1. Lecture 1 Introductions & Water
Biochemistry
Lecture 1
Introductions & Water

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

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

4. Levels of Complexity
Lipids

5. The Inner Life of the Cell

6. 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!

8. Carbon and Functional Groups

9. Other biomolecules
PEP
NADP+
Phosphatidylcholine

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

11. Water

12. Hydrogen Bonds

13. Chapter 2, Figure 2.3, Types of noncovalent interactions

14. Chapter 2, Figure 2.1, Noncovalent bonding interactions between human growth hormone and its cellular receptor

15. Chapter 2, Figure 2.2, Covalent and noncovalent bond energies

17. Chapter 2, Figure 2.12, Hydration of ions in a solution

18. Water

19. Chapter 2, Figure 2.14, One unit of clathrate structure surrounding a hydrophobic molecule

20. Chapter 2, Figure 2.16a, Interactions of amphipathic molecules with water

21. pH
pH = -log[H+]

22. Acids

23. Buffers

24. Chapter 2, Figure 2.18, The effect of pH on overall surface charge of human ubiquitin

25. Chapter 2, Figure 2.24, Dependence of protein solubility on pH

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

27. 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