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Chemistry > Section 13 - groups in the periodic table > Flashcards

Section 13 - groups in the periodic table Flashcards

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1
Q

How is the periodic table arranged?

A

Elements with similar chemical or physical properties are in the same groups

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2
Q

Where are alkali metals?

A

In group 1

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3
Q

How are alkali metals similar to other metals?

A

They have similar physical properties, they ar malleable and conduct electricity

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4
Q

How are alkalis only specific to themselves?

A

They have relatively low melting points / soft so they’re easy to cut / very reactive / readily form compounds with non-metals

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5
Q

How do alkalis burn in their air and why?

A

They burn brightly / they’re easily oxidised

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6
Q

What is the main products from alkali?

A

Hydrogen

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7
Q

How does reactivity change when going down the alkali metals group?

A

They get more reactive

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8
Q

What happens when lithium reacts with water?

A

Bubbles fiercely on the surface

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9
Q

What happens when sodium reacts with water?

A

Melts into a ball and fizzes on the surface

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10
Q

What happens when potassium reacts with water?

A

It bursts into flames and flies about the surface

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11
Q

What do you looks at to explain the trend in reactivity in metal alkalis ?

A

Electronic configurations of alkali metal atoms

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12
Q

Why are alkalis so reactive?

A

Because they have 1 outer electron on its outer shell which it is easily give up

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13
Q

As you go down the groups and shells get added, what happens to the force of attraction between positive nucleus and negative outer electron?

A

The force of attraction decreases as they become further apart

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14
Q

Why are alkalis easier to react as they go down the table?

A

Because the positive nucleus and negative electron loosen the force of attraction making it weaker so more likely to remove

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15
Q

What is group 7 of the periodic table called?

A

Halogens

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16
Q

What type of molecules do halogens exist in?

A

Diatomic molecules

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17
Q

What is a diatomic molecule?

A

One atom held together by a single covalent bond

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18
Q

State some properties of halogens

A

Non-metallic / poor conductors of heat and electricity

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19
Q

Why do you need to take care when handling halogens?

A

They are all toxic and corrosive

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20
Q

What happen to the m/b points and the densities when you go down group 7?

A

The melting/boiling points and the densities increase as you go down

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21
Q

What colour is chlorine?

A

Green gas

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22
Q

What colour is bromine?

A

Brown liquid

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23
Q

What colour is iodine?

A

Purple/black solid

24
Q

What do halogens make when they react with metals?

A

Salts

25
Q

What do the salts made from halogens and metals contain?

A

Halide ions

26
Q

Name some uses for halide salts

A

Table salt / toothpastes / swimming pool disinfectant /

27
Q

What is the chemical compound for table salt?

A

Sodium chloride

28
Q

Why are halogens good disinfectants / bleaches?

A

They can kill microorganisms and remove colour from materials

29
Q

What is the test or chlorine?

A

Place damp litmus paper in chlorine gas, if chlorine is present it first turns red and then bleaches white

30
Q

What is formed when halogens and hydrogen is combined?

A

Hydrogen halides

31
Q

What can form an acidic solution?

A

Dissolving hydrogen halides in water

32
Q

Explain the steps of making water acidic with hydrogen and chlorine

A

Hydrogen and chlorine molecules collide and covalent bonds holding them together / covalent bongs between hydrogen and chlorine make new compound - hydrogen chloride / hydrogen chloride dissolved in water and break up molecules into H+ and Cl- — formation of H+ makes solution acidic

33
Q

What happens to the reactivity as you go down halogens group?

A

They get less reactive as they go down

34
Q

What does fluorine do to iron wool?

A

Burst into flames

35
Q

What does chlorine do to iron wool?

A

Glows brightly

36
Q

What does bromine do to iron wool?

A

Glows dull red

37
Q

What does iodine do to iron wool?

A

Hanged colour

38
Q

How else can you work out the order of reactivity of halogens?

A

Using displacement reactions

39
Q

What happens during a displacement reaction?

A

A more reactive element takes place of a less reactive element in the ionic compound (more reactive halogen displaces a less reactive halogen from a halide compound)

40
Q

What do we look at to explain the trend in reactivity for halogens?

A

Electronic configuration

41
Q

What is oxidation?

A

When a metal reacts with oxygen it loses electrons ‘LOSS OF ELECTRONS’

42
Q

What is reduction?

A

‘GAIN OF ELECTRONS’

43
Q

What does mnemonic ‘OILRIG’ mean?

A

Oxidation is loss reduction is gain

44
Q

What happens during displacement: reduction or oxidation?

A

Both - reduction-oxidation

45
Q

Because displacement has a oxidation and reduction at the same time, what type of reaction is this?

A

Redox reaction

46
Q

What is in group 0?

A

Noble gases

47
Q

State some properties of noble gases

A

Colourless / very low melting and boiling points / poor conductors if heat and electricity

48
Q

Why are noble gases unique?

A

They’re inert

49
Q

What does inert mean?

A

They don’t easily react with anything

50
Q

Why do noble gases has low b/m points?

A

Because they exist as single atoms so have no strong bonds between atoms

51
Q

What is krypton uses for?

A

Photography lighting - produces brilliant white light

52
Q

What is argon used for?

A

Denser than air - added to space in between then wine and the cork to stop oxygen in air reacting with wine

53
Q

How is helium useful?

A

Low density and is non-flammable so is sued in weather balloons

54
Q

How is neon useful?

A

Produces distinctive red-orange light when electricity passed through it - useful for long lasting illuminated signs

55
Q

Why are noble gases so unreactive?

A

They have a complete outer shell so they are already stable

Chemistry (6 decks)

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