Explain the trend in first ionisation energy as you go across Period 3

Overall, the first ionisation energies will increase. This is because as you go along the period, the atomic number increases and this causes a stronger electrostatic attraction between the outer electrons and the nucleus. There are 2 "dips" in this trend. There is a drop in energy from Magnesium to Aluminium. This is because in magnesium the outer electrons are in a 3s orbital, whereas in aluminium the outer electron is in a 3p orbital. The 3p orbital is further from the nucleus, and hence there is more electron shielding and distance from the nucleus so electrostatic attraction decreases. The second drop is from Phosphorus to Sulphur. This is because it is the first time electrons are paired up in 3p orbitals, so there is added electron-electron repulsion.

Answered by Charles W. Chemistry tutor

15571 Views

See similar Chemistry A Level tutors

Related Chemistry A Level answers

All answers ▸

Explain why the second ionisation energy of Magnesium is lower than the second ionisation energy of Sodium.


How does the 3D dash and wedge notation work?


25cm3 of a 0.10moldm-3 solution of sodium hydroxide reacts exactly in a titration with 15cm3 HCl. What is the concentration of the hydrochloric acid?


Discuss the 2 most-commonly encountered representations of benzene, providing an advantage and disadvantage for each


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