The values of Delta _iH_1, Delta _iH_2, Delta | vedclass

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(B) The successive ionization energies are given as: $\Delta _iH_1 = 7.5 \ eV$,$\Delta _iH_2 = 25.6 \ eV$,$\Delta _iH_3 = 48.6 \ eV$,and $\Delta _iH_4

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$1s^2 \ 2s^2 \ 2p^6 \ 3s^2 \ 3p^1$

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(B) The successive ionization energies are given as: $\Delta _iH_1 = 7.5 \ eV$,$\Delta _iH_2 = 25.6 \ eV$,$\Delta _iH_3 = 48.6 \ eV$,and $\Delta _iH_4 = 170.6 \ eV$. $A$ large jump in ionization energy indicates the removal of an electron from a stable,fully-filled or half-filled shell (noble gas configuration). Here,the jump from $\Delta _iH_3$ $(48.6 \ eV)$ to $\Delta _iH_4$ $(170.6 \ eV)$ is very large,which suggests that the atom has $3$ valence electrons. Among the given options,the configuration $1s^2 \ 2s^2 \ 2p^6 \ 3s^2 \ 3p^1$ (Aluminum,$Z=13$) has $3$ valence electrons in the $3s$ and $3p$ orbitals. Therefore,the correct electronic configuration is $1s^2 \ 2s^2 \ 2p^6 \ 3s^2 \ 3p^1$.

Element	Ionization enthalpy $(kJ \ mol^{-1})$ $(1^{st}, 2^{nd}, 3^{rd})$
$A$	$899, 1757, 14847$
$B$	$737, 1450, 7731$

The values of $\Delta _iH_1, \Delta _iH_2, \Delta _iH_3$,and $\Delta _iH_4$ for an atom are $7.5 \ eV, 25.6 \ eV, 48.6 \ eV$,and $170.6 \ eV$ respectively. Determine the electronic configuration of the atom.

Similar Questions

Consider the following ionization enthalpies of two elements $A$ and $B$.

Element Ionization enthalpy $(kJ \ mol^{-1})$ $(1^{st}, 2^{nd}, 3^{rd})$

$A$ $899, 1757, 14847$

$B$ $737, 1450, 7731$

Which of the following statements is correct?

The correct order of first ionisation enthalpy of the given elements is:

The first ionization enthalpies of $Li$,$Be$,and $C$ are $520$,$899$,and $1086 \ kJ \ mol^{-1}$ respectively. Which of the values $800$ or $900 \ kJ \ mol^{-1}$ is more likely for the first ionization enthalpy of $B$? Why?

The first ionisation energies of alkaline earth metals are higher than those of the alkali metals. This is because

The second ionization potential is

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