Explain the change in first ionisation energy across period 2

Ionisation energy increases overall because nuclear charge increases with no significant increase in shielding, so it becomes more difficult to remove the outer electron.Ionisation energy decreases going from beryllium to boron as an electron is now being removed from a 2p orbital rather than a 2s orbital. 2p orbitals are higher in energy so it is easier to remove an electron.Ionisation energy decreases going from nitrogen to oxygen because now electrons are paired in orbitals so the electron removed from oxygen is repelled more by the other electron in its orbital so is easier to remove.

Answered by Amelia I. Chemistry tutor

14162 Views

See similar Chemistry IB tutors

Related Chemistry IB answers

All answers ▸

Describe how σ and π bonds form.


Explain the general trend in first ionisation energy across period 2 in the periodic table.


How are Van der Waals interactions formed between molecules?


Explain whether the boiling point of 1-bromopentane will be higher, lower or the same as that of 2-bromo-2-methylbutane. (3)


We're here to help

contact us iconContact usWhatsapp logoMessage us on Whatsapptelephone icon+44 (0) 203 773 6020
Facebook logoInstagram logoLinkedIn logo

© MyTutorWeb Ltd 2013–2025

Terms & Conditions|Privacy Policy
Cookie Preferences