Complete the table by placing one tick (✔) in each row to indicate the sign of each type of energy change under standard conditions. [Table 6.a: energy change | always positive | always negative | either negative or positive bond energy | enthalpy change of formation |]

1. (a)Complete the table by placing one tick (✔) in each row to indicate the sign of each type of energy change under standard conditions. [Table 6.a: energy change | always positive | always negative | either negative or positive bond energy | enthalpy change of formation |][1]
2. (b)Explain what is meant by the term enthalpy change of atomisation.[1]
3. (c)The overall reaction for the atomisation of liquid bromine molecules, Br₂(l), is shown. Br₂(l) → 2Br(g) This happens via a two-step process. • Construct a labelled energy cycle to represent this atomisation process, including state symbols. • Use your cycle and relevant data from the Data Booklet to calculate the enthalpy change of vaporisation of Br2(l), ∆H°vap. The enthalpy change of atomisation of bromine, ∆Hat, = +112kJmol⁻¹. ∆H°vap[3]
4. (d)Suggest how the ∆H°vap of iodine, I2(l), would compare to that of bromine, Br₂(l). Explain your answer.[1]
5. (e)(i)Explain what is meant by the term enthalpy change of hydration.[1]
6. (e)(ii)Suggest why the enthalpy change of hydration of Br⁻(g) is more exothermic than that of I⁻(g).[2]