Consider carbon allotropes diamond and graphite. Unlike diamond, graphite conducts electricity. Why? 1. In graphite, there are hybrid orbitals used for bonding that contain electrons. 2. In diamond, all the electrons are in sigma bonds which allow conductivity of electricity. 3. In graphite, there are unhybridized p- orbitals that extend over the entire sheet forming a delocalized pi (1) bonding network where electrons are free to move. 4. In diamond, the bonding electrons have enough energy to move and can therefore conduct electricity. 5. In graphite, the bonds are 109°, which is perfect for electricity conduction.

Consider carbon allotropes diamond and graphite. Unlike diamond, graphite conducts electricity. Why? 1. In graphite, there are hybrid orbitals used for bonding that contain electrons. 2. In diamond, all the electrons are in sigma bonds which allow conductivity of electricity. 3. In graphite, there are unhybridized p- orbitals that extend over the entire sheet forming a delocalized pi (1) bonding network where electrons are free to move. 4. In diamond, the bonding electrons have enough energy to move and can therefore conduct electricity. 5. In graphite, the bonds are 109°, which is perfect for electricity conduction.

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter7: Chemical Bonding And Molecular Structure

Section: Chapter Questions

Problem 7.105PAE

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