M5S9 – Born Haber Cycles

For which of these changes is the enthalpy change the standard enthalpy of atomisation of bromine?

The energy change for this process:

Br_(g) + e^- -> Br^-_(g)is called the:

The standard enthalpy change when one mole of an ionic compound forms from free gaseous ions is called the:

These are four values for the hydration enthalpies of ions:

-361 kJ mol^-1, -559 kJ mol^-1, -2003 kJ mol^-1, -2537 kJ mol^-1.

These ions from left to right are:

What is the enthalpy of solution of lithium bromide given that:

the lattice enthalpy for LiBr = -818 kJ mol^-1

enthalpy of hydration of Li⁺ ions = -559 kJ mol^-1

enthalpy of hydration of Br^- ions = -309 kJ mol^-1

The lattice enthalpy for magnesium oxide is -3850 kJ mol^-1.

The energy needed to break up 0.1 mol MgO into gaseous ions at 298K is:

[1] -38.5 kJ mol-1

[2] -385 kJ mol^-1

[3] +385 kJ mol^-1

[4] +3850 kJ mol^-1

For which of these compounds would expect the best agreement between the values of the lattice energy derived from experimental data (with the help of the Born-Haber cycle) and the values calculated from theory on the assumption that the bonding in the crystals is purely ionic?

The extent to which the negative ions are polarised by neighbouring positive ions in these crystals increase from left to right in which of these series?

(i) KF - KCl - KBr

(ii) LiI - NaI - KI

(iii) NaBr - MgBr₂ - AlBr₃

(iv) MgF₂ - CaF₂ - SrF₂

The magnitude (numerical value) of the lattice enthalpy for these compounds increase from left to right putting first the compound with the least negative value?

(i) LiCl - LiBr - LiI

(ii) MgO - BaO - BaS

(iii) NaCl - KCl - RbCl

(iv) NaF - MgF₂ - AlF₃

For which of these species is the value of the electron affinity positive?

(i) F

(ii) Cl

(iii) O

(iv) O^-