Tetrahedral Molecules

Part of the Structure and Bonding section of Coddy's Chemistry journey. Lesson 18 of 49.

Four groups, no lone pairs: tetrahedral, every bond angle 109.5°.

Methane and tetrachloromethane: a central carbon with four atoms around it

Four bonds and no lone pairs: a tetrahedron, drawn here flat

A flat drawing of CH₄ looks like a cross with 90° angles. In space the bonds spread further, to 109.5°. Examples: CH₄, CCl₄, CHCl₃, SiH₄.

Challenge

Trichloromethane, CHCl₃, was once used to put patients to sleep before surgery. Carbon is bonded to one hydrogen and three chlorine atoms. What shape is it, and what is its bond angle?

Try it yourself

Shape viewerDescribe the molecule CHCl₃

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 PlanarTetrahedral MoleculesPyramids and Bent Molecules Bond Angles Recap - Shape Detective

6Metals and Giant Structures

Metallic Bonding Diamond and Graphite Giant Covalent Structures Four Kinds of Substance Recap - Material Match