Lecture 1 Introductions & Water Biochemistry Lecture 1 Introductions & Water
Bloom’s Taxonomy Richard C. Overbaugh, Lynn Schultz Old Dominion University
Biochemistry is the chemistry of Living Systems The Chemistry of Carbon and Water Themes for this course: The transformation of energy Levels of complexity
Levels of Complexity Lipids
The Inner Life of the Cell http://multimedia.mcb.harvard.edu/anim_innerlife.html
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!
Carbon and Functional Groups
Other biomolecules PEP NADP+ Phosphatidylcholine
Bioenergetics Cell Reactants Products Steady State = constant flux Structural differences between reactants and products Concentration differences between reactants and products
Water
Hydrogen Bonds
Chapter 2, Figure 2.3, Types of noncovalent interactions
Chapter 2, Figure 2.1, Noncovalent bonding interactions between human growth hormone and its cellular receptor
Chapter 2, Figure 2.2, Covalent and noncovalent bond energies
Chapter 2, Figure 2.12, Hydration of ions in a solution
Water
Chapter 2, Figure 2.14, One unit of clathrate structure surrounding a hydrophobic molecule
Chapter 2, Figure 2.16a, Interactions of amphipathic molecules with water
pH pH = -log[H+]
Acids
Buffers
Chapter 2, Figure 2.18, The effect of pH on overall surface charge of human ubiquitin
Chapter 2, Figure 2.24, Dependence of protein solubility on pH
Hendeson Hasselbalch Equation HA H+ + A-
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