6. The bond angle for H-N-H in the Ammonia molecule is 107°, whereas the bond angle for H-P-H in the molecule PH3 is 93°. Explain: a. Why the H-N-H bond angle is 107°. b. Why the H-P-H bond angle is 93°.
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1. Why are double bonds and triple bonds shorter than single bonds? 2. VSEPR geometry predicts that the bond angles in formaldehyde (CH2O), a trigonal planar molecule, will be 120° throughout all three angles. However, analysis showed that the H-C-H bond angle is slightly smaller at 116.5°, while the two H-C-O angles are slightly larger at 121.8°. Explain this difference in the predicted bond angle vs actual bond angle. 3. VSEPR geometry also predicts that the bond angles in tetrahedral molecules are 109.5°. However, in the case of ammonia (NH3), analysis showed that the H-N-H bond angles are 107.3°. Explain this difference in the bond angle. 4. What is electronegativity, and why is it used to determine bond polarity? 5. Which among the molecules above has a resonance structure? What did you find to be common among them that is required to have a resonance structure?
Kaden B.
Explain why the H-N-H bond angle of ammonia is 107 °.
Preeti K.
The H-N-H bond angles in ammonia, NH3, and phosphine (the formal name is "phosphane"), PH3, are 107° and 93°, respectively. Apparently, the nitrogen atom in ammonia uses nearly fully developed sp3 hybrid orbitals while the phosphorus atom in phosphine does so to a much smaller extent. What are possible reasons why hybridization of s and p orbitals works well on nitrogen, but not on phosphorus?
Sri K.
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