1. Catalyst Draw the orbital diagram for Boron.
Give the 4 quantum numbers of the highest energy electron in Boron.

2. ChemicalBonding

3. Types of Bonds
Ionic
Covalent
Metallic

4. Metallic Bonds Electrons are shared by many atoms
Electrons free to move
Two or more metals

6. Metallic Compounds Generally high MP Hard & lustrous Less brittle
Conductors

7. Ionic Bonds
Electrons are transferred from one atom to another creating (+) & (-) ions
Metal & nonmetal

9. Ionic Compounds
Held together by electrostatic charge
Very high MP
Brittle

10. Covalent Bonds Electrons are shared by two atoms Two nonmetals
Weaker than ionic

12. Covalent Compounds
Low MP
Two nonmetals
Flexible
Some exceptions

13. Network Covalent or Macromolecules
VHMP
Extremely hard

14. Distinguishing Bonds
Use the difference in electronegativity

16. Bonds Types Ionic-transfer electrons
Polar covalent-electrons are not shared evenly, unequal distribution of charge
Non polar covalent-electrons shared equally

17. Bond Types Ionic: DEN > 2.0 Covalent: DEN < 1.7
Polar Covalent: 0.5<DEN<1.7
Non polar covalent :DEN< 0.5
Nothing is absolute

18. What about 1.6-2.0? 1.6<ΔEN<2.0:
if a metal is involved, then the bond is considered ionic.
only nonmetals are involved, the bond is considered polar covalent.

19. Classify Each type of Bond: 1. Na-Cl. 4. Al-Cl 2. C-F. 5. H-I 3. Fe-Cr
Classify Each type of Bond: 1. Na-Cl 4. Al-Cl 2. C-F 5. H-I 3. Fe-Cr 6. P-O

21. Lewis Dot Diagrams
Representation of valence electrons and bonds in a molecule or polyatomic ion

22. F K In an IONIC bond, electrons are lost or gained,
resulting in the formation of IONS
in ionic compounds. F K

23. How to draw the LDDs for COVALENT Compounds
“Count” the total valence electrons.
Determine the central atom, usually the 1st element in the formula (Note: H can never be a central atom)
Bond the central atom with the “others” using a single bond, shown as a line.
Subtract the electrons bonded (2 per bond)
Distribute the remaining electrons as lone pairs or form multiple bonds when needed to follow the octet rule (except H)

24. Single, Double, Triple Bond
Single Bond = 2 electrons shared
Double Bond = 4 electrons shared
Triple Bond = 6 electrons shared

25. Bond Strength Single Bond-longest, least energy
Double Bond-shorter, more energy
Triple bond-shortest, most energy

26. Guided Practice
Draw LDD for NaCl & CH2O

27. CW: Draw LDDs for: *next to each include the type of bond BeCl2 5. H2O
BF C2H6
CH C3H6
NH CF2O

28. Drill: 1) Illustrate the bond that will be formed when Sr and P bond
Drill: 1) Illustrate the bond that will be formed when Sr and P bond. What is the formula of the compound? What are the charges? 2) Draw the structure of H2O. Agenda: Continue illustrating Lewis Dot Diagrams of Molecules

29. Expanded Octets
Central atom is surrounded by more than 4 pairs of shared electrons
Sometimes easy to see, sometimes have to do the LDD to figure it out
If after drawing the skeleton structure, the number of electrons available is greater than the number required to give each atom an octet, distribute the extra electrons around the central atom as unshaired pairs.

30. LDDs
SF6
ClF3

31. Recognize polyatomic ions
Same rules apply, but you will add or subtract the charge to the total.
CO3-2 is a polyatomic ion; thus, the three Os must connect to the C

32. SO4-2 PO3-3 Polyatomic Ions
Same rules apply, just enclose it in the bracket then put the charge. However, the total valence should include the charges. If negative, add. If positive, subtract.
SO4-2 PO3-3

33. Draw LDDs for:
CO3-2

34. Drill: Draw LDDs for:
PCl3 SiO2

35. Resonance Structures
Equally valid Lewis Dot Diagrams for molecules or polyatomic ions that have the same shape.

36. O
O N O O
O N O -1 -1

37. Those that don’t follow
Sometimes atoms may not follow the octet rule
Columns 1A-3A

38. Expanded Octets
Sometimes atoms can be surrounded by more than 8 electrons (central atom)
Columns 5A-8A

39. Draw LDDs for:
PH5
SCl5-1

40. Drill: Draw LDDs:
SF4-2
XeF4

41. Drill: Draw the LDDs of the following: 1) SiBr4 2) ICl2- 3) TeF4 Agenda: 1) Practice predicting bonds using electronegativity differences 2) Determine the shapes of molecules

42. Electron Cloud Repulsion
In molecules each electron cloud repels other clouds enough to spread as far apart as possible

43. VSEPR Valence Shell Electron Pair Repulsion
Electron pairs repel each other to spread out as much as possible

44. Bonding Orbitals Type Hybrid VSEPR
2 lobes sp AX2
3 lobes sp2 AX3
4 lobes sp3 AX4
5 lobes sp3d AX5
6 lobes sp3d2 AX6

45. Molecular Geometry

47. Drill: Draw LDDs:
ICl3
IF4+1

48. Drill: Draw LDDS and predict the shape of the following:
CF4
SeBr6
SiOF2
NI3
5) IBr2-

49. Drill: Draw LDDS and predict the shape of the following: (P7)
CS2
PBr5
SeCl4
AsI3
5) IF2-

50. Drill: Draw the LDDs and predict the shape of the following molecules: 1) BeCl2 (Take note Be belongs to 2A) 2) XeCl2 3) SeI6 *For Period 1, pass your papers from yesterday forward Agenda: 1) Explain hybridization and identify hybrid orbitals 2) Draw structures with more than 1 central atom

51. Occurs when electron orbitals overlap
Covalent Bonding
Occurs when electron orbitals overlap

52. Orbitals
Max 2 e- per orbital

53. Hybridization
When s, p, and/or d orbitals (electron clouds) mix to make a new type of multi-lobed orbital

54. Hybrid Orbitals
sp sp3d
sp2 sp3d2
sp3

55. Hybridizations sp 2 lobes sp2 3 lobes sp3 4 lobes sp3d 5 lobes

56. Bonding Orbital Shape 2 lobes: Linear 180o
3 lobes: Trigonal planar 120o
4 lobes: Tetrahedral 109.5o
5 lobes: Hexahedral 120&180o
6 lobes: Octahedral 90&180o

57. Drawing LDDs for Carbon Chains
If there is more than one carbon, connect the carbons by connecting single dots between one carbon & another

58. Drawing LDDs
Repeat connecting the dots until all singled dots are connected making sure to obey the octet rule if possible

59. Drawing LDDs for Carbon Chains
If there is more than one carbon, connect the carbons by connecting single dots between one carbon & another

60. Draw LDDs for:
C4H8
C4H6

61. Draw LDDs for:
C3H6
C2H6

62. Drill: 1) Draw the LDD and identify the hybrid orbital of the following: 1) CCl4 2) PO33- 2) Bring out a sheet of paper Agenda: Answer a review classwork on chemical bonding

63. DRILL (For today’s Classwork)
Bring out 1 sheet of paper
Fold it lengthwise then crosswise twice to produce 8 folds
Number your boxes vertically. Don’t forget to write your name! 1) 5) 2) 6) 3) 7) 4) 8)

64. Front: LDD, Gen Formula, Shape, Hybrid Orbital
Left Side
SeO2
BrAt5
CTe2
OF2
Right Side
5) CH2Cl2
6) NO3-
7) SiF4
8) FBr3

65. Back: Others Left Side Differentiate Metallic, Ionic, Covalent Bond
Identify the type using the Electronegativity values (sm P.Table)
a) Ba and Se
b) Ge and F
c) O and Cl
d) S and N

66. Drill: 1) Draw the LDD and identify the shape of the following: 1) CH2O 2) SiAt4 3) BCl3 Agenda: Continue the review classwork on chemical bonding

67. Coverage of the Quiz tomorrow: 1) Types of Bonds – read the notes, even terms like lone pairs, VSEPR, molecular geometry, hybridization, etc. you should know 2) Forming Ionic Compounds along with the Ions and Formula 3) Predicting the Types of Bond using the Electronegativity 4) Showing Covalent Bonding through LDDs 5) Determining the Shape, Gen. Formula, Hybrid Orbital 6) Structures of Carbon Chains

68. Back: Others
Left Side
Next 4 - Ionic Bond – Show the transfer of electrons, ions and formula of the following pairs:
3) Ga and S
4) Pb and I
Right Side
5) Na and O
6) Sr and N

69. Back: Others Right Side For 7 and 8, draw the LDDs of: 7) C6H12

70. Drill: Week 5 of Quarter 2 Dec 7, 2015 Draw LDDs of:
C4H8 SiOF2
Agenda:
Differentiate polar from nonpolar.
Identify the intermolecular forces of attraction between substances

71. Polar vs. Nonpolar
Polar Covalent – unequal sharing of electrons (partial + & - charges called dipole) – when different elements are bonded to the central atom and/or when it has lone pairs
Non polar Covalent – equal distribution of electrons – when same elements are bonded & no lone pairs

72. Exceptions
Square Planar – non polar

73. CW: Draw LDDs. Give the shape, hybrid orbital and polarity:
SeO4 -2 SCl4
CH2O XeF3+1

74. Sigma Bonds(s) End to end orbital overlap
All single bonds are sigma bonds
All multiple bonds contain one sigma bond

76. Pi Bonds (p) Side by side orbital overlap
Multiple bonds contain p bonds

78. Multiple Bonds
Double: 1 s & 1 p
Triple: 1 s & 2 p

81. Coordinate Covalent Bonds
A covalent bond in which the two electrons are donated by one atom

82. Coordinate Covalent Bond
H3N: BF3
H3N-BF3
H3N BF3

83. Intermolecular Forces of Attraction (IMFA)
Weak temporary attractions between atoms from one molecule to another or another part of a larger molecule

84. Drill: Draw LDDs and predict polarity of:
1)IF4+ 2)SeCl2 3)OI2
Agenda:
Identify the intermolecular forces of attraction between substances

86. Intermolecular Forces
Hydrogen-bond
Dipole-dipole
Dipole-induced dipole
London dispersion forces

87. Hydrogen Bond Strongest of the intermolecular forces
Occurs when H is bound to one highly EN element (N,O, F) & connects to another

89. Dipole
Between Polar bonds or Polar molecules

90. Dipole
H F
d+ d-

91. Dipole-Dipole
When two polar molecules connect

92. Dipole-Induced Dipole
When a polar molecule gets near a non-polar one, it induces the non-polar one to become polar; thus, they connect

93. London Dispersion
Instantaneous attraction for fractions of seconds in which non-polar molecules connect
Very weak force

94. Draw LDDs for: BeH2 (no octet) PO43- BCl3 (no octet) SO2
- Is it POLAR or NONPOLAR?
-IMFA a)1&2,b)3&4,c)1&3,d)2&3?

96. Draw LDDs & Predict Polarity:
CF4 2) CO2
3) SeCl4 4) XeF4
- Is it POLAR or NONPOLAR?
-IMFA a)1&2,b)3&4,c)1&3,d)2&3?