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chemistry > Topic 4 - Inorganic Chem & Periodic Table > Flashcards

Topic 4 - Inorganic Chem & Periodic Table Flashcards

Inorganic Chemistry and the periodic table

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1
Q

Why does ionisation energy decrease down G2 ? (reactivity increases)

A
  1. extra electron shell (shielding)
  2. outer electrons further away from the nucleus (lower electrostatic attraction)
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2
Q

What are the solubility trends depending on the compound anion?

A
  1. Group 2 elements that contain single charged negative ions INCREASE in solubility down the group
  2. Compounds that contain double charged negative ions DECREASE in solubility down the group
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3
Q

What happens when G2 burns in oxygen ?

A

produces metal oxides (solid white)

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4
Q

What is the solubility trends as you go down Group 2 when you react with hydroxide?

A

Increases down the group

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5
Q

What happens when G2 reacts with chlorine ?

A

produces metal chlorides (solid white)

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6
Q

Which G2 does not produce an alkaline when added to water ?

A
  1. beryllium (oxide) - doesn’t react with water
    beryllium (hydroxide) - insoluble
  2. magnesium (oxide) - reacts slowly
    magnesium (hydroxide) - low solubility
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7
Q

What is the solubility trends as you go down Group 2 when you react with sulfate?

A

Decreases down the group

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8
Q

What sulfate is insoluble in water?

A

Barium sulfate

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9
Q

What are compounds like magnesium hydroxide known to be ?

A

sparingly soluble because they have a low solubilty

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10
Q

EQUATION when metal oxides react with water

A

MO(s) + H2O(l) -> M(OH)2(aq)

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11
Q

EQUATION when metal hydroxides react with water

A

M(OH)2(s) –+H2O(l)–>M(OH)2(aq)

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12
Q

EQUATION when metal hydroxides react with dilute acid

A

M(OH)2(aq) + 2HCl(aq) –> MCl2 (aq) +2H2O(l)

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13
Q

EQUATION when metal oxides react with dilute acid

A

MO(s) +2HCl(aq) –> MCl2(aq) + H2O(l)

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14
Q

What is the flame colour of Li?

A

Red

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15
Q

Trend of thermal stability in G1 and G2 ?

A

increases down a group

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16
Q

What is the flame colour of Na?

A

orange/yellow

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17
Q

What is the flame colour of K?

A

lilac

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18
Q

What is the flame colour of Rb?

A

red

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19
Q

What is the flame colour of Cs?

A

blue

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20
Q

How are G1/G2 carbonate and nitrate ions made unstable ?

A

they are large anions made unstable by the presence of a cation as it polarises the anion (distorting it) - greater distortion = less stable

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21
Q

What is the flame colour of Ca?

A

brick-red

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22
Q

What is the flame colour of Sr?

A

crimson

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23
Q

What is the flame colour of Ba?

A

green

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24
Q

How do you do a flame test in 3 steps:

A
  1. MIX a small amount of the compound you’re testing with a few drops of hydrochloric acid.
    2.HEAT a piece of platinum or nichrome wire in a hot Bunsen flame to clean it
    3.DIP the wire into the compound/acid mixture. Hold it in a very hot flame and note the colour produced.
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25
Q

What causes most distortion ?

A

smaller cations - higher charge density

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26
Q

Why do bunsen burners produce different colours depending on the compound used?

A

Energy absorbed from flame= electrons move to higher energy levels.

Colours seen as the electrons fall back down to lower energy levels=release energy in the form light.

Difference in energy as electron move from higher and lower levels determines the wavelength of the light released= makes the colour of the light.

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27
Q

EXPLAIN the trend in thermal stability of G1/G2 ?

A

further down the group = larger cation = lower charge density = less distortion = more stable carbonate/nitrate ion

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28
Q

Which compounds are more thermally stable ? (G1 or G2)

A

Group 1

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29
Q

Why are G2 compunds less thermally stable than G1 compunds ?

A
  • the greater the charge on cation, the greater the distortion and less stability
  • G2 have +2 charge compared to a +1 charge
  • therefore less stable
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30
Q

How to test the thermal stability of nitrates.

A
  1. measure how long it takes until a certain amount of oxygen is produced
  2. measure how long until an amount of brown gas is produced
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31
Q

How to test the thermal stability of carbonates

A
  1. how long it takes for an amount of CO2 to be produced

CO2 test- add limewater which is a saturated solution of calcium hydroxide.Turns cloudy

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32
Q

Do Group 1 carbonates decompose? and if they do which one can decompose.

A

they are thermally stable - you can’t heat them w a bunsen burner to make them decompose

HOWEVER THERE IS ALWAYS ONE SPECIAL ONE, Li2CO3 which decomposes to Li2O and CO2

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33
Q

Do Group 2 carbonates decompose?

A

they do decompose and they form an oxide and carbon dioxide

General formula: MCO3 –> MO + CO2
E.g. CaCO3 –> CaO + CO2

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34
Q

Do G2 nitrates decompose ?

A

yes - forms metal oxide, nitrogen dioxide and oxygen

general formula : 2M(NO3)2
—-> 2MO + 4NO2 + O2

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35
Q

What is the colour of fluorine?

A

pale yellow

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36
Q

What type of reaction is a halogen and halide reaction?

A

redox (displacement)

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37
Q

Explain the displacement reaction between halogens and halides (in terms of redox)

A

Thing being displaced is oxidised
Thing that does displacing is reduction

38
Q

What is the colour of chlorine?

A

green

39
Q

What is the colour of bromine?

A

red-brown

40
Q

What is the colour of iodine?

A

grey

41
Q

What is the physical state of fluorine?

A

gas

42
Q

What is the physical state of chlorine?

A

gas

43
Q

What is the physical state of bromine?

A

liquid

44
Q

ionic equation for chlorine water (Cl2) (colourless) + potassium chloride (KCl) (colourless)

A

no reaction

45
Q

What is Halogens natural state they exist in?

A

Covalent Diatomic Molecules

46
Q

Are Halogens polar or non- polar and why?

A

Non-polar because they have low solubility in water

47
Q

Colour of chlorine when in water and hexane

A

both virtually colourless

48
Q

ionic equation for chlorine water (Cl2) (colourless) + potassium bromide (KBr) (colourless)

A

Cl2 + 2(Br)- —> 2(Cl)- + Br2

orange

49
Q

Colour of bromine when in water and hexane

A

yellow/orange and orange/red

50
Q

Colour of Iodine when in water and hexane

A

Brown and pink/violet

51
Q

ionic equation for chlorine water (Cl2) (colourless) + potassium iodide (KI) (colourless)

A

Cl2 + 2(I)- —> 2(Cl)- + I2

brown

52
Q

ionic equation for bromine water (Br2) (orange) + potassium chloride (KCl) (colourless)

A

no reaction

53
Q

ionic equation for bromine water (Br2) (orange) + potassium bromide (KBr) (colourless)

A

no reaction

54
Q

ionic equation for bromine water (Br2) (orange) + potassium iodide (KI) (colourless)

A

Br2 + 2(I)- —> 2(Br)- + I2

brown2

55
Q

ionic equation for iodine solution (I2) (brown) + potassium chloride (KCl) (colourless)

A

no reaction

56
Q

ionic equation for iodine solution (I2) (brown) + potassium bromide (KBr) (colourless)

A

no reaction

57
Q

ionic equation for iodine solution (I2) (brown) + potassium iodide (KI) (colourless)

A

no reaction

58
Q

How to make the colour changes of halogen-halide reactions easier to see ?

A

shake reaction mixture with and organic solvent eg hexane
halogen will dissolve in organic solvent and settle out as a distinct layer above the aqueous solution

59
Q

Reactivity trend of group 7 ?

A

less reactive down group

60
Q

What ‘agent’ are halogens in terms of redox

A

oxising agents - usually react by gaining an electron therefore are reduced and oxidise other substance

61
Q

Explain the reactivity trend of group 7 ?

A

atoms become larger = electrons further away = shielding = harder for nucleus to attract electron to form ion

62
Q

what is the trend for melting and boiling point in G7

A

increases down the group

63
Q

EXPLAIN the trend for mp/bp in G7

A

increase in electron shells = stronger London forces = harder to overcome intermolecular forces

64
Q

Which halides will chlorine replace

A

bromide and iodide

65
Q

which halides will bromine replace

A

iodide

66
Q

which halide will iodide replace

A

none

67
Q

what happens when you mix cold chlorine gas and dilute aqueous sodium hydroxide

A

bleach is formed

68
Q

Trend of reducing power in halides ?

A

increases down the group

69
Q

EXPLAIN the trend of reducing power of halides ?

A

attraction of the outermost electron and nucleus weakens down the group (shielding and distance) therefore are oxidised more easily

70
Q

what happens when halides react with concentrated sulfuric acid?

A

produces hydrogen hallide

71
Q

explain the reaction of KF or KCl with H₂SO₄ ? include equation

A

KF (s) + H₂SO₄ (l) →KHSO₄ (s) + HF (g)

  • misty fumes seen as gas comes into contact with moisture in air
  • fluoride/chloride ions not strong enough reducing agents to reduce H₂SO₄ therefore reaction stops
  • oxidation numbers stay the same = not redox
72
Q

explain the reaction of KBr with H₂SO₄ ? include equation

A

reaction 1: KBr (s) + H₂SO₄ (l) →KHSO₄ (s) + HBr (g)

reaction 2: 2HBr (aq) + H₂SO₄ (l) →Br₂ (g) + SO₂ (g) + 2H₂O (l)

  • first = misty fumes
  • second = bromide ions stronger reducing agents = redox reaction
  • second = choking fumes of SO₂ and orange fumes of Br₂
73
Q

When halides react with H₂SO₄ what oxidation states should be assessed?

A

halide and sulfur

74
Q

explain the reaction of KI with H₂SO₄ ? include equation

A

reaction 1: KI (s) + H₂SO₄ (l) →KHSO₄ (s) + HI (g)

reaction 2: 2HI (g) + H₂SO₄ (l) → I₂ (s) + SO₂ (g) + 2H₂O (l)

reaction 3 : 6HI (g) + SO₂ → H₂S (g) + 3I₂ (s) + 2H₂O

  • first = same initial reaction
  • second = iodide ion reduce H₂SO₄
  • third = iodide ions very strong reducing agent therefore keeps going and reduces SO₂ to H₂S
  • third = H₂S gas is toxic and smells of bad eggs
75
Q

What type of gas are hydrogen halides ?

A

acidic

76
Q

What happens when hydrogen halides dissolve in water ?

A

produces misty fumes of acidic gas (can happen with moisture in air)

77
Q

What happens when hydrogen halides react with ammonia gas ?

A

white fumes produced

78
Q

What can be used as a test for halide ? and why

A

addition of silver ions as coloured precipitate formed

79
Q

Describe the test for halide ions ?

A
  1. add dilute nitric acid to remove ions that may interfere with reaction
  2. add silver nitrate solution
  3. precipitate of silver halide formed
80
Q

What happens when fluoride is added to silver nitrate solution ?

A

no precipitate as AgF is soluble

81
Q

What colour precipitate is formed when chloride reacts with silver nitrate ?

A

white (milk)

82
Q

What colour precipitate is formed when bromide reacts with silver nitrate ?

A

cream (cream)

83
Q

What colour precipitate is formed when iodide reacts with silver nitrate ?

A

yellow (butter)

84
Q

Why is a test for halide solutions difficult to identify when silver nitrate added ?

A

colours are very similar

85
Q

What can be added to the silver nitrate test for halide ions ?

A

ammonia solution

86
Q

What happens when silver chloride (white) reacts with ammonia solution ?

A

dissolves to give colourless solution

87
Q

What happens when silver bromide (cream) reacts with ammonia solution ?

A

precipitate remains unchanged = dilute ammonia
dissolves and colourless = concentrated ammonia

88
Q

What happens when silver iodide (yellow) reacts with ammonia solution ?

A

does not dissolve even in concentrated ammonia solution

89
Q

Describe the test for carbonate ions (CO₃²⁻) or hydrogencarbonate ions (HCO₃⁻)

A
  1. when either react with hydrochloric acid they fizz as carbon dioxide produced
  2. test for carbon dioxide with limewater = turns it cloudy
  3. bubble gas though test tube of limewater and watch
90
Q

Describe the test for sulfates (the sulfate ion SO₄²⁻ )

A
  1. add dilute hydrochloric acid followed by barium chloride solution
  2. HCl added to remove traces of carbonate ions from previous test as would also produce a precipitate
  3. if sulfate ions present in original compound, white precipitate of barium sulfate formed
91
Q

Describe the test for ammonium compounds - include equation

A
  1. add sodium hydroxide in a test tube with supposed compound with NH₄⁺
  2. heat gently
  3. hold damp litmus paper over test tube and if NH₃ given off should turn blue

NH₄X (aq) + NaOH (aq)→NH₃ (g) + H₂O (l) + NaX (aq)

chemistry (10 decks)

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