Problem Set 2

Problem Set 2 - , , g or u , where appropriate). b) How...

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Problem Set 2 Chemistry 173a/268a Due: Oct 26, 2007 1. Draw the Lewis dot structures for the following molecules: a) ClF 3 b) XeF 4 c) SO 2 d) ClO 2 F 3 e) TeCl 4 f) IO 3 - g) ICl 2 + 2. Using the VSEPR model, predict the shape of each of the molecules above. Provide both the (i) arrangement of the ‘electron regions’ and (ii) molecular geometry. 3. a) Draw the MO diagrams for NO - , NO, and NO + . b) Give the bond order for each. c) Give the magnetic properties of each. d) Place these three species in order of increasing bond length and explain your reasoning. e) Place NO - , NO, NO + , N and O in order of increasing ionization energy and explain your reasoning. 4. a) Draw the orbital combinations for linear CH 2 and construct the corresponding MO diagram (N.B. label your molecular orbitals as
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Unformatted text preview: , , g or u , where appropriate). b) How many molecular orbitals does CH 2 possess? c) How many bonding and anti-bonding orbitals does CH 2 possess? d) Does CH 2 contain any non-bonding orbitals. If so, why? e) Is this molecule diamagnetic or paramagnetic? f) What is the point group of this molecule? 5. Compare and contrast the following concepts as they pertain to Lewis theory and molecular orbital theory: a) bond b) multiple-bond c) lone pair . 6. For each of the following molecules, provide the (i) symmetry operations and (ii) point group: F Cl F Cl Cl Cl F F C(CFClMe) 4 N N C CH 2 D CD 3 D 2 HC CH 3 F F F F g) h) SO 3 i) CN-j) H 2 O a) b) c) d) e) f) B F Br Cl...
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This note was uploaded on 08/06/2008 for the course CHEM 173A taught by Professor Unknown during the Spring '08 term at UCSB.

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