 Hybridization 1s Overlap of 1sH-1sH s-bond

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Presentation transcript:

 Hybridization 1s Overlap of 1sH-1sH s-bond How is the bond formed in H2 molecule? H● + ●H → H-H H ● 1s Overlap of 1sH-1sH Increase in the electron density on the line connecting the two nuclei.  s-bond

s-bond How is the bond formed in HF molecule? H● + ●F → H-F Overlap of 1sH-2pF s-bond How is the bond formed in F2 molecule? Overlap of 2pF-2pF

How is the bond formed in CH4 molecule? Problem: Only two unpaired electrons in C atom!! CH2!!!! Now: 4 unpaired electrons in C atom  4 bonds! 2s 1s 2p Problem: bonds are not equivalent: 1 bond 3 bonds

Bond angle H-C-H = 90º NOT 109.5º can not be correct! Hybridization

No. of hybrid orbitals = No. of mixed orbitals

N H How is the bond formed in NH3 molecule? 2p N H Overlap of 1sH-2pN?? Problem: bonds are perpendicular to each other!! N 3 bonds Actually 107º which is close to 109.5 º not to 90 º.

2s 1s 2p Overlap of sH-sp3N 2s 1s 2p O H Bond angle 90º!!

No. of mixed orbitals = No. of s bonds + No. of lone EP CH4: 4+0 = 4 (1 s + 3 p) = 4 sp3 NH3: 3+1 = 4 (1 s + 3 p) = 4 sp3 H2O: 2+2 = 4 (1 s + 3 p) = 4 sp3

p-BOND Increase in electron density above and below the connecting line.

the fourth is different. How is the bond formed in C2H4 molecule? 2s 1s 2p 120º 3 equivalent bonds, But the three bonds must be perpendicular!! 3 equivalent bonds, the fourth is different. Only two bonds.

What is the hybridization of C atom in C2H4? sp2 no. of s-bonds=3 no. of lone EP=0 3+0=3 one s + two p → sp2

Only two bonds are equivalent. How is the bond formed in C2H2 molecule? 2s 1s 2p 3 equivalent bonds, and the three bonds must be perpendicular!! Only two bonds are equivalent.

   

Overlap of sH-spC Overlap of spC-spC Overlap of pC-pC What is the hybridization of C atom in C2H2? sp no. of s-bonds=2 no. of lone EP=0 2+0=3 one s + one p → sp

How is the bond formed in PCl5 molecule? Cl P Cl Cl Cl 5 equivalent bonds. 3s 3p 3d 3s 3p 3d 3d sp3d

   Overlap of pCl-sp3dP Overlap of sp3Cl-sp3dP

How is the bond formed in SF6 molecule? F F F S F 6 equivalent bonds. 3s 3p 3d 3s 3p 3d 3d sp3d2

   Overlap of pF-sp3d2S Overlap of sp3F-sp3d2S

disordered tetrahedral Key number No. of mixed orbitals = No. of s bonds + No. of lone EP Key number Hybridi-zation Group Type Molecular Geometry 2 sp AX2 linear 3 sp2 AX3 planar triangular AX2E V-shaped 4 sp3 AX4 tetrahedral AX3E trigonal pyramidal AX2E2 5 sp3d AX5 trigonal bipyramidal AX4E disordered tetrahedral AX3E2 T-shaped AX2E3 6 sp3d2 AX6 octahedral AX5E square pyramidal AX4E2 square planar

Exercise: Explain the bonds in N2, CO2, BF3? H-F What is the hybridization of F in HF? No. of mixed orbitals = No. of s bonds + No. of lone EP = 1 + 3 = 4 HF bond is formed by the overlap of sH with sp3F Better than overlap of 1sH-2pF In sp3 hybridization, the repulsion between the lone EPs around the F atom is less than that in the unhibridized atom (Lone EPs in p-orbitals are only 90º away from each other). Exercise: Explain the bonds in N2, CO2, BF3?