Explain how successive ionization energies account for the existence of three main energy levels in the sodium atom.

Make the student observe and analyse the electronic configuration of sodium and the trends in ionization energies for this element. We note a large increase in ionization energy between the 1st and 2nd electrons and between the 9th and 10th electrons. The large increase in ionization energy means that there is a much greater nuclear charge on the successive electrons as we get closer to the nucleus. The extent of this difference for those specific electrons shows that the the second electron is much closer to the nucleus that the first one, meaning that we have changed energy level. The same thing applies for the 9th and 10th electrons. Given that we noted 2 significant increases in energy levels, this shows that there are 3 main energy levels.(Support this with a diagram for better understanding).

Answered by Yasmin T. Chemistry tutor

8595 Views

See similar Chemistry IB tutors

Related Chemistry IB answers

All answers ▸

There are three halogenoalkanes with halogens F, Br and I. Each undergo an SN2 reaction. How does the rate of reaction differ between the three halogenoalkanes?


What is the structure of fluoroform (CFH3)? Does it have a dipole, explain your answer.


Explain the substitution reaction of a primary halogenoalkane with sodium hydroxide.


Describe how sigma and pi bonds form and describe how single and double bonds differ.


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