Which of the following pairs of elements would have more negative electron gain enthalpy.

Answer the following question (Based on EA, Delta_(eg)H^(ɵ) and IE ). (a) IE_(1) of Li is 5.4 eV "atom"^(-1) and the EA of Cl is 3.6 eV "atom"^(-1) . Calculate Delta_( r)H^(ɵ) in "kcal mol"^(-1) and kJ mol^(-1) for the reaction Li_((g))+Cl_((g)) rarr Li_((g))^(o+)+Cl_((g))^(ɵ) formed at such a low pressure that resulting ions do not combine with each other. (b) The IE of atoms X and Y are 400 and 300 kcal mol^(-1) respectively. EA's of these atoms are 80.0 and 85.0 K cal mol^(-1) . Explain as which of the atoms has higher EN . ( c) Explain why EA of S is -200 kJ mol^(-1) but the second EA is +649 kJ mol^(-1) ? (d) Which of the following pairs of elements would have more negative electron gain enthalpy (Delta_("eg")H^(ɵ)) ? (i) F or Cl , (ii) O or F (e) What would be the second electron gain enthalpy (Delta_(eg)H_(2)^(ɵ)) of oxygen as positive, more negative or less negative than first (Delta_(eg)H_(1)^(ɵ)) ? Explain. (f) Which has less negative Delta_(eg)H^(ɵ) oxygen or sulphur?

Which of the following pairs of elements would have a more negative electron gain enthalpy? a. O or F , b. F or Cl

S has more negative electron gain enthalpy than O why ?

Which of the following pairs would have a higher negative electron gain enthalpy ? {:((i)N or O, (ii) For Cl),((iii)Br or I, (iv) B or Al):}

Of the two elements given in each of the following cases, choose the element having a more negative electron gain enthalpy. Explain. F and Cl

Of the two elements given in each of the following cases, choose the element having a more negative electron gain enthalpy. Explain. N and O

Which of the following elements have the most negative electron gain enthalpies corresponding to the largest release of enegry?