(D) The atomic number of beryllium $(Be)$ is $4$ and boron $(B)$ is $5$. Since $B$ has a higher atomic number than $Be$,it has a greater nuclear charg

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

lesser nuclear charge and greater first ionisation enthalpy

(D) The atomic number of beryllium $(Be)$ is $4$ and boron $(B)$ is $5$. Since $B$ has a higher atomic number than $Be$,it has a greater nuclear charge. The electronic configuration of $Be$ is $1s^2 2s^2$ (fully filled $s$-orbital),while $B$ is $1s^2 2s^2 2p^1$. Due to the stable fully filled $2s$-orbital in $Be$,it requires more energy to remove an electron compared to $B$. Therefore,$Be$ has a lesser nuclear charge and a greater first ionisation enthalpy compared to $B$.

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

Difficult

In comparison to boron,beryllium has

JEE MAIN 2019 All JEE MAIN

A
greater nuclear charge and greater first ionisation enthalpy
B
lesser nuclear charge and lesser first ionisation enthalpy
C
greater nuclear charge and lesser first ionisation enthalpy
D
lesser nuclear charge and greater first ionisation enthalpy

Explore More

Browse All

Question Bank

All Subjects

Class 11 Questions

Class 11

Chemistry Questions

Chapter

Classification of Elements and Periodicity in Properties

Subtopic

Ionisation energy

Previous Year

JEE MAIN 2019 Paper All JEE MAIN years →

Given below are two statements:
Statement $I$: The second ionization enthalpy of $B$,$Al$ and $Ga$ is in the order of $B > Al > Ga$.
Statement $II$: The correct order in terms of first ionization enthalpy is $Si < Ge < Pb < Sn$.

DifficultJEE MAIN 2026

View Solution

Given below are two statements: one is labelled as Assertion $A$ and the other is labelled as Reason $R$:
Assertion $A:$ The first ionisation enthalpy decreases across a period.
Reason $R:$ The increasing nuclear charge outweighs the shielding across the period.
In the light of the above statements,choose the most appropriate from the options given below:

DifficultJEE MAIN 2024

View Solution

What factors should be considered to understand the trends in ionization enthalpy values? Explain.

Medium

View Solution

In which of the following arrangements,the order is $NOT$ according to the property indicated against it?

DifficultAIIMS 2015

View Solution

Ionization enthalpy of an atom is equal to

Medium

View Solution

Vedclass Products

For Students

Vedclass Test Series

Mock tests in real JEE/NEET style with performance analysis. 5-day free trial.

Start Free Trial

For Teachers

Exam Paper Generator

Generate Set A/B/C/D exam papers from 7.5L+ questions in 2 minutes. 3 chapters free.

Try Free

For Institutes

Online Exam Module

Live online exams with unlimited students, 360° analytics & white-label branding.

See Demo

In comparison to boron,beryllium has

Similar Questions

Given below are two statements:Statement $I$: The second ionization enthalpy of $B$,$Al$ and $Ga$ is in the order of $B > Al > Ga$.Statement $II$: The correct order in terms of first ionization enthalpy is $Si < Ge < Pb < Sn$.

What factors should be considered to understand the trends in ionization enthalpy values? Explain.

In which of the following arrangements,the order is $NOT$ according to the property indicated against it?

Ionization enthalpy of an atom is equal to

Vedclass Test Series

Exam Paper Generator

Online Exam Module

Given below are two statements:
Statement $I$: The second ionization enthalpy of $B$,$Al$ and $Ga$ is in the order of $B > Al > Ga$.
Statement $II$: The correct order in terms of first ionization enthalpy is $Si < Ge < Pb < Sn$.