(B) The ionization potential (or ionization energy) increases across a period and decreases down a group. Among the given options,$He$ (Helium) is a n

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(B) The ionization potential (or ionization energy) increases across a period and decreases down a group. Among the given options,$He$ (Helium) is a noble gas located at the top of Group $18$. Due to its extremely small atomic size and stable electronic configuration $(1s^2)$,it requires the highest amount of energy to remove an electron compared to the other elements listed. Therefore,$He$ has the highest ionization potential.

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

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The element with the highest value of ionization potential is

A
Potassium
B
Helium
C
Hydrogen
D
Xenon

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Class 11 Questions

Class 11

Chemistry Questions

Chapter

Classification of Elements and Periodicity in Properties

Subtopic

Ionisation energy

For one of the elements,various successive ionization enthalpies (in $kJ \cdot mol^{-1}$) are given below:

$I.E.$ $1^{st}$ $2^{nd}$ $3^{rd}$ $4^{th}$ $5^{th}$

Value $577.5$ $1810$ $2750$ $11580$ $14820$

The element is:

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Which of the following configurations represents atoms of the elements having the highest second ionization energy?

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The correct order of first ionization enthalpy for the given four elements is:

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

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The $1^{st}$ ionization enthalpy for $Mg$ is $+737 \text{ kJ/mol}$. The most probable estimated value of the $2^{nd}$ ionization enthalpy of $Mg$ is . . . . . . .

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$I.E.$	$1^{st}$	$2^{nd}$	$3^{rd}$	$4^{th}$	$5^{th}$
Value	$577.5$	$1810$	$2750$	$11580$	$14820$

The element with the highest value of ionization potential is

Similar Questions

For one of the elements,various successive ionization enthalpies (in $kJ \cdot mol^{-1}$) are given below: $I.E.$ $1^{st}$ $2^{nd}$ $3^{rd}$ $4^{th}$ $5^{th}$ Value $577.5$ $1810$ $2750$ $11580$ $14820$ The element is:

Which of the following configurations represents atoms of the elements having the highest second ionization energy?

The correct order of first ionization enthalpy for the given four elements is:

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

The $1^{st}$ ionization enthalpy for $Mg$ is $+737 \text{ kJ/mol}$. The most probable estimated value of the $2^{nd}$ ionization enthalpy of $Mg$ is . . . . . . .

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Online Exam Module

For one of the elements,various successive ionization enthalpies (in $kJ \cdot mol^{-1}$) are given below:

$I.E.$ $1^{st}$ $2^{nd}$ $3^{rd}$ $4^{th}$ $5^{th}$

Value $577.5$ $1810$ $2750$ $11580$ $14820$

The element is: