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Alevel Chemistry Edexcel > Topic 4 - Inorganic Chemistry and Periodic Table > Flashcards

Topic 4 - Inorganic Chemistry and Periodic Table Flashcards

1
Q

How does the reactivity change down group 2?

A

increases

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2
Q

Why does the reactivity increase down group 2?

A
  • more electrons/electron shells
  • outer electrons further from nucleus
  • weaker electrostatic attraction between nucleus and outer electrons
  • less energy required to remove electrons
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3
Q

How does the ionisation energy change down group 2?

A

decreases

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4
Q

Why does the ionisation energy decrease down group 2?

A
  • more electrons/electron shells
  • outer electrons further from nucleus
  • weaker electrostatic attraction between nucleus and outer electrons
  • less energy required to remove electrons
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5
Q

How does the atomic radii change down group 2?

A

increases

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6
Q

Why does the atomic radii increase down group 2?

A
  • more electrons

- more electron shells

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7
Q

How does the solubility of sulphates change down group 2?

A

decrease

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8
Q

How does the solubility of hydroxides change down group 2?

A

increase

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9
Q

group 2 metal + oxygen ->

A

metal oxide

white solid

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10
Q

group 2 metal + water ->

liquid water

A

metal hydroxide + hydrogen

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11
Q

group 2 metal + water ->

steam

A

metal oxide + hydrogen

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12
Q

group 2 metal + chlorine ->

A

metal chloride

white solid

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13
Q

group 2 oxide + water ->

A

metal hydroxide

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14
Q

thermal decomposition of group 2 carbonates (and Li2CO3)

carbonates ->

A

metal oxide + carbon dioxide

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15
Q

thermal decomposition of group 1 nitrates (except LiNO3)

nitrate ->

A

metal oxide + nitrogen dioxide

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16
Q

What is thermal decomposition?

A

breaks down of a substance into two or more substances due to heat

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17
Q

What is thermal stability?

A

likelyhood of a substance to undergo a change at a particular temperature
-how easily a substance breaks down under heat

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18
Q

thermal decomposition of group 1 nitrates (except Li2NO3)
nitrate ->
XNO3

A

group 1 nitrate + oxygen

XNO2 +1/2 O2

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19
Q

thermal decomposition of group 2 nitrates
nitrate ->
X(NO3)2

A

metal oxide + nitrogen dioxide + oxygen

XO + 2NO2 + 1/2 O2

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20
Q

How do group 1 and 2 nitrates and carbonates change in thermal stability down the group?

A

increase in thermal stability

-require a higher temperature to thermally decompose

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21
Q

Describe the change in thermal stability down the group (1 or 2)

A

-ionic radii decreases (-more energy levels)
-volume of ion increases
-charge remains constant
∴ charge density decreases
-have less of a polarising power on negative ions
-cause less distortion of electron cloud
-higher thermal stability

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22
Q

Describe the change in thermal stability across a period

A
  • same period ∴ same number of energy levels
  • group further to right has more protons -greater nuclear charge so greater electrostatic attraction between nucleus and outer electrons
  • group 2 ions have higher charge and lower volume than group 1 ions ∴ higher charge density
  • cause more distortion of electron cloud of negative ion
  • lower thermal stability
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23
Q

What are the three aspects to Fajan’s rules that allow us to predict a compound’s distortion of electron density?

A
  • high charge of cation (+ve ion)
  • small cation (+ve ion)
  • large anion (-ve ion)
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24
Q

What does a higher charge and smaller ionic radii result in?

A
  • higher charge density
  • more distortion of electron density
  • less thermally stable
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25
Q

Describe the method of a flame test

A
  • nichrome wire loop is dipped into concentrated HCl and in the flame to clean it
  • dipped back in HCl and then into the sample
  • sample is held in flame and flame colour is observed
26
Q

What is the flame colour of Li+?

A

red

27
Q

What is the flame colour of Ca2+?

A

orange red (brick red)

28
Q

What is the flame colour of Sr2+?

A

deep red

29
Q

What is the flame colour of Ba2+?

A

pale green (yellow green)

30
Q

Describe how an emission spectra works

A
  • electrons absorb specific wavelengths of light so get excited and are promoted to a higher energy level
  • electrons then go back to their ground state and release wavelengths of energy equivalent to the gap of energy levels
  • wavelength of light emitted is seen as a flame or as an emission spectra
31
Q

How do melting and boiling points change down group 7?

A

increase

32
Q

Why do melting and boiling points increase down group 7?

A
  • have more electrons
  • therefore have stronger London forces
  • requires more energy to overcome IMF so mp/bps increase
33
Q

How does electronegativity change down group 7?

A

decreases

34
Q

Why does electronegativity decrease down group 7?

A
  • more electrons
  • more shielding
  • outer electrons further from nucleus
  • less nuclear attraction
35
Q

How does reactivity change down group 7?

A

decreases

36
Q

Why does reactivity decrease down group 7?

A
  • more electrons
  • more shielding
  • outer electrons further from nucleus
  • less nuclear attraction so harder to gain an electron
37
Q

How does atomic radii change down group 7?

A

increase

38
Q

Why does atomic radii increase down group 7?

A
  • more electrons and more energy levels
  • more shielding
  • outer electrons further from nucleus
  • less nuclear attraction
39
Q

How does oxidising power change down group 7?

A

decreases

40
Q

How does the reducing power of halides change?

A

increases down group

41
Q

general reaction of halogens in cold NaOH

X2 + 2NaOH ->

A

NaXO + NaX + H2O

42
Q

halogen + group 1/2 metal ->

A

halide salt (eg. NaCl)

43
Q

Why does chlorine make water safe to drink/swim in?

A

Chlorine reacts with water in a disproportionation reaction to produce hypochloride
-hypochloride ionises to make chlorate ions (ClO-) which kill bacteria

44
Q

halogen + iron ->

A

iron halide
FeX3 (for strong oxidising agents -Cl and Br)
(FeI2 for iodine as it is a weaker oxidising agent so can only remove one electron)

45
Q

halogen + metal halide ->

A

halogen + metal halide

displacement reaction

46
Q

halide salt + sulfuric acid (H2SO4) ->

A

depends on reducing ability of halide
generally: NaHSO4 + HX
(with strong reducing agents like iodide, HX then reacts with acid again to form hydrogen sulfide (H2S), halogen and water)

47
Q

halide + silver nitrate solution ->

AgNO3 + NaX ->

A

silver halide + sodium nitrate

AgX + NaNO3

48
Q

What colour precipitate do chloride ions form with silver nitrate?

A

white precipitate

49
Q

What colour precipitate do bromide ions form with silver nitrate?

A

cream precipitate

50
Q

What colour precipitate do iodide ions form with silver nitrate?

A

yellow precipitate

51
Q

Ag+(aq) + X-(aq) ->

A

AgX (s)

52
Q

Does silver chloride redissolve in ammonia solution? (NH3)

A

Yes, both in dilute and concentrated NH3

53
Q

Does silver bromide redissolve in ammonia solution? (NH3)

A

Doesn’t in dilute NH3 but does redissolve in concentrated NH3

54
Q

Does silver iodide redissolve in ammonia solution? (NH3)

A

Doesn’t redissolve in dilute or concentrated NH3

55
Q

How can you test for halide ions?

A
  • add silver nitrate solution (AgNO3) and observe colour of precipitate formed (white = Cl, cream = Br, yellow = I)
  • add ammonia (NH3) (Cl will redissolve in dilute NH3, Cl and Br will redissolve in concentrated NH3)
56
Q

hydrogen halide in water

A

dissolves

forms H+ and X-

57
Q

hydrogen halide + ammonia ->

HX + NH3 ->

A

ammonium halide
NH4X
(white fumes)

58
Q

How do you test for carbonate ions(CO3 2-)?

A

add dilute HCl
positive result: effervescence (fizzing) from carbon dioxide produced
-can test carbon dioxide by bubbling it through lime water using a delivery tube -will turn lime water cloudy

59
Q

How do you test for sulfate ions (SO4 2-)?

A

add dilute HCl (to remove any carbonate ions) followed by barium chloride solution (BaCl2)
positive result: white precipitate formed (BaSO4)

60
Q

How do you test for ammonium ions (NH4+)?

A

add sodium hydroxide solution
warm
positive result: produces ammonia (NH3)
-ammonia turns damp red litmus paper blue
-float a glass rod (previously dipped in HCl) and a white dense smoke will be produced (NH4Cl)

Alevel Chemistry Edexcel (19 decks)

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