Carbon monoxide gas, CO(g), and nitrogen gas, N₂(g), are both diatomic molecules. (a) The diagram shows the arrangement of outer electrons in a molecule of CO(g). [Figure X.X]

1. (a)(i)State one similarity and one difference in the way the atoms in a carbon monoxide molecule are bonded together compared to the atoms in a nitrogen molecule.[2]
2. (a)(ii)The table states the electronegativity values of carbon, nitrogen and oxygen atoms. electronegativity C 2.5 N 3.0 O 3.5 Use the electronegativity values and relevant details from the Data Booklet to complete the table below. number of electrons per molecule type(s) of intermolecular (van der Waals') force N₂ CO[2]
3. (b)N₂(g) is less reactive than CO(g) even though N₂(g) has a lower bond energy than CO(g). Suggest why CO(g) is more reactive than N₂(g).[1]
4. (c)(i)Both carbon monoxide and nitrogen are gases at room temperature and pressure. They both behave like ideal gases under certain conditions. State the two conditions necessary for these two gases to approach ideal gas behaviour.[1]
5. (c)(ii)Explain why N₂(g) behaves more like an ideal gas than CO(g) does at 20.0°C and 101kPa.[2]
6. (d)Calculate the amount, in mol, of pure nitrogen gas which occupies 100 cm³ at 101 kPa and 20.0°C. Use relevant information from the Data Booklet. Show your working. Assume nitrogen behaves as an ideal gas. mol[3]

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