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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
Q

What happens to an Atom’s Electrical Charge if it loses an Electron?

(2 marks)

A

If an Atom loses an electron, it becomes positively charged

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26
Q

What happens to an Atom’s Electrical Charge if it gains a Electron?

(1 mark)

A

If an Atom gains an electron, it becomes negatively charged.

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27
Q

Describe an Atom Symbol.

6 marks

A
  • Mass Number: top left
  • Atomic Number: bottom left
  • Element: Centre
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28
Q

What is used to calculate the number of Protons, Neutrons and Electrons in an atom.

(2 marks)

A

Mass number + Atomic number.

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29
Q

What is the Number of Protons equal to?

2 marks

A

Number of Protons = The Number of Electrons = Atomic Number

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30
Q

What is the Number of Neutrons equal to?

2 marks

A

Number of Neutrons = Mass Number – Atomic Number

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31
Q

What is the Electrical Charge of a Proton?

1 mark

A

Protons have a Positive Charge.

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32
Q

What is the Electrical Charge of a Neutron?

1 mark

A

Neutrons have a Neutral Charge/no Charge.

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33
Q

What is the Electrical Charge of an Electron?

1 mark

A

Electrons have a Negative Charge.

34
Q

Electrons orbit the nucleus in shells.
Describe these shells.

(6 marks)

A
  • 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
Q

What is the maximum number of Electrons first shell (nearest shell) can hold for elements with Atomic Numbers 1-20?

(1 mark)

A

2 Electrons

36
Q

What is the maximum number of Electrons the second shell can hold for elements with Atomic Numbers 1-20?

(1 mark)

A

8 Electrons

37
Q

What is the maximum number of Electrons the third shell can hold for elements with Atomic Numbers 1-20?

(1 mark)

A

8 Electrons

38
Q

What is the maximum number of Electrons the fourth shell can hold for elements with Atomic Numbers 1-20?

(1 mark)

A

2 Electrons

39
Q

What is an Electronic Configuration?

1 mark

A

An Electronic Structure of an Atom.

40
Q

Describe a Sodium Atom’s Electronic Configuration.

4 marks

A

Sodium has 11 electrons:

  • 2 Electrons in the first shell.
  • 8 Electrons in the second shell.
  • 1 Electron in the third shell.
41
Q

How can Sodium’s Electronic Configuration be shown?

3 marks

A

2,8,1

42
Q

How are Electrons shown in an Atomic Diagram?

1 mark

A

Electrons are shown as dots/crosses in an Atomic Model.

43
Q

Describe an Atoms radius (in Metres and Nanometres.)

3 marks

A

An Atoms Radius is about;

  • 0.1 nm
  • Or 0.0000000001 metres (1 × 10-10 m)
44
Q

Describe the Nucleus of an Atom.

1 mark

A

The Nucleus of an Atom is less than

1 / 10,000 the size of an atom.

45
Q

What are Isotopes?

4 marks

A

Isotopes are Atoms of an Element with the same Atomic Number, but a different Mass Number.

  • They have a different number of Neutrons.
46
Q

Number of subatomic particles in atoms of the 2 isotopes of chlorine:

(22 marks)

A 
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
Q

Chlorine exists as…?

1 mark

A

two common isotopes.

48
Q

Most elements contain a mixture of what?

2 marks

A

Isotopes - each present in a different amount.

49
Q

The term ‘weighted mean mass’ takes into account?

2 marks

A

The different contribution of each isotope to the overall mass.

50
Q

The contributions of all isotopes are combined to give…?

2 marks

A

The Relative Atomic Mass – the weighted mean of the Mass Numbers.

51
Q

What is the Relative Atomic Mass?

2 marks

A

The weighted mean (contribution of each isotope to the overall mass) of the Mass Numbers.

52
Q

Finish the equation:
Relative Atomic Mass (Ar - Small r)

(3 marks)

A

= (Mass number 1 x abundance) x (Mass number 2 x abundance) / Total abundance

53
Q

Relative atomic mass is not the same as…?

1 mark

A

Mass number

54
Q

What are Mass numbers?

3 marks

A

Whole numbers - because they are the Number of Protons plus the Number of Neutrons.

55
Q

Describe the Relative Atomic Mass.
What is it?

(5 marks)

A
  • 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
Q

What are Compounds?

2 marks

A

2 or more elements chemically combined.

57
Q

What does ‘Mono’ mean? ,

1 mark

A

One

58
Q

What does ‘Di’ mean?

1 mark

A

Two

59
Q

How many Atoms of Oxygen does Carbon Monoxide have?

1 mark

A

Carbon Monoxide has one atom of Oxygen.

60
Q

How many Atoms of Oxygen does Carbon Dioxide have?

1 mark

A

Carbon Dioxide has two atoms of Oxygen.

61
Q

What is the formula for Water?

1 mark

A

H2O

62
Q

What is the formula for Carbon Monoxide?

1 mark

A

CO

63
Q

What is the formula for Carbon Dioxide?

1 mark

A

CO2

64
Q

What is the formula for Sulfur Dioxide?

1 mark

A

SO2

65
Q

What is the formula for Sulfur Trioxide?

1 mark

A

SO3

66
Q

What is the formula for Nitrogen Monoxide?

1 mark

A

NO

67
Q

What is the formula for Nitrogen Dioxide?

1 mark

A

NO2

68
Q

What is the formula for Ammonia?

1 mark

A

NH3

69
Q

What is the formula for Hydrochloric Acid?

1 mark

A

HCl

70
Q

What is the formula for Nitric Acid?

1 mark

A

HNO3

71
Q

What is the formula for Sulfuric Acid?

1 mark

A

H2SO4

72
Q

What Elements are present in Water?

2 marks

A

Hydrogen + Oxygen.

73
Q

What Elements are present in Carbon Monoxide?

2 marks

A

Carbon + Oxygen.

74
Q

What Elements are present in Carbon Dioxide?

2 marks

A

Carbon + Oxygen.

75
Q

What Elements are present in Sulfur Dioxide?

2 marks

A

Sulfur + Oxygen.

76
Q

What Elements are present in Sulfur Trioxide?

2 marks

A

Sulfur + Oxygen.

77
Q

What Elements are present in Nitrogen Monoxide?

2 marks

A

Nitrogen + Oxygen.

78
Q

What Elements are present in Nitrogen Dioxide?

2 marks

A

Nitrogen + Oxygen.

79
Q

What Elements are present in Ammonia?

2 marks

A

Nitrogen + Hydrogen.

80
Q

What Elements are present in Hydrochloric Acid?

2 marks

A

Hydrogen + Chlorine.

81
Q

What Elements are present in Nitric Acid?

3 marks

A

Hydrogen + Nitrogen + Oxygen.

82
Q

What Elements are present in Sulfuric Acid?

3 marks

A

Hydrogen + Sulfur + Oxygen.

CCEA GCSE Chemistry (7 decks)

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