Consider the following conversions:
(i) O_{ | vedclass

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Question

(C) The electron gain enthalpy $(\Delta H_{eg})$ for $O$ is $-141 \ kJ/mol$ $(\Delta H_1)$.
The electron gain enthalpy for $F$ is $-328 \ kJ/mol$ $(\

Vedclass · Accepted Answer

$\Delta H_2$ and $\Delta H_3$ are negative while $\Delta H_1$ is positive

Vedclass · Answer

(C) The electron gain enthalpy $(\Delta H_{eg})$ for $O$ is $-141 \ kJ/mol$ $(\Delta H_1)$.
The electron gain enthalpy for $F$ is $-328 \ kJ/mol$ $(\Delta H_2)$.
The electron gain enthalpy for $Cl$ is $-349 \ kJ/mol$ $(\Delta H_3)$.
Since $\Delta H_3 < \Delta H_2 < \Delta H_1 < 0$,all three values are negative.
$Na_{(g)} 	o Na^{+}_{(g)} + e^-$ represents ionization energy,which is always positive $(\Delta H_4 > 0)$.
Option $C$ is incorrect because $\Delta H_1$ is also negative,not positive.

Consider the following conversions:
$(i) \ O_{(g)} + e^- \to O^{-}_{(g)} ; \Delta H_1$
$(ii) \ F_{(g)} + e^- \to F^{-}_{(g)} ; \Delta H_2$
$(iii) \ Cl_{(g)} + e^- \to Cl^{-}_{(g)} ; \Delta H_3$
$(iv) \ Na_{(g)} \to Na^{+}_{(g)} + e^- ; \Delta H_4$
Which of the following statements is incorrect?

Similar Questions

In which of the following processes is energy liberated?

Which halogen has the highest value of negative electron gain enthalpy?

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Electron affinity is the lowest for

Which element in each of the following pairs has a more negative electron gain enthalpy?
$(i)$ $O$ or $F$ $(ii)$ $F$ or $Cl$

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Consider the following conversions: $(i) \ O_{(g)} + e^- \to O^{-}_{(g)} ; \Delta H_1$ $(ii) \ F_{(g)} + e^- \to F^{-}_{(g)} ; \Delta H_2$ $(iii) \ Cl_{(g)} + e^- \to Cl^{-}_{(g)} ; \Delta H_3$ $(iv) \ Na_{(g)} \to Na^{+}_{(g)} + e^- ; \Delta H_4$ Which of the following statements is incorrect?