The first ionization potential of Na, Mg, Al | vedclass

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Question

(A) The first ionization potential $(IE_1)$ generally increases across a period from left to right due to an increase in effective nuclear charge.Howe

Vedclass · Accepted Answer

$Na  Al < Si$

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(A) The first ionization potential $(IE_1)$ generally increases across a period from left to right due to an increase in effective nuclear charge.However,there are exceptions due to stable electronic configurations.For $Na$ $([Ne] 3s^1)$,$Mg$ $([Ne] 3s^2)$,$Al$ $([Ne] 3s^2 3p^1)$,and $Si$ $([Ne] 3s^2 3p^2)$:$1$. $Mg$ has a fully filled $3s$ orbital,which is more stable than the $3p^1$ configuration of $Al$,making $IE_1$ of $Mg > Al$.$2$. The general trend is $Na  Al Thus,the correct order is $Na  Al < Si$.

The first ionization potential of $Na, Mg, Al$ and $Si$ are in the order:

Similar Questions

Generally,the first ionization energy increases along a period. But there are some exceptions. One which is not an exception is

Assertion : First ionization energy for nitrogen is lower than oxygen.
Reason : Across a period effective nuclear charge decreases.

Explain why there is a phenomenal decrease in ionisation enthalpy from carbon to silicon?

Ionization energy of gaseous $Na$ atoms is $495.5 \ kJ \ mol^{-1}$. The lowest possible frequency of light that ionizes a sodium atom is $(h = 6.626 \times 10^{-34} \ J \ s, N_A = 6.022 \times 10^{23} \ mol^{-1})$.

The correct order of ionisation energy of $C$,$N$,$O$,and $F$ is

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