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C1 Atomic Structure and Periodic Table

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Last updated about 1 month ago
236 questions
4.1.1.1 Atoms, Elements, and compounds
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4.1.1.2 Mixtures
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4.1.1.3 The Development of the model of the atom
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4.1.1.4 Relative electrical charges of subatomic particles
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4.1.1.5 Size and mass of atoms
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4.1.1.6 Relative Atomic Mass
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4.1.1.7 Electronic Structure
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4.1.2.1 The Periodic Table
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4.1.2.2 Development of the Periodic Table
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4.1.2.3 Metals and non-metals
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4.1.2.4 Group 0
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4.1.2.5 Group 1
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4.1.2.6 Group 7
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4.1.3 Properties of Transition Metals
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Question 1
1.

Question 2
2.

Give the element symbol for the following elements.
Question 3
3.

Copper

Question 4
4.

Fluorine

Question 5
5.

Gallium

Question 6
6.

Hydrogen

Question 7
7.

Indium

Give the element name that matches the symbol below.
Question 8
8.

Au

Question 9
9.

Ge

Question 10
10.

I (This is a capital "i")

Question 11
11.

He

Question 12
12.

W

Question 13
13.

What do we call a substance that cannot be broken down into simpler substances by chemical means?

Question 14
14.

Which term describes a substance composed of two or more elements that are chemically combined?

Question 15
15.

Made up of 2 or more different atoms bonded together.

Question 16
16.

Two or more atoms bonded together.

Question 17
17.

How many atoms make up this compound?

Question 18
18.

How many atoms of oxygen are there in Hâ‚‚Oâ‚‚

Question 19
19.

What is the correct name for NaCl?

Question 20
20.

What is the chemical name for the compound CaO?

Question 21
21.

The correct name for the compound KBr is?

Question 22
22.

What is the correct name for the compound MgBr2?

Question 23
23.

Question 24
24.
Other Answer Choices:
molecule
atom
Question 25
25.
Other Answer Choices:
Not an element
Element
Question 26
26.
Other Answer Choices:
Element
Molecule
Both!
Question 27
27.
Other Answer Choices:
Both!
Compound
Molecule
Question 28
28.

Question 29
29.

Tom mixed sand and water together for a science experiment. What is this combination called?

Question 30
30.

Which method is used to separate based on boiling point?

Question 31
31.

What is the process used to separate crystals?

Question 32
32.

Which technique is best for separating colored pigments in a substance?

Question 33
33.

What method is utilized to remove insoluble particles (solids) from a liquid?

Question 34
34.



Is the image above an image of an element, compound or mixture?

Question 35
35.

Is the image above an image of an element, compound or mixture?

Question 36
36.

Is the image above an image of an element, compound or mixture?

Question 37
37.

What is the main difference between a compound and a mixture?

Question 38
38.

What method of separation separates colours?

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Question 39
39.
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Question 41
41.
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Question 43
43.
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Question 45
45.
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Question 47
47.
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Question 49
49.

Question 50
50.

Question 51
51.

Question 52
52.

Question 53
53.

Question 54
54.

Draggable itemarrow_right_altCorresponding Item
arrow_right_alt
arrow_right_alt
arrow_right_alt
Question 55
55.

3
Question 56
56.

A chocolate chip cookie could be used as a model for JJ Thomson's theory of the structure of an atom.

Assess the model and write:

a) Two reasons it was a good model for JJ Thomson's theory
b) One reason why it is not a good model.

Question 57
57.

Draw and label a diagram for

a) John Dalton's model
b) JJ Thomson's model

Question 58
58.

Just like Rutherford, Jun is writing a conclusion from Geiger and Marsden's gold foil experiment. Help him write to explain the findings to show how the atomic model looked.

Jun needs to write:
a) The 3 different things that positive alpha particles did when fired at the gold foil
b) A conclusion for each of these findings
c) A description of the model of the atom that this new evidence provided

Question 59
59.

Which of these belong to the Plum Pudding Model and the Nuclear Model?

  • Contains protons
  • Contains only negative charges
  • Positive nucleus
  • Contains electrons
  • Ball of Positive charge
  • Electrons moving
  • Contains only positive charges
  • Contains opposite charges
  • Electrons embedded - not moving
  • Made up of mostly empty space
  • Negative nucleus
  • No nucleus
  • Ball of negative charge
  • Plum Pudding
  • Nuclear Model
  • Both
  • Neither
Question 60
60.

Question 61
61.

Draggable itemarrow_right_altCorresponding Item
arrow_right_alt
JJ Thomson
arrow_right_alt
Bohr
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Rutherford
arrow_right_alt
Dalton
arrow_right_alt
Chadwick
6
Question 62
62.

Compare the nuclear model to the current model, giving both similarities and differences.

Question 63
63.

Select two correct statements about Dalton’s model of atoms.

1
Question 64
64.

Which is the best representation of Dalton's model?

Question 65
65.

JJ Thomson said that there must be something smaller than an atom.

Question 66
66.

True! He said there was something smaller - what are they called?

1
Question 67
67.

Which image shows JJ Thomson’s model?

Question 68
68.

JJ Thomson’s model was called the currant bun model.

Question 69
69.

It was called the Plum Pudding model - why?

Question 70
70.

What happened to the alpha particles in Rutherford's gold foil experiment?

1
Question 71
71.

Which image shows Rutherford’s nuclear model?

1
Question 72
72.

Which image shows Bohr’s model?

Question 73
73.

What did later experiments show about the nucleus?

Question 74
74.

What subatomic particle did James Chadwick suggest existed?

Question 75
75.

Scientists noticed a difference in the atomic number and mass of an atom.

Question 76
76.

What is the charge of a proton?

Question 77
77.

Question 78
78.

Question 79
79.

What is the relative size of an electron?

Question 80
80.

What is the charge of a proton?

Question 81
81.

Why are atoms neutral? (hand mark)

Question 82
82.

What is the charge of a proton?

Question 83
83.

What is the relative size of an electron?

Question 84
84.

What is the relative size of an electron?

Question 85
85.

What is the charge of an ion formed when calcium loses 2 electrons?

Question 86
86.

Question 87
87.

Question 88
88.

Question 89
89.
Question 90
90.

What is the atomic number of carbon?

Question 91
91.

Which element has an atomic number of 11?

Question 92
92.

How many protons does Hydrogen (H) have in its nucleus?

Question 93
93.

What element in the periodic table has 8 protons?

Question 94
94.

What is the proton number of Helium (He)?

Question 95
95.

How many protons are in the nucleus of Carbon (C)?

Question 96
96.
Correct the information so that Lucas can submit his homework:

The atomic number tells you how many __________ are in the nucleus of an atom. Each element has a unique __________ number. The atomic number is always the __________ of the two numbers found for each element on a periodic table. For an atom, the number of protons is __________ the number of electrons.
Question 97
97.

How can the neutron number of an element be calculated?

Question 98
98.

What is the neutron number of an Oxygen atom whose atomic number is 8 and mass number is 16?

Question 99
99.

If an element has an atomic number of 6 and a mass number of 12, what is the number of neutrons?

Question 100
100.
Li: Protons_______ Neutrons_______ Electrons_______ Atomic Number_______ Atomic Mass_______
Question 101
101.
C: Protons_______ Neutrons_______ Electrons_______ Atomic Number_______ Atomic Mass_______
Question 102
102.
Xe: Protons_______ Neutrons_______ Electrons_______ Atomic Number_______ Atomic Mass_______
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Question 112
112.

Challenge: Atoms are very small, and their nucleus is even smaller. Research and explain the size of atoms and their nucleus.

3
Question 113
113.
What are the protons, electrons and neutrons of Helium-3?
P: _______
E: _______
N: _______
3
3
3
1
2
Question 119
119.

Give the symbol of the isotope described.

An isotope with 29 protons and 34 neutrons.

Question 120
120.

Give the symbol of the isotope described.

An isotope with 13 protons and 13 neutrons.

Question 121
121.

Give the symbol of the isotope described.

An isotope with 56 protons and 81 neutrons.

Question 122
122.

Give the symbol of the isotope described.

An isotope with 3 protons and 6 neutrons.

Question 123
123.

Give the symbol of the isotope described.

An isotope with 14 protons and 19 neutrons.

Question 124
124.
What are the protons, electrons, and neutrons of the element Potassium? P: _______ E: _______ N: _______
Question 125
125.

What element in the periodic table has 8 protons?

1
Question 126
126.

This is Scandium.

What is its atomic number?

1
Question 127
127.

How many protons does it have?

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Question 130
130.

What is an isotope?

Question 131
131.

They have a very _____ mass.

Question 132
132.

Electrons are a ________ particle.

Question 133
133.

They are located in ______ around the outside of an atom.

Question 134
134.

Which element has an atomic number of 11?

Question 135
135.

Question 136
136.

Question 137
137.

Calculate the relative atomic mass (Ar) of gallium to 3sf given that it consists of two isotopes with these abundances: Ga-69 = 60.1%, Ga -71 = 39.9%.

Question 138
138.

The data shows the mass numbers and abundances of naturally-occurring copper isotopes.

Cu-63 = 69%
Cu-65 = 31%

Calculate the relative atomic mass of copper. Give your answer to 1 decimal place.

Question 139
139.

Question 140
140.

What is the relative atomic mass of element X with isotopes 20 (80%) and 22 (20%)?

Question 141
141.

Calculate the relative atomic mass of isotope A (10, 50%) and isotope B (12, 50%).

Question 142
142.

If 70% of isotope 35 and 30% of isotope 37, what is the relative atomic mass?

Question 143
143.

Calculate the relative atomic mass of magnesium if Mg-24 has 78% abundance and Mg-26 has 22% abundance.

Question 144
144.

Given Cl-35 at 75% and Cl-37 at 25%, find the relative atomic mass of chlorine.

Question 145
145.

Question 146
146.

Question 147
147.

Question 148
148.

Question 149
149.

Match these elements to the correct electron configuration.

Draggable itemarrow_right_altCorresponding Item
Fluorine
arrow_right_alt
2,8
Carbon (C)
arrow_right_alt
2,8,1
Neon (Ne)
arrow_right_alt
2,8,2
Magnesium (Mg)
arrow_right_alt
2,4
Sodium (Na)
arrow_right_alt
2,7
Question 150
150.

How many valence electrons does neon have?

Question 151
151.

How many valence electrons does neon have?

Question 152
152.

Match these elements to the correct electron configuration.

Draggable itemarrow_right_altCorresponding Item
Neon (Ne)
arrow_right_alt
2,8
Sodium (Na)
arrow_right_alt
2,8,1
Fluorine
arrow_right_alt
2,8,2
Magnesium (Mg)
arrow_right_alt
2,4
Carbon (C)
arrow_right_alt
2,7
Instructions: fill in the boxes below to show the electron configuration of these atoms. Use your periodic table to help you. The example above shows you how.
Question 153
153.

Draw the electrons of Nitrogen

Question 154
154.

Draw the electrons of Lithium

Question 155
155.

Draw the electrons of Neon

Question 156
156.

Draw the electrons of Magnesium

Question 157
157.

Explain how electrons are arranged in electron shells

Question 158
158.

Fluorine has 9 electrons. How are they arranged?

Question 159
159.

Match the atom to its electron configuration

Draggable itemarrow_right_altCorresponding Item
Sodium (11)
arrow_right_alt
2,1
Potassium (19)
arrow_right_alt
2,8,1
Lithium (3)
arrow_right_alt
2,8,8,1
Question 160
160.

Chlorine ion (Cl-) has fewer electrons than a chlorine atom (Cl).

Question 161
161.

Atoms that lose electrons form positive ions.

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Question 168
168.
Question 169
169.
Question 170
170.
Question 171
171.
Question 172
172.
Question 173
173.

Draw the electron configuration for Sodium

Question 174
174.

Draw the electronic structure of Chlorine

Question 175
175.

Draw the electronic structure of Potassium

Question 176
176.

Question 177
177.

Question 178
178.

Question 179
179.

Question 180
180.

Question 181
181.

Question 182
182.
Question 183
183.
Question 184
184.
Question 185
185.
Question 186
186.
Question 187
187.
Question 188
188.
Question 189
189.
Question 190
190.
Question 191
191.

Who is the creator of the Modern periodic table?

Question 192
192.

What distinguished Mendeleev's Periodic Table?

Question 193
193.

Why are elements in the same group in Mendeleev's periodic table?

Question 194
194.

How did Mendeleev organise the elements in his periodic table?

Question 195
195.

Are most metals at room temperature solid, liquid, or gas?

Question 196
196.
  • Poor conductor of electricity and heat
  • Malleable (able to be hammered)
  • Ductile (can be made into wires)
  • Solid at room temperature
  • High density
  • Brittle
  • Lustrous (shiny)
  • Dull
  • Good conductor of electricity and Heat
  • Gas or liquid at room temperature
  • Low density
  • Metal
  • Non-Metal
Question 197
197.

Question 198
198.

Question 199
199.

Describe the pattern of reactivity of these elements and others in their group

Question 200
200.

Question 201
201.

Question 202
202.

Question 203
203.

Question 204
204.
Question 205
205.

Question 206
206.

Question 207
207.

List the names of the 6 elements that are known as the Alkali Metals

Question 208
208.

For the first 3 elements draw the electron shell configurations

Question 209
209.

How many electrons do they have on their outer shell?

Question 210
210.

Draw the ion formed from the Li atom

Question 211
211.

Draw the ion formed from the Na atom

Question 212
212.

Draw the ion formed from the K atom

Question 213
213.

Describe the pattern of reactivity of these elements.

Question 214
214.
Question 215
215.

Draw the ion formed from the F atom

Question 216
216.

Draw the ion formed from the Cl atom

Question 217
217.

Describe the pattern of reactivity of these elements and others in their group

Question 218
218.

Question 219
219.

Question 220
220.

Question 221
221.

Question 222
222.

Question 223
223.

Question 224
224.

Question 225
225.

Question 226
226.

Question 227
227.
Other Answer Choices:
Question 228
228.
Other Answer Choices:
Question 229
229.
Other Answer Choices:
Question 230
230.

Question 231
231.

Question 232
232.

Question 233
233.

Question 234
234.

Sort out the following elements whether they belong to Group 1 metals or Transition metals.

  • Copper
  • Iron
  • Sodium
  • Lithium
  • Transition Metal
  • Group 1 Metal
Question 235
235.

Identify the property from the provided options:

  • Soft and can be cut with a knife
  • Dense
  • Low density
  • High melting point
  • React slowly with water
  • React vigorously with water
  • Produce alkaline solutions when react with water
  • Form coloured compounds
  • Group 1 Metals
  • Transition Metals
Question 236
236.

Identify the property from the provided options:

  • Soft and can be cut with a knife
  • Dense
  • Low density
  • High melting point
  • React slowly with water
  • React vigorously with water
  • Produce alkaline solutions when react with water
  • Form coloured compounds
  • Group 1 Metals
  • Transition Metals
Question 40
40.
Question 42
42.
Question 44
44.
Question 46
46.
Question 48
48.
Question 103
103.
As Protons:_______ Electrons: _______
Neutrons: _______
Question 104
104.
Be Protons:_______ Electrons: _______
Neutrons: _______
Question 105
105.
In Protons:_______ Electrons: _______
Neutrons: _______
Question 106
106.
Ne Protons:_______ Electrons: _______
Neutrons: _______
Question 107
107.
Os Protons:_______ Electrons: _______
Neutrons: _______
Question 108
108.
Zn Protons:_______ Electrons: _______
Neutrons: _______
Question 109
109.
Sr Protons:_______ Electrons: _______
Neutrons: _______
Question 110
110.
Au Protons:_______ Electrons: _______
Neutrons: _______
Question 111
111.
Ta Protons:_______ Electrons: _______
Neutrons: _______
Question 114
114.
What are the protons, electrons and neutrons of Helium-4?
P: _______
E: _______
N: _______
Question 115
115.
What are the protons, electrons and neutrons of Helium-6?
P: _______
E: _______
N: _______
Question 116
116.
What are the protons, electrons and neutrons of Helium-7?
P: _______
E: _______
N: _______
Question 117
117.

Find the symbol for helium on your Periodic Table.

Which of the isotopes has the mass number closest to the mass number given on the Periodic Table?

Question 118
118.

Would the chemical properties of the isotopes of helium be the same or different?
Explain your answer. (hand mark)

Question 128
128.

What is its atomic mass?

Question 129
129.

How many neutrons does it have?

Question 162
162.

How many electrons does this have?

Question 163
163.

What is the electron structure?

Question 164
164.

How many electrons does this atom LOSE?

Question 165
165.

How many electrons does this have?

Question 166
166.

What is the electron structure?

Question 167
167.

How many electrons does this atom LOSE?