Assertion (A): Boron has a smaller first ioni | vedclass

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

Question

(C) Assertion $(A)$: Electronic configuration of Boron $(Z=5)$ is $[He] 2s^2 2p^1$. In the first ionisation ($IE_1$ or $\Delta_i H_1$),the electron is

Vedclass · Accepted Answer

Assertion and Reason both are correct statements and Reason is correct explanation for Assertion.

Vedclass · Answer

(C) Assertion $(A)$: Electronic configuration of Boron $(Z=5)$ is $[He] 2s^2 2p^1$. In the first ionisation ($IE_1$ or $\Delta_i H_1$),the electron is removed from the $2p^1$ orbital.Electronic configuration of Beryllium $(Z=4)$ is $[He] 2s^2$. The electron is removed from the fully filled $2s^2$ orbital,which is more stable and requires more energy.Thus,the Assertion is correct.Reason $(R)$: The $s$-orbital is spherical and closer to the nucleus,providing better shielding for the $2p$ electron from the nuclear charge. Consequently,the $2p$ electron in Boron experiences a lower effective nuclear charge compared to the $2s$ electrons in Beryllium,making it easier to remove.Therefore,the Reason is the correct explanation for the Assertion.

Assertion $(A)$: Boron has a smaller first ionisation enthalpy than beryllium.
Reason $(R)$: The penetration of a $2s$-electron to the nucleus is more than the $2p$-electron; hence,the $2p$-electron is more shielded by the inner core of electrons than $2s$-electrons.

Similar Questions

The incorrect statement is:

Given below are two statements:
Statement $I$: The first ionization energy of $Pb$ is greater than that of $Sn$.
Statement $II$: The first ionization energy of $Ge$ is greater than that of $Si$.
In the light of the above statements,choose the correct answer from the options given below:

Among the second period elements,the actual ionization enthalpies are in the order $Li < B < Be < C < O < N < F < Ne$. Explain why:
$(i)$ $Be$ has higher $\Delta_{i}H$ than $B$
$(ii)$ $O$ has lower $\Delta_{i}H$ than $N$ and $F$?

Which of the following orders for ionisation energy is correct?

Would you expect the first ionization enthalpies for two isotopes of the same element to be the same or different? Justify your answer.

Vedclass Test Series

Exam Paper Generator

Online Exam Module

Assertion $(A)$: Boron has a smaller first ionisation enthalpy than beryllium.Reason $(R)$: The penetration of a $2s$-electron to the nucleus is more than the $2p$-electron; hence,the $2p$-electron is more shielded by the inner core of electrons than $2s$-electrons.