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C2 Bonding, structure, and the properties of matter

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Last updated 25 days ago
166 questions
4.2.1.1 Chemical Bonds
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4.2.1.2 Ionic Bonding
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4.2.1.3 Ionic Compounds
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4.2.1.4 Covalent Bonding
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4.2.1.5 Metallic Bonding
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4.2.2.1 The Three states of Matter
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4.2.2.2 State Symbols
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4.2.2.3 Properties of Ionic Compounds
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4.2.2.4 Properties of small molecules
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4.2.2.5 Polymers
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4.2.2.6 Giant Covalent Structures
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4.2.2.7 Properties of Metals and Alloys and 4.2.2.8 Metals as Condudctors
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4.2.3 Structure and bonding of carbon
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4.2.4 Bulk and surface properties of matter including nanoparticles
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Question 1
1.

Draggable itemarrow_right_altCorresponding Item
Covalent bonding
arrow_right_alt
Transferring electrons
Metallic bonding
arrow_right_alt
Sharing electrons
Ionic bonding
arrow_right_alt
Delocalised electrons through structure
Alloy
arrow_right_alt
Mixture of a metal and another element
Question 2
2.

Draw the ion formed from the Li atom

Question 3
3.

Draw the ion formed from the Na atom

Question 4
4.

Draw the ion formed from the K atom

Question 5
5.

Draw the ion formed from the F atom

Question 6
6.

Draw the ion formed from the Cl atom

Question 7
7.

What type of bonding is shown in the video below? ALSO, explain how you know.

Question 8
8.

What is the ion formed when Magnesium (Atomic Number: 12) loses two electrons?

Question 9
9.

Draw dot and cross diagram - Calcium sulfide

Question 10
10.

Draw electron configuration diagrams to show how an atom of lithium becomes an ion

Question 11
11.

Potassium is in Group 1. How many electrons does it lose when it becomes an ion?

Question 12
12.

What kind of bonding is this?


Question 13
13.

What is the ion formed by Sodium (Na)?

Question 14
14.

What is the ion formed by Oxygen (O)?

Question 15
15.

What ion does Calcium (Ca) form?

Question 16
16.

What ion does Fluorine (F) form?

Question 17
17.

Which ion has a 2+ charge?

Question 18
18.

What is the ion formed when Magnesium (Atomic Number: 12) loses two electrons?

Question 19
19.

Draw the ion formed from the Li atom

Question 20
20.

Draw the ion formed from the Na atom

Question 21
21.

Draw the ion formed from the K atom

Question 22
22.

Draw the ion formed from the F atom

Question 23
23.

Draw the ion formed from the Cl atom

Question 24
24.

Lithium LOSES an electron (electrons are negative). What charge does it have?

Question 25
25.

Beryllium LOSES two electrons (electrons are negative). What charge does it have?

Question 26
26.

Magnesium LOSES two electron (electrons are negative). What charge does it have?

Question 27
27.

Fluorine GAINS an electron - what charge does it have?

Question 28
28.

Draw dot and cross diagram - Lithium fluoride

Question 29
29.

Draw dot and cross diagram - Magnesium chloride

Question 30
30.

Draw dot and cross diagram - Lithium Oxide

Question 31
31.

Draw dot and cross diagram - Calcium sulfide

Question 32
32.

Why do metals form positive ions, while non-metals form negative ions?

Question 33
33.

Use dot and cross diagram to show the electronic changes that occur during the reaction between calcium and fluorine.

Question 34
34.

Match the formulas of the following ionic compounds to their names.

Draggable itemarrow_right_altCorresponding Item
Mg3N2
arrow_right_alt
Sodium sulfide
MgO
arrow_right_alt
Potassium chloride
Na2S
arrow_right_alt
Magnesium oxide
KCl
arrow_right_alt
Lithium sulfide
Li2S
arrow_right_alt
Magnesium nitride
Question 35
35.

Match the names of the following ionic compounds to their formulas.

Draggable itemarrow_right_altCorresponding Item
Sodium oxide
arrow_right_alt
Be3P2
Rubidium bromide
arrow_right_alt
RbBr
Potassium nitride
arrow_right_alt
Na2O
Aluminum chloride
arrow_right_alt
AlCl3
Beryllium phosphide
arrow_right_alt
K3N
Question 36
36.

What is the formula for lithium sulfide?

Question 37
37.

What is the formula for potassium bromide?

Question 38
38.

What is the formula for beryllium nitride?

Question 39
39.

What is the formula for aluminum sulfide?

Question 40
40.

What is the formula for sodium phosphide?

Question 41
41.

When atoms gain or lose electrons, they do not form ions

Question 42
42.

When Li loses an electron, it becomes Li+1

Question 43
43.

Draw electron configuration diagrams to show how an atom of lithium becomes an ion

Question 44
44.

Draw electron configuration diagrams to show how an atom of fluorine becomes an ion

Question 45
45.

Potassium - Use your periodic table to find the number of electrons

Question 46
46.

Draw the atom Boron and how it becomes the ion B+3

Question 47
47.
In a giant ionic structure, there are strong electrostatic forces in all directions between _______ charged particles.
Question 48
48.
  • Ionic Compounds
  • Simple Molecules
Question 49
49.

How are these compounds classified?

  • Methane
  • Magnesium Oxide
  • Sodium Chloride
  • Carbon Dioxide
  • Small Covalent Compounds
  • Ionic Compounds
Question 50
50.

Describe the difference between an ionic and covalent bond.

Question 51
51.

Complete the figure below to show the outer shell electrons in a molecule of Si2H6

Question 52
52.

Give one limitation of using a dot and cross diagram to represent a molecule.

Question 53
53.

What kind of chemical bonding is taking place with Bromine?

Question 54
54.

This is Hydrogen Cyanide and it follows all the rules of covalent bonding. Use your knowledge of covalent bonding to complete the diagram. (Grade 7/8 Bonding Question)

Question 55
55.

How are these compounds classified?

  • Methane
  • Magnesium Oxide
  • Sodium Chloride
  • Carbon Dioxide
  • Small Covalent Compounds
  • Ionic Compounds
Question 56
56.

Describe the difference between an ionic and covalent bond.

Question 57
57.

The chlorine molecule forms a single bond. Please complete the diagram

Question 58
58.

A chemical bond formed when two atoms share one or more pairs of valence electrons.

Question 59
59.

Which one has the stronger bond?

Question 60
60.

Which of the following is a covalent compound?

Question 61
61.

How many valence electrons are shared in each covalent bond?

Question 62
62.

What kind of bonding is this?

Question 63
63.

In a metallic bond, where are the electrons located?

Question 64
64.

Give the definition of metallic bonding ( 1 mark)

Question 65
65.

Question 66
66.

Question 67
67.

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Question 70
70.

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Question 71
71.

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Question 72
72.

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Question 76
76.

What is the state of matter that has a definite shape and volume?

Question 77
77.

Which of the following are states of matter?

Question 78
78.

Water can exist in all three states of matter (solid, liquid, gas).

Question 79
79.

Can you give an example of a gas that you breathe in?

Question 80
80.

Ice is the solid state of water.

Question 81
81.

Drag the characteristics or details to the correct state of matter.

  • has a definite volume but no defined shape
  • has a volume that can change
  • are somewhat close together but can move freely
  • particles collide and move everywhere
  • particles vibrate in a fixed position
  • has a defined shape and volume
  • Solid
  • Liquid
  • Gas
Question 82
82.

What is matter with a definite shape and definite volume?

Question 83
83.

What is matter that has a definite volume, but NOT a definite shape.

Question 84
84.

Type the name for each change of state next to the letter that represents this change on the diagram below

Question 85
85.

Substances are usually the most dense when they are in the solid state.

Question 86
86.

Which of the following is NOT true? As thermal energy is added to a substance...

Question 87
87.

If a substance cools down, its molecules

Question 88
88.

If a substance heats up, its molecules

Question 89
89.

Question 90
90.

Question 91
91.

Question 92
92.

Why don’t covalent compounds conduct electricity?

Question 93
93.

Why are ionic substances soluble in water?

Question 94
94.

Why don’t covalent compounds conduct electricity?

Question 95
95.

Why do ionic compounds have high melting and boiling points?

Question 96
96.

Why are most ionic compounds soluble in water?

Question 97
97.

In our practical, did ionic compounds dissolve in water and become soluble?

Question 98
98.

Did the ionic compounds conduct electricity?

Question 99
99.

Did the ionic compounds have high or low melting points?

Question 100
100.

Match keyword to definition

Draggable itemarrow_right_altCorresponding Item
melting point
arrow_right_alt
A measure of how well a material conducts electricity.
thermal conductivity
arrow_right_alt
A measure of how well a material transfers energy when heated.
electrical conductivity
arrow_right_alt
Temperature at which a substance changes from solid to a liquid state.
Solubility
arrow_right_alt
A particle that enables electrical conductivity.
charge carrier
arrow_right_alt
How well a solute dissolves in a solvent
Question 101
101.

Which of the following ionic substances is not a good electrical conductor?

Question 102
102.

Why do ionic compounds have high melting and boiling points?

Question 103
103.

Why are most ionic compounds soluble in water?

Question 104
104.

Why is the melting point of magnesium oxide, MgO, higher than sodium chloride, NaCl?

Question 105
105.

Why don’t covalent compounds conduct electricity?

Question 106
106.

Why are ionic substances soluble in water?

Question 107
107.

What are the properties of ionic substances?

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Question 111
111.

Why do ionic compounds have higher melting points than simple covalent compounds?

Question 112
112.

Which of these is the property of ionic and small covalent molecules?

  • Does Not Conduct Electricity
  • Conducts Electricity when Dissolved
  • Forms Giant Ionic Lattice
  • High Melting Point
  • Low Melting Point
  • Usually Gas or Liquid
  • Small Covalent Molecule Properties
  • Ionic Properties
1
Question 113
113.

Giant structure or simple molecule?

1
Question 114
114.

Giant structure or simple molecule?

1
Question 115
115.

Giant structure or simple molecule?

Question 116
116.

Why do ionic compounds have higher melting points than simple covalent compounds?

Question 117
117.

Which of these is the property of ionic and small covalent molecules?

  • Does Not Conduct Electricity
  • Conducts Electricity when Dissolved
  • Forms Giant Ionic Lattice
  • High Melting Point
  • Low Melting Point
  • Usually Gas or Liquid
  • Small Covalent Molecule Properties
  • Ionic Properties
Question 118
118.

Poly(ethene) is produced from ethene.
The structure of ethene is:



Complete the structure of poly(ethene)

Question 119
119.
Complete the missing parts of the sentence

Polymers are _______ molecules made up of smaller, repeating units. Each smaller individual molecule is called a _______ and they join together in a process called _______ .
Question 120
120.

Which state of matter are most polymers at room temperature

1
Question 121
121.

Giant structure or simple molecule?

1
Question 122
122.

Giant structure or simple molecule?

1
Question 123
123.

Giant structure or simple molecule?

1
Question 124
124.

Giant structure or simple molecule?

Question 125
125.

Properties

  • Never conduct electricity
  • Almost never conduct electricity
  • Solids
  • Low melting and boiling points
  • Very high melting points
  • Gases or liquids
  • Giant Covalent Structures
  • Small Covalent Molecules
1
Question 126
126.

(a)Explain why silicon dioxide has a high melting point. (2 marks)

1
Question 127
127.

(a)Suggest why the melting point of silicon dioxide is higher than the melting point of sodium chloride. (1 mark)

1
Question 128
128.

(a)State why sodium chloride conducts electricity when molten. (1 mark)

Question 129
129.

Sort the covalent compounds

  • Silicon Dioxide
  • Water
  • Graphite
  • Hydrogen
  • Diamond
  • Oxygen
  • Giant Covalent Structure
  • Small Covalent Molecules
Question 130
130.

Which of these are giant covalent structures?

Question 131
131.

Giant covalent structures are not as strong as small covalent molecules due to their smaller size.

Question 132
132.

Giant covalent structures like diamond, graphite, and silicon dioxide generally have high melting and boiling points.

Question 133
133.

All giant covalent structures are insulators, as they cannot conduct electricity.

Question 134
134.

Which is NOT a common property of alloys?

Question 135
135.

Match the vocabulary terms to their definitions

Draggable itemarrow_right_altCorresponding Item
Malleabitilty
arrow_right_alt
Means a substance can be pounded or hammered into thin sheets. (can bend)
Ductility/Ductile
arrow_right_alt
means if an object can transfer heat or electricity
Physical State
arrow_right_alt
How an object reflects light
Luster
arrow_right_alt
How the surface of an object looks or feels
Texture
arrow_right_alt
if a substance can be made in to thin wire
Conductivity
arrow_right_alt
Refers to if an object is a solid, liquid or gas
Question 136
136.

Explain why metals can conduct electricity and are malleable? (2 marks)

Question 137
137.

What is the primary reason metals are good conductors of electricity?

Question 138
138.

What is an alloy?

Question 139
139.

Why do alloys typically have more advantageous properties than pure metals?

Question 140
140.

Match the property to the right type of covalent structure.

Draggable itemarrow_right_altCorresponding Item
Low melting and boiling points
arrow_right_alt
Giant covalent structures
High melting and boiling points
arrow_right_alt
Diamond
Does not conduct electricity
arrow_right_alt
Small covalent molecules
Question 141
141.

Which of the following properties do these structures hold in terms of their hardness?

  • Methane
  • Diamond
  • Graphite
  • Silicon dioxide
  • Hard
  • Soft
Question 142
142.

Match the property to the appropriate covalent form.

Draggable itemarrow_right_altCorresponding Item
Conducts electricity
arrow_right_alt
Graphite
Low hardness
arrow_right_alt
Small covalent molecules
Extremely hard and strong
arrow_right_alt
Diamond
Question 143
143.

Match the covalent structure with the correct description about structure.

Draggable itemarrow_right_altCorresponding Item
Layers can slide over each other
arrow_right_alt
Carbon nanotube
Form three-dimensional network
arrow_right_alt
Graphite
Regular network of carbon atoms in a hexagonal pattern
arrow_right_alt
Diamond and silicon dioxide
Question 144
144.

Match each statement with the right covalent structure(s).

Draggable itemarrow_right_altCorresponding Item
Usually gases or liquids at room temperature
arrow_right_alt
Small covalent molecules
Not soluble in water
arrow_right_alt
Giant covalent structures
Hard, lustrous and have high thermal conductivity
arrow_right_alt
Diamond
Question 145
145.

What is a distinctive feature of the structure of diamond?

Question 146
146.

Why can graphite conduct electricity?

Question 147
147.

Graphite and other giant covalent structures are easily dissolved in water.

Question 148
148.

What is this?

1
Question 149
149.

1a:

1
Question 150
150.

1b:

Question 151
151.

Which of the following is a correct conversion in the metric
system?

Question 152
152.

Which of the following values could describe the size of a
nanoparticle?

1
Question 153
153.

What is the surface area for the first cube?

1
1
1
1
1
Question 159
159.

How does the surface area to volume ratio change when a bulk
material is split into smaller nanoparticles?

Question 160
160.
Question 161
161.
Calculate the surface area to volume ratio for a nanoparticle that is a
cube with a side length of 15 nm, and one of 60 nm. No units are required

Surface area 1 = _______
Volume 1 = _______
SA:V 1 = _______

Surface area 2 = _______
Volume 2 = _______
SA:V 2 =_______
Question 162
162.

The properties of nanoparticles are identical to those of the same materials in
bulk form.

Question 163
163.

Justify your above answer

Question 164
164.

Titanium dioxide nanoparticles are used in sunscreen,
and silver nanoparticles are used in socks. Explain how the properties of these
nanoparticles makes them suitable for each application.

Question 165
165.

Consider the potential risks associated with the inhalation of nanoparticles.

Describe and explain what those risks could be.

Describe how society might address the use of nanoparticles in industry.

Question 166
166.

Explain how a high surface area to volume ratio of a substance used
as a catalyst affects the reactivity of particles.

Question 68
68.

What happens to particles in a solid when energy is added?

Question 69
69.

How do particles behave in a gas compared to a liquid?

Question 73
73.

Question 74
74.

Question 75
75.

Question 108
108.

What is the name of this compound?

Question 109
109.

What type of forces acts between the ions in an ionic compound?

Question 110
110.

What are two properties of ionic compounds?

Question 154
154.

What is the volume for the first cube?

Question 155
155.

What is the SA:V for the first cube?

Question 156
156.

What is the surface area for the second cube?

Question 157
157.

What is the volume for the second cube?

Question 158
158.

What is the SA:V for the second cube?