Why do the atomic radii of the elements decrease across Period 3 from sodium to chlorine?

The atomic radius of an atom is the distance from the atom's nucleus to its outermost electron. Moving across Period 3, the number of protons in the nucleus increases - for example sodium has 11 protons, and chlorine has 17 protons. Nuclear charge increases across the period, therefore the attraction between the positively charged nucleus and negatively charged electrons increases, so the atomic radii decreases. The number of electrons also increases across a period, but as each extra electron enters the same principal energy level, there is relatively little extra shielding.

Answered by Amy T. Chemistry tutor

27007 Views

See similar Chemistry A Level tutors

Related Chemistry A Level answers

All answers ▸

State and explain the trend in ionisation energies and its effect on the reactivity of groups containing metals.


Draw the reaction mechanism for the formation of ethanol from bromoethane and water and name the mechanism.


Explain why the second ionisation energy of boron is higher than the first ionisation energy of boron?


What's the difference between Aliphatic and Aromatic Molecules?


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