Assertion $(A)$: The first ionisation energy of $Be$ is greater than that of $B$.
Reason $(R)$: $2p$ orbital has lower energy than $2s$ orbital.
Reason $(R)$: $2p$ orbital has lower energy than $2s$ orbital.
- ABoth $A$ and $R$ are true and $R$ is a correct explanation for $A$.
- BBoth $A$ and $R$ are true but $R$ is not a correct explanation for $A$.
- C$A$ is true but $R$ is false.
- D$A$ is false but $R$ is true.
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Similar Questions
The given electronic configurations are for elements $X$,$Y$,and $Z$. Note that these configurations represent ions of the elements:
$X = [Ne] \, 3s^2 \, 3p^5$
$Y = [Ne] \, 3s^2 \, 3p^6$
$Z = [Ne] \, 3s^2 \, 3p^4$
Determine the correct statement regarding the energy changes associated with these configurations.
$X = [Ne] \, 3s^2 \, 3p^5$
$Y = [Ne] \, 3s^2 \, 3p^6$
$Z = [Ne] \, 3s^2 \, 3p^4$
Determine the correct statement regarding the energy changes associated with these configurations.
Difficult
View SolutionThe successive ionisation enthalpies of an element $X$ in $(kJ \ mol^{-1})$ are $1012$,$1907$,$2955$,$4955$,$6275$ and $21,260$ respectively. The element $X$ is:
Among $Be$, $B$, $Mg$ and $Al$, the second ionisation potential is maximum for
Which of the following elements has the highest metallic character?
Element $-$ $IP$ (Ionization Potential)
Element $-$ $IP$ (Ionization Potential)
Medium
View SolutionFor $Mg$,the values of $\Delta_iH_1$ and $\Delta_iH_2$ are $178 \, kcal \, mol^{-1}$ and $348 \, kcal \, mol^{-1}$ respectively. The enthalpy change for the reaction $Mg \to Mg^{2+} + 2e^-$ is ............. $kcal \, mol^{-1}$.
Medium
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