In the Nuffield textbook, the bond angle for ethane is 109.5. How can I explain this in terms of the electron clouds, as the shape does not form a tetrahedral position?
If you consider the molecule as a whole this is difficult, but if you consider each carbon atom you will see that each is surrounded by four bonding electron pairs so the angles will be the normal tetrahedral angle (see page 27 in the Nuffield Chemistry students’ book). So the angle is the same as in the simple tetrahedra. All you need to do in organic molecule, is look at each carbon atom in the structure and see how many bonding pairs of electrons it has around it. If it has four it will be tetrahedral. Multiple bonds count as ‘one’, so in ethene there is a double bond and two single bonds round each carbon atom. The molecule is planar with bond angles of 120o. For oxygen and nitrogen atoms you have to take into account any lone-pairs as well as the bonding electrons when explaining the shape of a molecule. Rev Risk assessment Before attempting any practical work based on the advice and suggestions on this website, you must do the following. Identify any hazards, assess the risks fro
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