Describe and explain the electrical conductivity of lithium oxide, Li2O, and lithium in their solid and molten states.

Lithium conducts electricity in its solid and molten states. Lithium exhibits metallic bonding and as such its valence electrons are delocalised in the liquid and solid state allowing electricty to be conducted.

Lithium oxide only conducts electricty in its molten state. It is an ionic compound and in solid Li2O the ions are fixed in position in an ionic lattice, the ions are not mobile and therefore cannot conduct electricty. However, when molten the ionic bonds are broken and the ions are mobile allowing electricty to be conducted. 

CF
Answered by Charlie F. Chemistry tutor

33299 Views

See similar Chemistry A Level tutors

Related Chemistry A Level answers

All answers ▸

What are the redox reactions involving carbonyls?


10cm^3 of 1M NaOH solution is mixed with 15cm^3 of 0.5M HCl, what is the resulting pH of the solution?


Why is phenol more reactive than benzene?


describe the structure of graphite


We're here to help

contact us iconContact ustelephone icon+44 (0) 203 773 6020
Facebook logoInstagram logoLinkedIn logo

MyTutor is part of the IXL family of brands:

© 2025 by IXL Learning