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GCSE Chemistry > C4 - The Periodic Table > Flashcards

C4 - The Periodic Table Flashcards

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1
Q

What is the plum pudding model?

A

There is a positively charged ‘pudding’ with negative electrons inside

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2
Q

How was the plum pudding model proved wrong?

A

They used a thin piece of gold and fired particles through it and most went through but some deflected backwards showing a positive nucleus

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3
Q

What is Bohr’s model?

A

There is a nucleus with fixed orbit shells with electrons on these

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4
Q

What is the nucleus?

A
  • Contains protons and neutrons

- It has a positive charge

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5
Q

What are the electrons?

A
  • Negatively charges
  • Move around on the shells
  • They have virtually no mass
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6
Q

What is the mass and charge of protons, neutrons and electrons?

A

Mass Charge
Proton. 1. 1
Neutron. 1. 0
Electron. 0.0005. -1

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7
Q

What is the mass number?

A

Total number of protons and neutrons (big number)

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8
Q

What is the atomic number?

A

Number of protons (small number)

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9
Q

What are isotopes?

A

They are the same except from have extra neutrons

Same atomic number but different mass number

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10
Q

What did Döbereiner make the periodic table look like?

A

He ordered them in relative atomic mass

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11
Q

What did Newland make the periodic table look like?

A

He put it in similar properties such as metals non metals…

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12
Q

What did Dmitri Mendeleev’s periodic table look like?

A

He put them in order of atomic mass and similar properties but left gaps for predicted elements

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13
Q

What do the periods in the periodic table represent?

A

The number of shells

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14
Q

What do the groups of the periodic table represent?

A

This shows the number of electrons on the outer shell

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15
Q

What is ionic bonding?

A

This is where a metal and a non metal transfers electrons

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16
Q

What is covalent bonding?

A

When two non metals share electrons

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17
Q

What happens as you go down group 1 metals?

A

They get more reactive as the outer electron is more easily lost

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18
Q

What are group 1 metals?

A

Alkali metals

19
Q

What is oxidation and reduction?

A

O xidation
I s
L oss

R eduction
I s
G ain

20
Q

What happens when group 1 metals react with water?

A

Hydrogen gas is produces meaning it fizzes, moves very fast, bubbles and sometimes ignites

21
Q

What flame is produced with lithium, sodium and potassium?

A 
Lithium = red flame
Sodium = yellow/orange flame
Potassium = lilac flame
22
Q

What are group 7 metals?

A

Halogens

23
Q

What happens as you go down the group 7 metals?

A

As you go down they get less reactive because it’s harder to gain an electron

24
Q

What happens when halogens are reacted?

A

They form salts

25
Q

What happens with more and less reactive halogens?

A

The more reactive ones will displace the less reactive ones

26
Q

What are some of the useful properties of metals?

A

They have a crystal structure:

  • High mp and bp
  • Strong
  • Good conductors
27
Q

What are super conductors?

A

Metals at very low temperatures so they loose there resistance

28
Q

What are super conductors used for?

A
  • Power cables
  • Electromagnets
  • Electronic circuits
29
Q

What are transition metals?

A

Similar to normal metals but make good catalysts

30
Q

Give examples of transition metals which are catalysts.

A

Iron (harber process)

Nickel (margarine)

31
Q

What is thermal decomposition?

A

This is the breaking down with heat

32
Q

What is an example of thermal decomposition using copper(II) carbonate?

A

Copper(II) carbonate > copper oxide + carbon dioxide

CuCO(3) > CuO + CO(2)

33
Q

What is a precipitation reaction?

A

This is when two solutions react and form an insoluble solid in the solution

34
Q

What is the precipitation reaction between copper(II) sulfate + sodium hydroxide?

A

Copper(II) sulfate + sodium hydroxide > copper(II) hydroxide + Sodium sulfate

35
Q

What colours are made with transition metals?

A

Copper(II) hydroxide = blue

Iron(II) hydroxide = grey/green

Iron(III) hydroxide = orange/brown

36
Q

How do we get our water?

A
  • Surface water

- Groundwater

37
Q

What are the four steps in water purification?

A
  • Mesh
  • Sand filtration (removes the large materials in it)
  • Sedimentation (makes fine particles clump together when iron sulphate is added)
  • Chlorination (kills microbes)
38
Q

What impurities are in tap water?

A
  • Nitrate residue
  • Lead compounds
  • Pesticide residue
39
Q

What can you test water for?

A

Dissolved ions

40
Q

How do you test for sulfate ions?

A

Use barium chloride

41
Q

How do you test for sulfate ions using barium chloride?

A

1) Add hydrochloric acid to the test sample
2) Add ten drops of barium chloride solution
3) If there is a white precipitate then its present

42
Q

How do you test for halide ions?

A

Use silver nitrates

43
Q

How do you test for halide ions using silver nitrate?

A

1) Add some dilute nitric acid to the test sample
2) Add 10 drops of silver nitrate solution
3) If halide ions are present a precipitate will be formed

44
Q

What do different coloured precipitates show when testing for halide ions?

A
  • Chloride ions = white precipitate
  • Bromide ions = cream precipitate
  • Iodide ions = pale yellow precipitate

GCSE Chemistry (4 decks)

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