Lewis Structures SCH3U/4C March 2016.

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Presentation transcript:

Lewis Structures SCH3U/4C March 2016

Lewis Structures We have seen Lewis diagrams for single elements, where we represent only the valence electrons for a particular element.

Lewis Structures A Lewis structure consists of the electron distribution in a compound and the formal charge on each atom.

How to Draw Lewis Structures Example: CO2 Determine whether the compound is ionic or covalent using electronegativity differences. C = 2.5 O = 3.0 EN = 0.5 (covalent) Determine the total number of valence electrons by adding the valence electrons for each atom involved: C = 4, O = 6x2 Total = 16

Divide the total number of valence electrons by two, to determine the number of electron pairs. Organize the atoms so there is a central atom (usually the least electronegative) surrounded by outer atoms O C O

8 EP – 2 EP = 6 EP : : : : 6 EP – 6 EP = 6 EP : : Distribute the electron pairs, keeping track of how many electron pairs (EP) remain: Place one pair between the central atom and each outer atom O : C : O Three more pairs on each outer atom : O : C : O : Redistribute the electrons to ensure each atom has a satisfied octet. : O :: C :: O : 8 EP – 2 EP = 6 EP : : : : 6 EP – 6 EP = 6 EP : :

Replace any bonding pairs with the appropriate bond (single or double) : O = C = O : Note that each oxygen molecule has 2 pairs of electrons that are not involved in bonding. These non-bonding electron pairs are known as lone pairs : :