Would you expect the first ionization enthalpies for two isotopes of the same element to be the same or different? Justify your answer.
(N/A) The ionization enthalpy of an atom depends on the number of electrons and the nuclear charge (number of protons).
Since isotopes of the same element have the same atomic number,they possess the same number of protons and electrons.
Therefore,the electronic configuration and the effective nuclear charge experienced by the valence electrons remain identical for both isotopes.
Consequently,the first ionization enthalpy for two isotopes of the same element is the same.
Since isotopes of the same element have the same atomic number,they possess the same number of protons and electrons.
Therefore,the electronic configuration and the effective nuclear charge experienced by the valence electrons remain identical for both isotopes.
Consequently,the first ionization enthalpy for two isotopes of the same element is the same.
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Which of the following is not the correct increasing order of ionisation energy?
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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 ............. $kcal \, mol^{-1}$.
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View SolutionBased on the values of $IE_1$ and $IE_2$,which of the following represents an alkali metal?
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View SolutionElectronic configurations of four elements $A$,$B$,$C$,$D$ are given below:
$A$) $1s^2 2s^2 2p^6 3s^1$
$B$) $1s^2 2s^2 2p^6 3s^2 3p^1$
$C$) $1s^2 2s^2 2p^6 3s^2$
$D$) $1s^2 2s^2 2p^6 3s^2 3p^2$
The correct order of first ionization enthalpy of these elements is:
$A$) $1s^2 2s^2 2p^6 3s^1$
$B$) $1s^2 2s^2 2p^6 3s^2 3p^1$
$C$) $1s^2 2s^2 2p^6 3s^2$
$D$) $1s^2 2s^2 2p^6 3s^2 3p^2$
The correct order of first ionization enthalpy of these elements is:
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