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Y9 Bonding Revision

Total questions: 113

Worksheet time: 1hrs 17mins

Name
Class
Date
1.
Which consists of carbon atoms?
a)
graphite
b)
diamond
c)
fullerene
d)
all of these
2.
Which has a 2D hexagonal layered structure?
a)
graphite
b)
diamond
c)
fullerene
d)
all of these
3.
Which has a every carbon atom covalently bonded to three others?
a)
graphite
b)
diamond
c)
fullerene
d)
two of these
4.
What structure is shown in the diagram?
a)
Diamond
b)
Graphite
5.
Which has weak dispersion forces in between layers?
a)
graphite
b)
diamond
c)
fullerene
d)
none of these
6.
Which has a free delocalized electron between layers that gives rise to electrical conductivity ?
a)
graphite
b)
diamond
c)
fullerene
d)
none of these
7.
Which is used in pencils ?
a)
graphite
b)
diamond
c)
fullerene
d)
none of these
8.
Which is used as electrodes in an electrochemical cell?
a)
graphite
b)
diamond
c)
fullerene
d)
none of these
9.
Which has a 3D hexagonal structure?
a)
graphite
b)
diamond
c)
fullerene
d)
none of these
10.
Which has every carbon atom covalently bonded to four other atoms?
a)
graphite
b)
diamond
c)
fullerene
d)
none of these
11.
Which is extremely hard?
a)
graphite
b)
diamond
c)
fullerene
d)
none of these
12.
Which is used as a cutting tool and in jewelry?
a)
graphite
b)
diamond
c)
fullerene
d)
none of these
13.
Which has the formula C60?
a)
graphite
b)
diamond
c)
fullerene
d)
none of these
14.
Which is made of balls or cages of carbon?
a)
graphite
b)
diamond
c)
fullerene
d)
none of these
15.
Which is a semiconductor?
a)
graphite
b)
diamond
c)
fullerene
d)
none of these
16.
Define the term allotropes
a)
Atoms with same proton number but different number of neutrons
b)
Atoms with same proton number but different mass number
c)
Atoms in different arrangement in structure
d)
Atoms in different arrangement and different physical form
17.
What kind of bonding does atoms in graphite has?
a)
Covalent bonding with all atoms
b)
Each carbon, bonded covalently to 3 other carbon atoms in a 3D lattice
c)
Each carbon, bonded covalently to 4 other carbon atoms.
d)
Each carbon, bonded covalently to 3 other carbon atom in 2D held by intermolecular
18.
Which of the following is true about C60 ?
a)
Each carbon bonded covalently to 3 other carbon atoms in a hexagonal ball like structure
b)
Each carbon bonded covelently to 4 other carbon atoms in layers
c)
a giant lattice structure
d)
pentagonal in shape
19.
What structure is shown in the diagram?
a)
Diamond
b)
Graphite
c)
fullerene
20.
Which statement is a true comparison of diamonds and graphite?
a)
diamonds are extremely hard and colorless where as graphite is a very soft gray substance. 
b)
diamonds are extremely soft and colorless where as graphite is a very hard gray substance.
c)
Diamonds are made only from carbon where as graphite is a carbon compound containing metal electrons
21.
which answer shows the correct number of C-C covalent bonds in its allotropes? 
a)
Diamond 3, Graphite 3, fullerene 3
b)
Diamond 4, Graphite 3, fullerene 3
c)
Diamond 4, Graphite 3, fullerene 4
d)
Diamond 4, Graphite 4, fullerene 3
22.

Which of the following names matches the chemical formula N2O3?

a)

Dinitrogen triople oxide

b)

Nitrogen oxide

c)

Dinitrogen trioxide

d)

Trioxide nitrogen

23.

What is the correct chemical formula for phosphorus trihydride?

a)

P2H3

b)

P4H2

c)

PH3

d)

P3H3

24.

Which of the following is the chemical formula for sulfur hexachloride?

a)

SCl6

b)

S6Cl

c)

S6Cl6

d)

S1Cl6

25.
When an atom loses an electron, it becomes a:
a)
positive ion
b)
negative ion
c)
neutral ion
d)
neutral atom
26.
Which of the following is NOT a property of ionic compounds?
a)
They have very high melting points
b)
They conduct electricity when in solution
c)
They have high boiling points
d)
They are insoluble in water
27.
How are covalent bonds explained?
a)
When one atom takes the other atom's electron
b)
When the atom shares an electron with an another atom
c)
When the two nucleus merge
d)
When the neutrons leave the nucleus
28.
Where are the nonmetals located on the periodic table? 
a)
Blue
b)
Red
c)
Green
29.
What is the correct formula for this molecule?
a)
NH
b)
N3H
c)
NH3
d)
NH4
30.
Ionic bonds exist between a metal with a non-metal.
a)
True
b)
False
31.
Magnesium (Mg) and Oxygen (O) form an ________ bond.
a)
Ionic
b)
Covalent
c)
Metallic
d)
Nothing
32.
Calcium (Ca) and 2 chlorine (Cl) atoms make a covalent compound.
a)
True
b)
False
33.

What usually forms the negative ion?

a)

nonmetals

b)

metal

c)

none

34.
Which of the following is NOT formed by a covalent bond?
a)
K2S
b)
H2O
c)
I2
d)
CO2
35.

Simple molecular molecules generally have

a)

low melting and boiling points

b)

high melting and boiling points

c)

ionic bonds

d)

metallic bonds

36.

Which structures conduct electricity as a liquid but not as a solid?

a)

Metallic

b)

Covalent

c)

Ionic

d)

All of the above

37.

Which structure has a sea of free electrons?

a)

Ionic

b)

Covalent

c)

Metallic

d)

All of the above

38.
What is an atom or group of atoms that has an electric charge?
a)
ion
b)
metal
c)
nonmetal
d)
ionic compound
39.
If a potassium atom loses one electron, a positive ion results.
a)
TRUE
b)
FALSE
40.
Which of the following describes covalent bonds?
a)
Bonds form because of opposite charges
b)
Bonds form to fill outer electron shells
c)
Electrons are transferred between atoms
d)
Covalent bonds are magical
41.

Covalent bonds are formed between...

a)

two or more metal atoms

b)

two or more non-metal atoms

c)

a metal and a non-metal atom

42.

Covalent bonds are formed when electrons are transferred between atoms.

a)

True

b)

False

43.

Atoms can only share electrons in the (a)   shell.

44.

Fluorine is a diatomic molecule. Fluorine is in Group 7. How many electrons are shared in this covalent bond?

(a)  

45.

Oxygen is a diatomic molecule. Oxygen is in Group 6. How many electrons are shared in this covalent bond?

(a)  

46.

The structure of ammonia is shown in the diagram. What is the formula for ammonia?

a)

NH3

b)

HN3

c)

N3H

d)

HN3

47.

What are the disadvantages of using displayed formulae, like the one shown?

a)

The 3D structure of the molecule is not shown.

b)

They can show how atoms are bonded in large molecules.

c)

They do not show which atom each electron comes from.

d)

They can be used to find the structural formula of the molecule.

48.

Select the properties of simple covalent substances.

a)

Low melting and boiling points.

b)

High melting and boiling points.

c)

Do not conduct electricity.

d)

Good conductors of electricity.

49.

Why do simple covalent substances not conduct electricity?

a)

They have low melting points.

b)

They have low boiling points.

c)

There are no delocalised electrons or free ions to carry the charge.

d)

The molecules are too large.

50.

Covalent structures have low melting and boiling points because it does not take much energy to break the _____ intermolecular forces.

a)

weak

b)

strong

51.
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
52.
How are covalent bonds explained?
a)
When one atom takes the other atom's electron
b)
When the atom shares an electron with an another atom
c)
When the two nucleus merge
d)
When the neutrons leave the nucleus
53.
What region of the periodic table contains atoms that form covalent bonds?
a)
the left side
b)
the middle
c)
the right side
d)
top left
54.
Is carbon considered a metal or a non-metal?
a)
metal
b)
nonmetal
c)
other
55.
What can be generalized about covalent bonds?
a)
Electrons will be exchanged.
b)
Electrons will be transferred.
c)
Electrons will be given and taken.
d)
Electrons will be shared.
56.
What is it called if there are three-pairs of electrons being shared?
a)
Triple bond
b)
Bond length
c)
Tribond
d)
Chocolate Mousse
57.
What two types of atoms make a covalent bond?
a)
2 Nonmetals
b)
1 Nonmetal & 1 Metal
c)
2 Metals
d)
2 Noble Gases
58.
How many electrons are shared in a double bond?
a)
2
b)
4
c)
6
d)
8
59.

What is it called if there are two-pairs of electrons being shared?

a)

Single covalent bond

b)

Double covalent bond

c)

Triple covalent bond

d)

None of the above

60.

What is it called if there is one-pair of electrons being shared?

a)

Single covalent bond

b)

Double covalent bond

c)

Triple covalent bond

d)

None of the above

61.

How many electrons are bonded to the C atom on the left?

(a)  

62.

How many electrons are there surrounding/bonded to the P atom?

(a)  

63.

How many electrons are bonded to the S atom in the above structure of methane-sulphonic acid?

(a)  

64.
The word "nano" means:
a)
one millioneth
b)
one billioneth
c)
one thousandth
d)
one trillioneth
65.

Which 2 of the following technologies are currently made using nanotechology?

a)

odor-free socks

b)

vegetarian meatballs

c)

vaccinations

d)

wrinkle-resistant fabrics

66.
Nanotechnology allows the manipulation of atoms or molecules to create or modify materials at the nanoscale.
a)
True
b)
False
67.

What is nanotechnology?

a)

Study and manipulation of technology that is micro sized

b)

Study and manipulation of matter that is small but can still be seen by the human eyes

c)

Study and manipulation of matter at a scale of 1-100 nano meters

d)

Study and manipulation of matter that moves at a speed measured in nano seconds

68.
What is a buckyball?
a)
A carbon atom (C60)
b)
Nickname for Mercedes-Benz's futuristic concept car (C111)
c)
Plastic explosives nanoparticle (C4)
d)
Concrete nanoparticle with a compressive strength of 20 nanonewtons (C20)
69.

Why the properties of nanomaterials are different significantly compared to bulk materials?

a)

Increased relative surface area

b)

Decreased relative surface area

c)

Increased lattice parameters

d)

Lower down the melting temperature

70.
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.
71.
There are more metals than non metals in the periodic table.
a)
True
b)
False
72.
At room temperature, most metals are
a)
liquid
b)
solid
c)
gas
d)
an alloy
73.
What does malleable mean?
a)
able to be shaped
b)
will break easily
c)
can be used for wire
d)
is shiny
74.
Which of these is NOT an alloy?
a)
bronze
b)
copper
c)
brass
d)
stainless steel
75.
Electrons that are free to move in metals
a)
delocalized electrons
b)
oxidation number
c)
chemical bond
d)
salts
76.
What is the ability of a substance to be pulled into a thin strand?
a)
Malleability
b)
Ductility 
c)
Conductivity
d)
Solubility
77.
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
78.
A mixture of two or more metals is called:
a)
mixture
b)
solution
c)
compound
d)
alloy
79.

Which of the following is an alloy?

a)

stainless steel

b)

chromium

c)

nickel

d)

lead

80.

Metallic bonding is...

a)

a type of covalent bond.

b)

a type of ionic bond.

c)

an attraction between positive ions and a sea of delocalised electrons.

81.
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
82.

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

83.
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.
84.

Name some household appliances that are made of metal. Why are metals chosen to make these appliances?

4 lines
85.

Which of these are properties of metals?

a)

ductile and malleable

b)

low melting or boil point

c)

high melting/boiling point

d)

conduct electricity

e)

soluble in water

86.

what charge do the metal ions have in metallic bonding?

a)

negative

b)

positive

c)

neutral

87.

what one word/phrase describes the electrons in metallic bonding

a)

delocalised

b)

swimming

c)

sea of electrons

d)

fixed

e)

flying

88.

Why do the electrons in metals move about freely?

a)

There are overlapping orbitals that allow outer electrons of atoms to move about freely throughout the entire

b)

Electrons are repelled

c)

Bonds are broken between electrons and cations

89.

Draw the structure of a metal.

90.

Metals have ​ (a)   melting and boiling points because of the ​ (b)   electrostatic forces of ​ between ​ (c)   ions and ​ (d)   electrons. A ​ (e)   amount of energy is required to break these forces.

Choose from the below words
high
strong
positive
delocalised
large
low
small
weak
fixed
91.

Metals are good conductors of heat...

a)

because they are shiny and reflect heat.

b)

because the absorb heat.

c)

the electrons are delocalised and able to move, colliding with cations to transfer themal energy.

d)

because the cations can move freely to transfer thermal energy.

92.

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

93.
The ability of a material to deform, usually by stretching along its length. This property allows us to make wires.
a)
conductivity
b)
ductility
c)
malleability
d)
hardness
94.
The ability of a material to be shaped in all directions without cracking or breaking.
a)
hardness
b)
ductility
c)
malleability
d)
conductivity
95.

Metals are ​ (a)   because when a metal is hit, the metallic layers ​ (b)   each other. The ​ (c)   electrons ​ (d)   along with the cations. The metallic bond ​ (e)   break.

Choose from the below words
malleable and ductile
slide over
delocalised
move
does not
brittle
repel
does
96.

Which name is given to mixtures of metals?

a)

Alloys

b)

Compounds

c)

Ores

d)

Salts

97.

Which two elements form an alloy when heated together?

a)

Chlorine and Hydrogen

b)

Chlorine and zinc

c)

Copper and hydrogen

d)

Copper and zinc

98.

Which diagram represents an alloy?

a)

A

b)

B

c)

C

d)

D

99.

What type of alloy does the diagram represent?

a)

interstitial

b)

substitution

100.
Elements on the LEFT side of the periodic table will most likely form:
a)
Positive ions
b)
Negative ions
c)
Neutral Ions
d)
None of these
101.
A mixture of two or more metals is called:
a)
mixture
b)
solution
c)
compound
d)
alloy
102.

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

103.
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
104.
What is the formula of Sodium oxide?
a)
Na2O
b)
NaO2
c)
Na2O2
d)
Na2O
105.

What is the name of the compound with the chemical formula CrCl3 ?

a)

chromium (III) chlorate

b)

chromium trichloride

c)

chromium(II) chloride

d)

chromium(III) chloride

106.

What is the correct chemical formula for sodium sulfate?

a)

NaSO4

b)

Na2SO4

c)

Na(SO4)2

d)

Na2(SO4)2

107.

A formula unit can best be described as

a)

the chemical formula for an ionic compound

b)

a charged group of covalently bonded atoms

c)

the chemical formula for a molecule

d)

the arrangement of ions in an ioinc crystal

108.

Which of the following pairs of elements would NOT react to form an IONIC compound?

a)

sulfur and phosphorus

b)

sodium and iodine

c)

iron and oxygen

d)

aluminum and bromine

109.
Ionic compounds are ordinarily found as
a)
plasma
b)
liquids
c)
gasses
d)
crystalline solids 
110.
What is the chemical formula for calcium nitrate?
a)
CaNO3
b)
Ca(NO2)2
c)
Ca(NO3)2
d)
Ca3N2
111.

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.

112.

Which of the following would have the lowest melting point?

a)

MgCl2

b)

Al2O3

c)

CO2

d)

AlP

113.

Nonmetals tend to form ions by

a)

destroying electrons

b)

gaining electrons

c)

losing electrons

d)

sharing electrons

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