Identify and explain the trend in atomic radius across a period

The atomic radius across a period in the periodic table tends to decrease from left to right. As you move across a period the number of electrons from one element to the next increases by one. The electron is added in the same valence shell which increases electron repulsion which slightly increases the atomic radius but this is a very small. As you move across a period an extra proton is aded from one element to the next, increasing the positive charge of the nucleus and therefore increasing the attractive force between the nucleus and the valence shell. This increased electrostatic attraction pulls the valence shell closer to the nucleus so the atomic radius decreases.

OM
Answered by Olavo M. Chemistry tutor

19234 Views

See similar Chemistry IB tutors

Related Chemistry IB answers

All answers ▸

What is the difference between SN1 and SN2 reactions, and how do you determine via which mechanism the reaction will proceed?


In reaction kinetics, what parameters affect the rate of the reaction?


Sort the following substances MgO, Na, H2O, H2S, NaCl, in the order of increasing melting temperature.


Draw the full curly mechanism for the reaction between Bromo-Methane and NaOH. What reaction is it?


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