Human Physiology Santa Monica College SPRING 2011

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

Review of syllabus

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. www.physiologyplace.com Clarify questions you may have Study groups Good attendance

Chapter 2: Atoms, Ions and Molecules

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.

Remember to answer concept questions and questions at end of chapter-2 pp. 47-48 (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. 21-23,26-27, 30-31, 36, 38, 40, 43, 44 Questions related to graphs and figures Pg. 26, 37, 42-43

Atoms are composed of: Quarks Superstrings

Quarks and superstrings

Radiation and nuclear medicine

Simplest kinds of matter Composed of one type of atom

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

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

Example of Polar Covalent Bond Water

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

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

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

Ionic Interaction 17 electrons 11 electrons 18 electrons 10 electrons

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

Saltwater Which is the solute? Which is the solvent?

We measure concentration of solutes in solution as: Percent Molarity

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.

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. 1000 ml- 180= 820 ml

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

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

A common biological buffer The sponge! H2CO3 H+ + HCO3- Notice how the hydrogen ion moves from the “bound” state to a “free state”

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

Carbohydrates Carbon Hydrogen Oxygen (CH20)n

Lipids Insoluble in water Carbon, Hydrogen, Oxygen Non polar

Protein Primary Secondary Tertiary Quaternary

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