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

3552 Views

See similar Chemistry A Level tutors

Related Chemistry A Level answers

All answers ▸

The standard enthalpy of formation of glucose is -1273.3kJ/mol, and for carbon dioxide it is -393.5kJ/mol, and for water -285.8 kJ/mol. What is the standard enthalpy of combustion of glucose, C6H12O6?


Why is methylamine a stronger base than aminobenzene?


How does the first ionization enthalpy change down group 2?


Calcium nitride contains 81.1% by mass of the metal. Calculate the empirical formula of calcium nitride. Show your working.


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