1. Human Physiology
Santa Monica College
SPRING 2011

2. Topics to be covered: Physiology Syllabus Chapter 2 Basic Chemistry
Molecules and their interaction
Read Chapter 2
Chapter 1
What is physiology
Scientific process
Read Chapter 1

3. Review of syllabus

4. Resources to help you do well in physiology
Read chapters before discussion
Use “concept checks” found in the text
Answer the questions at the end of each chapter and answer the concept questions throughout the chapter. Answers for both are available either at the back of the textbook or end of the chapter.
Clarify questions you may have
Study groups
Good attendance

5. Chapter 2: Atoms, Ions and Molecules

6. Outline of concepts to be reviewed
Atoms and Elements
Molecules and Bonds
Solutions and Solutes
Concentration pH
Major classes of organic macro-molecules
Protein Interactions: will be presented on a separate power point.

7. Remember to answer concept questions and questions at end of chapter-2 pp (excluding question 32)
These are not to hand-in but you will find these questions help you to both review the material and identify where you may have questions.
Concept questions for chapter-2 are on pages
Pg ,26-27, 30-31, 36, 38, 40, 43, 44
Questions related to graphs and figures
Pg. 26, 37, 42-43

8. Atoms are composed of:
Quarks Superstrings

9. Quarks and superstrings

11. Radiation and nuclear medicine

12. Simplest kinds of matter
Composed of one type of atom

13. Bonding and Interactions Between Atoms
Covalent Bonding
Hydrogen Bonding
Ionic Interactions
Van der Waals Forces

14. Covalent Bonds Sharing of electrons
A molecule may have polar covalent bond.
A molecule may have non-polar covalent bond.

15. Example of Polar Covalent Bond
Water

16. Molecular Interactions
Within H20 molecules
Covalent bonds
Between H20 molecules
Hydrogen bonds

18. Polarity affects solubility of drugs.
Polar molecules
Hydrophilic
Non-Polar molecules
Hydrophobic

19. Let’s look at Na+Cl- as an example of ionic interactions.

20. Ionic Interaction
17 electrons
11 electrons
18 electrons
10 electrons

21. Solutions Solutions= Solutes+Solvent
For example: saltwater is a solution

22. Saltwater
Which is the solute?
Which is the solvent?

23. We measure concentration of solutes in solution as:
Percent
Molarity

24. You want to prepare a 10% glucose solution.
You weigh out _________grams of glucose.
Dissolve the glucose to a total volume of ___________ milliters (ml) of solution.

25. Now you want to prepare a 1 Molar (M) C6H1206 solution.
You weigh out ________ grams glucose and dissolve it in a total of volume of ________liter of solution.
180 grams glucose
in a total volume of 1 liter
i.e ml- 180= 820 ml

26. pH=log(1/[H+]) pH
What is it?
Why is it important?

27. What is a buffer?
Think “chemical sponge”
“bound H+”
“free H+”

28. A common biological buffer
The sponge!
H2CO H+ + HCO3-
Notice how the hydrogen ion moves from the “bound” state to a “free state”

29. Organic Macro-Molecules of the Body
Carbohydrates
Lipids & steroids
Proteins
Nucleic Acids

30. Carbohydrates
Carbon
Hydrogen
Oxygen
(CH20)n

32. Lipids
Insoluble in water
Carbon, Hydrogen, Oxygen
Non polar

34. Protein
Primary
Secondary
Tertiary
Quaternary

36. Nucleic Acid: Two examples are DNA& RNA
(DNA & RNA will be further discussed in more detail later in the course.)