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A2 Chemistry > Inorganic > Flashcards

Inorganic Flashcards

(48 cards)

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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

21
Q

Silicon oxide

22
Q

Phosphorus oxide

23
Q

Sulphur oxides

24
Q

Chlorine oxides

25
Fluoride and chloride ions reducing ability
Won't reduce concentrated sulphuric acid
26
Bromide ions reduction on concentrated sulphuric acid
Reduces sulphuric acid to sulphur dioxide. | Bromide ions are oxidised to bromine
27
Iodide ions reduction of sulphuric acid
Sulphuric acid reduces to hydrogen sulphide. | The iodide ions are oxidised to iodine
28
Trend in reducing ability of halide ions
Increase going down the group
29
Suggest why the melting point of magnesium oxide is much higher than the melting point of magnesium chloride.
Charge on ion bigger than on chloride Oxide ion is smaller than chloride These cause stronger electrostatic attraction
30
Why is Al(OH)3 insoluble in water ?
Large lattice energy Strong covalent bonds Positive enthalpy of solution Positive Gibbs free energy change
31
What would you observe when magnesium reacts with water at high temperatures?
White powder | Bright white flame
32
Equation with magnesium reacts with water
Mg + H2O --> MgO + H2
33
Why does magnesium have a higher melting point than sodium?
Mg2+ has higher charge than Na+ | It attracts delocalised electrons more strongly
34
What properties of silicon dioxide are as a result of its structure and bonding?
``` High melting and boiling point Hard Brittle Not malleable Insoluble Non conductor ```
35
What are 2 properties of MgO caused by their structure and bonding which can be tested?
High melting point | Molten oxide conducts electricity
36
Explain the structure and bonding in phosphorus (V) oxide which causes its melting point to be lower than silicon dioxide.
Molecular with covalent bonding | Intermolecular forces are easy to overcome
37
Why is phosphor (V) oxide represented as P4O10 rather than P2O5?
Exists as P4O10 | Molecular formula
38
Why does phosphorus (V) oxide have a higher melting point hat sulphur (IV) oxide?
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
Why can an excess of MgO be used to neutralise H3PO4?
It is sparingly soluble so can be filtered off
40
Why would using an excess of NaOH to neutralise phosphoric (V) acid in a lake lead to environmental problems?
An excess of NaOH would make the lake alkaline and kill wildlife
41
What's the electron arrangement of copper (I)?
[Ar] 3d10
42
What is observed when aqueous ammonia is added to cobalt (II) chloride until in excess and forms Co(H2O)4(OH)2?
Blue/pink ppt forms Co(H2O)4(OH)2 Precipitate dissolves in XS ammonia
43
What is observed when aqueous ammonia is added to cobalt (II) chloride until in excess and forms [Co(NH3)6]2+?
Forms yellow coloured solution | Darkens on standing in air
44
What is observed when aqueous ammonia is added to cobalt (II) chloride until in excess and forms [Co(NH3)6]3+?
Due to oxidation by O2 in air
45
What is observed when sodium carbonate reacts with iron (II) sulphate?
Green ppt | FeCO3
46
What is observed when sodium carbonate reacts with iron (II) sulphate?
Brown/red ppt [Fe(H20)3(OH)3] Effervescence as carbon dioxide is evolved
47
Why do separate solutions of iron (II) sulphate and iron (III) sulphate of equal concentrations have different pH values?
Fe3+ has a larger charge and smaller size than Fe2+ | Fe3+ polarises a Logan water molecules to a greater extent
48
Give two reasons why copper extraction using scrap iron is more environmentally friendly than reduction by carbon.
Lower energy consumption Benefits of less copper ore mining Less CO2 released

A2 Chemistry (14 decks)

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