2. Atomic Structure and Properties
Chemistry of Life
Atomic Structure and Properties
Chemical Bonding
Macromolecules
Chemical reactions

3. Prior Knowledge
Write everything you know about the following equation.
C6H12O O CO2 + 6H2O

4. Atoms The basic unit of matter is an ATOM.
Atoms are broken into 3 parts
Protons (+ charge) found in the nucleus
Neutrons (no charge) found in the nucleus
Electrons ( - charge) found in constant motion around the nucleus (orbitals)
A substance made up of only one type of atom is called an element (N2)
A substance made up of more than one type of atom is called a compound. (ex H2O)

7. Electrons can be added or lost to create a charged atom called an ion.
A typical atom can exist in two different forms which affect the atomic properties:
Neutrons can be added (common) or lost (uncommon) to form isotopes. Uses?
Electrons can be added or lost to create a charged atom called an ion.
Losing electrons create a positive charge (cation)
Gaining an electron forms a negative charge (anion)
Interactions of atoms are mostly a product of moving electrons (bonding, electricity, conduction, etc)

12. Chemical bonds 3 main types of bonds (two biological)
Metallic Bonds form between two metals (very strong) example Fe3
Ionic Bonds form from sharing of electrons (weak) example NaCl
Covalent Bonds form from the sharing of electrons. (Strong) example CH4

14. CO2
NH3CH2CO2

15. Identify
MgF2
CaO
N2O3
Li3N
C6H12O6

16. Transfer of electrons Sharing of electrons Weak bonds Strong Bonds
Ionic Bonds Covalent Bonds
Transfer of electrons Sharing of electrons
Weak bonds Strong Bonds
Metal and non-metal Two non-metals
Enegativity 1.8 or more Enegativity 1.2 or less
Examples: Examples:
NaCl, CaO, MgF2 CO2, F2, P4S10

17. Properties of H2O
Water molecules are neutral (no net charge). Why then is water one of the best electrical conductors?
Water is a polar molecule which forms both covalent and ionic bonds.
Polar covalent bonds form between Hydrogen and Oxygen creating a (+) charge on the H and a (-) charge on the O.
Hydrogen bonds from between water molecules. The positive H attracts the negative O. The result is a matrix with unlimited bonds.

20. Cohesion is the attraction between molecules of the same substance.
Adhesion is the attraction between molecules of different substances.
Mixtures are formed by two or more molecules which are phyiscally joined but not chemically.
Solutions: all components are spread evenly
Solute: dissolved substance (solid) ex. salt
Solvent: substance doing the dissolving (liquid) ex H2O

22. Acids / Bases What happens when you split a water molecule?
You get two charged molecules that are the basis of many chemical reactions
Acids are formed from large concentrations of H+ ions (hydrogen ions). pH scale from 1 - 6
Bases are formed from large concentrations of OH- ions (hydroxide ions) pH scale from 8 – 14
Water consists of both ions and thus is neutral at pH of 7.

24. Organic Chemistry
Organic chemistry is the study of compounds with bonds between carbon atoms.
Carbon compounds are the base to all living organisms (organic).
There are 4 groups of large organic compounds called macromolecules.

25. Carbohydrates Sugars / starches
Mainly used for energy and structure in organisms
Simplest of the four macromolecules
Monosaccharides – simple sugars (glucose)
Polysaccharides – complex chain of monosaccharides (starch)

26. Lipids Fats, oils Contain mostly carbon and hydrogen
Source of stored energy for organisms
Found in membranes and barriers (skin)
Non-water soluble (does not allow water to pass)

27. Proteins
Made up of long chains of amino acids (bonded through hydrolysis)
Contain nitrogen, carbon, hydrogen, and oxygen. The most complex macromolecule.
Proteins have a variety of functions:
Structure and support (forms bone and muscle)
Regulates cell process and controls chemical reaction rates
Transports materials
Fights diseases

29. Comparing Macromolecules
What element is different between Proteins and sugars?

30. Sugar Structure

31. Lipid structure

32. Protein Structure

34. Nucleic Acids Contains nitrogen, oxygen, carbon, hydrogen, phosphorus
Stores genetic information
Transmits genetic information (codes for proteins)

35. Chemical Reactions
Your body is a complex system going through thousands of chemical reactions every second.
Energy, protein production, waste removal, oxygen transport, muscle contractions, are all examples of chemical reactions.

36. What is the difference between a chemical and physical reaction?
C6H12O O CO2 + 6H2O
Reactants Products
Chemical reactions break chemical bonds in the reactants to form new (different) products
Exothermic Reaction – releases energy
Reactants are larger than products
Endothermic Reaction – requires energy
Products are larger than reactants

37. Types of Chemical Reactions
Decomposition (Break down)
Synthesis (Build-up)
Single displacement (re-arranging)
Double displacement (re-arranging)
Combustion (burning)
What are the products and reactants?

38. Does water and carbon dioxide naturally combine to make sugar?
No, it requires a specific amount of energy applied to the two chemicals to start the chemical reaction. This is called Activation Energy.
Organisms are able to control reactions by using substances called catalysts which can control the rate of a reaction.
Some of the most important catalysts are found inside your body and cells, these biological catalysts are called Enzymes.

39. Enzymes (biological catalysts) work by attaching to a substance (substrate) at a specific recognition site called an active site.
This is the same process used by antibodies and to fight off diseases. Why then can your body not fight off the disease called HIV or AIDS? (what type of cell fights diseases?)