Chemistry 2000 (Spring 2014) Problem Set #3: Valence Bond Theory Solutions
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1 hemistry 2000 (Spring 2014) Problem Set #3: Valence Bond Theory Solutions Answers to Questions in Silberberg (only those w/out answers at the back of the book) 10.2 sp 2 sp Four hybrid orbitals form when four atomic orbitals of a central atom mix. Whenever orbitals are mixed in any way, the number of orbitals produced must be the same as the original number of orbitals Mixing one p orbital and one s orbital gives two sp hybrid orbitals sp 2 ( has trigonal planar electron group geometry) sp 2 (both have trigonal planar electron group geometry) sp ( has linear electron group geometry) is sp 2 (it has trigonal planar electron group geometry) of the 3 group is sp 3 (it has tetrahedral electron group geometry) with double bonds to and O is sp (it has linear electron group geometry) (1) is sp 3 (it has tetrahedral electron group geometry) (2) is sp 2 (it has trigonal planar electron group geometry) O(3) is sp 3 (it has tetrahedral electron group geometry) (4) is sp 3 (it has tetrahedral electron group geometry) (5) is sp 2 (it has trigonal planar electron group geometry) (6) is sp 2 (it has trigonal planar electron group geometry) 28 should have bond angles that are a little less than likely about 107. should have bond angles that are approximately 120. should have bond angles that are approximately is sp 2 hybridized, so the hybrid orbitals are said to be formed from its 2s, 2p x and 2p y orbitals. The lone pairs on reside in sp 2 orbitals. o. The in 3 are sp 3 hybridized. The in the ring are sp 2 hybridized.
2 Additional Practice Problems 1. The structural formula of glycine is shown below. ame the hybrid orbital set used by each central atom when VB theory is applied to glycine and indicate how many unhybridized 2p orbitals remain on each central atom. : O: Suggested Approach for This Type of Question: 1. Add lone pairs to convert structural formula to Lewis dot structure. 2. Determine electron group geometry for each 'central' atom. 3. hoose hybrid orbital set based on electron group geometry. O 2. DA consists of three types of molecules connected together. The coding molecules are called nitrogenous bases (because they are bases that contain nitrogen). The molecule shown below is adenine, one of the four nitrogenous bases in DA. ame the hybrid orbital set used by each of the three bolded atoms when VB theory is applied to adenine. Also, indicate the number of unhybridized 2p orbitals remaining on each bolded atom. ow many σ bonds are there in one molecule of adenine? 16 ow many π bonds are there in one molecule of adenine? 4 3. Acetyl chloride ( 3 Ol) has the connectivity shown: Draw the best Lewis structure for acetyl chloride. Indicate the molecular geometry at each central atom. (of 3 ) = tetrahedral (of Ol) = trigonal planar What is the hybridization of the following atoms when VB theory is applied to acetyl chloride: (of 3 ) = sp 3 (of Ol) = sp 2 (d) ow many sigma bonds are there in one molecule of acetyl chloride? 6 (e) ow many pi bonds are there in one molecule of acetyl chloride? 1 : O: l :
3 4. Acetonitrile ( 3 ) has the connectivity shown: Draw the best Lewis structure for acetonitrile. Indicate the molecular geometry at each central atom. (of 3 ) = tetrahedral (of ) = linear What is the hybridization of the following atoms when VB theory is applied to acetonitrile: (of 3 ) = sp 3 (of ) = sp (d) ow many sigma bonds are there in one molecule of acetonitrile? 5 (e) ow many pi bonds are there in one molecule of acetonitrile? 2 : 5. The Lewis structure for 2 2 is shown below. onsider this molecule according to valence bond theory. ame the set of hybrid atomic orbitals used by each atom. sp 2 learly indicate which orbitals contribute to each σ bond in 2 2. :(sp 2 ) (1s) :(sp 2 ) (1s) :(sp 2 ) (sp 2 ) learly indicate which orbitals contribute to each bond in 2 2. :(2p) (2p)
4 6. Use diagram(s) to explain how sp orbitals are formed. learly indicate the number, type and geometry of all orbitals involved. An s orbital and a p orbital in the same shell of the same atom combine to make two sp orbitals: 7. Use diagrams in your answers to the following questions. What is the main difference between a hybrid atomic orbital and a molecular orbital? ybrid atomic orbitals are formed by mixing orbitals on the same atom. Molecular orbitals are formed by mixing orbitals on different atoms. (In both cases, the total number of orbitals is not changed. Mixing two atomic orbitals gives two new orbitals be they hybrid atomic orbitals or be they molecular orbitals.)
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