Physiology

• Only can test 'naturla run'
• Determine Subjective vs Objective
• Qualitative vs Quantitative

• Meter = Base unit of length
• Gram = Base unit of mass
• Liter = Base unit of volume
• Celsius = Base unit of Temperature

• Observation
• Hypothesis (must be testable)
• Experiments (test hypothesis)
• Results & Data
• Conclusion (accept or reject hypothesis)

• Cellular / Molecular (in vitro = outside body)
• Animal Experiments (in vivo = inside body) (90% fail at this level)
• Clinical Trials - Phase I: Tested on healthy human volunteers
• Clinical Trials - Phase II: Tested on target population
• Cinical Trials - Phase III: Tested on wide variety (age, ethnic groups, and levels of health) all over the country
• Cinical Trials - Phase IV: Tested for other possible uses

• Maintain stable, constant condition.
• Multiple dynamic equilibrium adjustment and regulation mechanisms make homeostasis possible.
• Body Temperature = 37C
• Blood pH = 7.3 - 7.4

The output of the system acts to oppose the input of the system. If overall feed back is negative, system will be stable. Example = maintaining blood pressure

• 'A produces more of B which in turn produces more of A'
• Examples - Blood Clotting & Contractions during childbirth
• 

Feed-forward control is exemplified by the normal anticipatory regulation of heartbeat in advance of actual physical exertion. Feed-forward control can be likened to learned anticipatory responses to known cues.

• Carbon
• Hydrogen
• Nitrogen
• Oxygen
• Phosporus
• Sulfur

• Proton: Located in Nucleus. Positive Charge (+). 1 AMU
• Neutron: Located in Nucleus. Neutral Charge. 1 AMU
• Electron: Located in Orbital. Negative Charge (-). 0 AMU

• Atomic Number: Number of Protons
• Atomic Mass: Number of protons and Neutrons

• Must fill all previous shells first
• First orbital holds 2 Electrons
• All adjacent orbitals hold 8 Electrons

• Outer orbitals are shared.
• Organic Molecules bound in this manner.
• Non-polar: Equal sharing of Electrons (Example H₂)
• Polar: Unequal sharing of Electrons (Example H₂O)

• Transfer of Electrons (Example NaCl)
• Atoms seek to stabilize by completing their outer orbitals.
• Inorganic molecules typically bond in this manner.

• Hydrgoen atoms are slightly attracted to electronegative atoms
• Examples: Oxygen, Nitrogen
• Found in Protein, Enzymes, and DNA

Slight attraction of non-poplar molecules.

• Carbon based
• Covalent bonds allow for large compounds

• Combined with Condensation / Dehydration RXN
• Taken apart with Hydrolysis RXN

• Suffix -ose
• Formula: C_nH_2nO_n
• Monosaccharides are simple sugars (Glucose)
• Two monosaccharides can be joined covalently to form a disaccharide (Glucose + Glucose = Maltose + H₂O)
• Numerous monosaccharides joined together are called polysaccharides (Glycogen)

• Hydrophobic
• Insoluble in polar solvents (water)
• Stored in the body as triglyceride.
• glycerol + 3 fatty acids = triglyceride + 3 H₂O
• Palmitic Acid (saturated): single covalent bonds
• Linolenic Acid (unsaturated): at least one double bond