Lewis Structures visualize molecular structure

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Presentation transcript:

Lewis Structures visualize molecular structure assume most atoms will have octet of electrons 1. Determine number of valence electrons 2. Place least electronegative atom at center Using e- pairs, bond central atom to surrounding atoms 4. Complete octets on surrounding atoms 5. Place remaining e- on central atom. Use multiple bonds to complete octet, if necessary

: : : : : : : F N F : : : : : F : N F : nitrogen trifluoride NF3 valence e- N = 5 5 + (3 x 7) = 26 e- F = 7 central atom = N bond F to N : : : : : : : F N F 6 e- complete octets : : : : : F 24 e- surrounding atoms : 26 e- complete octet N F : central atom include lone pairs

: : : : : O C : O : : : : O : : C O C O : : C O C O : carbonate ion 4 + (6 x 3) = 22e- valence e- C = 4 O = 6 charge = 2- 24e- : : C=O bond shorter C O bond : : : O C : O 6e- stronger : : : : O : 24e- : C O resonance structures C O : : C O C O :

: : H : C : H H : C : : O : H : : : : O : . .. . . .. formaldehyde CH2O 4 + 6 + (2 x 1) = 12e- 4 - 0 - 4 = 0 4 - 2 - 3 = -1 : : H : C : H which is best structure? H : C : : O : H : : : : formal charge O 6 - 2 - 3 = 1 : compare e- in isolated atom to 6 - 4 - 2 = 0 e- in Lewis structure formal charge = valence e- - lone pair e- - ½ shared e- formal charge = 0 preferred . C .. N . . .. O

: : : O : N : O : H : : : : : O : O N O H O O N O H O O N O H O nitric acid HNO3 valence e- N = 5 5 + (3 x 6) + 1 = 24 e- O = 6 oxy acid O-H H = 1 : : : O : N : O : H central atom = 8 e- N : : : : : O 24 e- bond O to N : +1 bond H O N O H O O N O H O complete octets -1 -1 +1 +1 surrounding atoms O N O H O complete octet central atom -1

: : : : : N : O N O : Exceptions to octet rule 1. Molecules with odd number of electrons Lewis structures electron pairs unpaired e- free radical NO 5 + 6 = 11e- start with 12e- : : : : : N : O N O : 5 5 - 3 - 2 = 0 - 4 - 2 = -1 6 - 4 - 2 = 0 6 - 3 - 2 = +1

: : : F F : B : : : F : : Exceptions to octet rule 2. Incomplete octets (fewer than 8 e-) B Be (Al) boron trifluoride BF3 3 + (3 x 7) = 24e- : : : F F : B : : : F : :

Cl : Cl : Cl : P Cl : Cl : Exceptions to octet rule 3. Expanded octet more than 8 e- only Period 3 and above must have d orbitals phosphorous pentachloride PCl5 5 + (5 x 7) = 40e- Cl : Cl : Cl : P Cl : Cl :