1. Inorganic Chemistry - Applications

2. Hydrogen Bonding (1). Hydrogen Bonds – Hydrogen (cation) attracted to nitrogen, oxygen (anions) Attraction between ions (electrostatic) – ‘Weak bond’ – Van der Waals forces (2). Examples – Surface tension in water – DNA

3. Hydrogen Bonding Hydrogen Bonding Animation (link) Hydrogen Bonding Animation

4. Why is hydrogen bonding important? Water molecules are attracted to each other – Bonds are easily broken- modifies climate – Breaks down ionic compounds (ions in the body) – Digestion – breaks down food compounds Holds DNA strands together – Easily broken (replication) – Easy to reform (brings new strands together)

5. Chemical Reactions and Energy (1). Types of Chemical Reactions (page 38) – Synthesis reaction – Decomposition reactions (2). Synthesis reactions – Store energy – formation of ATP – Starch (3). Decomposition reactions – Energy releasing – Glycogen or Starch ---  glucose – (4). Oxidation – Reduction reactions

6. Chemical Reactions and Energy (1). Energy and Chemical Reactions – ATP stores chemical energy in it’s bonds – Glucose is ‘used by the cells’ to produced ATP – Phosphate bonds are broken --  energy released Cellular work (2). Oxidation and Reduction reactions – See notes online

7. Mixtures and Solutions (1). Mixtures – Composed of two or more components – Physically mixed (no chemical reaction) (2). Types of Mixtures – Solutions Solvent vs solute – Solute particles do not settle out Homogeneous mixtures Transparent, individual atoms and molecules

8. Mixtures (3). Colloids – Heterogeneous – Larger solute particles; do not settle out; scatter light – Cytosol of the cell (4). Suspensions – Heterogeneous – Large solutes; settle out – Blood

9. Solutions, Ionic Balance (1). Body fluids must maintain proper ionic balance – Inorganic solutes (salts), acids and bases are called ‘electrolytes’ – Ionize in water – Ions must be balanced Water balance in cells

10. Concentrations of Solutions (1). Percentage concentration – 5% glucose solution (2). Molarity – Moles/L – Mole = elements atomic weight 1 mole of carbon = 12 g 1 mole of glucose = 180 g 1 mole of HCl = 36 g – 1 M solution of HCl = 1 mole (36 g)/L