Why does the first ionisation energy of atoms generally increase across a period?

The first ionisation energy is defined as the energy required to remove one mole of electrons from each atom of a mole of gaseous atoms. As we go along a period in the periodic table, the atomic number increases. As the atomic number increases, the number of protons in the nucleus increases. This causes the electrostatic attraction between the nucleus and the outermost electron to generally become stronger across a period.

Answered by Chemistry tutor

3589 Views

See similar Chemistry A Level tutors

Related Chemistry A Level answers

All answers ▸

Elements in the periodic table show a trend in atomic radius. State and explain the trend in atomic radius from Li to F.


What are moles and how do you calculate them?


Explain why the first ionisation energy of sulfur is different from that of phosphorus.


State 2 features of a system that is in dynamic equilibrium.


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