(A) The ionization enthalpy generally increases across a period from left to right due to an increase in effective nuclear charge. For the elements $L

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(A) The ionization enthalpy generally increases across a period from left to right due to an increase in effective nuclear charge. For the elements $Li$,$Be$,$B$,and $N$ in the second period,the expected order is $Li However,$Be$ $(1s^2 2s^2)$ has a fully filled $2s$ orbital,and $N$ $(1s^2 2s^2 2p^3)$ has a half-filled $2p$ subshell,both of which are exceptionally stable. Due to this,$Be$ has a higher ionization enthalpy than $B$. Therefore,the correct order is $Li < B < Be < N$.

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

Easy

The correct order of the first ionization enthalpies of the following elements is:

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A
$Li < B < Be < N$
B
$Li < Be < B < N$
C
$N < Be < B < Li$
D
$N < B < Be < Li$

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Class 11 Questions

Class 11

Chemistry Questions

Chapter

Classification of Elements and Periodicity in Properties

Subtopic

Ionisation energy

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Which of the following electronic configurations is associated with the biggest jump between the second and third ionization energies?

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The first three ionisation energies (in $kJ/mol$) of three representative elements are given below:

Element $IE_1$ $IE_2$ $IE_3$

$P$ $495.8$ $4562$ $6910$

$Q$ $737.7$ $1451$ $7733$

$R$ $577.5$ $1817$ $2745$

Which of the following options is incorrect?

Difficult

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The sum of $IE_1 + IE_2$ and $IE_3 + IE_4$ for elements $P$ and $Q$ are given below:

Element $IE_1 + IE_2$ $(kJ/mol)$ $IE_3 + IE_4$ $(kJ/mol)$

$P$ $2.45$ $8.82$

$Q$ $2.85$ $6.11$

Then,according to the given information,the incorrect statement$(s)$ is/are:

Element	$IE_1 + IE_2$ $(kJ/mol)$	$IE_3 + IE_4$ $(kJ/mol)$
$P$	$2.45$	$8.82$
$Q$	$2.85$	$6.11$

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What is the significance of the terms 'isolated gaseous atom' and 'ground state' while defining the ionization enthalpy and electron gain enthalpy?

Medium

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Which of the following electrons should have the highest value of ionisation energy (for the same value of the principal quantum number)?

Easy

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Element	$IE_1$	$IE_2$	$IE_3$
$P$	$495.8$	$4562$	$6910$
$Q$	$737.7$	$1451$	$7733$
$R$	$577.5$	$1817$	$2745$

The correct order of the first ionization enthalpies of the following elements is:

Similar Questions

Which of the following electronic configurations is associated with the biggest jump between the second and third ionization energies?

The first three ionisation energies (in $kJ/mol$) of three representative elements are given below: Element $IE_1$ $IE_2$ $IE_3$ $P$ $495.8$ $4562$ $6910$ $Q$ $737.7$ $1451$ $7733$ $R$ $577.5$ $1817$ $2745$ Which of the following options is incorrect?

The sum of $IE_1 + IE_2$ and $IE_3 + IE_4$ for elements $P$ and $Q$ are given below: Element $IE_1 + IE_2$ $(kJ/mol)$ $IE_3 + IE_4$ $(kJ/mol)$ $P$ $2.45$ $8.82$ $Q$ $2.85$ $6.11$ Then,according to the given information,the incorrect statement$(s)$ is/are:

What is the significance of the terms 'isolated gaseous atom' and 'ground state' while defining the ionization enthalpy and electron gain enthalpy?

Which of the following electrons should have the highest value of ionisation energy (for the same value of the principal quantum number)?

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The first three ionisation energies (in $kJ/mol$) of three representative elements are given below:

Element $IE_1$ $IE_2$ $IE_3$

$P$ $495.8$ $4562$ $6910$

$Q$ $737.7$ $1451$ $7733$

$R$ $577.5$ $1817$ $2745$

Which of the following options is incorrect?

The sum of $IE_1 + IE_2$ and $IE_3 + IE_4$ for elements $P$ and $Q$ are given below:

Element $IE_1 + IE_2$ $(kJ/mol)$ $IE_3 + IE_4$ $(kJ/mol)$

$P$ $2.45$ $8.82$

$Q$ $2.85$ $6.11$

Then,according to the given information,the incorrect statement$(s)$ is/are: