1. Chemistry – study of matter and the changes it undergoes

2. Only 1 kind of atom
2 or more different kinds of atoms

4. Element is a pure substance made up of only one kind of atom.

6. Families (groups) – vertical columns
Elements in a family have similar properties
Periods – rows, left to right add another proton and electron – filling up outer energy (valence) level

7. Elements are Made of Atoms
The single smallest unit of an element that retains all of the chemical and physical properties of its parent element is called an atom.
Atoms are made up of smaller, subatomic pieces called protons, neutrons and electrons
Helium

8. Atoms are composed of three types of subatomic particles
Electrons: have a negative charge and are the smallest part of an atom
Protons: have a positive charge and mass of 1amu
Neutrons: have no charge
1 neutron = 1 amu
Protons and neutrons clump to make the nucleus
The electrons surround the nucleus and form the much larger electron cloud.

9. Atomic Number Atomic number defined as the number of protons
Because atoms are neutral: # electrons = # protons
Atoms of the same element always have the same atomic number 2 3 11

10. Chemical Bonds
Atoms are not stable unless their valence (outermost) energy level is filled.
By forming bonds with other atoms, valence levels are filled.
Barium

11. Two types of bonds
Atoms may fill their valence levels one of two ways:
share electrons with other atoms to form a covalent bond or
Atoms can gain or lose electrons to create an ionic bond

12. Ionic Bonds (Salts)
Formed when electrons are transferred between atoms – one loses and the other gains
Atom that has gained or lost an electron is now charged and called an ion
Atom that loses electrons becomes + and the one that gains is -

13. Covalent Bonds
Electrons are shared: single pair shared = single covalent bond, 2 pairs shared = double covalent bond

14. Chemical Formulas
Tell kinds and numbers of atoms in one molecule (or smallest unit) of a substance
Subscripts tell the number of atoms of the element to the upper left (of the subscript).
Eg. H2O
Tells us there are 2 atoms of H and 1 of O in one molecule of water (if no subscript, then it is understood to be 1)

15. CO2
1 carbon dioxide molecule has 1 carbon atom bonded to 2 oxygen atoms.

16. Chemical Equations
Represent chemical reactions, which obey the law of conservation of matter – the kinds and numbers of atoms that enter into the reaction also come out!
Coefficients tell how many of the molecules they precede are involved.
Eg. 2Mg + O MgO
Read as magnesium plus oxygen yields magnesium oxide
Substances to the left of the arrow are reactants, and substances to the right are products
In this reaction, 2 atoms of magnesium react with 2 atoms of oxygen to produce 2 molecules of magnesium oxide.

18. pH refers to the concentration of H+ or OH- ions
Lower pH – higher concentration of H+ and the greater the acidity
Higher pH – higher concentration of OH- and the greater the alkalinity (base)
Organisms – and tissues within organisms have specific pH requirements.

19. Inorganic Molecules Simple Structure H20, 02, NH3, CO2
Inorganic even though it contains carbon - exception

20. Biological Macromolecules Organic (contain carbon)
(polymer)
Building
Blocks
(monomers)
Function
Sources
Protein
Amino acids
Structure, enzymes, hormones
Eggs, fish, chicken, meat, nuts, legumes, dairy
Carbohydrates
polysaccharides (starch – cellulose)
Monosaccharides
Simple sugars
(glucose)
Energy
Fruit, veggies, bread, potatoes,
pasta, grains
Lipids (fats and oils)
Fatty acids and
Glycerol (Not monomers)
Energy, structure, hormones
Vegetable oils (olive, safflower), animal fats (butter)
Nucleic acids
DNA & RNA
Nucleotides
Carry genetic code and direct protein synthesis
Cells

21. CARBOHYDRATES Sugars, Starches, Cellulose
Contain C,H,O in a ratio of 1:2:1
Ratio of H:O is 2:1 just like H2O
Eg. C6H12O6
Energy & energy storage

22. cellulose
starch
sugar

23. Glucose
A monosaccharide C6H12O6,
major source of energy in the body.

24. Monosaccharide + monosaccharide
disaccharide

25. Polymerization
Smaller units (monomers) are bonded together to make larger units (polymers)
A disaccharide such as maltose or sucrose is made from the dehydration synthesis (condensation reaction or removal of H2O) of 2 monosaccharides
If more than 2 monosaccharides are bonded through dehydration, a polysaccharide (starch) is made. Cellulose is an example

26. PROTEINS Composed of monomers called amino acids
Contain C, H, O, sulfur and nitrogen!
Structure and chemicals that affect other body processes: enzymes, hormones

28. Peptide bond
A dipeptide results

29. Amino Acids

30. There are 20 different types of amino acids found in the natural world.

31. LIPIDS Fats, oils and waxes
Contain C,H,O with a very high ratio of carbon and hydrogen to oxygen.
Composed of fatty acids and glycerol
Uses:
Cell membrane structure
Energy
Some Hormones
Insulation

32. Lipids Include all of the fats, oils and waxes
Lipids Include all of the fats, oils and waxes. They have higher ratios of Carbon & Hydrogen than oxygen.

33. Saturated vs Unsaturated Fats unsaturated has double bonds

34. Nucleic Acids DNA & RNA: carry genetic code
Made of repeating units called nucleotides:
Sugar + phosphate + N base
Contain P

35. nucleotide