How does the ionization energy of the element | vedclass

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(B) As we move down Group $1$ (alkali metals),the atomic size increases due to the addition of new shells. Due to the increase in atomic size,the vale

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Decreases down the group

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(B) As we move down Group $1$ (alkali metals),the atomic size increases due to the addition of new shells. Due to the increase in atomic size,the valence electron becomes farther from the nucleus,and the effective nuclear charge experienced by the valence electron decreases. Consequently,the force of attraction between the nucleus and the valence electron decreases,making it easier to remove the electron. Therefore,the ionization energy decreases down the group.

List-$I$ (Salt)	List-$II$ (Flame colour wavelength)
$(a)$ $LiCl$	$(i)$ $455.5 \text{ nm}$
$(b)$ $NaCl$	$(ii)$ $670.8 \text{ nm}$
$(c)$ $RbCl$	$(iii)$ $780.0 \text{ nm}$
$(d)$ $CsCl$	$(iv)$ $589.2 \text{ nm}$

How does the ionization energy of the elements of Group $1$ change as we move down the group?

Similar Questions

Match List-$I$ with List-$II$:

List-$I$ (Salt) List-$II$ (Flame colour wavelength)

$(a)$ $LiCl$ $(i)$ $455.5 \text{ nm}$

$(b)$ $NaCl$ $(ii)$ $670.8 \text{ nm}$

$(c)$ $RbCl$ $(iii)$ $780.0 \text{ nm}$

$(d)$ $CsCl$ $(iv)$ $589.2 \text{ nm}$

Choose the correct answer from the options given below:

Give two uses of $KOH$.

Which of the following statements is incorrect?

Which one among the following metals is the weakest reducing agent?

$Na$ and $Li$ are placed in dry air. We get

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