T2-S10-898989-elab

T2-S10-898989-elab - Test 2 CH101-001, 5 mar 2010, code...

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Test 2 CH101-001, 5 mar 2010, code 898989 NAME: ______________ Question 1 Consider the ion BrO 2 1- You may assume the bromine atom is in the middle. Perform a Lewis type calculation. Determine the formal charges (FC), oxidation states (Ox) and the bond order (BO). Also consider the shape and the proper name of the molecular ion. Select the correct answer: A. The shape is bent, the name is the bromite and Ox(Br) = +3 B. The shape is linear and Ox(Br) = -1 C. The formal charges are: FC(Br)=+3 and FC(O)=-2 D. There are ten lone pairs and the name is bromate. E. There are two resonance structures, such that the bond order of both Br-O bonds is 1½. Question 2 Consider the molecule CH 2 NH. Two of the hydrogen atoms are attached to the carbon atom and one to the nitrogen. Applying Lewis and VSEPR rules predict the shape of the molecule and the bond order of this species. A. The bond order of the C-N bond is 1. The C-N-H angle is 120 o B. The bond order of the C-N bond is 3 The C-N-H angle is 180 o C. The bond order of the C-N bond is 1 The C-N-H angle is 108 o D. The bond order of the C-N bond is 2. The C-N-H angle is 180 o E. The bond order of the C-N bond is 2 The C-N-H angle is 120 o Question 3 Are these statements true? A. Hybridization theory works well in describing the bonding in most organic molecules. B. Nonbonding electron pairs are often thought to be associated to more than atom, whereas lone pairs are assumed to be localized on one atom only. C. Antibonding orbitals always have one or more nodal planes more than the corresponding bonding combination. D. All of the above.
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C O O O C O O O C O O E. None of the above. Question 4 When calculating the electronic structure of the carbonate ion CO 3 2- according to the Lewis assumptions we arrive at three equivalent structures as shown. Select the correct statement A. The description with three resonance forms results from the erroneous assumption that electron pairs (e.p.) can only be shared by two atoms. In reality the bond order is 1.333 for each bonding region, because one e.p. is shared over the whole molecule. B. This molecular ion always has two longer bonds of order 1 and one shorter one of order 2 C.
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T2-S10-898989-elab - Test 2 CH101-001, 5 mar 2010, code...

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