1. Organic Compounds, Chemical Reactions, Acids, Bases, and the pH Scale

2. Organic compounds
Contain Carbon in their structures. Usually many carbons are linked together to form a carbon backbone.

3. Carbohydrates Includes sugar and starch
They are classified based on their size and solubility.
can be:
Monosaccharide- one sugar
Disaccharide- two sugars
Polysaccharide- many sugars

4. Lipids A.k.a. fats Insoluble in water.
Allows for a long term way to store energy.
Includes:
Triglycerides
phospholipids
steroids
Eicosaniods

5. Proteins
Any of a large group of nitrogenous organic compounds that are essential constituents of living cells; consist of polymers of amino acids; essential in the diet of animals for growth and for repair of tissues.
Includes:
Amino acids
Globular proteins
Fibrous proteins

6. Enzymes
Specialized proteins that facilitate a reaction. They can speed up or slow down a reaction.
pH and temperature affect an enzyme’s function.

7. Chemical equations Chemicals reacting= reactants
Chemicals formed= products
Reactants  products
A + B  AB

8. Types of chemical reactions
Synthesis reaction- formation of new bonds.
A + B  AB
A and B were once separate atoms, but have now come together by forming a bond, creating molecule AB.

9. Decomposition Reactions
Decomposition reaction- breaking of previous bonds.
AB  A + B
AB was once a single molecule. After a reaction occurs (like an enzyme splitting a larger molecule) A and B are now separate atoms.

10. Exchange Reactions
Exchange reaction are a combination of synthesis and decomposition reaction.
AB + C  AC +B
AB + CD  AD + CB
Old bonds between molecules are broken, and the new atoms exchange partners, forming new molecules.

11. Factors that influence chemical reactions
Temperature
Concentration
Particle size
Catalysts (enzymes)

12. Acids
is traditionally considered any chemical compound that, when dissolved in water, gives a solution with a hydrogen ion activity greater than in pure water
i.e. a pH less than 7.0 in its standard state
pH: 0-6.9
Eaxmple of an acid: HCl

13. Bases Produces hydroxide ions in solution. (-OH-)= hydroxide
pH=
Example of a base: NaOH

14. What is pH?
pH is a measure of the acidity or alkalinity of a solution.
Low pH= highly acidic
High pH= highly basic

15. The pH scale

16. Polarity and Acidity
What are the environmental risks associated with acids being polar and water being polar?
Hint

17. Buffers Designed to prevent sharp changes in pH.
Without them, if we ingest anything that has a pH difference from our own blood, we may accidently alter our pH too far and cause ourselves serious bodily harm, if not death.

18. Cohesion and adhesion forces

19. Cohesion the intermolecular attraction between like-molecules.
In this definition, like= same
Co=together!

20. Adhesion
the tendency of dissimilar particles or surfaces to cling to one another.
In this definition, dissimilar = different