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Molecular Models Lab. # of bonds Shape Resonance? O 2 2 (1 ,1  )linearNo H 2 O2 (2  ) bentNo NH 3 3 (3  ) trigonal pyramidNo CH 4 4 (4  ) tetrahedralNo.

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Presentation on theme: "Molecular Models Lab. # of bonds Shape Resonance? O 2 2 (1 ,1  )linearNo H 2 O2 (2  ) bentNo NH 3 3 (3  ) trigonal pyramidNo CH 4 4 (4  ) tetrahedralNo."— Presentation transcript:

1 Molecular Models Lab

2 # of bonds Shape Resonance? O 2 2 (1 ,1  )linearNo H 2 O2 (2  ) bentNo NH 3 3 (3  ) trigonal pyramidNo CH 4 4 (4  ) tetrahedralNo

3 N 2 3 (1 ,2  ) bentNo HCN4 (2 ,2  ) linearNo CO 2 4 (2 ,2  ) linear Yes N 2 O 4 (2 ,2  ) linear Yes # of bonds Shape Resonance?

4 SO (4  ) tetrahedral No NO (2 ,1  ) bent Yes NO (3 ,1  ) trigonal planarYes H 2 CO4 (3 ,1  ) trigonal planar No # of bonds Shape Resonance?

5 HCO (3 ,1  ) trigonal planarYes  C 2 H 6 7 (7  )  No  C 2 H 4 6 (5 ,1  )  (planar!)No  C 2 H 6 O 8 (8  )  No # of bonds Shape Resonance?

6  N 2 H 4 5 (5  )  No  CH 4 O5 (5  )  No SO 3 4 (3 ,1  ) trigonal planar Yes SO 2 3 (2 ,1  ) bent Yes # of bonds Shape Resonance?

7 SO (3  ) trigonal pyramid No SCN -1 4 (2 ,2  ) linear Yes Br 2 1 (1  ) linear No O 3 3 (2 ,1  ) bent Yes # of bonds Shape Resonance?

8  N 2 O 4 7 (5 ,2  )  Yes  C 2 O (5 ,2  )  Yes HF1 (1  ) linear No ICl 1 (1  ) linear No # of bonds Shape Resonance?

9 NH (4  ) tetrahedral No H 3 O + 3 (3  ) trigonal pyramid No BCl 3 3 (3  ) trigonal planar! No PCl 5 5 (5  ) trigonal bipyramid No # of bonds Shape Resonance?

10 # of bonds Shape Lone Pairs O 2 2linear2 H 2 O2bent2 NH 3 3 trigonal pyramid1 CH 4 4 tetrahedral0 (On central atom)

11 N 2 3bent1 HCN4linear0 CO 2 4linear 0 N 2 O 4linear 0 # of bonds Shape Lone Pairs (On central atom)

12 SO tetrahedral 0 NO bent 1 NO trigonal planar0 H 2 CO 4 trigonal planar 0 # of bonds Shape Lone Pairs (On central atom)

13 HCO trigonal planar0  C 2 H 6 7    C 2 H 4 6  (planar!)   C 2 H 6 O 8   # of bonds Shape Lone Pairs (On central atom)

14  N 2 H 4 5    CH 4 O5   SO 3 4 trigonal planar 0 SO 2 3 bent 1 # of bonds Shape Lone Pairs (On central atom)

15 SO trigonal pyramid 1 SCN -1 4 linear 0 Br 2 1 linear 3 O 3 3 bent 1 # of bonds Shape Lone Pairs (On central atom)

16  N 2 O 4 7    C 2 O   HF1 linear 3 ICl 1 linear 3 # of bonds Shape Lone Pairs (On central atom)

17 NH tetrahedral 0 H 3 O + 3 trigonal pyramid 1 BCl 3 3 trigonal planar! 0! PCl 5 5 trigonal bipyramid 0 # of bonds Shape Lone Pairs (On central atom)

18 Symmetry? Polar bonds? Polar? O 2 YesNoNo H 2 ONoYesYes NH 3 NoYesYes CH 4 YesNoNo

19 N 2 Yes No No HCNNoYesYes CO 2 Yes Yes No N 2 O No Yes Yes Symmetry? Polar bonds? Polar?

20 SO 4 -2 Yes Yes * NO 2 -1 No Yes * NO 3 -1 Yes Yes * H 2 CONo Yes Yes Symmetry? Polar bonds? Polar?

21 HCO 2 -1 No Yes *  C 2 H 6 Yes No No  C 2 H 4 Yes No No  C 2 H 6 O No Yes Yes Symmetry? Polar bonds? Polar?

22  N 2 H 4 No? Yes Yes  CH 4 ONo Yes Yes SO 3 Yes Yes No SO 2 No Yes Yes Symmetry? Polar bonds? Polar?

23 SO 3 -2 No Yes * SCN -1 No Yes * Br 2 Yes No No O 3 No No No Symmetry? Polar bonds? Polar?

24  N 2 O 4 YesYes No  C 2 O 4 -2 Yes Yes * HFNo Yes Yes ICl No Yes Yes Symmetry? Polar bonds? Polar?

25 NH 4 + Yes Yes * H 3 O + No Yes * BCl 3 Yes Yes No PCl 5 Yes? Yes No Symmetry? Polar bonds? Polar?

26 Hybridization Multiples? Angle O 2 sp 2 1 double H 2 Osp 3 No NH 3 sp 3 No CH 4 sp 3 No

27 N 2 sp1 triple-- HCNsp1 triple180 CO 2 sp2 doubles180 N 2 O sp2 doubles180 Hybridization Multiples? Angle

28 SO 4 -2 sp 3 No109.5 NO 2 -1 sp 2 1 double<120 NO 3 -1 sp 2 1 double120 H 2 COsp 2 1 double120 Hybridization Multiples? Angle

29 HCO 2 -1 sp 2 1 double120  C 2 H 6 sp 3 No109.5  C 2 H 4 sp 2 1 double120  C 2 H 6 O sp 3 No109.5&<109.5 Hybridization Multiples? Angle

30  N 2 H 4 sp 3 No<109.5  CH 4 Osp 3 No109.5&<109.5 SO 3 sp 2 1 double120 SO 2 sp 2 1 double<120 Hybridization Multiples? Angle

31 SO 3 -2 sp 3 No<109.5 SCN -1 sp2 doubles180 Br 2 sp 3 No-- O 3 sp 2 1 double<120 Hybridization Multiples? Angle

32  N 2 O 4 sp 2 2 doubles120  C 2 O 4 -2 sp 2 2 doubles120 HFsp 3 No-- ICl sp 3 No-- Hybridization Multiples? Angle

33 NH 4 + sp 3 No109.5 H 3 O + sp 3 No<109.5 BCl 3 sp 2 !No!120 PCl 5 dsp 3 !No!90 & 120 Hybridization Multiples? Angle

34 O 2 H 2 O NH 3 CH 4

35 N 2 HCN CO 2 N 2 O (N is in the center!)

36 SO 4 -2 (Notice the charge?) NO 2 -1 NO 3 -1 H 2 CO

37 HCO 2 -1  C 2 H 6  C 2 H 4  C 2 H 6 O

38  N 2 H 4  CH 4 O SO 3 SO 2

39 SO 3 -2 SCN -1 Br 2 O 3

40  N 2 O 4  C 2 O 4 -2 ( C-C in the center!) HF ICl (that’s iodine monochloride)

41 NH 4 + H 3 O + BCl 3 PCl 5

42 O 2 H 2 O NH 3 CH 4

43 N 2 HCN CO 2 N 2 O (N is in the center!)

44 SO 4 -2 (Notice the charge?) NO 2 -1 NO 3 -1 H 2 CO

45 HCO 2 -1  C 2 H 6  C 2 H 4  C 2 H 6 O

46  N 2 H 4  CH 4 O SO 3 SO 2

47 SO 3 -2 SCN -1 Br 2 O 3

48  N 2 O 4  C 2 O 4 -2 ( C-C in the center!) HF ICl (that’s iodine monochloride)

49 NH 4 + H 3 O + BCl 3 PCl 5


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