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Unformatted text preview: 2]. Suggest a mechanism consistent with this rate law, being sure to label steps as fast and slow. (Hint: It is easiest to assume the first step is slow.) NO2(g) + F2(g) NO2F(g) + F(g) (slow) 1 if equilibrium arrows used for slow Step 1: +2 slow step matches rate law +1 slow/fast labels (fast) F(g) + NO2(g) NO2F(g) Step 2: +2 steps add to overall equation 1 each unbalanced reaction 5 9. Consider the substitution reaction of H2SBH3 with NH3, which generates two product molecules (ignore the states of matter), assuming that no species exceeds the octet rule. Given the following information: Step 1: There are two products in the first step; one product, which is an intermediate, has a trigonal planar molecular geometry. Step 2: The intermediate from Step 1 reacts in Step 2 to form a compound with two sp3 hybridized atoms. Overall: One bond is formed and one bond is broken. One of the products has a bent molecular geometry and smells like rotten eggs. (a) Propose a mechanism for this reaction. (b) Draw the Lewis structures of both products, including all lone pairs and formal charges. +2 Step 1: H2SBH3 H2S + BH3 H
H Step 2: BH3 + NH3 H3NBH3 +2 H
H 1 for each incorrect species and each unbalance...
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This note was uploaded on 09/20/2012 for the course CHEM 1252 taught by Professor Jew during the Fall '12 term at UNC Charlotte.
- Fall '12