(D) Ionization energy is defined as the minimum amount of energy required to remove the most loosely bound electron from an isolated gaseous atom in i

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The energy required to remove the outermost electron of an atom of the element

(D) Ionization energy is defined as the minimum amount of energy required to remove the most loosely bound electron from an isolated gaseous atom in its ground state. The process can be represented as: $M(g) + \text{Energy} \rightarrow M^+(g) + e^-$. Therefore,option $D$ is the correct definition.

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

Easy

The ionization energy of an element is defined as:

A
The same as the electron affinity of the element
B
Equal in magnitude but of opposite sign to the electron affinity of the element
C
The energy released when an electron is added to an atom of the element
D
The energy required to remove the outermost electron of an atom of the element

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Class 11

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Classification of Elements and Periodicity in Properties

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Ionisation energy

When first ionisation energy is plotted against the atomic number,the peaks in the curve are occupied by

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The second ionisation potential of an element $M$ is the energy required to

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Correct increasing order of first ionisation potential is

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If first ionization enthalpies of element $X$ and $Y$ are $419 \ kJ \ mol^{-1}$ and $590 \ kJ \ mol^{-1}$,respectively and second ionization enthalpies of $X$ and $Y$ are $3069 \ kJ \ mol^{-1}$ and $1145 \ kJ \ mol^{-1}$,respectively. Then the correct statement is :-

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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:

MediumKCET 2015

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

The ionization energy of an element is defined as:

Similar Questions

When first ionisation energy is plotted against the atomic number,the peaks in the curve are occupied by

The second ionisation potential of an element $M$ is the energy required to

Correct increasing order of first ionisation potential is

If first ionization enthalpies of element $X$ and $Y$ are $419 \ kJ \ mol^{-1}$ and $590 \ kJ \ mol^{-1}$,respectively and second ionization enthalpies of $X$ and $Y$ are $3069 \ kJ \ mol^{-1}$ and $1145 \ kJ \ mol^{-1}$,respectively. Then the correct statement is :-

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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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: