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Chemistry A level > Topic 4 - inorganics > Flashcards

Topic 4 - inorganics Flashcards

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1
Q

How does ionisation energy change down group 2?

A

Decreases as more shielding

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2
Q

How does group 2 from Be - SR react with oxygen?

A

All burn vigorously except Be. 2M + O2 –> 2MO

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3
Q

How does Barium react with oxygen?

A

Vigorously. Ba + O2 –> 2BaO2

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4
Q

What is the trend on reactions of group II with water? and comparison to group 1?

A

Group 2 less reactive than comparative group 1. Increases in vigour down the group.

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5
Q

What is the equation for Mg and water?

A

Mg + H2O –> MgO + H2

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6
Q

What is the equation for Ca, Sr or Ba in water?

A

M + 2H2O –> M(OH)2 + H2

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7
Q

Explain water happens with Be and water?

A

Beryllium doesn’t react with water

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8
Q

What is the equation for group II and chlorine?

A

M + Cl2 –> MCl2

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9
Q

How do group II oxides react with water?

A

Form M(OH)2 except BeO

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10
Q

How do group II oxides react with dilute acids?

A

Forms salt and water

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11
Q

Why do group II hydroxides react with acids?

A

They are bases

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12
Q

How does group II sulphates solubility change?

A

Less soluble down the group.

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13
Q

How does group II hydroxides solubility change?

A

More soluble down group. All partially soluble

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14
Q

What changes the thermal stability of carbonates?

A

More stable = stronger CO bond = anion polarised less = large cation = more stable down group

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15
Q

How does thermal stability of group 1 carbonates change?

A

Li not stable under bunsen heat(Li2CO3 –> Li2O + CO2). All others are increasingly more stable

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16
Q

How does thermal stability of group 2 carbonates change?

A

More stable down group but, all decompose under heat to form MCO3 –> MO + CO2

17
Q

How does group II thermal stability of nitrates change down group?

A

More stable down group. Forms 2MO + 4NO2 + O2

18
Q

How does group 1 thermal stability of nitrates change?

A

More stable down group. All decompose (except Li) to MNO2 + O2. Lithium forms Li2O + NO2 + O2

19
Q

What are the flame tests of group 1 and II?

A

LI+ - Red. Na+ - yellow. K+ - Lilac. Ca2+ - Brick red. Sr2+ - Crimson. Ba2+ - Apple green

20
Q

What is chlorine’s appearance at rtp, in aq solution and hydrocarbon solution?

A

Green gas at rtp. Pale green in solutions.

21
Q

What is Bromine’s appearance at rtp, in aq solution and hydrocarbon solution?

A

Red/Brown liquid at rtp. Orange/Yellow in aq. Red in hydrocarbon solution.

22
Q

What is Iodine’s appearance at rtp, in aq solution and hydrocarbon solution?

A

Grey/black solid at rtp. Brown in aq. Violet in hydrocarbon solution.

23
Q

How does electronegativity change down group 7?

A

Decreases down the group as bigger element less electronegative.

24
Q

How does mtp change for group 7?

A

Increases down group as more London forces.

25
Q

What is noticeable about group 7 reactions with metals and non-metals?

A

More exothermic up the group with metals. More explosive up group with non-metals. E.g. Chlorine + H2 exlplode in sunlight, bromine needs catalyst and Iodine is very slow.

26
Q

How do group 7 act as oxidising agents?

A

Stronger oxidising agents up group as gain e- more easily.

27
Q

How do group 7’s reactions with conc. H2SO4 change?

A

Better reducing agents down group as lose electron more easily. Meaning HI and HBr form I2 and Br2 but KCl only forms HCl

28
Q

How do you test for a halide?

A

Add nitric acid and silver nitrate. Cl- forms white ppt. Br- cream and I- yellow.

29
Q

How can you test halide ppts after silver nitrate test?

A

Add ammonia solution, AgCl dissolves, AgBr only in conc. and AgI doesn’t.

30
Q

Are hydrogen halides soluble?

A

Yes, in water for acids.

31
Q

Why don’t we use Astatine?

A

It is radioactive

32
Q

Test for carbonate ion?

A

Add dilute acid, test gas with limewater. Goes cloudy as CO2 produced.

33
Q

Test for sulfate ion?

A

Add dilute HCl to solution followed by Barium Chloride. Forms white ppt.

34
Q

Test for Ammonium ion?

A

Warm with NaOH. Hold damp red litmus. Ammonia gas turns it blue

Chemistry A level (6 decks)

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