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A2 Chemistry > Inorganic > Flashcards

Inorganic Flashcards

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1
Q

General trend in ionisation energies going across period 3?

A

Increase except at Al and S.
This is due to different orbitals of lower energy.
General trend is due to increasing nuclear charge and decreasing distance from nucleus.

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2
Q

Trend in atomic radius for period 3?

A

Decreases going across, because the number of electrons increases with the nuclear charge, creating a greater force of attraction.

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3
Q

Electronegativity trend for period 3

A

Increases going along,

Nuclear charge increases with power to attract

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4
Q

Melting and boiling trends for period 3

A

Increases with Metallics
Slight decrease with giant Covalent
Gradual decrease with simple molecular

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5
Q

Sodium with water

A

2Na + 2H2O –> 2NaOH + H2

Exothermic reaction
Colourless solution

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6
Q

Magnesiums reaction with water

A

Slow reaction with water
Mg + 2H2O –> Mg(OH)2 + H2

Burns in steam
Mg + H2O –> MgO + H2

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7
Q

Aluminiums reaction with water

A

Slow reaction due strong aluminium oxide layer on metal which continues to build up during the reaction

3Al + 3H2O –> Al2O3 + 3H2

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8
Q

Silicons reaction with water

A

Depends on type of silicon used

So + 2H2Oo –> SiO2 + 2H2

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9
Q

Phosphorus reaction with water

A

None

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10
Q

Sulphur reaction with water

A

None

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11
Q

Chlorine reaction with water

A

Dissolves in water to give green solution.

Cl2 + H2O HCl + HOCl

In sunlight chloric acid decomposes to form more HCl

2Cl2 + 2H2O –> 4HCl +O2

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12
Q

Argon reaction with water

A

None

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13
Q

Sodium reaction with oxygen

A

Burn in oxygen with an orange flame to produce a white solid mixture of sodium oxide and sodium peroxide

4Na + O2 –> 2Na2O
Or
2Na + O2 –> Na2O2

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14
Q

Magnesium reaction with oxygen

A

Burns in oxygen with intense white flame to give white solid MgO

2Mg + O2 –> 2MgO

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15
Q

Aluminium reaction with oxygen

A

Will burn if powdered, due to strong oxide layer. White sparkles

4Al + 3O2 –> 2Al2O3

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16
Q

Silicons reaction with oxygen

A

Will burn if heated strongly enough

Si + O2 –> SiO2

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17
Q

Phosphorus reaction with water

A

White phosphorus catches fire spontaneously in air, burning with a white flame and producing clouds of white smoke (P2O6 + P4O10)
Proportions of these depend on amount of oxygen available, in an excess, product is almost all phosphorus (V) oxide

P4 + 3O2 –> P4O6
Or
P4 + 5O2 –> P4O10

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18
Q

Sodium oxide

A

Na2O

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19
Q

Magnesium oxide

A

MgO

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20
Q

Aluminium oxide

A

Al2O3

21
Q

Silicon oxide

A

SiO2

22
Q

Phosphorus oxide

A

P4O10

P4O6

23
Q

Sulphur oxides

A

SO3

SO2

24
Q

Chlorine oxides

A

Cl2O7

Cl2O

25
Q

Fluoride and chloride ions reducing ability

A

Won’t reduce concentrated sulphuric acid

26
Q

Bromide ions reduction on concentrated sulphuric acid

A

Reduces sulphuric acid to sulphur dioxide.

Bromide ions are oxidised to bromine

27
Q

Iodide ions reduction of sulphuric acid

A

Sulphuric acid reduces to hydrogen sulphide.

The iodide ions are oxidised to iodine

28
Q

Trend in reducing ability of halide ions

A

Increase going down the group

29
Q

Suggest why the melting point of magnesium oxide is much higher than the melting point of magnesium chloride.

A

Charge on ion bigger than on chloride
Oxide ion is smaller than chloride
These cause stronger electrostatic attraction

30
Q

Why is Al(OH)3 insoluble in water ?

A

Large lattice energy
Strong covalent bonds
Positive enthalpy of solution
Positive Gibbs free energy change

31
Q

What would you observe when magnesium reacts with water at high temperatures?

A

White powder

Bright white flame

32
Q

Equation with magnesium reacts with water

A

Mg + H2O –> MgO + H2

33
Q

Why does magnesium have a higher melting point than sodium?

A

Mg2+ has higher charge than Na+

It attracts delocalised electrons more strongly

34
Q

What properties of silicon dioxide are as a result of its structure and bonding?

A 
High melting and boiling point
Hard
Brittle
Not malleable
Insoluble
Non conductor
35
Q

What are 2 properties of MgO caused by their structure and bonding which can be tested?

A

High melting point

Molten oxide conducts electricity

36
Q

Explain the structure and bonding in phosphorus (V) oxide which causes its melting point to be lower than silicon dioxide.

A

Molecular with covalent bonding

Intermolecular forces are easy to overcome

37
Q

Why is phosphor (V) oxide represented as P4O10 rather than P2O5?

A

Exists as P4O10

Molecular formula

38
Q

Why does phosphorus (V) oxide have a higher melting point hat sulphur (IV) oxide?

A

P4O10 is a larger molecule with a greater surface area and more electrons, so it has stronger VDWs forces which require more energy to break.

39
Q

Why can an excess of MgO be used to neutralise H3PO4?

A

It is sparingly soluble so can be filtered off

40
Q

Why would using an excess of NaOH to neutralise phosphoric (V) acid in a lake lead to environmental problems?

A

An excess of NaOH would make the lake alkaline and kill wildlife

41
Q

What’s the electron arrangement of copper (I)?

A

[Ar] 3d10

42
Q

What is observed when aqueous ammonia is added to cobalt (II) chloride until in excess and forms Co(H2O)4(OH)2?

A

Blue/pink ppt forms
Co(H2O)4(OH)2
Precipitate dissolves in XS ammonia

43
Q

What is observed when aqueous ammonia is added to cobalt (II) chloride until in excess and forms [Co(NH3)6]2+?

A

Forms yellow coloured solution

Darkens on standing in air

44
Q

What is observed when aqueous ammonia is added to cobalt (II) chloride until in excess and forms [Co(NH3)6]3+?

A

Due to oxidation by O2 in air

45
Q

What is observed when sodium carbonate reacts with iron (II) sulphate?

A

Green ppt

FeCO3

46
Q

What is observed when sodium carbonate reacts with iron (II) sulphate?

A

Brown/red ppt
[Fe(H20)3(OH)3]
Effervescence as carbon dioxide is evolved

47
Q

Why do separate solutions of iron (II) sulphate and iron (III) sulphate of equal concentrations have different pH values?

A

Fe3+ has a larger charge and smaller size than Fe2+

Fe3+ polarises a Logan water molecules to a greater extent

48
Q

Give two reasons why copper extraction using scrap iron is more environmentally friendly than reduction by carbon.

A

Lower energy consumption
Benefits of less copper ore mining
Less CO2 released

A2 Chemistry (14 decks)

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