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

3105 Views

See similar Chemistry A Level tutors

Related Chemistry A Level answers

All answers ▸

what is entropy in terms of disorder?


Explain why xenon has a lower first ionization energy than neon.


Describe the shape of, and bonding in, a molecule of benzene and explain why benzene does not readily undergo addition reactions.


For the following reaction, you obtained 7.2 g of sodium sulfate, starting from 10 g of sulfuric acid. Sodium hydroxide is in excess. What is the % yield? H2SO4 + 2NaOH → Na2SO4 + 2H2O


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