Why does nuclear radius decrease and first ionisation energy increase across the period?

As we move across the period electrons occupy the same outer electron shell, having roughly the same distance to the nucleus. Moving across the period nuclear charge increases as the number of protons in the nucleus increases, conversly nuclear shielding remains about the same across the row meaning the effective nuclear attraction rises and therefore the nuclear radius also reduces. Because the attraction betweent outer electrons and the nuclear is higher, more energy is required to ionise the atom (remove an electron).

JM
Answered by James M. Chemistry tutor

3139 Views

See similar Chemistry A Level tutors

Related Chemistry A Level answers

All answers ▸

How does the ionisation energy differ across period 2 from Li to Ne?


Give the two reactions required in order to convert an alcohol into a hydroxynitrile. Include reactants and conditions. (6 marks)


Explain the unusually high boiling point of HF


What is the definition of a Brownsted-Lowry base?


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