Chemistry

Electron affinity: Cl(g) + e? Cl?(g) ?E = ?349 kJ/mol Ionization energy: Cl(g) Cl+(g ) + e? ?E = 1251 kJ/mol Substance to be an acid Disolve in water to form acidic solution or React with a base Metals Form cations in aq M M2+ + 2e? Low I1 Metals + non-metals salt (ionic compound) Metal oxides basic: Metal oxides + H20 metal hydroxide (OH-) (not all) Metal + O2 metal O2- (Ionic Solid) Acid + metal salt (aq) + H2 (g) Acid + metal OH- salt (aq/s) + H2O (l) Acid + metal O2- salt (aq/s) + H2O (l) Acid + metal HCO2-3 salt (aq/s) + CO2 (g) + H2O (l) Acid + metal HCO-2 salt (aq/s) + CO2 (g) + H2O (l) Acid + metal S2- salt (aq/s) + SO2 (g) + H2O (l) Acids + Metals Soluble Water Acid Product NiO (clear) No HNO3 (clear) Ni(NO3)2 (Green)

Lewis Symbols As a pictorial understanding of where the electrons are in an atom, we represent the electrons as dots around the symbol for the element. The number of electrons available for bonding are indicated by unpaired dots. These symbols are called Lewis symbols. Place the electrons on four sides of a square around the element symbol.
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Chapter 9- Molecular Geometry and Bonding Theories 9.1 Molecular Shapes Lewis structures give atomic connectivity: they tell us which atoms are physically connected to which atoms. Whenever two atoms or ions are strongly attached to each other we say there is a chemical bond. Three general types of chemical bonds: ionic , covalent and metallic. We will encounter 11 basic molecular shapes: The shape of a molecule is determined by its bond angles. Bond angles The angles made by the lines joining the nuclei of the atoms in a molecule Consider CCl4: Experimentally we find all Cl?C?Cl bond angles are 109.5?. Valence Shell Electron Pair Repulsion (VSEPR) model.