Given below are two statements:Statement (I): | vedclass

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(D) Statement $(I)$: The first ionisation enthalpy generally increases across a period from left to right. The correct order for these elements is $Ar

Vedclass · Accepted Answer

Statement $I$ is false but Statement $II$ is true

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(D) Statement $(I)$: The first ionisation enthalpy generally increases across a period from left to right. The correct order for these elements is $Ar > Cl > Mg > Na$. Therefore, the given order $Na > Mg > Cl > Ar$ is incorrect. Thus, Statement $(I)$ is false.Statement $(II)$: The electronic configuration of $Ca$ $(Z=20)$ is $[Ar] 4s^2$. The first two electrons are removed from the $4s$ orbital. The third electron must be removed from the $3p^6$ orbital, which is a stable noble gas configuration (Argon core). Removing an electron from a stable, fully-filled shell requires a very high amount of energy. Thus, Statement $(II)$ is true.

Given below are two statements:
Statement $(I)$: The first ionisation enthalpy of the elements $Na$, $Mg$, $Cl$ and $Ar$ follows the order $Na > Mg > Cl > Ar$.
Statement $(II)$: Among $Ca$, $Al$, $Fe$ and $B$, the third ionisation enthalpy is very high for $Ca$.

Similar Questions

Assertion $(A)$: The first ionisation energy of $Be$ is greater than that of $B$.
Reason $(R)$: $2p$ orbital has lower energy than $2s$ orbital.

Outermost electronic configurations of four elements $A, B, C, D$ are given below:
$A: 3s^{2}$
$B: 3s^{2} 3p^{1}$
$C: 3s^{2} 3p^{3}$
$D: 3s^{2} 3p^{4}$
The correct order of first ionization enthalpy for them is:

The incorrect relation among the following is

Which of the following sets is correct regarding the ionization potential?

The correct sequence of elements in decreasing order of first ionisation energy is

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Given below are two statements:Statement $(I)$: The first ionisation enthalpy of the elements $Na$, $Mg$, $Cl$ and $Ar$ follows the order $Na > Mg > Cl > Ar$.Statement $(II)$: Among $Ca$, $Al$, $Fe$ and $B$, the third ionisation enthalpy is very high for $Ca$.