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UK GCSE Chemistry > Chemistry - Atomic Structure (C2) > Flashcards

Chemistry - Atomic Structure (C2) Flashcards

Revision on Atomic structure and the C2 Structure

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1
Q

Define Atom

A

The smallest part of an element that can still be recognised as that element

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2
Q

Define Element

A

A substance made up of only one atom

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3
Q

Define Molecule

A

A substance made of two or more different atoms chemically bonded together (can be atoms of the same type)

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4
Q

Define Mixture

A

A substance made of more than one thing not chemically bonded together

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5
Q

State the three subatomic particles

A

Protons, Neutrons, Electrons

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6
Q

State the relative charges of the subatomic particles

A

Protons +1, Neutrons 0, Electrons -1

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7
Q

State the masses of the subatomic particles

A

Protons 1, Neutrons 1, Electrons 0

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8
Q

How are the subatomic particles arranged in an atom?

A

Protons and Neutrons in the nucleus and electrons orbiting the outer shells.

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9
Q

What is the plum pudding model?

A

A ball of positive charge with negative electrons studded into it

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10
Q

What did Rutherford’s alpha scattering experiment prove?

A

Atoms have a small dense nucleus with a positive charge

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11
Q

How did Bohr adapt the model of the atom?

A

He said electrons orbit the nucleus at specific distances

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12
Q

What is the atomic number of an atom?

A

The number of protons in an atom

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13
Q

What is the mass number of an atom?

A

The number of protons + the number of neutrons in an atom

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14
Q

How do you calculate the number of neutrons in an atom?

A

Mass number - atomic number

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15
Q

How are the electrons arranged in atoms?

A

Orbiting the nucleus in shells

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16
Q

How many electrons can go in the first shell?

A

2

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17
Q

How many electrons can go in the other shells?

A

8

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18
Q

How were elements arranged in the early attempts of the periodic table?

A

By atomic weight

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19
Q

How are elements in the periodic table arranged?

A

By atomic number

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20
Q

How are elements in the periodic table arranged?

A

By atomic number

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21
Q

What are groups in the periodic table?

A

The columns, numbered 1, 2, 3, 4, 5, 6, 7, 0/8

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22
Q

What do you know about elements in the same group?

A

They have similar properties (reactions) as they have the same number of electrons in the outer shell

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23
Q

What can the group tell you about the electrons in an atom?

A

How many electrons in the outer shell. E.g. carbon is in group 4 so has 4 electrons in the outer shell

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24
Q

What are periods in the periodic table?

A

The rows in the periodic table

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25
Q

What can the period tell you about the electrons in an atom?

A

How many shells an atom has. E.g. carbon is in the second period so has two shells

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26
Q

Why did Mendeleev swap the order of some elements?

A

So they were in the same group as elements they had similar chemical properties with

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27
Q

Why did Mendeleev leave gaps in his periodic table?

A

For elements that had not been discovered yet

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28
Q

What is an ion?

A

A charged particle

An atom which has lost or gained an electron

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29
Q

How many electrons does calcium have?

A

20 (same as atomic number!)

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30
Q

How many electrons does silicon have?

A

14 (same as atomic number!)

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31
Q

How are the electrons in sulphur arranged?

A

2.8.6 (18 electrons total)

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32
Q

How are the electrons in magnesium arranged?

A

2.8.2 (12 electrons total)

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33
Q

How many electrons are in the outer shell of boron?

A

3 (it is in group 3!)

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34
Q

How many electrons are in the outer shell of phosphorous?

A

5 (it is in group 5!)

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35
Q

How many electrons are in the outer shell of sodium?

A

1 (it is in group 1!)

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36
Q

An element has three shells and three electrons in the outer shell. What element is it?

A

Aluminium (group 3, period 3

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37
Q

How many electrons are in the outer shell of Gallium?

A

3 (it is in group 3!)

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38
Q

How can solids be separated from liquids?

A

Filtration

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39
Q

What is crystallisation?

A

When a solution is heated until crystals start to form then left to cool until all the water evaporates

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40
Q

What does distillation do?

A

Separates mixture of liquids with different boiling points

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41
Q

What decides what element an atom is?

A

The number of protons. E.g. carbon always has 6 protons

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42
Q

Why do atoms have no charge?

A

They have the same number of protons and electrons

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43
Q

What is the approximate radius of an atoms

A

0.1nm (1x10-10m)

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44
Q

How big is the radius of the nucleus compared to that of the atom?

A

1/10000 the size (so 1x10-14m)

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45
Q

What is an isotope?

A

An atom with the same number of protons but a different number of neutrons.

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46
Q

How do you calculate the relative atomic mass of an isotope?

A

Multiply the isotope mass by the abundance for each isotope, add them together and divide the answer by 100

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47
Q

What type of ions do metals form?

A

Positive ions as they lose electrons to get a full outer shell - Cations

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48
Q

What type of ions do non-metals form?

A

Negative ions as they gain electrons to get a full outer shell - Anions

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49
Q

In terms of electrons, what do group 1 (the alkali metals) elements have in common?

A

1 electron in the outer shell

50
Q

What do atoms become ions?

A

To get a noble gas formation as these are very stable

full outer shell

51
Q

Describe ionic boning

A

When a metal losses electron(s) to become a positive cation and a non-metal gains these electron(s) to become a negative anion
The anion and cation have strong electrostatic forces of attraction and form an ionic bond

52
Q

What does a dot and cross diagram show?

A

How ionic and covalent bonds are formed

See Figure 10

53
Q

What structures do ionic bonds form?

A

Giant Ionic Lattice

54
Q

Describe Giant Ionic Lattices

A

Regular lattice
Alternating positive and negative ions
(See Figure 11)

55
Q

What force are Giant Ionic Lattices held together by?

A

Strong electrostatic forces of attraction between oppositely charged particles

56
Q

Describe some of the properties of ionic compounds

A

High melting and boiling point

Conduct electricity as liquids or if dissolved in water but not as solids

57
Q

Why do ionic compounds have high melting/ boiling points?

A

Many strong ionic bonds between ions

A lot of energy is required to break these bonds

58
Q

Why do ionic bonds conduct electricity as liquids or if dissolved in water but not as solids?

A

In solids the ions are trapped in the regular lattice and thus can not carry charge
In liquids the ions are free to move and can thus carry charge
When dissolved in water the ions separate and are free to move and can thus conduct electricity

59
Q

Describe covalent bonding

A

When non-metals bond by sharing electrons

60
Q

How do covalent bonds work?

A

The electrons in the outer shell are attracted to the nuclei of both atoms and thus hold them together through electrostatic force of attraction

61
Q

How strong are covalent bonds?

A

Very strong

62
Q

What causes some elements to be diatomic?

A

They covalently bond to each other to become stable

63
Q

What are the three models for simple molecular covalent bonds?

A

Dot and cross
Displayed formula
3D model
(See Figure 12)

64
Q

What type of substances do covalent bonds form?

A

Simple molecular or giant covalent structures

65
Q

How strong are the intermolecular forces attraction in simple molecular covalent bonds?

A

Very weak

66
Q

Why are the melting/ boiling points of simple molecular covalent bonds so low?

A

Despite strong covalent bonds, intermolecular forces of attraction in covalent molecules are very weak and not much energy is needed to separate them

67
Q

Describe the conductivity of simple molecular compounds

A

None, they are not charged

68
Q

Describe a polymer

A

Chain of repeating monomers

69
Q

Describe the bonding in polymers

A

Covalent

70
Q

How do we draw polymers?

A

We draw a single repeating unit

See Figure 13

71
Q

What are macromolecules?

A

Giant Covalent Structures

72
Q

Describe properties of macromolecules

A

High melting and boiling point
Do not generally conduct electricity
- (graphite in an exception)

73
Q

What 3 Macromolecules do I need to know?

A

Diamond
Graphite
Silicon Dioxide

74
Q

What is the boiling point of diamond and why?

A

Non-existent due to the strong covalent bonds in every direction
(Not possible to create on Earth)

75
Q

Describe how hard diamond is and why

A

Diamond is extremely hard due to the strong covalent bonds in every direction

76
Q

Describe the structure of diamond

A

Rigid
Forms all 4 potential bonds
(See Figure 14)

77
Q

Describe the structure of Graphite

A

Hexagonal layers
Weak intermolecular forces
One free electron per atom
(See Figure 14)

78
Q

Describe the structure of Silicon Dioxide

A

One silicon atom for every two oxygen
Very strong covalent bonds
(See Figure 14)

79
Q

What three Allotropes of Carbon do I need to know?

A

Diamond
Graphite (graphene)
Fullerenes

80
Q

What is an allotrope of Carbon?

A

Different structural forms of carbon in the same state

81
Q

Describe the conductivity of diamond

A

None, it forms all four potential bonds and thus does not have any free electrons

82
Q

Why is graphite soft and slippery?

A

There are no covalent bonds between layers, only weak intermolecular forces which can be easily broken

83
Q

Describe the conductivity of graphite

A

It is conductive of both heat and electricity as it only forms 3/4 potential bonds and thus has a delocalised electron which can carry charge

84
Q

Describe Graphene

A

A single layer of graphite

85
Q

How thick is graphene?

A

1 atom

86
Q

Why is graphene used in tents rackets or bows?

A

It is very light and strong

87
Q

How many atom molecules are in Buckminsterfullerene?

A

60 (C60)

88
Q

Describe Fullerenes

A

Molecules of carbon shaped as either closed tubes or hollow balls
(See Figure 15)

89
Q

What are fullerenes used for?

A

They can trap other molecules so are used to deliver drugs
Have large surface area so can be used as industrial catalysts
Also make good lubricants

90
Q

What kind of structures do metals form

A

Giant metallic structures

91
Q

Describe metallic bonding

A

The metals loose an electron to form positive cations and the delocalised electrons form a sea around the cations
(See Figure 16)

92
Q

Why are most metals solid at room temperature?

A

Electrostatic forces of attraction between ions and delocalised electrons are strong and thus a lot of energy is needed to break this

93
Q

Why are metals good conductors?

A

They have delocalised electrons which can carry charge and energy

94
Q

Why are metals malleable?

A

All of the ions are the same size and thus can roll over each other easily

95
Q

What are alloys?

A

A compound of different metals

96
Q

Why are alloys harder than pure metals?

A

The atoms are not all the same size and thus do not slide over each other

97
Q

What are the three states of matter?

A

Solid
Liquid
Gas

98
Q

Describe the structure of a solid

A 
Strong forces of attraction between particles
Regular lattice arrangement
Particles in a fixed position
Fixed shape and volume
Particles vibrate 
(See Figure 17)
99
Q

Describe the structure of a liquid

A 
Weak forces of attraction between particles
Constantly moving in random motion
Take the shape of their container
Free to move around each other
Constant volume
(See Figure 17)
100
Q

Describe the structure of a gas

A 
Very weak forces of attraction between particles
Take the shape of their container
No definite shape or volume
Travel in straight lines
Rarely touch
(See Figure 17)
101
Q

What happens when a solid is heated?

A

Melting
As the particles gain energy the vibrate more
Eventually the bonds between particles weaken and they become a liquid
(See Figure 17)

102
Q

What happens when a liquid is heated?

A

Evaporation
The particles gain energy and move around each other faster
Eventually the bonds between particles weaken and they become a gas
(See Figure 17)

103
Q

What happens when a gas is heated?

A

The particles gain energy and expand
This increases the pressure
(See Figure 17)

104
Q

What happens when a solid is cooled?

A

The particles loose energy and stop vibrating as much

105
Q

What happens when a liquid is cooled?

A

Freezing
The particles loose energy and stop moving as much
Eventually bonds form and it becomes a solid
(See Figure 17)

106
Q

What happens when a gas is cooled?

A

Condensing
The particles loose energy and stop moving as much
Eventually bonds form and it becomes a liquid
(See Figure 17)

107
Q

What is sublimation?

A

When an element goes straight from solid to gas

See Figure 17

108
Q

What is another name for coarse particles?

A

Dust

109
Q

What is the diameter of a coarse particle?

A

Between 2.5X10^-6m and 1X10^-5m

Between 2, 500nm and 10, 000nm

110
Q

What is the diameter of a fine particle?

A

Between 1X10^-7m and 2.5X10^-6m

Between 100nm and 2, 500nm

111
Q

What is the diameter of a nanoparticle?

A

Between 1X10^-9 and 1X10^-7

Between 1nm and 100nm

112
Q

What is the equation for surface are to volume ratio?

A

Surface area to volume ratio = surface area / volume

113
Q

Why are nanoparticles useful?

A

They have large volume to surface area ratios

114
Q

Why does having a large surface area to volume ratio make for good catalysts?

A

Reactions happen on the outside of particles, therefore if more of the particle is the surface, more reactions can occur

115
Q

What could nanoparticles be used for in medicine?

A

Delivering drugs right into cells when necessary

116
Q

Why are silver nanoparticles useful?

A

They have antibacterial properties

117
Q

What can silver nanoparticles be used for?

A

They can be put into

  • surgical masks
  • wound dressings
  • deodorant
118
Q

What are advantages of using nanoparticles in suncream?

A

Better skin coverage

Protects from harmful UV rays

119
Q

What are disadvantages of using nanoparticles in suncream?

A

We do not know if they could harm your body cells

We do not know if once washed away, they may damage the environment

120
Q

Why should products with nanoparticles be clearly labelled?

A

We still do not know their long-term effects

UK GCSE Chemistry (9 decks)

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