Inorganic Chemistry - Applications

Inorganic Chemistry - Applications

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

Hydrogen Bonding

• Hydrogen Bonding Animation (link)

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)

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

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

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

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

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

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