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11 Nov 2019
Can someone help me with steps 1-3 for question 1-52 letter (e)
For each of the following compounds, Give the hybridization and approximate bond angles around each atom except hydrogen. Draw a three-dimensional diagram, including any lone pairs of electrons. (a) H_3 O^+ (b) ^-OH (c) CH_2CHCN (d) (CH_3)_3 N (e) [CH_3NH_3]^+ (f) CH_3COOH (g) CH_3CHNH (h) CH_3OH (i) CH_2O For each of the following compounds and ions, Draw a Lewis structure. Show the kinds of orbitals that overlap to form each bond. Give approximate bond angles around each atom except hydrogen. In most amines, the nitrogen atom is sp^3 hybridized, with a pyramidal structure and bond angles close to 109 degree. In urea, both nitrogen atoms are found to be planar, with bond angles close to 120 degree. Explain this surprising finding.
Can someone help me with steps 1-3 for question 1-52 letter (e)
For each of the following compounds, Give the hybridization and approximate bond angles around each atom except hydrogen. Draw a three-dimensional diagram, including any lone pairs of electrons. (a) H_3 O^+ (b) ^-OH (c) CH_2CHCN (d) (CH_3)_3 N (e) [CH_3NH_3]^+ (f) CH_3COOH (g) CH_3CHNH (h) CH_3OH (i) CH_2O For each of the following compounds and ions, Draw a Lewis structure. Show the kinds of orbitals that overlap to form each bond. Give approximate bond angles around each atom except hydrogen. In most amines, the nitrogen atom is sp^3 hybridized, with a pyramidal structure and bond angles close to 109 degree. In urea, both nitrogen atoms are found to be planar, with bond angles close to 120 degree. Explain this surprising finding.
Irving HeathcoteLv2
3 Apr 2019