(C) Step $1$: The ionization potential $(IP)$ decreases as we move down a group in the periodic table due to an increase in atomic size and the shield

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(C) Step $1$: The ionization potential $(IP)$ decreases as we move down a group in the periodic table due to an increase in atomic size and the shielding effect.Step $2$: Since $K$ is located below $Na$ in Group $1$, its $IP$ must be lower than that of $Na$ $(5.48 \, eV)$.Step $3$: Among the given options, $4.34 \, eV$ is the only value less than $5.48 \, eV$.

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

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If the $IP$ of $Na$ is $5.48 \, eV$, the ionisation potential of $K$ will be ............ $eV$.

A
Same as that of $Na$
B
$5.68$
C
$4.34$
D
$10.88$

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Class 11

Chemistry Questions

Chapter

Classification of Elements and Periodicity in Properties

Subtopic

Ionisation energy

Amongst the elements with the following electronic configurations,which one of them may have the highest ionisation energy?

DifficultAIPMT 2009

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For the second period elements,the correct increasing order of first ionisation enthalpy is:

MediumNEET 2019

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Which of the following electronic configurations represents the element with the lowest ionization energy?

Easy

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Which diagram of ionization energy is correct for the elements $Cu$,$Ag$,and $Au$?

Easy

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Define ionisation enthalpy. Discuss the factors affecting ionisation enthalpy of the elements and its trends in the periodic table.

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If the $IP$ of $Na$ is $5.48 \, eV$, the ionisation potential of $K$ will be ............ $eV$.

Similar Questions

Amongst the elements with the following electronic configurations,which one of them may have the highest ionisation energy?

For the second period elements,the correct increasing order of first ionisation enthalpy is:

Which of the following electronic configurations represents the element with the lowest ionization energy?

Which diagram of ionization energy is correct for the elements $Cu$,$Ag$,and $Au$?

Define ionisation enthalpy. Discuss the factors affecting ionisation enthalpy of the elements and its trends in the periodic table.

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