Name ……………………………………………………………………………………

1.	Liquid ammonia, NH3, and water, H2O, both show hydrogen bonding.
(i)	Draw a labelled diagram to show hydrogen bonding between two molecules of liquid ammonia.

[3]
 
(ii)	Water has several anomalous properties as a result of its hydrogen bonding.
	Describe and explain one anomalous property of water which results from hydrogen bonding.
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[2]
[Total 5 marks]

2.	The figure below shows the boiling points of four hydrides of Group 6 elements.

(i)	Explain, with the aid of a diagram, the intermolecular forces in H2O that lead to the relatively high boiling point of H2O.

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[3]
 
(ii)	Suggest why H2S has a much lower boiling point than H2O.
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[1]
[Total 4 marks]
3.	Describe and explain the density of ice compared with water.
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[Total 2 marks]

4.	Water forms hydrogen bonds which influences its properties.
	Explain, with a diagram, what is meant by hydrogen bonding and explain two anomalous properties of water resulting from hydrogen bonding.
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[Total 6 marks]
 
5.	The O–H bonds in water and the N–H bonds in ammonia have dipoles.
(i)	Why do these bonds have dipoles?
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[1]
(ii)	Molecules of NH3 are able to form hydrogen bonds. Draw a diagram to show the hydrogen bonding in ammonia. Include any relevant lone pairs and dipoles.

[2]
[Total 3 marks]

ON FILE PAPER (estimate no more than ½ A4) complete the following:

6.	In this question, one mark is available for the quality of spelling, punctuation and grammar.
The halogens chlorine, bromine and iodine each exist as diatomic molecules at room temperature and pressure.
The halogens all have van der Waals’ forces.
·	Explain how van der Waals’ forces are formed.
·	Explain the trend in volatilities of the halogens chlorine, bromine and iodine.
[Total 6 marks]

7.	In this question, one mark is available for the quality of written communication.
	Describe the intermolecular bonding in CH4 and in H2O.
Use clear diagrams in your answer.
[Total 6 marks]

Total: 32 marks