By Sören Prip Beier, Peter Dybdahl Hede
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Extra resources for Essentials of Chemistry, 2nd edition
Example text
The octet rule has to be satisfied for all the atoms in the molecule. Therefore it is necessary with double bonds between the carbon atom and the oxygen atoms. That way the Lewis structure for carbon dioxide has now told us that in this molecule the carbon atom is placed in the centre. Each oxygen atom is double bonded to the carbon atom and two lone pairs are “attached” to each oxygen atom. But from the Lewis structure we know nothing about the actual molecular geometry. We know that hydrogen (from the 1st period) wants to be surrounded by two electrons and that elements from the 2nd period want to satisfy the octet rule by being surrounded by eight electrons.
The number of dots corresponds to the number of valence electrons. When the atom is surrounded by eight electrons the octet rule is satisfied. The electrons are often placed in pairs. Such an electron pair is called a lone pair. By use of Lewis’ theory and atoms in ”electron dot forms” we are prepared to look at how atoms are arranged inside the molecules relative to each other. When the so-called Lewis structure of a molecule or composite ion is to be written on a piece of paper, the following guidelines have to be followed: 1) Determine the total number of valence electrons for the molecule/composite ion.
In this chapter we will use our knowledge about atomic orbitals to answer the following question: Why do two hydrogen atoms join and form a H2 molecule when for example two helium atoms rather prefer to stay separate than to form a He2 molecule? We are also going to look at the geometry of different molecules by using orbital theory. That way we can find the answer to the following question: Why is a CO2 molecule linear (O-C-O angle = 180°) when a H2O molecule is V-shaped (H-O-H angle 180°)? When we have been looking at different molecules we are going to move into the world of metals.