Diamond and Graphite

Part of the Structure and Bonding section of Coddy's Chemistry journey. Lesson 35 of 49.

Diamond and graphite are both pure carbon: two forms of one element, differing in how the atoms are joined.

Diamond: each carbon makes four covalent bonds to four other carbons, in every direction. One giant structure: very hard, melts above 3500 °C, no free electrons, does not conduct.

Methane: a carbon atom joined to four hydrogen atoms by four single bonds

Carbon makes four single bonds, as it does to its neighbors in diamond

Graphite: each carbon bonds to three others in flat sheets. The fourth electron moves along the sheet, so graphite conducts; the sheets slide, so it is soft.

Challenge

In diamond each carbon atom is joined to four others by single bonds, just as the carbon in methane is joined to four hydrogen atoms. Draw the Lewis structure of methane, CH₄.

Try it yourself

Lewis boardDraw the Lewis structure of CH₄

Test yourself

This lesson includes a short quiz. Start the lesson to answer it and track your progress.

All lessons in Structure and Bonding

2Covalent Bonds

Sharing Electrons Counting Valence Electrons Drawing Lewis Structures Double and Triple Bonds Lone Pairs Formal Charge Lewis Structures of Ions Recap - Molecule Builder

5Forces Between Molecules

London Forces Dipole-Dipole Forces Hydrogen Bonds Boiling Points Like Dissolves Like Recap - Boiling Contest

8Practice Problems

Recap - Polar Bonds Survey Recap - Pigments and Hexane Recap - Butanol and Ether Recap - Dots on an Oxide

3Shapes of Molecules

Electron Groups Linear and Trigonal Planar Tetrahedral Molecules Pyramids and Bent Molecules Bond Angles Recap - Shape Detective

6Metals and Giant Structures

Metallic BondingDiamond and GraphiteGiant Covalent Structures Four Kinds of Substance Recap - Material Match