Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

a2 chemistry > Inorganic > Flashcards

Inorganic Flashcards

You may prefer our related Brainscape-certified flashcards:
AP® Chemistry flashcards Periodic Table flashcards
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.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

Electronegativity trend for period 3

A

Increases going along,

Nuclear charge increases with power to attract

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

Melting and boiling trends for period 3

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Sodium with water

A

2Na + 2H2O –> 2NaOH + H2

Exothermic reaction
Colourless solution

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Magnesiums reaction with water

A

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

Burns in steam
Mg + H2O –> MgO + H2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Silicons reaction with water

A

Depends on type of silicon used

So + 2H2Oo –> SiO2 + 2H2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Phosphorus reaction with water

A

None

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Sulphur reaction with water

A

None

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

Argon reaction with water

A

None

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Magnesium reaction with oxygen

A

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

2Mg + O2 –> 2MgO

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

Aluminium reaction with oxygen

A

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

4Al + 3O2 –> 2Al2O3

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

Silicons reaction with oxygen

A

Will burn if heated strongly enough

Si + O2 –> SiO2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

Sodium oxide

A

Na2O

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

Magnesium oxide

A

MgO

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions