1. Biochemistry
Lecture 1

2. Bloom’s Taxonomy
Richard C. Overbaugh, Lynn Schultz Old Dominion University

3. Student Objectives for this course
Calculate bioenergetic parameters and evaluate carbon molecules reactions
Reproduce and explain key metabolic processes: glycolysis, TCA cycle, electron transport and oxidative phosphorylation, fatty acid oxidation
Analyze protein structure and function and evaluate different methods used to assess and test structure and function
Trace key metabolites through key pathways, design experiments to test carbon flux
Compare and contrast modes of metabolism regulation and judge the effects of different modes

4. Biochemistry is the chemistry of Living Systems
The Chemistry of Carbon and Water
Themes for this course:
The transformation of energy
Levels of complexity

5. Cells

6. Cells

7. Levels of Complexity
Lipids

8. The Inner Life of the Cell

9. Why Carbon What can we learn from this?
Bond
Strength (kJ/mol)
C – C
347 – 356
C = C
611
837
C – O
336
C – H
356 – 460
Si – Si
230
Si – O
368
O – O
146
O = O
498
N – N
163
N = N
418
946
What can we learn from this?
C – C bond is stronger than C – O
Stable in oxygen rich environment!
Two C – C bonds are stronger than one C = C
Chains are stable!
C – H bond is strong
Hydrocarbons stable at room temperature!

10. Important Functional Groups
Alcohol
Thiol
Amine
Ether
Thioether
Peroxide
Disulfide
Aldehyde
Ketone
Carboxylic acid
Ester
Anhydride
Amide
Thioester
Phosphate
Phosphoester
Phosphoanhydride

12. Carbon and Functional Groups

13. Other biomolecules
PEP
NADP+
Phosphatidylcholine

14. Bioenergetics Cell Reactants Products Steady State = constant flux
Structural differences between reactants and products
Concentration differences between reactants and products

15. Water

16. Hydrogen Bonds

17. Water

18. Colligative Properties

19. pH
pH = -log[H+]

20. Acids

21. Buffers

22. Hendeson Hasselbalch Equation
HA H+ + A- 

23. Summary Biochemistry is the chemistry of living things
Which is the chemistry of carbon and water
Carbons unique bonding properties
Water: hydrogen bonds and ionization
Buffers and pH