1. LECTURE 6.2

2. BONDING AND THE PERIODIC TABLE
Ionic Bonding
Covalent Bonding
Metallic Bonding
Van der Waals Bonding
Hydrogen Bonding

3. THE THREE PRIMARY OR STRONG BONDS
Metal to Non-Metal: Ionic (Chapter 15)
Non-Metal to Non-Metal: Covalent (Chapter 16)
Metal to Metal: Metallic (Chapter 17)

4. THE SECONDARY OR WEAK BONDS
Hydrogen: Between “Electropositive” and “Electronegative” Elements. Permanent Dipoles (Chapter 19)
WATER!
van der Waals: Fluctuating Dipoles (Chapter 18)
NOBLE GASES

5. THE IONIC BOND
The establishment of the "Noble gas configuration" by electron transfer from metallic atoms to non-metallic atoms. The electrostatic bond is thus formed between positively charged metallic ions (cations), and negatively charged ions (anions).
Ionic bonds are non-directional.

6. THE IONIC BOND
Always produces compounds. Examples include NaCl (common salt), Na2O (natron) and magnesium oxide (MgO), where one species is metallic (the cation) and is from groups I-III or the transition metals: the other species is non-metallic (the anion),* and is from Groups V, VI or VII. Most importantly, ionically bonded solids are non-metallic and inorganic – they are ceramics.
* A Negative ION.

7. THE IONIC BOND
Ionic Bond: arises from the electrostatic attraction between cations and anions. Because the cations are everywhere positive, and the anions are everywhere negative, the bond is non-directional.

8. THE COVALENT BOND
The attainment of the "magical octet" of outer shell electrons by atoms sharing pairs of valence electrons.
Each shared electron pair constitutes a single bond.
Covalent bonds are directional.

9. THE COVALENT BOND
Occurs in non-metallic (Groups IV, V, VI and VII) elements to form e.g., network solids (diamond carbon and silicon) and molecular gases (hydrogen, oxygen).
Covalent bonding also occurs in compounds, as in the network solids SiC (both Group IV elements), and SiO2 (Groups IV and VI respectively) and molecular gases (e.g., carbon dioxide).

10. COVALENT BOND
Covalent Bond: arises from the electrostatic attraction between cations/cation cores and shared electron pairs. The electrons are said to be localized, because they are confined, primarily between adjacent cations
Hence, the covalent bond is directional.

11. THE METALLIC BOND
The bonds formed between an array of positively charged metallic cations and a "sea" of negatively charged, free-electrons, the latter being "donated" from the outer shells of the constituent atoms.
Metallic bonds are non-directional.
Occurs for all metallic elements and their alloys (i.e., Group I, I and III metals and for the transition metals), to form close-packed solids

12. METALLIC BOND
Metallic Bond: arises from the electrostatic attraction between cation cores and an electron cloud. The electrons are said to be delocalized, because they are not confined, to any cation core, but are “free” to move between the cation cores.
Hence, the metallic bond is non-directional.

13. RUTHERFORD-BOHR MODELS

14. IONIC BONDING IN MAGNESIUM OXIDE

15. THE CRYSTAL STRUCTURE OF MATGNESIUM OXIDE

16. AN IONIC COMPOUND; AB2

17. HYDROGEN: THE SIMPLEST MOLECULE

18. THE METHANE MOLECULE, PARAFFINS AND MOLECULAR WEIGHT

19. ELECTRON-DOT REPRESENTATIONS OF COVALENTLY-BONDED ELEMENTS

20. STRUCTURE OF COVALENTLY BONDED ELEMENTS

21. THE MONOMER AND TETRAMER OF DIAMOND-CARBON

22. THE MONOMER AND CRYSTAL STRUCTURE OF DIAMOND

23. THE “HARD-SPHERE” AND “BALL AND STICK” MODELS OF DIAMOND-CARBON

24. COVALENTLY BONDED NETWORK SOLID