1. Chemistry of Life

2. Structure of an Atom Size Subatomic particles Nucleus Proton Neutron
Quarks
Electrons
Outside the nucleus
Different distances (levels, clouds)
Move randomly
Size

3. How are Elements Different?
Atomic number
# of protons
Mass #
# of protons + # of neutrons
Atomic mass

4. Use the Periodic Table Carbon Most common form of carbon Carbon – 14
Atomic #
# of protons
# of electrons
Mass #
# of protons + # of neutrons
Most common form of carbon
Carbon – 14
14 = mass #
# of protons
# of electrons
# of neutrons
Isotope : same # of protons, but different # of neutrons from most common form

5. Boron – 11 Boron – 10 # of protons # of electrons # of neutrons
Isotope?
Boron – 11
# of protons
# of electrons
# of neutrons
Isotope?

6. Daily Review
Determine the number of protons, neutrons and electrons in each of the following
Fluorine-20
Helium-4
Which of those compounds is an isotope?

7. Water – Why is it important?
Makes up a lot of living things
Many useful/helpful properties
Polarity
Lopped side appearance
One side slightly positive
Creates solutions
Because of charge can dissolve
Other polar and ionic (fully charged)
2 or 3 types of compounds
Examples
Can break apart other substances
Creates suspensions

8. Is more dense as a liquid
Can hold lots of heat
Takes more energy to heat up
Releases energy back more slowly
Examples
Is more dense as a liquid

9. Hydrogen Bonds Very strong between molecules
Very strong between molecules
Each water can have 4 H- bonds
Causes
Cohesion
Adhesion
Capillary action
Surface tension

10. pH Water breaks down to H+ and OH- pH = how much H+ Acids Bases
pH of 7 means H+ and OH- are equal
Acids
pH lower than 7
Lower # = stronger
Examples
Bases
pH higher than 7
Higher # = stronger
Buffers
Help with homeostasis

11. Daily Review
Define:
Cohesion
Adhesion pH
Describe 4 reasons why water is a versatile molecule that is important to living beings
Stomach acid has a pH of 2 and ocean water has a pH of 8
Which one is acidic?
Which one is closer to being neutral?

12. Other Basic Chemistry Atom Atoms are generally neutral Ions Molecule
Atom with a charge
Sodium
11 protons + 11 electrons = neutral
Gains or loses electrons
11 protons + 10 electrons = +1
Caffeine

13. Chemical Bonds Make molecules An attraction, not a physical thing
Hydrogen
Ionic
Involves ions
Gaining/losing electrons
Very strong
Covalent
Sharing electrons
Not as strong
More common

14. Elements of life C, H, N, O, P, S Organic Inorganic Contains C and H
C, H, N, O, P, S
Organic
Contains C and H
Covalent bonds
Usually large molecules
In living things
Inorganic
No C (unless simple, like CO or CO2)
Examples – water, O2, N2

15. Macromolecule Definition Polymer Made of monomers
Each bond created releases water
Breaking a bond releases water

16. Polymers of Biology

17. Carbohydrates Disaccharides Basics Monosaccharides 2 sugars
Sucrose = glucose + fructose
Lactose = glucose + galactose
Carbohydrates
Basics
1C:2H:1O
Main source of energy
Structural
Monosaccharides
Simple sugar
Glucose
Galactose
Fructose

18. Complex Carbohydrates
Polysaccharides
Starch
Storage in plants
Glucose units
Glycogen
Storage in animals
Released from liver
Cellulose
Structure in plants
Wood

19. Daily review Fill in the chart with the missing vocabulary terms
Carbohydrates
Composed on one subunit
Composed of 2 subunits
Composed of more than 2 subunits
Daily review
Fill in the chart with the missing vocabulary terms
Define:
Ions
Chemical bond
Macromolecule
Polymer
Give examples of monosaccharides, disaccharides, and polysaccharides

20. Lipids Fats, waxes, oils, steroids, hormones Insoluble in water
Lipids
Fats, waxes, oils, steroids, hormones
Insoluble in water
Glycerol + fatty acid(s)
Functions
Cell structure
More efficient energy storage (9 vs. 4 calories)
Communication
Steroids
Ring of carbons
Hormones
Cholesterol

21. Saturated vs. unsaturated
Saturated
All single carbon bonds
Solid
Examples
Unsaturated
Carbon to carbon double bond(s)
Liquid
Good vs. bad

22. Nucleic acids Contains C, H, N, O, P Made from nucleotides
5-carbon sugar
Phosphate group
Nitrogenous base (5 different)
Purpose – genetic information
DNA, RNA

23. Daily review Name what each is made of and a use for each:
Carbohydrate
Nucleic acid
Lipid
What is the difference between a saturated and unsaturated fat?

24. Proteins Contain C, H, N, O Made of amino acids
Very specific order or amino acids
Complex 3d shape
Chain of amino acids = polypeptide chain
Folds and crumples
May have multiple subunits
Function
Structural
Nutrient storage
Transportation
Identification of cells (defense)
Enzymes

25. Proteins are sensitive
Proteins are sensitive
Change shape easily
Denature
Caused by changes in
Temperature pH
Salt concentration
Molecules present
May permanently disable the protein or cause it to malfunction
Frying an egg

26. Chemical reactions Atoms don’t change Atoms rearranged
Chemical bonds broken and formed
Usually requires energy - activation energy
Getting energy slows down the reaction

27. Enzymes Lock and key Will not work if denatured
Proteins
Catalyst
Not changed
Lowers activation energy
Speeds up reaction
Lock and key
Substrate
Active site
Will not work if denatured
Used in most biological processes