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

Answered by Maria T. Chemistry tutor

3185 Views

See similar Chemistry A Level tutors

Related Chemistry A Level answers

All answers ▸

2.11g of MgCl2 is added to 30cm3 of water. Find the concentration of chloride ions in the solution.


Write a balanced equation for the oxidation of Iron from the 2+ oxidation state to the 3+ oxidation state using the manganate ion.


State and explain the general trend in first ionisation energy across Period 3


Explain why phenol is nitrated more readily than benzene.


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