1C ODea hndt 2

1C ODea hndt 2 - a. PH 3 b. NO 2-c. C 2 H 2 d. CO 3 2-e. N...

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CLAS Chem 1C Handout 2 Ch 13 Bonding (13.10 – 13.12) Rules for drawing Lewis structures : 1. Add up all the valence electrons for the molecule. If the molecule has a negative charge, add electrons, if it has a positive charge, subtract electrons. 2. Form single bonds between the atoms first (two electrons per bond). 3. Arrange the remaining electrons to satisfy the duet rule (2 e-) for hydrogen and the octet rule (8 e-) for other elements. 1. Draw Lewis structures for the following. Show resonance where applicable.
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Unformatted text preview: a. PH 3 b. NO 2-c. C 2 H 2 d. CO 3 2-e. N 2 f. HCN g. ClO 2-h. N 2 O 4 How to calculate formal charge : FC = (# of valence e- on free atom) - (# of e- belonging to atom in Lewis structure) 2. Draw all the resonance structures for the ion OCN-. Which is the most stable? 3. Draw two Lewis structures for the following molecules, one that obeys the octet rule and one that minimizes formal charge. a. SO 4 2-b. POCl 3 c. BeF 2 d. XeO 4...
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1C ODea hndt 2 - a. PH 3 b. NO 2-c. C 2 H 2 d. CO 3 2-e. N...

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