lecture23 (11-29-2006) Ch 11

lecture23 (11-29-2006) Ch 11 - Chemistry 2A-c F2006...

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1 Chemistry 2A Chemistry 2A -c F2006 c F2006 (Ch10 (Ch10 -48)265 48)265 Molecular Shapes and Dipole Moments Polar molecules: H—Cl δ + δ - Dipole moment: μ=δ d Debye (unit): 1 D=3.34x10 -30 C.m Example : HCl δ = μ /d =(1.03 D) (3.34x10 -30 C.m/D)/(127.4x10 -12 m) = 2.70x10 -20 C electron charge=1.6x10 -19 C δ /e - =0.17 HCl is 17% ionic capacitor
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2 Chemistry 2A Chemistry 2A -c F2006 c F2006 (Ch10 (Ch10 -49)266 49)266 O=C=O μ =0 O H H μ≠ 0 CO 2 is non-polar: linear H 2 O is polar- bent
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3 Chemistry 2A Chemistry 2A -c F2006 c F2006 (Ch10 (Ch10 -50)267 50)267 Bond length (r e ) and bond energy (D e ) r e D e r V(r)
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4 Chemistry 2A Chemistry 2A -c F2006 c F2006 (Ch10 (Ch10 -51)268 51)268 Bond order and bond length Bond order =1 (single bond) Bond order =2 (double bond) Bond order =3 (triple bond)
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5 Chemistry 2A Chemistry 2A -c F2006 c F2006 (Ch10 (Ch10 -52)269 52)269
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Concept of bond formation A chemical bond with electron density in between the nuclei is called a σ bond 1s 1 1s 1 OVERLAP to form a region of increased electron density between the atoms. The better the overlap, the stronger the bond. Chemistry 2A
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lecture23 (11-29-2006) Ch 11 - Chemistry 2A-c F2006...

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