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Understanding Chemical Bonding: Basic Concepts and Types

Explore the fundamental concepts of chemical bonding, such as metallic, ionic, and covalent bonds, as well as lattice energy and transition metal ions. Learn about Lewis' representation of valence electrons and the forces that hold atoms together.

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Understanding Chemical Bonding: Basic Concepts and Types

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  1. Chapter 8.1-8.3 Basic Concepts of Chemical Bonding

  2. Chemical Bonding • Force of attraction that holds atoms together

  3. Types of Bonds • Metallic bond • e- are free to move around the metal atoms e- • e.g. Fe,Co, Ni, etc. • Metals are shiny • Good conductors of heat & electricity • Malleable

  4. Types of Bonds • Ionic Bond • Bond between (+) and (-) ions. • Ex. NaCl  Na+ … Cl- • Covalent Bond • Due to sharing of e-. H•*H  H – H

  5. Lattice Energy (LE) • Energy required to separate gaseous ions from a mole of a solid ionic compound. NaCl (s)  Na+ (g) + Cl- (g) ∆H latt = 788 kJ/mol

  6. Ionic bond is due to electrostatic attraction. Coulomb's Law: E Q1 Q2 d Q1 - charge on 1st atom Q2 - charge on 2nd atom d - distance between charges Problems: 8.22,25 (P337) Effect of charge & effect of size? LiCl, NaBr, RbBr, MgO

  7. Transition Metal Ions • In forming ions e- is first removed from the outermost s orbital. e.g. Ti  (Ar) 4s2 3d2 Ti +2 (Ar) 3d2

  8. Non Transition ion • e- is removed from the outermost orbital (does not have to be a s orbital). e.g. C  1s2 2s22p2 C+ 1s2 2s22p1

  9. Lewis’ Representation of Valence e- Outermost s and p e- . Li  1s22s1 : Ca  (Ar) 4s2

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