State and explain the trend in ionisation energies and its effect on the reactivity of groups containing metals.

First ionisation energies decrease down groups in the Periodic Table:-larger atomic radius-increased nuclear charge is outweighted by increased shielding-reactivity increases down the group as it's easier to lose electrons-there is less attraction on electrons

MT
Answered by Maria T. Chemistry tutor

3195 Views

See similar Chemistry A Level tutors

Related Chemistry A Level answers

All answers ▸

What is a 'foolproof' way to balance any combustion reaction?


What is meant by the 'First Ionisation Energy' of an element?


How do you decide what the sign of the enthalpy change should be?


Explain why Magnesium has a greater second ionisation energy than strontium


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