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Objective: To learn to draw the Lewis structure for a molecule or ion, determine the geometry of the electron pairs and the geometry of the molecule or ion.

Date Posted: 30/07/2020
Category: Chemistry
Due Date: 05/08/2020
Instruction
Procedure: In order to draw correct Lewis structures, follow the steps given below. 1) Calculate total number of valence electrons in the structure (add group numbers for each atom). a) If structure is a positive ion, subtract electrons equal to the charge. b) If structure is a negative ion, add electrons equal to the charge. 2) Draw a symmetrical skeleton structure connecting atoms bonded with a dash. a) Generally the least electronegative atom is the central atom (but never hydrogen as it always forms only one bond). b) In ternary acids (ones containing polyatomic ions), hydrogen bonds to oxygen and not to the central atom. c) If several structures are possible, choose the one where atoms have the usual number of bonds (usual number of bonds = 8 – group number) 3) Count each dash bonding atoms as two electrons then add lone pairs (non bonding pairs) to atoms surrounding the central atom until each has eight electrons around it (except H – 2 electrons). 4) Add remaining electrons as lone pairs on the central atom. a) If you are two electrons short on the central atom, move a lone pair from a surrounding atom to become a bonding pair and form a double bond. b) If you are four electrons short on the central atom, move two lone pairs from surrounding atoms to become bonding pairs and form a triple bond or two double bonds. c) If you have extra electrons, place them as lone pairs on the central atom (central atom may have up to twelve electrons around it).
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