7 7.1 Chapter 7 Covalent Bonding

Size: px

Start display at page:

Download "7 7.1 Chapter 7 Covalent Bonding"

기윤 삼
5 years ago
Views:

1 7 7.1 Chapter 7 Covalent Bonding

2 7 7.2? Lewis : Lewis

3 7 7.3 (valance electron) # of valance e- = # of group (core electron) (Bond) (ionic bond) : metal-nonmetal (covalent bond) : nonmetal-nonmetal (metallic bond) : metal-metal

4 Lewis Lewis,, ( ). (dot ) H + F H F 2H + O H O H H 2 O HF H 8 (octet).. : Octect Rule

5 7 7.5 Lewis Step 1. Step 2. Step 3. Step 4. Step 5.

6 7 7.6 Step 1. Central atom : F Terminal atom : H, O, Halogen

7 Step 2. (valence electrons) = =( ) H # of valance e - = 1,. OCl - ion: = 14 valence e - CH 3 OH molecule: 4 + 4(1) + 6 = 14 valence e - SO 3 2- ion: 6 + 3(6) + 2 = 26 valence e

8 7 7.8 Step 3. 1 (= ) 4 H O Cl H C O H O S O H O

9 7 7.9 Step 4. : OCl - ion: 14-2 = 12 valence e - left CH 3 OH molecule: = 4 valence e - left SO 2-3 ion: 26-6 = 20 valence e - left : Terminal atom (Octect rule), : H ( O Cl ) - H C O H ( O S O ) 2- H O

10 Step 5. Octect Rule Terminal atom C, N, O, P, S

11 ) NO - 3 S1. O N O O S2. # valence e - = = 24 S3. O N O O S4. # of valence e - left: 24-6 = 18

12 S4. Terminal atom O N O N 6. 2 : O N O N 2? 10 valence e - N N O O

13 2) CH

14 3) PF

15 4) CO

16 5) CH 3 CO

17 ) 8 : F Be F F B F F

18 ) (expanded octet) : ) XeF 4 : 36 valence e -. octet structure 32, 4, 12 F F Xe F F

19 (Resonance Forms) (delocalization) : Stabilization NO 3-3 : O = N O O N O O N = O O O 3 ( hybrid). octet rule Lewis. O :

20 (Molecular Geometry) VESPR : Valance Shell Electron Pair Repulsion. P-block 2 6, : BeF linear 2 BeF 3 triangular planar CF 4 tetrahedral PF 5 triangular bipyramid SF 6 octahedral

21 7 7.21

22 AX 2 (linear) 180 BeF 2 AX 3 (Tiangular) 120 BF 3 AX 4 AX 5 (Tetrahedral) CH 4 90,120, PF 5 (Trigonal bipyramid) 180 AX 6 (Octahedral) 90, 180 SF 6

23 (lone pair electron) (lone pair elctron): AX 2 E (GeF 2 ) :bent, 120 AX 3 E (NH 3 ) :triangular pyramid, 109 AX 2 E 2 (H 2 O) :bent, 109

24 ELECTRON PAIRS

25 ELECTRON PAIRS

26 7 7.26

27 : BF 3 and SO 3 : both AX 3, same geometry BeF 2 and CO 2 : both AX 2, both linear F Be F O=C=O H C C H

28 (molecular Shape) 1. Lewis 2. ( + ) 3. VSEPR 4. (lone pair electron)

29 (Polarity)

30 7 7.30, H H E.N. = 0 H C E.N. = 0.3 H F E.N. = 1.8 (- pole at F atom)

31 : HCl,Cl 2 H Cl Cl Cl polar nonpolar : O F Be F CH 4 CH 3 Cl H H nonpolar polar nonpolar polar

32 ; (Hybridization) Bonding Model Valance Bond Theory Molecular Orbital Theory MOT( ) s p. s, p, d ( hybrid orbitals ).

33 CH 4 :sp

34 s + p 2 sp 2s 2p Be in BeF 2 ( ) ( )( )( ) s + 2 p 3 sp 2 2s 2p B in BF 3 ( ) ( )( )( ) s + 3 p 4 sp 3 2s 2p C in CH 4 ( ) ( ) ( ) ( )

35 sp

36 ( ) sp 3 d, sp 3 d 2 2 (e.g.. N, O, F) 2d.

37 (Unshared Pairs) (H 2 O, NH 3 ). O S = O sp 2 hybridization for sulfur O = C = O sp hybridization for carbon

38 ( ) ( ) bond :,.. bond : (extra),, (lobe)..

39 CH 4

40 7 7.40

41 ( ) CO 2 2 sigma bonds; 2 pi bonds SO 2 2 sigma bonds; 1 pi bond N 2 1 sigma bond; 2 pi bonds

Microsoft PowerPoint - Chap7note

Microsoft PowerPoint - Chap7note 강의개요 Chapter 7 Covalent Bonding Lewis 구조 : 옥테트규칙 Lewis구조그리기 공명구조 분자의기하학적구조 극성 결합의극성 분자의극성 원자궤도함수와혼성궤도함수 Copyright 2005 연세대학교이학계열일반화학및실험 (1) 강의노트 7.1 Lewis Structures; The ctet Rule A Lewis structure shows