(C) The first ionization energy $(IE_1)$ of $3^{rd}$ period elements follows the order: $Na < Al < Mg < Si < S < P < Cl < Ar$. Magnesium $(Mg)$ has a

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(C) The first ionization energy $(IE_1)$ of $3^{rd}$ period elements follows the order: $Na Magnesium $(Mg)$ has a higher $IE_1$ than $Na$ $(Z)$ but lower than $Cl$ and $Ar$ ($X$ and $Y$). Therefore,$X$ and $Y$ are $Ar$ and $Cl$,and $Z$ is $Na$.

Class 11 Chemistry Classification of Elements and Periodicity in Properties Ionisation energy

Medium

The first ionization energy of magnesium is smaller as compared to that of elements $X$ and $Y$,but higher than that of $Z$. The elements $X$,$Y$ and $Z$,respectively,are :

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A
chlorine,lithium and sodium
B
argon,lithium and sodium
C
argon,chlorine and sodium
D
neon,sodium and chlorine

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Class 11 Questions

Class 11

Chemistry Questions

Chapter

Classification of Elements and Periodicity in Properties

Subtopic

Ionisation energy

Previous Year

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Which of the following electronic configurations represents the highest second ionization energy for an element?

Easy

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Match the following List-$I$ and List-$II$ and select the correct answer using the codes given below.
List-$I$ (Successive Ionization Enthalpy) $\left( kJ \, mol^{-1} \right)$ List-$II$
Element $IE_1$ $IE_2$ $IE_3$ Code Element
$1$ $2080$ $3963$ $6130$ $(a)$ $H$
$2$ $520$ $7297$ $11810$ $(b)$ $Li$
$3$ $900$ $1758$ $14810$ $(c)$ $Be$
$4$ $800$ $2428$ $3660$ $(d)$ $B$
- - - - $(e)$ $Ne$

Medium

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Assertion $(A)$: Boron has a smaller first ionisation enthalpy than beryllium.
Reason $(R)$: The penetration of a $2s$-electron to the nucleus is more than the $2p$-electron; hence,the $2p$-electron is more shielded by the inner core of electrons than $2s$-electrons.

EasyAP EAMCET 2020

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Discuss and compare the trend in ionisation enthalpy of the elements of group-$1$ with those of group-$17$ elements.

Difficult

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The correct order of first ionization potential $(IP)$ is:

Medium

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Element	$IE_1$	$IE_2$	$IE_3$	Code	Element
$1$	$2080$	$3963$	$6130$	$(a)$	$H$
$2$	$520$	$7297$	$11810$	$(b)$	$Li$
$3$	$900$	$1758$	$14810$	$(c)$	$Be$
$4$	$800$	$2428$	$3660$	$(d)$	$B$
-	-	-	-	$(e)$	$Ne$

The first ionization energy of magnesium is smaller as compared to that of elements $X$ and $Y$,but higher than that of $Z$. The elements $X$,$Y$ and $Z$,respectively,are :

Similar Questions

Which of the following electronic configurations represents the highest second ionization energy for an element?

Assertion $(A)$: Boron has a smaller first ionisation enthalpy than beryllium.Reason $(R)$: The penetration of a $2s$-electron to the nucleus is more than the $2p$-electron; hence,the $2p$-electron is more shielded by the inner core of electrons than $2s$-electrons.

Discuss and compare the trend in ionisation enthalpy of the elements of group-$1$ with those of group-$17$ elements.

The correct order of first ionization potential $(IP)$ is:

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Assertion $(A)$: Boron has a smaller first ionisation enthalpy than beryllium.
Reason $(R)$: The penetration of a $2s$-electron to the nucleus is more than the $2p$-electron; hence,the $2p$-electron is more shielded by the inner core of electrons than $2s$-electrons.