The ionization energy of an element is defined as:
- AThe same as the electron affinity of the element
- BEqual in magnitude but of opposite sign to the electron affinity of the element
- CThe energy released when an electron is added to an atom of the element
- DThe energy required to remove the outermost electron of an atom of the element
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Electronic 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:
Ionization enthalpy of an atom is equal to
Medium
View SolutionWhich of the following electronic configurations represents the element with the lowest ionization energy?
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View SolutionWhich of the following species has the highest ionisation potential?
Medium
View SolutionThe ionization energy of hydrogen is:
Easy
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