Explain the trend in the first ionisation energies of the group 1 elements

The general trend is a decrease in first ionisation energy, which is because as you descend the group the number of energy levels surrounding the positively charged nucleus increases. This means that the outermost electrons are held further away from the positive nucleus, and experience more shielding from the inner shells. This therefore means that the electrostatic attraction between the positive nucleus and negative outermost electron is weakened, so less energy is required for this attraction to be overcome and the electron to be liberated.

CB
Answered by Caitlin B. Chemistry tutor

5615 Views

See similar Chemistry A Level tutors

Related Chemistry A Level answers

All answers ▸

At what temperature does the reaction become feasible? When ΔH = 492.7 kJmol^-1 and ΔS = 542.6 JK^-1mol^-1.


What is the standard enthalpy change of formation and how does it differ from the standard enthalpy change of reaction?


State and explain the general trend in the first ionisation energy across a period.


When aqueous barium chloride is added to a solution containing sulfate ions a white precipitate is formed. i)Write the ionic equation for the formation of this precipitate.


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