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CCEA GCSE Chemistry > Atomic Structure > Flashcards

Atomic Structure Flashcards

1
Q

What is all matter is made of?

1 mark

A

Atoms

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2
Q

What is “atom” is derived from?

2 marks

A

Ancient Greek word atomos: “something that cannot be divided.”

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3
Q

What is the ‘Plum Pudding Model’?

3 marks

A

The scientific idea (early model) that an atom is a sphere of positive charge, with negatively charged electrons in it.

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4
Q

What was Ernest Rutherford opinion (Peer Review) of the Plum Pudding Model?

(3 marks)

A

Ernest Rutherford disproved of the PP model and suggested that an atom had a Positive Nucleus at its centre, orbited by Negatively-Charged Electrons.

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5
Q

Describe Ernest Rutherford’s Atom Model.

3 marks

A

Positive Nucleus at the Atom’s centre, orbited by Negatively-Charged Electrons.

1932: James Chadwick discovered the neutron – a particle with no charge in the nucleus of the atom. The modern idea of the atom was complete.

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6
Q

What was James Chadwick’s Atom discovery?

5 marks

A

1932: James Chadwick discovered the Neutron - particle with no charge in the Nucleus of the atom.
- Completing the Modern Atomic Model.

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7
Q

Who discovered the Neutron?

2 marks

A

James Chadwick discovered the Neutron in the centre of an Atoms Nucleus.

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8
Q

Describe The Modern Atomic Model.

6 marks

A

A central, positively-charged Nucleus that contains:

  • positively-charged protons
  • neutral neutrons

Negatively-charged electrons orbit the Nucleus in shells.
An atom’s nucleus gives it most of its mass.

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9
Q

What gives an Atom most of its mass?

1 mark

A

An atom’s Nucleus gives it most of its mass.

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10
Q

Name the 3 Atomic Models.

4 marks

A
  • Plum Pudding Model
  • Ernest Rutherford’s Model
  • Modern Atomic Model; inspired by previous models plus James Chadwick’s discovery.
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11
Q

What was the earliest Atomic Model?

1 mark

A

Plum Pudding Model

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12
Q

Name the 3 Subatomic Particles.

3 marks

A
  • Protons
  • Neutrons
  • Electrons
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13
Q

Give the Relative Mass of a Proton.

1 mark

A

1

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14
Q

Give the Relative Mass of a Neutron.

1 mark

A

1

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15
Q

Give the Relative Mass of an Electron.

1 mark

A

1 / 1840

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16
Q

Give a Protons Relative Charge.

1 mark

A

+1

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17
Q

Give a Neutrons Relative Charge.

1 mark

A

0

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18
Q

Give an Electrons Relative Charge.

1 mark

A

-1

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19
Q

Give a Protons location in an Atom.

1 mark

A

Protons are found in the Nucleus of an Atom.

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20
Q

Give a Neutrons location in an Atom.

1 mark

A

Neutrons are found in the Nucleus of an Atom.

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21
Q

Give an Electrons location in an Atom.

1 mark

A

Electrons are found in shells around the Nucleus of an Atom.

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22
Q

Describe an Atomic number.

2 marks

A

An Atomic Number is the Number of Protons in an atom’s Nucleus.

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23
Q

Describe a Mass number.

2 marks

A

A Mass Number is the total Number of Protons + Neutrons.

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24
Q

What is an Atoms Electrical charge?

3 marks

A

An Atom has a Neutral/no overall charge, because it has an equal Number of Protons and Electrons.

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25
What happens to an Atom’s Electrical Charge if it loses an Electron? (2 marks)
If an Atom loses an electron, it becomes positively charged
26
What happens to an Atom’s Electrical Charge if it gains a Electron? (1 mark)
If an Atom gains an electron, it becomes negatively charged.
27
Describe an Atom Symbol. | 6 marks
- Mass Number: top left - Atomic Number: bottom left - Element: Centre
28
What is used to calculate the number of Protons, Neutrons and Electrons in an atom. (2 marks)
Mass number + Atomic number.
29
What is the Number of Protons equal to? | 2 marks
Number of Protons = The Number of Electrons = Atomic Number
30
What is the Number of Neutrons equal to? | 2 marks
Number of Neutrons = Mass Number – Atomic Number
31
What is the Electrical Charge of a Proton? | 1 mark
Protons have a Positive Charge.
32
What is the Electrical Charge of a Neutron? | 1 mark
Neutrons have a Neutral Charge/no Charge.
33
What is the Electrical Charge of an Electron? | 1 mark
Electrons have a Negative Charge.
34
Electrons orbit the nucleus in shells. Describe these shells. (6 marks)
- Different shells = different max number of Electrons. - Each shell a different distance away; first + lowest available shell (nearest Nucleus) filled first - when full, Electrons begin to fill the next shell.
35
What is the maximum number of Electrons first shell (nearest shell) can hold for elements with Atomic Numbers 1-20? (1 mark)
2 Electrons
36
What is the maximum number of Electrons the second shell can hold for elements with Atomic Numbers 1-20? (1 mark)
8 Electrons
37
What is the maximum number of Electrons the third shell can hold for elements with Atomic Numbers 1-20? (1 mark)
8 Electrons
38
What is the maximum number of Electrons the fourth shell can hold for elements with Atomic Numbers 1-20? (1 mark)
2 Electrons
39
What is an Electronic Configuration? | 1 mark
An Electronic Structure of an Atom.
40
Describe a Sodium Atom’s Electronic Configuration. | 4 marks
Sodium has 11 electrons: - 2 Electrons in the first shell. - 8 Electrons in the second shell. - 1 Electron in the third shell.
41
How can Sodium’s Electronic Configuration be shown? | 3 marks
2,8,1
42
How are Electrons shown in an Atomic Diagram? | 1 mark
Electrons are shown as dots/crosses in an Atomic Model.
43
Describe an Atoms radius (in Metres and Nanometres.) | 3 marks
An Atoms Radius is about; - 0.1 nm - Or 0.0000000001 metres (1 × 10-10 m)
44
Describe the Nucleus of an Atom. | 1 mark
The Nucleus of an Atom is less than | 1 / 10,000 the size of an atom.
45
What are Isotopes? | 4 marks
Isotopes are Atoms of an Element with the same Atomic Number, but a different Mass Number. - They have a different number of Neutrons.
46
Number of subatomic particles in atoms of the 2 isotopes of chlorine: (22 marks)
``` 35Cl; Atomic Number - 17 Mass Number - 35 Number of Protons - 17 Number of Neutrons - (35 - 17) = 18 Number of Electrons - 17 ``` ``` 37Cl; Atomic Number - 17 Mass Number - 37 Number of Protons - 17 Number of Neutrons - (37 - 17)= 20 Number of Electrons - 17 ```
47
Chlorine exists as...? | 1 mark
two common isotopes.
48
Most elements contain a mixture of what? | 2 marks
Isotopes - each present in a different amount.
49
The term ‘weighted mean mass’ takes into account? | 2 marks
The different contribution of each isotope to the overall mass.
50
The contributions of all isotopes are combined to give...? | 2 marks
The Relative Atomic Mass – the weighted mean of the Mass Numbers.
51
What is the Relative Atomic Mass? | 2 marks
The weighted mean (contribution of each isotope to the overall mass) of the Mass Numbers.
52
Finish the equation: Relative Atomic Mass (Ar - Small r) (3 marks)
= (Mass number 1 x abundance) x (Mass number 2 x abundance) / Total abundance
53
Relative atomic mass is not the same as...? | 1 mark
Mass number
54
What are Mass numbers? | 3 marks
Whole numbers - because they are the Number of Protons plus the Number of Neutrons.
55
Describe the Relative Atomic Mass. What is it? (5 marks)
- an Average Mass; takes into account all of the Isotopes + their Abundance. - not always a whole number. - but on data reports a lot of the Relative Atomic Masses are rounded to whole numbers.
56
What are Compounds? | 2 marks
2 or more elements chemically combined.
57
What does ‘Mono’ mean? , | 1 mark
One
58
What does ‘Di’ mean? | 1 mark
Two
59
How many Atoms of Oxygen does Carbon Monoxide have? | 1 mark
Carbon Monoxide has one atom of Oxygen.
60
How many Atoms of Oxygen does Carbon Dioxide have? | 1 mark
Carbon Dioxide has two atoms of Oxygen.
61
What is the formula for Water? | 1 mark
H2O
62
What is the formula for Carbon Monoxide? | 1 mark
CO
63
What is the formula for Carbon Dioxide? | 1 mark
CO2
64
What is the formula for Sulfur Dioxide? | 1 mark
SO2
65
What is the formula for Sulfur Trioxide? | 1 mark
SO3
66
What is the formula for Nitrogen Monoxide? | 1 mark
NO
67
What is the formula for Nitrogen Dioxide? | 1 mark
NO2
68
What is the formula for Ammonia? | 1 mark
NH3
69
What is the formula for Hydrochloric Acid? | 1 mark
HCl
70
What is the formula for Nitric Acid? | 1 mark
HNO3
71
What is the formula for Sulfuric Acid? | 1 mark
H2SO4
72
What Elements are present in Water? | 2 marks
Hydrogen + Oxygen.
73
What Elements are present in Carbon Monoxide? | 2 marks
Carbon + Oxygen.
74
What Elements are present in Carbon Dioxide? | 2 marks
Carbon + Oxygen.
75
What Elements are present in Sulfur Dioxide? | 2 marks
Sulfur + Oxygen.
76
What Elements are present in Sulfur Trioxide? | 2 marks
Sulfur + Oxygen.
77
What Elements are present in Nitrogen Monoxide? | 2 marks
Nitrogen + Oxygen.
78
What Elements are present in Nitrogen Dioxide? | 2 marks
Nitrogen + Oxygen.
79
What Elements are present in Ammonia? | 2 marks
Nitrogen + Hydrogen.
80
What Elements are present in Hydrochloric Acid? | 2 marks
Hydrogen + Chlorine.
81
What Elements are present in Nitric Acid? | 3 marks
Hydrogen + Nitrogen + Oxygen.
82
What Elements are present in Sulfuric Acid? | 3 marks
Hydrogen + Sulfur + Oxygen.

CCEA GCSE Chemistry (7 decks)

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