2. Atoms Molecules What are the building blocks? Subatomic particles
Protons
Electrons
s orbital
p orbital
d orbital
Hybrids
Carbon
Hydrogen
Oxygen
Nitrogen
Phosphorus
Chlorine
Atoms
Methane
Formaldehyde
Hydrogen cyanide
Phosphorus pentachloride
Molecules

3. Electron: Both wave and particle

4. Electron: Both wave and particle

5. It’s all about building blocks
CHEMISTRY
It’s all about building blocks

8. Number of available connections (bonds)
Carbon Nitrogen Oxygen Hydrogen
Number of available connections (bonds)

9. H
Methane C H H H

10. Methanol H C O H H H

11. FORCE & ENERGY N S S N The forces at work are: Electromagnetic:
Repulsion of like charges: proton-proton and electron-electron Attraction of unlike charges: proton-electron.
Magnetic:
Electron spin introduces magnetic forces. Electrons with opposite spins produce opposite magnetic poles. Opposite magnetic poles attract. Opposite spin is required for electrons to occupy the same orbital. N S S N

13. Lewis Structures & Molecular Shape

14. Lewis Structures
Gilbert Lewis

15. Lewis Structures Keeps track of valence (bonding) electrons
Predicts formula for many compounds
Predicts charge of compounds
Predicts stability of compounds
Predicts molecular shape if combined with other theories.
nitrate=NO3-

16. Why interest in Molecular Shape?
Predicts polar compounds (ones with ends with opposite charges)
Predicts solubility
Predicts interaction with light (link)
Predicts crystal structure δ- δ- δ+ δ- δ+ δ- δ- δ-

17. Methane building blocks
Lewis Structure
VSEPR
Valence Shell Electron Pair Repulsion

18. Carbon
1s2 2s2 2p2 s p d f

19. 3 sp Methane: Carbon 1s 2s 2px 2py 2pz sp3 sp3 sp3 sp3 Promote
Hybridize sp 3 x
109.5o z
Methane: Carbon

21. VSEPR http://www.chem.purdue.edu/gchelp/vsepr/

23. Orbitals

24. Lewis Structures

25. PF3
5 + 7x3 = 26 valence electrons 1 2 3 4 5

26. P F P
Magic 8 P F P F
4 groups of electrons, which will repel each other. P F

27. P P F
PF3 F F s p
1s2 2s2 2p6 3s2 3p3 d f

28. P F AB3N 1 central atom=A 3 bonding atoms = B3
4 groups of electrons, which will repel each other. P F
1 central atom=A
3 bonding atoms = B3
1 non-bonding pairs of electrons = N
AB3N -

29. AB3N

30. AB3N

33. Number of electron groups
Hybridization
Number of electron groups
Hybridization 2 sp 3
sp2 4
sp3 5
sp3d 6
sp3d2 P F

34. Polar? δ+ P F δ- F δ- F δ-
P = 2.1
F = 4.0
Electronegativity

36. SCl2
6 + 7x3 = 27 valence electrons 1 2 3 4 5

37. Magic 8 S Cl S Cl S Cl S Cl -
4 groups of electrons, which will repel each other.

38. P P F
PF3 F F s p
1s2 2s2 2p6 3s2 3p3 d f

39. S Cl AB2N2 1 central atom=A 2 bonding atoms = B2
4 groups of electrons, which will repel each other. S Cl
1 central atom=A
2 bonding atoms = B2
2 non-bonding pairs of electrons = N2
AB2N2 -

40. AB2N2

41. Number of electron groups
Hybridization
Number of electron groups
Hybridization 2 sp 3
sp2 4
sp3 5
sp3d 6
sp3d2 Cl S Cl S Cl

42. Polar ? δ+ S Cl δ- δ-
S = 2.5
Cl = 3.0
Electronegativity

43. CS2
4 + 6x2 = 16 valence electrons 1 2 3 4 5

44. Magic 8 C S C S C S C S -
2 groups of electrons, which will repel each other.

45. C S AB2 VESPR Sketch 1 central atom=A 2 bonding atoms = B2
2 groups of electrons, which will repel each other. C S
1 central atom=A
2 bonding atoms = B2
Zero non-bonding pairs of electrons
AB2 -

46. AB2

47. Hybridization C S 2 sp 3 sp2 4 sp3 5 sp3d 6 sp3d2 # of electron groups
Electron geometry 2 sp 3
sp2 4
sp3 5
sp3d 6
sp3d2
for carbon
Straight
Trigonal
Tetrahedral
Trigonal bipyramidal
Octahedral C S
for sulfur

48. H C N sp Linear C S 2s + 2px 1s 2s 2px 2py 2pz sp sp Promoted
Hybridized H C N sp
Linear C S
2s + 2px
Carbon in hydrogen cyanide or carbon disulfide:

49. Polar ? C S
S = 2.5
C = 2.5
Electronegativity

50. KrF2
8 + 7x2 = 22 valence electrons 1 2 3 4 5

51. OK for period 3 elements or higher
Violated Magic 8 F Kr
OK for period 3 elements or higher Kr F Kr F Kr F
5 groups of electrons, which will repel each other. -

52. Kr F AB2N3 VESPR Sketch 1 central atom=A 2 bonding atoms = B2
5 groups of electrons, which will repel each other. Kr F
1 central atom=A
2 bonding atoms = B2
3 non-bonding pairs of electrons
AB2N3 -

53. AB2N3 Kr F

54. Polar ? No δ+ Kr F δ- δ-
Kr = 3.0
F = 4.0
Electronegativity

55. PO33-
5 + 6x3 + 3 = 26 valence electrons 1 2 3 4 5

56. P F
Magic 8 P O 3- P O P O - - 3- P O
4 groups of electrons, which will repel each other.

57. P O AB2N VESPR Sketch 3- 1 central atom=A 3 bonding atoms = B3
2 groups of electrons, which will repel each other. P O 3-
1 central atom=A
3 bonding atoms = B3
1 non-bonding pairs of electrons=N
AB2N -

58. P O 3-

59. Hybridization P O 3- 2 sp 3 sp2 4 sp3 5 sp3d 6 sp3d2
# of electron groups
Hybridization
Electron geometry 2 sp 3
sp2 4
sp3 5
sp3d 6
sp3d2
Straight
Trigonal
Tetrahedral
Trigonal bipyramidal
Octahedral
Trigonal pyramidal P O 3-
for P & O

60. Polar ? δ+ 3- P O O δ- δ- O δ-
O = 3.5
P = 2.1
Electronegativity

61. Now it’s your turn

62. 3 sp d Trigonal Bipyrimidal Phosphorus Pentachloride: Phosphorus 2 3s
sp3d sp3d sp3d sp3d sp3d
Neon 2 3s
3px
3py
3pz
dxz dyz dxy dx2-y2 dz2
Hybridized
90o
Promoted
sp d 3
120o
Trigonal Bipyrimidal
120o
Phosphorus Pentachloride: Phosphorus

63. PF3 s p
1s2 2s2 2p6 3s2 3p3 d f

64. l=0 s l=1 p l=2 d * * * l=3 * f * * Period 1 Period 2 Period 3
Principle number n
l=0 s
l=1
Period 1
Period 2
Period 3
Period 4
Period 5
Period 6
Period 7
n=1 l=0 m=0
n=2 l=0 m=0
n=2 l=1 m=-1
n=2 l=1 m=-0
n=2 l=1 m=+1
n=2 l=1 m=0
n=3 l=0 m=0
n=3 l=1 m=-1
n=3 l=1 m=0
n=3 l=1 m=+1
n=4 l=0 m=0
n=3 l=2 m=-2
n=3 l=2 m=-1
n=3 l=2 m=0
n=3 l=2 m=+1
n=3 l=2 m=+2
n=4 l=1 m=-1
n=4 l=1 m=0
n=4 l=1 m=+1
n=5 l=0 m=0
n=4 l=2 m=-2
n=4 l=2 m=-1
n=4 l=2 m=0
n=4 l=2 m=+1
n=4 l=2 m=+2
n=5 l=1 m=-1
n=5 l=1 m=0
n=5 l=1 m=+1
n=6 l=0 m=0
n=5 l=2 m=-2
n=5 l=2 m=-1
n=5 l=2 m=0
n=5 l=2 m=+1
n=5 l=2 m=+2
n=6 l=1 m=-1
n=6 l=1 m=0
n=6 l=1 m=+1
n=7 l=0 m=0
n=6 l=2 m=-2
n=6 l=2 m=-1
n=6 l=2 m=0
n=6 l=2 m=+1
n=6 l=2 m=+2
n=7 l=1 m=-1
n=7 l=1 m=0
n=7 l=1 m=+1
n=4 l=3 m=-3
n=4 l=3 m=-2
n=4 l=3 m=-1
n=4 l=3 m=0
n=4 l=3 m=+1
n=4 l=3 m=+2
n=4 l=3 m=+3
n=5 l=3 m=-3
n=5 l=3 m=-2
n=5 l=3 m=-1
n=5 l=3 m=0
n=5 l=3 m=+1
n=5 l=3 m=+2
n=5 l=3 m=+3 p
l=2 d * * *
l=3 f * * *

66. Electron Configuration
Period 1
Period 2
Period 3
Period 4
Period 5
Period 6
Period 7 He 3d 4d