Chem200HWChap9

Chem200HWChap9 - explain your reasoning. 6. Write all the...

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Chapter 9 1. Predict the shape, the bond angles and the polarity for the following compounds: PCl 6 - , PCl 5 , SiCl 4 , C 2 H 2 , NF 3 , IF 5 , SO 2 , AsH 3 , BF 3 , O 3 , HCN 2. How many σ and π bonds are there in all the compounds in question 1. 3. Determine the hybridization of the central atom in the followings compounds: HCOOH, NH 2 CH 3 , HCN, and OC(NH 2 ) 2 . 4. Identify the hybrid orbitals used by C, N, O, S, and I in the following molecules and ions: N 2 H 2 , CH 3 OH, SF 4 , IF 4 + . 5. Knowing that carbon has a valence of four in nearly all its compounds and can form chains and rings of C atoms a) Draw two possible structures for C 3 H 4 . b) Determine all bond angles in each structure. c) Determine the hybridization of each carbon atom in the two structures. d) Ascertain whether the two structures are resonance structures or not and
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Unformatted text preview: explain your reasoning. 6. Write all the Lewis structures that give delocalized bonds in the following compounds: CH 2 CHCHCH 2 , CH 2 CHCHCHO, NCCHCHCH 3 , NCCHCHOH. 7. Be 2 does not exist. Explain why. But what about the Be 2 + ion? Describe its molecular orbital electron configuration and give its net bond order. Do you expect the ion to be stable? 1 8. When potassium reacts with O 2 , potassium superoxide, KO 2 , is produced. The superoxide ion is O 2-, write the molecular orbital electron configuration of the ion and predict its bond order and magnetic character. 2...
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Chem200HWChap9 - explain your reasoning. 6. Write all the...

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