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[OBSELETE] S - Chem > topic 4 > Flashcards

topic 4 Flashcards

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1
Q

what is the reactions of group 2 metals with oxygen

A

metal + oxygen -> metal oxide

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2
Q

what is the reactions of group 2 metals with chlorine

A

metal + chlorine -> metal chloride

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3
Q

what is the reaction of group 2 metals with water

A

metal + (cold) water -> metal hydroxide + hydrogen

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4
Q

what are the group 1 flame colours

A

lithium- red
sodium- yellow
potassium- lilac
rubidium- red
caesium- blue

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5
Q

what are the group 2 flame colours

A

magnesium- no flame colour
calcium- orange-red
strontium- red
barium- pale green
copper- blue-green

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5
Q

why does magnesium have no flame colour

A

energy released isnt in visible light spectrum

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5
Q

what colour is chlorine at room temperature

A

pale green gas

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5
Q

what colour is bromine at room temp

A

brown liquid

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5
Q

what colour is iodine at room temp

A

grey-black solid

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5
Q

what colour is chlorine in aqueous solution

A

pale green

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5
Q

what colour is bromine is aqueous solution

A

orange/yellow

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5
Q

what colour is iodine in aqueous solution

A

brown

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5
Q

what colour is chlorine when dissolved in a hydrocarbon solvent

A

pale green

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5
Q

what colour is bromine when dissolved in hydrocarbon solvent

A

red

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6
Q

what colour is iodine in hydrocarbonsolvent

A

purple

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7
Q

what is the experimental procedure for thermal decomposition

A

-measure some of the carbonate into a test tube
- fit a delivery tube to the test tube and clamp it so that the delivery tube end in a second test tube containing limewater
- heat the test tube containing the carbonate and then heat it more strongly

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8
Q

how can you test for chlorine

A

chlorine turns damp blue litmus red and then bleaches it
chlorine also displaces bromine and iodine from bromide or iodide solutions

9
Q

how can you test for bromine

A

bromine is orang/red when dissolved in an organic solvent
bromine displaces iodine from an iodide solution

10
Q

how can you test for iodine

A

iodine turns starch black
is also decolourised by thiosulphate solution
its brown in water but purple in organic solvents

11
Q

what kind of solvents do halogens dissolve in

A

non polar solvents such as hexane

12
Q

why does the colour change occur in halogen displacement reactions

A

when the halogn is displaced, the solution turns into the colour of the halogen that is displaced in aqueous solution
e.g if iodine is displaced, aqueous solution would turn brown (which is its colour when dissolved in aqueous solution)

13
Q

why does reducing power increase down group 7?

A

this is because the halide ion becomes larger
outer electrons are further from the nucleus
less attraction between the nucleus and the outer e-
easier to lose e- do it can be used to reduce other species (and donate its electron)

14
Q

when concentrated sulfuric acid is added to (e.g potassium) chloride what can be produce

A

misty white fumes
hydrogen halide is formed
KHSO4

15
Q

when concentrated sulfuric acid is added to (potassium) bromide what can be produced

A

brown misty fumes
bromine gas is formed
sulphur dioxide is formed

16
Q

when concentrated sulfuric acid is added to (potassium) iodide what can be produced

A

iodine gas
water
sulphur dioxide
suphur
hydrogen sulphide

17
Q

what are the colours of the precipitates formed when silver nitrate is added to halides

A

silver halide forms
silver chloride- white
silver bromide- cream
silver iodide- yellow

18
Q

what is the effect of sunlight on the halides

A

chloride- white precipitate turns purple- grey
bromide- cream precipitate turns green- yellow
iodide- no effect

19
Q

what happens when ammonia solution is added to halides

A

chloride- precipitate dissolves in dilute and conc. ammonia solution
bromide- precipitate dissolves in conc. ammonia solution
iodide- doesnt dissolve

20
Q

what is the disproportionation reaction of chlorine with water

A

Cl2(g) + H2O(l) -> HClO(aq) + HCL(aq)

21
Q

what is the reaction of chlorine with cold dilute sodium hydroxide

A

disproportionates to chlorate (I) and chloride
2NaOH + CL2 -> NaCl + NaClO + H2O

22
Q

what is the reaction of chlorine with hot concentrated sodium hydroxide solution

A

3Cl + 6NaOH -> 5NaCl + NaClO3 + 3H2O

23
Q

how do you test for carbonate ions

A

add dilute hydrochloric acid is added to the test compound
bubbles of gas produced which is carbon dioxide
limewater is used to confirm that the gas is CO2

24
Q

how to test for sulphate ions

A

detected using barium chloride
- add a few drops of dilute hydrochloric acid
- then add a few drops of barium chloride solution
- a white precipitate of barium sulphate forms if sulphate ions are present

25
Q

how can you test for ammonium ions (NH4+)

A
  • add dilute sodium hydroxide and gently warm
    is ammonium ions present - ammonia gas will form
  • ammonia gas turns damp red litmus paper blue
26
Q

What is the formula for group 1 carbonates

A

X2CO3

27
Q

What is the formula for group 2 nitrates

A

X(NO3)2

28
Q

What is the formula for group 1 nitrates

A

XNO3

29
Q

What is the formula for group 2 carbonates

A

XCO3

30
Q

why is iodine unable to displace bromine or chlorine

A

its a weaker oxidising agent than them both

31
Q

how can you compare the rate of decomposition of carbonates

A

use of delivery tube to bubble gas into limewater
compare time taken for lime water to go cloudy

32
Q

what is the trend in reactivity of haloalkanes

A

increases down the group
this is because the C-X bond enthalpy decreases

[OBSELETE] S - Chem (19 decks)

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