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Advanced Higher Chemistry

Advanced Higher Chemistry. Unit 1 Shapes of molecules and Polyatomic Ions. Shapes of Molecules. We can predict the shape of molecules or polyatomic ions (group ions) by looking at the number of electron pairs. There are two types of electron pairs: bonding and non-bonding (lone pairs).

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Advanced Higher Chemistry

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  1. Advanced Higher Chemistry Unit 1 Shapes of molecules and Polyatomic Ions

  2. Shapes of Molecules • We can predict the shape of molecules or polyatomic ions (group ions) by looking at the number of electron pairs. • There are two types of electron pairs: bonding and non-bonding (lone pairs).

  3. Electron Pairs • Bonding electron pairs are the two electrons you would find in a covalent bond. • Non-bonding (or lone pairs) are electrons which are already paired on the atom.

  4. Shapes • The direction of a covalent bonds is determined by the number of orbitals occupied by electron pairs and the repulsion between these orbitals . • Non-bonded pairs have a greater repulsive effect than that of a bonded pair.

  5. Order of repulsion • The order of repulsion is:bonded:bonded<bonded:lone<lone:lone

  6. Linear • Two filled orbitals, two bonding pairs.Cl ÷ Be ÷ Cl • Beryllium chloride has two bonded pairs of electrons. These two pairs will be as far apart as possible resulting in the bonds being 180 degrees apart.

  7. Trigonal Planar • Three filled orbitals, al bonding pairs.

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