If first ionization enthalpies of element X a | vedclass

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Question

(A) For element $X$: The difference between the $2^{nd}$ and $1^{st}$ ionization enthalpy is $3069 - 419 = 2650 \ kJ \ mol^{-1}$,which is very large.

Vedclass · Accepted Answer

$X$ is an alkali metal and $Y$ is an alkaline earth metal.

Vedclass · Answer

(A) For element $X$: The difference between the $2^{nd}$ and $1^{st}$ ionization enthalpy is $3069 - 419 = 2650 \ kJ \ mol^{-1}$,which is very large. This indicates that the removal of the second electron requires breaking a stable noble gas configuration,characteristic of an alkali metal.For element $Y$: The difference between the $2^{nd}$ and $1^{st}$ ionization enthalpy is $1145 - 590 = 555 \ kJ \ mol^{-1}$,which is relatively small. This indicates that the second electron is removed from the same valence shell,characteristic of an alkaline earth metal.Therefore,$X$ is an alkali metal and $Y$ is an alkaline earth metal.

If first ionization enthalpies of element $X$ and $Y$ are $419 \ kJ \ mol^{-1}$ and $590 \ kJ \ mol^{-1}$,respectively and second ionization enthalpies of $X$ and $Y$ are $3069 \ kJ \ mol^{-1}$ and $1145 \ kJ \ mol^{-1}$,respectively. Then the correct statement is :-

Similar Questions

The first ionization enthalpy $(\Delta_{i} H)$ values of the third period elements,$Na, Mg$ and $Si$ are respectively $496, 737$ and $786 \, kJ \, mol^{-1}$. Predict whether the first $\Delta_{i} H$ value for $Al$ will be more close to $575$ or $760 \, kJ \, mol^{-1}$? Justify your answer.

Assertion $(A)$: First ionisation enthalpy of oxygen is less than that of nitrogen.
Reason $(R)$: Atoms with half-filled or completely filled orbitals are less stable.
The correct option among the following is:

Which elements in a period have the maximum and minimum ionization enthalpy?

Which of the following statements is incorrect?

The first ionisation potential is maximum for

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