d)

All of the above

40.

An example of a covalent compound is...

a)

Oxygen gas (O2)

b)

Potassium bromide (KBr)

c)

Strontium iodide (SrI2)

d)

Pure iron (Fe)

41.

Elements such as diamond and graphite are examples of...

a)

simple covalent molecules

b)

metallic

c)

ionic

d)

giant covalent

42.

Low melting and boiling points that rarely conduct electricity.

a)

simple covalent molecules

b)

metallic

c)

ionic

d)

giant covalent

43.

Melting points are very high and they rarely conduct electricity as solid or liquid.

a)

simple covalent molecules

b)

metallic

c)

ionic

d)

giant covalent

44.

Excellent conductors as solid and liquid due to a sea of delocalised electrons.

a)

simple covalent molecules

b)

metallic

c)

ionic

d)

giant covalent

45.

Giant structures with high melting and boiling points but only conduct electricity when molten or dissolved in a solution.

a)

Small molecular covalent

b)

Metallic

c)

Ionic

d)

Giant covalent

46.

Which of these is a small molecular compound?

a)

NaCl

b)

CO2

c)

Fe2

d)

MgCl2

47.

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

48.
Nonmetals tend to 
a)
gain electrons
b)
lose electrons
49.

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

50.

Which type of bond is formed from the sharing of electrons?

a)

ionic bond

b)

covalent bond

51.

What set of elements is most likely to form a covalent compound?

a)

Na and O

b)

Na and K

c)

O and C

52.

Which set of elements is most likely to form an ionic compound?

a)

Na and O

b)

C and O

c)

Na and K

53.

Melted and dissolved compound conducts electricity.

a)

ionic compound

b)

covalent compound

54.

Have very strong intermolecular forces

a)

ionic compounds

b)

covalent compounds

55.

Which of the following describes covalent bonds?

a)

Bonds form because of opposite charges

b)

electrons are shared to fill outer electron shells

c)

Electrons are transferred between atoms

d)

Covalent bonds are magical

56.
Ionic Bonding involves...
a)
The transfer of protons
b)
The transfer of nuetrons 
c)
The transfer of electrons
d)
None Of the above
57.
What elements generally make an ionic bond?
a)
metal and nonmetal
b)
2 or more nonmetals
c)
metal
d)
none of the above
58.

Why do atoms form bonds?

a)

to increase their potential energy by filling up their valence shell

b)

to lower their potential energy by filling up their valence shell

c)

to increase their atomic number

59.

Which of the following is a covalent compound?

a)

CaO

b)

NaCl

c)

MgCl2

d)

CH4

60.

Is the following compound ionic or covalent?

LiBr

a)

Ionic

b)

Covalent

61.

Is the following compound ionic or covalent?

PBr5

a)

Ionic

b)

Covalent

62.

Is the following compound ionic or covalent?

A material with a high melting point

a)

Ionic

b)

Covalent

63.

Is the following compound ionic or covalent?

A material that is hard and brittle

a)

Ionic

b)

Covalent

64.

Is the following compound ionic or covalent?

A material that LOSES and GAINS electrons

a)

Ionic

b)

Covalent

65.

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.

66.
The reason that a sodium atom bonds with a chlorine atom is because
a)
Sodium transfers an electron to Chlorine
b)
oppositely charged ions form a strong electrostatic attraction
c)
ions are the same size
d)
the ions have a full outer shell
67.
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.
68.
There are more metals than non metals in the periodic table.
a)
True
b)
False
69.
At room temperature, most metals are
a)
liquid
b)
solid
c)
gas
d)
an alloy
70.
What does malleable mean?
a)
able to be shaped
b)
will break easily
c)
can be used for wire
d)
is shiny
71.
Which of these is NOT an alloy?
a)
bronze
b)
copper
c)
brass
d)
stainless steel
72.

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

a)

Malleability

b)

Ductility

c)

Conductivity

d)

Solubility

73.
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
74.
A mixture of two or more metals is called:
a)
mixture
b)
solution
c)
compound
d)
alloy
75.
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
76.

Which of the following is an alloy?

a)

stainless steel

b)

chromium

c)

nickel

d)

lead

77.
Metallic bonding is...
a)
a type of covalent bond.
b)
a type of ionic bond.
c)
an attraction between positive ions and electrons.
78.
What is the ability of a substance to allow heat, sound, or electricity to flow through it?
a)
Malleability
b)
Ductility
c)
Solubility
d)
Conductivity
79.

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

80.
I can hit a metal with a hammer without the metal shattering because of its __________.
a)
Ductility
b)
Malleability
c)
Conductivity
d)
Lustrousness
81.
Why are alloys generally used to make everyday objects?
a)
Alloys are often stronger and less active than pure metals.
b)
Alloys have higher melting point than pure metals.
c)
Alloys are less expensive to produce than pure metals.
d)
Alloys have ionic bonds instead of metallic bonds.
82.
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.
83.
There are more metals than non metals in the periodic table.
a)
True
b)
False
84.
What does malleable mean?
a)
able to be shaped
b)
will break easily
c)
can be used for wire
d)
is shiny
85.
Which of these is NOT an alloy?
a)
bronze
b)
copper
c)
brass
d)
stainless steel
86.
What is the ability of a substance to be pulled into a thin strand?
a)
Malleability
b)
Ductility 
c)
Conductivity
d)
Solubility
87.
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
88.
A mixture of two or more metals is called:
a)
mixture
b)
solution
c)
compound
d)
alloy
89.
Which of the following is an alloy?
a)
sterling silver
b)
chromium
c)
nickel
d)
lead
90.
Metallic bonding is...
a)
a type of covalent bond.
b)
a type of ionic bond.
c)
an attraction between positive ions and electrons.
91.
Electrons that are free to move in metals
a)
delocalized electrons
b)
oxidation number
c)
chemical bond
d)
salts
92.
What is the ability of a substance to be rolled or pounded into a thin sheet?
a)
Malleability
b)
Ductility
c)
Conductivity
d)
Solubility
93.
What is the ability of a substance to allow heat, sound, or electricity to flow through it?
a)
Malleability
b)
Ductility
c)
Solubility
d)
Conductivity
94.

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

95.

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"

96.

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

97.

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

98.
There are more metals than non metals in the periodic table.
a)
True
b)
False
99.
At room temperature, most metals are
a)
liquid
b)
solid
c)
gas
d)
an alloy
100.
I can hit a metal with a hammer without the metal shattering because of its __________.
a)
Ductility
b)
Malleability
c)
Conductivity
d)
Lustrousness
101.
In metals, the _______ electrons form a shared sea of electrons.
a)
Metallic
b)
Inner
c)
Outer
d)
Ionic
102.
What do metals conduct?
a)
heat
b)
electricity
c)
both
d)
neither
103.
In general, what can be said of the melting points of metals?
a)
They are low.
b)
They are high.
c)
They are lower than nonmetals.
d)
They do not have melting points.
104.
Why are alloys generally used to make everyday objects?
a)
Alloys are often stronger and less active than pure metals.
b)
Alloys have higher melting point than pure metals.
c)
Alloys are less expensive to produce than pure metals.
d)
Alloys have ionic bonds instead of metallic bonds.
105.
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
106.
NH4NO3
a)
soluble
b)
insoluble
107.
AgCl
a)
soluble
b)
insoluble
108.
NaCl
a)
soluble
b)
insoluble
109.
K2SO4
a)
soluble
b)
insoluble
110.
FeS
a)
soluble
b)
insoluble
111.
Ca(OH)2
a)
soluble
b)
insoluble
112.
BaSO4
a)
soluble
b)
insoluble
113.
NaC2H3O2
a)
soluble
b)
insoluble
114.
K2CO3
a)
soluble
b)
insoluble
115.
CaCO3
a)
soluble
b)
insoluble
116.
KBr
a)
Soluble
b)
Insoluble
117.
Zinc Hydroxide
a)
Soluble 
b)
Insoluble
118.
Silver Iodide
a)
Soluble 
b)
Insoluble 
119.
Zinc Carbonate
a)
Soluble 
b)
Insoluble 
120.
KOH
a)
Soluble 
b)
Insoluble
121.
Silver acetate
a)
Soluble 
b)
Insoluble
122.
NiCl2
a)
Soluble 
b)
Insoluble
123.
PbI2
a)
Soluble
b)
Insoluble
124.
NaC2H3O2
a)
soluble
b)
insoluble
125.
K2CO3
a)
soluble
b)
insoluble
126.
CaCO3
a)
soluble
b)
insoluble
127.
BaSO4
a)
soluble
b)
insoluble
128.
Ca(OH)2
a)
soluble
b)
insoluble
129.
FeS
a)
soluble
b)
insoluble
130.
K2SO4
a)
soluble
b)
insoluble
131.
AgCl
a)
soluble
b)
insoluble
132.
NH4NO3
a)
soluble
b)
insoluble
133.

What of these is always soluble?

a)

Nitrates

b)

Phosphates

c)

Carbonates

d)

Hydroxides

134.
BaCl2
a)
soluble
b)
insoluble
135.
Fe(C2H3O2)3
a)
soluble
b)
insoluble
136.

Which factor affecting solubility is shown in the picture?

a)

temperature

b)

height

c)

stirring

d)

particle size

137.

Which factor is shown in the picture?

a)

temperature

b)

particle size

c)

stirring

d)

use of spoon

138.

Why do sugar particles dissolve faster in hot water?

a)

water particles move slow

b)

water particles move fast

c)

water particles settle down

d)

water particles stay on top

139.

How does particle size affect solubility?

a)

bigger particles dissolve faster

b)

smaller particles can occupy the space in water faster

c)

bigger particles spread faster than smaller particles

140.

What are the factors that affect solubility?

a)

rate of stirring

b)

particle size

c)

temperature

d)

all of these

141.

Which of the following does not affect solubility of solutes?

a)

Tempearture

b)

Color

c)

Size particles

d)

Kind of solute

142.
In a solid to liquid mixture, an increase in temperature means...
a)
increase in solubility
b)
decrease in solubility
143.
Stirring the solution increases or decreases the solubility?
a)
increases
b)
decreases
144.

Which will dissolve faster crushed table salt or crystal of table salt?

a)

crushed table salt

b)

crystal of table salt

145.

What combination would dissolve a solid solute the fastest?

a)

high temperature, no stirring

b)

no heat, no stirring

c)

sugar cube, no heat

d)

high temperature, stirring

146.

What would dissolve most slowly?

a)

Large crystals in stirred water

b)

Large crystals in unstirred water

c)

Small crystals in stirred water

d)

Small crystals in unstirred water

147.

Is shaking increases the solubility of a solution?

a)

Yes

b)

No

c)

Maybe

148.

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 moving electrons.

149.
At room temperature, most metals are
a)
liquid
b)
solid
c)
gas
d)
an alloy
150.
What is the ability of a substance to be pulled into a thin strand?
a)
Malleability
b)
Ductility 
c)
Conductivity
d)
Solubility
151.

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"

152.

Electrons that are free to move in metals are called (a)   electrons

153.

Why do metals conduct electricity?

a)

They are shiny

b)

The electrons are delocalised and able to move

c)

The electrons are held tightly within the lattice

d)

The electrons are shared between two metal ions

154.

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

155.

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

156.

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

157.
I can hit a metal with a hammer without the metal shattering because of its __________.
a)
Ductility
b)
Malleability
c)
Conductivity
d)
Lustrousness
158.
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
159.
A mixture of two or more metals is called:
a)
mixture
b)
solution
c)
compound
d)
alloy

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