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A-Level Chemistry > 3.3 Chemistry of the p-block > Flashcards

3.3 Chemistry of the p-block Flashcards

1
Q

Why are they called the p-block elements?

A

Each of the p-block elements have their outer electron in the p orbital.

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2
Q

Which two p-block elements have amphoteric behaviour?

A

Al/ Al3+
Pb/ Pb2+

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3
Q

What is the chemical equation for the reaction between aluminium oxide and sulfuric acid?

A

Al2O3 + 3H2SO4 —> Al2(SO4)3 + 3H2O

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4
Q

What is the chemical equation for the reaction between aluminium oxide and sodium hydroxide?

A

Al2O3 + 2NaOH + 3H2O —> 2NaAl(OH)4

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5
Q

What is the chemical equation for the reaction between lead oxide and hydrochloric acid?

A

PbO + 2HCl —> PbCl2 + H2O

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6
Q

What is the chemical equation for the reaction between lead oxide and sodium hydroxide?

A

PbO + NaOH + H2O —> NaPb(OH)3

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7
Q

What is the inert pair effect?

A

The tendency of electrons in the outer s orbital to remain unionised and unshared. It is used to explain the increasing stability of the oxidation states that are two less that the group valency for Groups 3, 4 and 5 (also known as groups 13, 14 and 15).

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8
Q

Describe how the stability of oxidation states changes down Group 3

A

In Group 3 the stability of the +1 oxidation state increases down the group.
The Tl+ ion is much more common than the Tl3+ ion, whereas at the top of the group the Al+ ion is very rare due to its instability and hence the Al3+ ion is more common.

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9
Q

Describe how the stability of oxidation states changes down Group 4

A

In Group 4, stability of the +4 oxidation state reduces down the group, whilst stability of the +2 oxidation state increases down the group.

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10
Q

Describe how the stability of the oxidation states changes down Group 5

A

In Group 5, stability of the +5 oxidation state reduces down the group, whilst stability of the +3 oxidation state increases down the group.

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11
Q

Describe the structure and bonding in Al2Cl6

A

Aluminium Hexafluoride (Al2Cl6) is a donor-acceptor dimer. It is made up of two separate, identical molecules which are linked together by two dative bonds. Two atoms of chlorine share their lone pair of electrons with two atoms of aluminium to form the dative bonds.

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12
Q

Describe the structure and bonding in NH3BF3

A

NH3BF3 is a donor-acceptor compound.
There is a dative coordinate bond formed between the nitrogen and boron atoms, where nitrogen supplies both the electrons for the covalent bond.

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13
Q

Describe the structure of cubic boron nitride

A

The cubic form of boron nitride consists of alternately linked boron and nitrogen atoms. The structure is a tetrahedral bond network which is similar to that of the carbon atoms in a diamond. The lone pair of electrons on a nitrogen are accepted by boron to give this giant 3D covalent lattice.

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14
Q

Describe the structure of hexagonal boron nitride

A

Hexagonal boron nitride has a layered structure which is similar to graphite. The layers form a 2D giant covalent network. The alternate boron and nitrogen atoms link together and form hexagonal rings in thin layers which are held together by weak intermolecular forces.

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15
Q

Explain which boron nitride structure is suitable to be used as a lubricant

A

The hexagonal boron nitride structure has weak intermolecular forces between the layers and so these layers can slide, making it suitable to be used as a lubricant.

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16
Q

Identify the reducing agent in the following reaction
CuO + CO —> Cu + CO2

A

Cu: 2+ —> 0 (reduced)
C: 2+ —> 4+ (oxidised)
The reducing agent is carbon monoxide.

17
Q

What is the chemical equation for the reaction between PbO2 and hydrochloric acid?
Identify the oxidising agent

A

PbO2 + 4HCl —> PbCl2 + 2H2O + Cl2
The oxidising agent is Pb(IV) / Pb4+

18
Q

Describe the general acid-base behaviour trend of Group 4 oxides

A

Acidity of the Group 4 oxides decreases as you go down the group. The oxides towards the bottom are more basic, however they don’t completely lose their acidic character so they are described as amphoteric.

19
Q

Explain the acid-base properties of carbon dioxide and lead oxide in relation to their position in Group 4

A

Carbon is at the top of Group 4 so carbon dioxide is acidic in nature and can react with bases.
Lead is towards the bottom of Group 4 so lead oxide is amphoteric in nature, meaning it can react with acids and bases.

20
Q

Compare the reactions of CCl4, SiCl4 and PbCl2 with water

A

CCl4 does not react with water
SiCl4 reacts violently with water
PbCl2 is partially soluble in cold water but more soluble in hot water.

21
Q

Why does CCl4 tend not to react with water

A

For the reaction to take place, the oxygen’s lone pair from water needs to bond to the carbon atom in CCl4. The reaction doesn’t occur for various reasons:
The chlorine atoms are very bulky and the carbon atom is very small so it is hard for the oxygen to get near the carbon atom. There is also a lot of repulsion between the various lone pairs as the oxygen atom gets close to the chlorine atoms, which makes the transition state very unstable. Also, there is not a convenient empty orbital for the oxygen to bond to on the carbon atom.

22
Q

How is SiCl4 able to react with water?

A

The silicon atom is relatively big so there is space for the oxygen atom on water to attack the silicon atom. Silicon also has empty 3d orbitals which can accept a lone pair of electrons from the oxygen atom.

23
Q

Explain how PbCl2 reacts with water

A

PbCl2 has a lot of ionic character and therefore can be thought of as being ionic in its reaction with water. PbCl2 is slightly soluble in cold water but much more soluble in hot water.

24
Q

What is the chemical equation for the reaction of SiCl4 with water?

A

SiCl4 + 2H2O —> SiO2 + 4HCl

25
Q

What is the chemical equation for the reaction of Pb2+ ions with OH- ions?

A

Pb2+ + 2OH- —> Pb(OH)2
Pb(OH)2 dissolves in excess OH- :
Pb(OH)2 + 2OH —> [Pb(OH)4]2-

26
Q

What is the chemical equation for the reaction of Pb2+(aq) with Cl- ions?

A

Pb2+ + 2Cl- —> PbCl2
With excess Cl-:
PbCl2 + 2Cl- —> [PbCl4]2-

27
Q

What is the chemical equation for the reaction of Pb2+(aq) ions with I- ions?

A

Pb2+ + 2I- —> PbI2

28
Q

What is a disproportionate reaction?

A

A reaction in which a species simultaneously undergoes oxidation and reduction to form two different products.

29
Q

What chemical equation for the disproportionation reaction that chlorine undergoes with cold sodium hydroxide?

A

2NaOH + Cl2 —> NaClO + NaCl + H2O

30
Q

What is the chemical equation for the disproportionation reaction that chlorine undergoes with warm sodium hydroxide?

A

6NaOH + 3Cl2 —> NaClO3 + 5NaCl + 3H2O

31
Q

What is the chemical equation for the disproportionation reaction that chlorine undergoes with water?

A

Cl2 + H2O <—> 2H+ + Cl- + ClO-

32
Q

Why are chlorine and chlorate ions used in water treatment?

A

They kill bacteria which makes the water safe. This is a result of their oxidising power.

33
Q

How do sodium chloride and sodium fluoride react with concentrated sulfuric acid?

A

Chlorides and fluorides are not oxidised by sulfuric acid:
NaCl + H2SO4 —> NaHSO4 + HCl
NaF + H2SO4 —> NaHSO4 + HF

34
Q

How do bromide ions react with concentrated sulfuric acid?

A

Bromide ions can reduce concentrated sulfuric acid:
2Br- + H2SO4 + 2H+ —> Br2 + SO2 + 2H2O

35
Q

How do iodide ions react with concentrated sulfuric acid?

A

Iodide ions are stronger reducing agents than bromide ions:
8I- + H2SO4 + 8H+ —> 4I2 + H2S + 4H2O

A-Level Chemistry (9 decks)

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