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MPW chemistry > group 2, group 7 and ions tests > Flashcards

group 2, group 7 and ions tests Flashcards

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1
Q

what are group 2 elements called?

A

Alkaline earth metals

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2
Q

what does ‘alkaline in alkaline earth metals mean?

A

the oxides of these metals releases OH- ions in solution

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3
Q

what does ‘earth’ in alkaline earth metals mean?

A

Very abundant in the earths crust

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4
Q

what structure do all gorup 2 elements have?

A

All Group 2 metals have the giant metallic lattice structure

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5
Q

how do group 2 metals conduct electricity?

A

Metals conduct electricity when solid or liquid because the electrons are delocalised and can move

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6
Q

why do group 2 metals have High Melting and Boiling Points

A

It takes a lot of energy to break the strong electrostatic attraction between the ions and the delocalised electrons

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7
Q

give the general equation for metals + oxygen

A

2M(s) + O2(g) —–> 2MO(s)

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8
Q

give the general equation for metals + water

A

M(s) + 2H2O(l) —> M(OH)2(s) + H2(g)

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9
Q

give the general equation for metals + steam

A

M(s) + H2O(g) —–> MgO(s) + H2(g)

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10
Q

give the general equation for metals + an acid (use H2SO4)

A

M + H2SO4 —-> MSO4 + H2

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11
Q

What is the reactivity of metals like down a group?

A

More Reactive Down the Group

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12
Q

What do metals get more reactive down the group/why does ionisation energy decrease down the group?

A
  1. There are more shells of electrons.
  2. Therefore, the outer electrons are further from the nucleus and more shielded.
  3. So the nuclear attraction for the outer electron is less.
  4. The outer electrons are more easily lost.
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13
Q

What is a common use for calcium oxide/hydroxide?

A

Neutralisation of acidic soils

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14
Q

what is a common ise for magnesium hydroxide or calcium carbonate?

A

Neutralises stomach acids when you have a stomach ache

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15
Q

What is produced when a metal oxide reacts with water?

A

metal hydroxide is only produced

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16
Q

what occurs to the pH of hydroxides down the group?

A

increases

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17
Q

ACID + BASE —–>

A

SALT + WATER

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18
Q

ACID + CARBONATE ——>

A

SALT + WATER + CARBON DIOXIDE

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19
Q

Do group 2 loose or gain electrons, if so are they oxidised or reduced, if so are they reducing agents or oxidising agents?

A

loose electrons
oxidised
reducing agents

20
Q

what are the name of the group 7 elements?

A

Halogens

21
Q

what is the structure of the group 7 elements, and what are the bonds and forces present?

A

simple molecular lattice, covalent bonds, london forces

22
Q

what type of molecules are the halogens?

A

diatomic

23
Q

how are covalent bonds described?

A

short and strong

24
Q

how are london forces described?

A

long and weak

25
Q

what state are F2, Cl2, Br2, and I2?

A

F2, Cl2 = gas
Br2 = liquid
I2 = solid

26
Q

describe and explain the mp and bp of the halogens

A

The boiling points and melting points of the halogens increase as you go down the group:
The molecules have more electrons.
So the London forces between the molecules are stronger.
Therefore, more energy is needed to break them.

27
Q

what is the half equation for flourine?

A

F2 + 2e- → 2F-

28
Q

describe and explain the reactivty of the halogens

A

Reactivity decreases down Group 7:
Halogen atoms get larger with more shells of electron
More inner shells shield incoming electrons more from the nucleus
Incoming electrons don’t get as close to the nucleus
So the attraction for incoming electrons is weaker
So ions form less easily

29
Q

what is a disproportionation reactions?

A

The simultaneous oxidation and reduction of the same species

30
Q

good use of chlorine

A

Chlorine kills bacteria (Sterilisation)

31
Q

Why do some people not want the water to be chlorinated?

A

chlorine is toxic

32
Q

chlorine disproportionation

A

Cl2 + H2O HCl + HOCl

33
Q

how does a displacement reaction work?

A

the more reactive reactiant replaces the less reactive one

34
Q

colour of iodine in cyclohexane

A

pink/purple/violet

35
Q

colour of bromine in cyclohexane

A

orange

36
Q

How to test for halogens

A
  1. add silver nitrate solution to see a precipitate

2. add dilute ammonia, and then conc ammonia to see the precipitate dissolve

37
Q

Chloride ion with silver nitrate

A

A white precipitate in silver nitrate

This dissolves in dilute ammonia and conc ammonia

38
Q

Bromide ion with silver nitrate

A

A cream precipitate in silver nitrate

This doesn’t dissolves in dilute ammonia, but will in conc ammonia

39
Q

Iodide ion with silver nitrate

A

A yellow precipitate in silver nitrate

This doesn’t dissolve in any ammonia at all, no matter how hot or concentrated

40
Q

what is the test for a carbonate, and how can you prove it is a carbonate?

A

Add dilute acid (normally nitric acid), there should be effervecence/fizzing
bubble through limewater, and a white ppt should form (turns the lime water white/cloudy)

41
Q

what is the test for a sulfate?

A

add barium nitrate, a white ppt should form

42
Q

what is the correct order for the ion tests?

A
  1. carbonate
  2. sulfate
  3. halide
43
Q

why carbonate first?

A

sulfate nor halide ions produce a gas with a dilute acid, therfore if no bubble are produced then you can carry on

44
Q

why sulfate second?

A

baso4 is white and insolube. barium carbonate is also white

45
Q

test for ammonium ions

A

boil in dilute sodium hydoxide, and test with damp rest litmus, the gas produced should turn the red litmus blue

MPW chemistry (14 decks)

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