1. Bonding

2. Types of Bonds Ionic Covalent Metallic

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

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

5. Metallic Bonds No debate about metallic bonds Easy to identify Will not be discussed

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

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

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

9. Covalent Compounds Low MP Two nonmetals Flexible Some exceptions

10. Network Covalent or Macromolecules VHMP Extremely hard

11. Molecule Any compound that can exist as an entity by itself

12. Distinguishing Bonds Distinguishing ionic & covalent bonds can be difficult, but generally determined by difference electronegativity

13. Bonds Types Ionic Polar covalent Non polar covalent

14. Bond Types Ionic:  EN > 2.0 Covalent:  EN < 2.0 Polar Covalent: 0.5<  EN <2.0 Non polar covalent :  EN < 0.5 Nothing is absolute

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

16. Coordinate Covalent Bond H 3 N:BF 3 H 3 N-BF 3 H 3 NBF 3

17. Dipole Polar bonds Polar molecules

18. Dipole H F  +  -

19. Ionic Bonding - +

20. Covalent Bonding Occurs when electron orbitals overlap

21. Orbitals On the board Max 2 e - per orbital

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

23. Hybrid Orbitals spdsp 3 sp 2 d 2 sp 3 sp 3

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

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

26. Bonding Orbitals TypeHybrid VSEPR 2 lobessp AX 2 3 lobessp 2 AX 3 4 lobessp 3 AX 4 5 lobes dsp 3 AX 5 6 lobes d 2 sp 3 AX 6

27. VSEPR Orbitals

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

30. Draw the Bonding Electron Dot Diagrams for Each Element

31. Bonding Electron Dot Diagrams Electron dot diagrams that go through 4 singles before any electrons are paired up

32. 1A: 1 single 2A: 2 singles 3A: 3 singles 4A: 4 singles 5A: 1 pair & 3 singles 6A: 2 pair & 2 singles 7A: 3 pair & 1 single 8A: 4 pair

33. Drill: Equate each of the following: sp 3 AX 2 2 lobes spAX 3 4 lobes dsp 3 AX 4 6 lobes sp 2 AX 5 3 lobes d 2 sp 3 AX 6 5 lobes

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

35. Drawing LDDs Draw the bonding electron dot diagram for each element in the molecule with the element with the most unpaired e - near the center

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

37. Drawing LDDs Connect a single dot on one atom to a single dot on another (never two on the same atom)(never connect one dot to more than one other dot)

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

39. Drawing LDDs Recognize polyatomic ions H 2 CO 3 : CO 3 -2 is a polyatomic ion; thus, the three Os must connect to the C

40. Drawing LDDs Redraw the molecule neatly making sure to include all dots

41. Draw LDDs for: BeCl 2 H 2 O BF 3 C 2 H 6 CH 4 C 3 H 6 NH 3 CH 2 O

42. Drawing LDDs Draw EDDs Connect Cs if multiple Connect single dots Recognize Polyatomic Ions Redraw neatly

43. Draw LDDs for: H 2 C 2 O 4 C 4 H 6

44. Draw the LDD for: C 4 H 9 NO 2 C 4 H 8 N 2 O 2

45. Coordinate Covalent Bond A covalent bond in which both electrons are donated by one atom

46. Draw LDDs for: SO 4 -2 SO 2

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

48. O O N O O O N O

49. Draw LDDs: HNO 3 C 4 H 5 NO

50. Draw LDDs for: PH 3 PO 3 -3 KCN C 4 H 8 O

51. Expanded Octets Sometimes atoms can be surrounded by more than 8 electrons Columns 5A-8A

52. If more atoms are bound to the central atom than its unpaired electrons, then split some paired electrons

53. Example: 5 things bound to P P

54. Hint When drawing expanded LDDs for polyatomic ion, adjust the charge of the central atom

55. Draw LDDs for: PH 5 SCl 5 -1

56. Draw LDDs for: PO 4 -3 P 2 O 7 -4 K 2 SO 4 C 5 H 8 O

57. Draw LDDs for: BeH 2 AlCl 3 SO 2 CF 4 NH 3 H 2 O

58. Hybridizations sp2 lobes sp 2 3 lobes sp 3 4 lobes

59. Bond Angles sp~180 o sp 2 ~120 o sp 3 ~109.5 o

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

62. Pi Bonds (  ) Side by side orbital overlap Multiple bonds contain  bonds

64. Multiple Bonds Double: 1  & 1  Triple: 1  & 2 

67. Intermolecular Forces Weak temporary attractions between atoms from one molecule to another or another part of a larger molecule

68. Intermolecular Forces Sometimes called: Van der Waals Forces

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

71. Hydrogen Bond Strongest of the intermolecular forces Occurs when H is bound to one highly EN element & connects to another

73. Dipole-Dipole When two polar molecules connect

74. 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

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

77. Draw Lewis Dot Diagram for: ICl 5 Determine: bond  s, hybridization, VSEPR, & shape

78. Identify as ionic, covalent, or metallic bonds Na-Cl Fe-Cr S-ClH-Cl Mg-SC-C N-OFe-Fe

79. Draw LDDs for: HONOH 3 PO 4 CO 2 C 3 H 4 O 2

80. Draw LDDs & Predict All for: CF 4 NH 3 BF 3 CO 2 SeCl 4 XeF 4

81. Draw LLDs & Predict All For: H 3 PO 4 ICl 5 IF 3 CO SeCl 4 C 4 H 6 O 2

82. Draw LDDs & predict VSEPR, Hybridization, bond  s, & shape of: XeF 4 SCl 4 XeO 4

83. List & describe the four types of intermolecular forces

84. Draw Lewis Dot Diagrams of: C 4 H 5 NO 2