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AQA GCSE Chemistry > Atomic Structure and the Periodic Table > Flashcards

Atomic Structure and the Periodic Table Flashcards

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1
Q

Atom

A

Smallest part of an element that can exist

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2
Q

Element

A

A substance that contains only one type of atom

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3
Q

Compounds [3]

A
  1. Contains two or more different types of atoms
  2. Which are chemically combined
  3. In fixed proportions
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4
Q

Mixtures [2]

A
  1. Contains two or more elements or compounds

2. Which are NOT chemically combined

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5
Q

What are the two parts of an equation?

A
  1. Reactants

2. Products

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6
Q

Describe the law of conservation of mass [3]

A
  1. Total mass of products = Total mass of reactants

2. As no atoms are lost or made

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7
Q

What are the two ways in which components of compounds can be separated?

A
  1. Electrolysis

2. Chemical reactions

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8
Q

What are the characteristics of the components of a mixture?

A

They retain their original characteristics

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9
Q

What is filtration used to separate?

A

Soluble solids/ (dissolved to liquids) from insoluble solids

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10
Q

Describe the process of filtration [4]

A
  1. Place a filter paper into a funnel
  2. Pour the liquid through the paper
  3. The solid cannot pass through the paper and so remains
  4. The liquid passes into a beaker
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11
Q

What is crystallisation used to separate?

A

A soluble solid from a solution

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12
Q

Describe the process of crystallisation [3]

A
  1. GENTLY HEAT the solution in an evaporating disk using a burner
  2. Once Crystals begin to form, LEAVE TO COOL
  3. After the solution has turned into crystals, DRY and FILTER remaining liquid
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13
Q

What are the 2 ways to dry crystals?

A
  1. Pat with filter paper

2. Using a warm oven

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14
Q

What does simple distillation separate?

A

A solvent from a solution

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15
Q

Describe the process of removing salt from water using simple distillation [3]

A
  1. Salty water is HEATED
  2. Water vapour COOLS in a condenser and drips into a beaker
  3. Water has condensed and salt remains
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16
Q

What does fractional distillation separate?

A

Mixtures in which the components have different boiling points

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17
Q

Describe the process of separating a mixture using Fractional Distillation [3]

A
  1. Vapour RISES through column which is hot at bottom and cool at top
  2. Vapours CONDENSE at section with temperature lower than their boiling point
  3. Liquids led away from column
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18
Q

What is chromatography used to separate?

A

To separate mixtures of coloured soluble components

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19
Q

What is the indicator that a substance is pure on a chromatogram?

A

Produces one spot

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20
Q

What is the indicator that a substance is impure on a chromatogram?

A

Produces two or more spots

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21
Q

What is the formula for the Rf value?

A

Distance travelled by adults/ Distance travelled by solvent

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22
Q

Who created the Plum pudding model of the atom?

A

Thompson

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23
Q

Describe the Plum Pudding model of the atom [2]

A
  1. Atoms contained tiny, negative electrons

2. Surrounded by a sea of positive charge

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24
Q

Why was there a need for a new model? (Plum Pudding)

A

In 1898, Thompson discovered the electron

25
Q

Describe the Geiger and Marsden experiment

A
  1. Bombarded a thin sheet of gold with alpha particles

2. Most of the positive atoms passed through but some were deflected at acute angles (1/10000)

26
Q

What were the conclusions drawn from the Geiger and Marsden experiment?

A
  1. Positive charge in an atom is concentrated in a very small area
  2. This area is known as the nucleus (nuclear model)
27
Q

What did Bohr deduce?

A

Electrons must orbit at specific distances to prevent them spiralling inwards

28
Q

How big is the nucleus in comparison to the atom?

A

1/10000 of the atomic radius

29
Q

Atomic Number

A

Number of Protons in an atom

30
Q

Mass Number

A

Sum of Protons and Neutrons in an atom

31
Q

Formula for the number of neutrons

A

Mass Number-Atomic Number

32
Q

Isotopes

A

Isotopes of an element have the same number of protons but a different amount of neutrons

33
Q

How to atoms form ions?

A

By gaining or losing electrons

34
Q

What is the electron configuration number?

A

2:8:8

35
Q

What does Electron configuration show?

A

How electrons are arranged around the nucleus

36
Q

Who put together the first instance of the Periodic Table?

A

John Newlands

37
Q

How did John Newlands organise his periodic table and why was this problematic? [4]

A
  1. Organised by atomic weight
  2. Noticed periodicity
  3. But missing elements caused issues
  4. Following atomic weight only, meant some elements were in the wrong place
38
Q

Who created the modern version of the periodic table?

A

Dimitri Mendeleev

39
Q

How did Dimitri Mendeleev organise his periodic table? [4]

A
  1. Left gas for future found elements
  2. Placed elements in ‘groups’ with similar properties
  3. Used gaps to predict existence and properties of new elements
  4. Later realised (after discovery of sub-atomic particles) he organised in atomic number
40
Q

How do you find out the outer shell electron number of an atom?

A

Look at the number of the group it is in

41
Q

Explain the properties of Group 0 Elements [3]

A
  1. FULL outer shell of electrons
  2. => Very STABLE electronic configuration
  3. => They are very UNREACTIVE
42
Q

What is the pattern of Boiling points and reactivity within Group 1 of the periodic table? [2]

A
  1. LOW Melting and Boiling points that DECREASE down the group
  2. INCREASE reactivity down the group
43
Q

Why do group 1 elements increase in reactivity down the group? [2]

A
  1. They have 1 outer shell electron
  2. Further from influence of Nucleus as number of shells increase
  3. => Therefore, they can be EASILY LOST
44
Q

What is Group 1 also known as?

A

Alkali Metals

45
Q

How are alkali metals stored and why? [2]

A
  1. React vigorously with water, oxygen and moisture in air

3. => Stored underneath oil

46
Q

What happens when an alkali metal reacts with water? [2]

A
  1. Metal hydroxide formed

2. Hydrogen gas given off

47
Q

What happens when an alkali metal dissolves in water?

A

An alkali solution is produced

48
Q

What happens when an Alkali Metal reacts with non metals?

A

Ionic compounds are formed

49
Q

What are Group 7 elements known as?

A

Halogens

50
Q

Describe the pattern of reactivity within Group 7 of the periodic table?

A

Decreases down the group

51
Q

Why do Group 7 elements decrease in reactivity down the group? [2]

A
  1. They have 7 outer shell electrons
  2. Further away from the influence of the nucleus as number of shells increase
  3. Therefore, it is HARDER to gain an electron
52
Q

What happens when Halogens react with metals?

A

They form ionic salts

53
Q

What is the rule for the displacement of Halogens? [2]

A
  1. A more reactive halogen will displace a less reactive halogen
  2. From an aqueous solution of its salt
54
Q

Where are transition metals located within the periodic table?

A

Between groups 2 and 3

55
Q

Name 2 properties of Transition Metals [2]

A
  1. Malleable

2. Good conductors

56
Q

State 2 uses of transition metals [2]

A
  1. Used as Catalysts=> speed up reactions

2. Circuitry

57
Q

Compare Transition metals to alkali metals [3]

A
  1. Stronger
  2. Higher melting points
  3. Less reactive
58
Q

Explain how forces of attraction affects melting and boiling points in simple substances [3]

A
  1. Bonds are strong covalent between molecules
  2. Forces of attraction are much weaker
  3. Only a little amount of energy is required to overcome the forces of attraction here

AQA GCSE Chemistry (10 decks)

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