Explain why the second ionisation energy of boron is higher than the first ionisation energy of boron.

Boron is the 5th element in the periodic table, and has an electron configuration 1s22s22p1. The first ionization energy of Boron is the energy required to remove the single 2p electron, while the second ionization energy of boron is the energy required to remove one of the two 2s electron. If we already have removed the 2p electron, then we are left with a positively charged Boron ion, and it is harder to remove another electron from an already positively charged species. Moreover, the 2s electrons are closer to the nucleus and are held in the atom with a greater force. That is why the second ionization energy of Boron is higher.

AI
Answered by Adelina I. Chemistry tutor

36092 Views

See similar Chemistry A Level tutors

Related Chemistry A Level answers

All answers ▸

How can you test for aldehydes and ketones?


The bond angle in a molecule of ammonia (NH3) is 107 degrees so why, when part of a transition metal complex is the bond angle 109.5 degrees.


What are the stereochemical implications of bimolecular and unimolecular nucleophilic substitution?


Explain the trend in first ionisation energy as you go across Period 3


We're here to help

contact us iconContact ustelephone icon+44 (0) 203 773 6020
Facebook logoInstagram logoLinkedIn logo

© MyTutorWeb Ltd 2013–2025

Terms & Conditions|Privacy Policy
Cookie Preferences