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A Level Chemistry- KE > inorganic chemistry and the periodic table > Flashcards

inorganic chemistry and the periodic table Flashcards

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1
Q

why does ionisation energy decrease down group 2?

A

-electron shells of elements increase by 1 down G2
-extra inner shells shield outer electrons from attraction of positive nucleus
-atomic radius increases=outer electrons further away from nucleus=reduction in electrostatic attraction
-these factors make it easier to remove outer electrons∴ionisation energy decreases

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2
Q

does the increase in positive charge of the nucleus (due to extra protons) affect ionisation energy of group 2 elements?

A

no, effect is overridden by extra shells

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3
Q

what is the trend in reactivity down group 2?

A

increases down the group

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4
Q

what is the trend in ionisation energy down group 2?

A

decreases down the group

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5
Q

why does reactivity increase down group 2?

A

elements of G2 react by losing outer 2 electrons ∴ higher ionisation energies makes it more difficult to lose the outer 2 electrons ∴ will be less reactive

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6
Q

what happens when a group 2 metal reacts with water?

A

forms a metal hydroxide and hydrogen
Ca + 2H₂O→Ca(OH)₂ + H₂

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7
Q

How does Be react with water?

A

doesn’t react

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8
Q

How does Mg react with water?

A

very slowly

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9
Q

How does Ca react with water?

A

steadily

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10
Q

How does Sr react with water?

A

fairly quickly

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11
Q

How does Ba react with water?

A

rapidly- effervescence

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12
Q

what happens when a group 2 metal burns in oxygen?

A

solid white oxide formed
2Ca + O₂→2CaO

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13
Q

what happens when a group 2 metal reacts with chlorine?

A

forms solid white chlorides
Ca + Cl₂ → CaCl₂

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14
Q

what are the oxides and hydroxides of group 2?

A

bases

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15
Q

what happens when oxides and hydroxides of group 2 react with dilute acids?

A

they neutralise the dilute acids because they are bases,, also form solutions for corresponding salts

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16
Q

what happens when oxides and hydroxides of group 2 react with water?

A

form alkaline solutions,, more alkaline as you go down the group

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17
Q

why do oxides form more strongly alkaline solutions as you go down the group?

A

the hydroxides get more soluble

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18
Q

what is the trend in solubility of group 2 hydroxides (and other singly charged ions) down the group?

A

increased solubility

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19
Q

what is the trend in solubility of group 2 doubly charged negative ions (e.g. SO₄²⁻ sulfates) down the group?

A

decrease solubility

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20
Q

is barium sulfate completely insoluble?

A

yes

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21
Q

what substance helps detect carbonate ions and hydrocarbonate ions?

A

HCl

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22
Q

what happens when HCl and CO₃²⁻/HCO₃⁻ react?

A

they fizz and give off CO₂
CO₃²(s) + 2H⁺(aq) → CO₂(g) + H₂O(l)

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23
Q

how can you test for CO₂?

A

lime water goes cloudy

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24
Q

how do you test for sulfates?

A

HCl and Barium Chloride

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25
Q

how do you identify a sulfate ion?

A

-add dilute HCl followed by Barium chloride solution
-if white participate of barium sulfate forms it means the original compound contained a sulfate

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26
Q

why is HCl added in the test for sulfate ions?

A

to get rid of traces of carbonate ions so they don’t affect results

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27
Q

how to test for ammonium compounds?

A

-damp red litmus paper
-because ammonia gas (NH₃) is alkaline it will turn the red litmus paper blue

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28
Q

how to test for ammonium ions (NH₄⁺)?

A

-add sodium hydroxide to unknown substance into a test tube and gently heat the mixture
-if ammonia is given off NH₄⁺ ions are present
-this can be tested using damp litmus paper

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29
Q

why does litmus paper need to be damp when testing for ammonia gas?

A

so the gas can dissolve and make the colour change

30
Q

why is beryllium oxide an exception from the oxides of the group 2 metals?

A

it does not react with water

31
Q

what happens when oxides of group 2 are with water?

A

they react readily and form soluble metal hydroxides that are very alkaline due to the OH⁻

32
Q

why is magnesium oxide an exception from the oxides of the group 2 metals?

A

reacts slowly and the hydroxide formed is not very soluble

33
Q

what is thermal decomposition?

A

when a substance breaks down when heated

34
Q

the more thermally stable a substance is…..

A

the more heat it will take to break it down

35
Q

what colour will the reaction mixture turn if bromine is displaced?

A

orange

36
Q

what colour will the reaction mixture turn if iodine is displaced?

A

brown

37
Q

how else can you see the results of a halide-halogen redox reaction?

A

by shaking the mixture with hexane (organic solvent) so halogen will dissolve and settle as a distinct layer above aqueous solution

38
Q

how is chlorine used in water treatment to kill bacteria?

A

-mixing chlorine and water is a disproportionation reaction which produces HCl and HClO(hypochlorous acid)
-HClO ionises to make chlorate ions which kill bacteria in water

39
Q

flame colour Li?

A

red

40
Q

flame colour Na?

A

orange/yellow

41
Q

flame colour K?

A

lilac

42
Q

flame colour Rb?

A

red

43
Q

flame colour Cs?

A

blue

44
Q

flame colour Ca?

A

brick-red

45
Q

flame colour Sr?

A

crimson

46
Q

flame colour Ba?

A

green

47
Q

why do the flames colour of group 1 and 2 elements vary?

A

-energy absorbed from flame causes electrons to move to higher energy levels
-colour seen as electron falls back to lower energy level releasing energy in the form of light
-difference in energy between higher and lower levels determines wavelength of light released (determines colour of light)

48
Q

why does thermal stability of carbonates and nitrates increase down groups 1 and 2?

A
49
Q

halogen + group 1/2 metal?

A

halide salt

50
Q

how are halide salts formed?

A

halogen oxidises group 1/2 metals (halogen reduced itself)

51
Q

why should reactions involving halogens be carried out in a fume cupboard?

A

halogens are toxic

52
Q

what happens when a cold alkali reacts with a halogen?

A

disproportionation reaction (halogen is simultaneously reduced and oxidised)

53
Q

how is bleach formed?

A

disproportionation reaction with chlorine gas + cold dilute aqueous 2NaOH

NaCl also formed and water

54
Q

what is the chemical name for bleach?

A

sodium chlorate I (NaClO)

55
Q

what is the trend in reducing power for the halides? (halogen ions)

A

reducing power decreases down the group because=
-ions get bigger down the group=electrons further away from nucleus=attraction gets weaker=electron is lost easily
-there are extra inner electron shells so shielding effect is greater

56
Q

what happens in the reaction of KF/KCl with sulfuric acid?

A

-HF/HCl produced, misty fumes
-Fluoride and chloride ions are not strong enough reducing agents to reduce sulfuric acid so reaction stops
-not a redox reaction

57
Q

what happens in the reaction of KBr with sulfuric acid?

A

-HBr formed (first step),, misty fumes
-HBr further reduces sulfuric acid (as it is a stronger oxidizing agent) into Br₂+SO₂+H₂O (second step),, orange fumes of bromine released,,redox reaction

58
Q

are halide ions reduced or oxidised in their reactions with H₂SO₄?

A

oxidised, they lose electrons and become positive

59
Q

what happens in the reaction of KI with sulfuric acid?

A

-HI formed (first step)
-HI reduces H₂SO₄ into I₂+SO₂+H₂O
-iodine ions are strong reducing agents so further reduce SO₂ to H₂S which smells of rotten egg

60
Q

why are iodine ions the strongest reducing agents?

A

because iodine ions reduces sulfur in H₂SO₄
from +6 to 0,,,, Br goes from +6 to +4

61
Q

what happens what hydrogen halides gases dissolve in water?

A

they become acids as hydrogen halides are acidic gases e.g. hydrogen chloride to hydrochloric acid

62
Q

what happens when a hydrogen halide reacts with ammonia gas?

A

white fumes produced forming NH₄Cl

63
Q

What to halide ions react with to form precipitate which is a test for halides?

A

silver nitrate solution AgNO₃

64
Q

what is the hazard of silver nitrate?

A

corrosive

65
Q

what precipitate is formed in the silver nitrate test for fluoride?

A

there is no precipitate as AgF is soluble

66
Q

what precipitate is formed in the silver nitrate test for chloride?

A

white (milk)

67
Q

what precipitate is formed in the silver nitrate test for bromide?

A

cream (cream)

68
Q

what precipitate is formed in the silver nitrate test for iodide?

A

yellow (butter)

69
Q

How can you further tell what halide has been identified from silver nitrate test if precipitates look similar?

A

add ammonia solution

70
Q

what happens when ammonia solution is added to AgCl precipitate?

A

precipitate dissolves in dilute ammonia solution to make colourless liquid

71
Q

what happens when ammonia solution is added to AgBr precipitate?

A

only dissolves in concentrated ammonia solution to give colourless solution (would not happen in dilute)

72
Q

what happens when ammonia solution is added to AgI precipitate?

A

doesn’t dissolve at all regardless of concentration

A Level Chemistry- KE (15 decks)

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