(A) The first ionisation potential $(I.P.)$ generally increases from left to right across a period due to an increase in effective nuclear charge.For

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(A) The first ionisation potential $(I.P.)$ generally increases from left to right across a period due to an increase in effective nuclear charge.For the elements $B$ (Boron),$C$ (Carbon),and $N$ (Nitrogen),which belong to the $2^{nd}$ period,the order of increasing first $I.P.$ is $B Therefore,the correct sequence is $B < C < N$.

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

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Among the following options,the sequence of increasing first ionisation potential will be

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A
$B < C < N$
B
$B > C > N$
C
$C < B < N$
D
$N > C > B$

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Class 11

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Classification of Elements and Periodicity in Properties

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Ionisation energy

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With reference to the concept of ionisation potential,which one of the following sets is correct?

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The increasing order of the first ionization enthalpies of the elements $B$,$P$,$S$ and $F$ (lowest first) is:

MediumAIEEE 2006

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Which of the following electronic configurations has the highest ionization enthalpy?

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Mercury is the only metal which is liquid at $0 \, ^oC$. This is due to its:

MediumAIPMT 1995

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The second ionization potential is

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Among the following options,the sequence of increasing first ionisation potential will be

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With reference to the concept of ionisation potential,which one of the following sets is correct?

The increasing order of the first ionization enthalpies of the elements $B$,$P$,$S$ and $F$ (lowest first) is:

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