1. Bonding and Properties

2. All Compounds Covalent Ionic Metallic Polar Nonpolar
Molecular Polymeric Network
Polar Nonpolar

3. WS – Bond and Property Chart

4. Types of Compounds
IONIC
COVALENT
METALLIC

5. IONIC + -

6. + + + + + + + +
METALLIC + + + + + + + +

7. CO-VALENT + +

8. IONIC COMPOUNDS

9. NaCl

10. NaCl

11. CaCO3

12. Ionic Bonds / Compounds
Oppositely charged atoms / IONS are created that attract magnetically
Cation (+) attracts Anion (-)
Ionic Compounds are called Salts or Ceramics

13. Ionic Compounds Are Crystals

17. KEY CONCEPT: Ionic Compounds are Crystals made of Alternating Positive and Negative Particles

18. Ionic Compounds Are Brittle Because………..

19. + - + - - + + - + - - - + - +

20. - + - + + + - - - - + + - + + - - + + -

21. - + - + + + - - - - + + - + + - - + + -

22. Ionic Compounds Have High Melting Points because…….

23. Ionic Compounds Have Solubility in Water (Polar), but not in Oil (Nonpolar) because………

24. Ionic Compounds Conduct as Liquids and When Dissolved Because…….

25. e-
Light e-
Na+
Na+ e-
Na0 e- e-

26. The Electric Pickle

27. Examples of Ionic Compounds (Salts)
NaCl – Flavoring and Preservative
Na3PO4 – Common Preservative
CuSO4 – Fungicide
Na2CO3 – Leavening Agent
AgNO3 – Black & White Photography

28. + + + + + + + +
METALLIC + + + + + + + +

29. Metallic Bonds and Compounds
A free flowing, shared pool of electrons attracted to a group of positive ions (Note: the atoms are NOT actually ionic)
Loose sharing of electrons between among many metal nuclei.

31. Metals like ionic compounds usually have highly ordered atomic structure (crystalline)

32. Key concept of metallic compounds: Loose pool of electrons which can move between metal atoms which are in a crystalline arrangement.

33. Malleability of Metals
Community pool of electrons
helps cohesiveness (changing shape e.g. malleability & ductility)
Bonds are electrons being shared between atoms, if no sharing then the atoms would fall apart most easily

34. Bending Metals + + + + + + + + + + + + + + + + + + + + + + + + + + + +

35. Bending Metals + + + + + + + + + + + + + + + + + + + + + + + + + + + +

36. Bending Metals + + + + + + + + + + + + + + + + + + + + + + + + + + + +

37. Community Pool of Electrons leads to conductivity of heat and electricity

40. Metals typically have a high melting point because the community pool of electrons lessens the ability of metals to move freely from each other.

41. Metal compounds are typically called Alloys

42. Alloys Stainless Steel – Fe, Cr, Ni, Cu, etc.
Niobium-titanium Superconducting Alloy
Brass – CuZn and Bronze – CuSn
Lightweight Planes - AlTi Alloys
Mangalloy – Strong and Tough

43. Lab - Thermal Conditioning of Metals

44. Annealing is a heat treating process which makes material softer and less brittle by producing uniform material properties and a higher crystalline structure.
A material can be annealed by heating it to a specific temperature and then letting the material slowly cool to room temperature.

45. Tempering is a heat treatment for making material harder
Tempering is a heat treatment for making material harder. The metal is heated to a specific temperature and rapidly cooled (quenched) in a bath of water, brine, oil, or air to increase its hardness.
Tempering freezes atoms into a more random arrangement which makes the material stronger, but more brittle.

46. Partial Annealing after Tempering will provide greater strength, but not as much brittleness

47. 7

53. Making Metals Strong Carbon Content and Tempering
Carbon makes steel hard. It fills open spaces making the metal have a tighter pack, but bonds are weaker between Fe and C then between Fe and Fe.

55. Mangalloy

57. Hardness Measures

58. CO-VALENT

59. COVALENT Atoms share pairs of electrons
Atoms are bonded because ELECTRONS are STRONGLY PULLED by TWO ATOMS
Atoms share pairs of electrons
Each pair of shared electrons creates one bond.

60. H2

62. Covalent Compounds
Because Nonmetals have High Electronegativities a universal property of Covalent Compounds is Low Conductivity of Electricity.
Otherwise, covalent compounds have a wide variety of properties including textures, hardness, malleabilities, melt points

63. Why are covalent compounds so diverse?

64. All Compounds Covalent Ionic Metallic Molecular Polymeric Network
Polar Nonpolar

65. Key concept of Molecular Covalent: Small groups with covalently bonded atoms are called MOLECULES

66. Small Covalent Compounds = Molecules
Polar Examples
Water: H2O
Sugar: C6H12O6
Nonpolar Examples
Air: N2, O2, CO2
Wax: C25H52
H - H

67. B/C Molecules are Small ……
Molecules can be all three states of matter, but they are the only type of compound that can be a gas at room temperature.

68. B/C Molecules are Small ……
the lowest melt points compound
will dissolve in substances of similar polarity

69. Key concept of Polymeric Covalent: Polymers are LARGE and LONG chains of Covalently Bonded Atoms with a REPEATING PATTERN

70. POLYethylene

71. Examples are DNA, Plastics, Protein, Wood/Paper, Rubber, Cotton

72. B/C Polymers are Larger they…
Are usually solids, but flexible
have medium melt points
Are harder to dissolve

73. Key concept of Polymeric Covalent: Networks are very large covalent compounds with widespread CONTINUOUS bonding

74. Covalent Network
The amount of bonds makes networks very stable

75. B/C Networks have SO much bonding they...
Are solids (crystalline solids)
have very high melt points
do not dissolve in water

76. Examples of Networks Diamonds: C Graphite: C Sand: SiO2
Silicon for Computer Chips: Si
NOTICE: The formula is a ratio of the elements. The formula does NOT represent the number of atoms in a network. Even my small, 9.6 g piece of silicon has 21,000,000,000,000,000,000,000 atoms.

78. Basic Unit of Compounds vs. Melting Point Temperature

79. Differences in Melting Point Temperatures+ -
H2O
H2O
H2O
H2O
H2O
H2O
H2O
H2O
Ionic (e.g. NaCl)
Molecular Covalent C
Network Covalent (diamond)

80. Metallic Compounds + + + + + + + + + + + +

81. Dissolving

82. Dissolving Ionic Compounds

85. Dissolving Sugar Molecules (C6H12O6)

86. Network Covalent (diamond)
Dissolving + -
H2O
H2O
H2O
H2O
H2O
H2O
H2O
H2O
Ionic (e.g. NaCl)
Molecular Covalent C
Network Covalent (diamond)

87. END

89. Potential Energy as a function of nuclear proximity

90. Crystal Lattice
A Lattice is an array of points repeating periodically in three dimensions.
Shapes will depend on Chemical Formula

91. Lattice Energy
Force of attraction will influence how much energy it takes to break the ions apart
Melting Point
Solubility
Strength of Solid

92. Acids and Bases
Acids and bases are small discrete units like molecules
Acids and bases break down in water to form ions
We will discuss acids and bases as a separate unit toward the end of the year

93. Sharing of electrons (electronegativity) is a gradient
Nonpolar
Ionic

94. Electronegativity 0-0.3 nonpolar covalent 0.3 to 1.7 polar covalent
Above 1.7 is ionic
A bond between two metals is a metallic bond

95. How do we typify compounds? Bonding Lab 1
As chemists we want to relate
the observable data to the
microscopic structure so we can
categorize, predict, engineer
Does NaCl behave they way it does partly because it is made of ions and IONICALLY BONDED?
Does Water H2O behave like it does because of has POLAR COVALENT Bonds? As chemists we want to relate
Does Water H2O behave like it does because of has POLAR COVALENT Bonds?

96. Oxidation Numbers represent when bonded and doesn’t represent anything real vs. Charge is real
Oxidation number is when as a compound and charge is when it is as an ion

97. + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + +