Define the term 'first ionisation energy' and explain why the first ionisation energy shows a general increase across period 2

The first ionisation energy is the energy required to remove an electron from each atom in one mole of gaseous atoms to produce +1 charged gaseous ions.The first ionisation energy shows an general increase across period 2 at the number of shells stay the same but the nuclear charge increases. Therefore electrons experience a greater attraction to the nucleus as the shielding remains the same

NN
Answered by Naledi N. Chemistry tutor

4393 Views

See similar Chemistry A Level tutors

Related Chemistry A Level answers

All answers ▸

How does a change in temperature affect the Kc value when the forward reaction is exothermic?


Draw the full structual diagram of ethyl-ethanoate, labeling relevent bond angles and explain why the molecule has this structure.


What factors affect the lattice enthalpy of an ionic solid?


Why is the enthalpy of hydration of a chloride ion more negative than that of a bromide ion, using your knowledge of the attractive forces involved.


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