This question is about the ionisation energy of elements across a period. a) Define ionisation energy. b) Explain the trend in ionisation energy across a period.

a) Ionisation energy is the minimum amount of energy required to remove an electron from each atom of one mole of gaseous atoms.
b) Across a period, the ionisation energy increases due to the increase in protons within the nucleus, this increases the nuclear charge of the atom and also draws the outer electrons in towards the nucleus, in turn decreasing the atomic radius. Both factors lead to a greater attraction between the nucleus and outer electrons, making it harder to remove an electron from the atom.

EC
Answered by Emma C. Chemistry tutor

1302 Views

See similar Chemistry A Level tutors

Related Chemistry A Level answers

All answers ▸

Write equations for the reaction of propanoic acid with methanol and name any organic products.


How do you go about answering titration equations?


But-1-ene reacts with HBr to form a saturated compound, name and draw the mechanism, then explain how three isomeric products are formed.


Calculate the empirical formula of a compound containing 77.7% Iron and 22.3% of oxygen.


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