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Life’s Water: Necessary and Abundant
Human H2O content:
Life on Europa (Jupiter moon) only considered if H2O is present Even in unusually
cold hearty Antarctic bacteria (e.g. -2C) H2O is essential
Compound MW BP MP
H2S Sulfide 34 -60 -85H2Se Selenide 81 -4 -50H2Te Telluride 130 -2 -49
H2O Water 18 100 0
Water Unlike its Molecular Neighbors
As the molecule becomes heavier how should this affect boiling point and melting point?
Unusual Physical Properties of H2O
Adhesion – sticks to other molecules
Cohesion – sticks to itself
High surface tension
Water Hydrogen Bonding: Weak But Abundant
Distance for:
Covalent
H-bonding
Non-interacting
Van der Waals radius
Van der Waals Radius: distance from nucleus to effective electron surface
Where is H-bonding on this graph?
Oxygen Electronic configuration? Bond angle?
Hydrogen Bonding in Water
DNA Base Pair Hydrogen Bonding
100
400
200.1
Relative Bond Strengths
Where do dipole-dipole interactions fit into this ranking?
Hydrogen-Bonding Requirement
Differential electronegativity
S – H - - - - - SName the following interactions:
Water: the Universal Solvent
Polar solvents weaken electrostatic interactions
Dielectric Solvent Constants1
1Dielectric solvent constant is a measure of the ability of a solvent to diminish electrostatic attraction between dissolved ions
Exclusion of non-polar substances from a water phase
Entropy driven ∆G = ∆H - TΔS
Hydrophobic Effect
Single Tail Amphipathic Molecules: Micelles
What is the driving force for this reaction?
Double Tail Amphipathic Molecules: Bilayer
A Bilayer Limits Movement of Polar Substances
Amphipathic molecules contain both hydrophobic and hydrophilic portions
Driving Force for Protein Folding: Hydrophobic Effect
Is a molecule always charged or uncharged?
pH Versus pKA
Ka/pKa Values
Le Chatelier’s Principle
When a system in a state of dynamic equilibrium is acted upon by some outside stress, the system will, if possible, shift to a new position of equilibrium in order to minimize the effect of the stress.
Acetic Acid Titration Curve
What is the effective buffering range?
Conceptionally: pKA is the pH at which the ionized
and unionized forms are equal. HA ↔ H+ + A-
KA = [A-][H+]/[HA]
KA[HA]/[A-] = [H+]
log KA + log [HA]/[A-] = log [H+]
pH = pKA – log [HA]/[A-]
Henderson-Hasselbalch Equation
pH = pKA – log [HA]/[A-]
pKA = -log KA and pH = -log [H+]
pH Value of Biological Fluids
Inverse Relationship: [H+] and [OH-]
H2O ↔ H+ + OH-
K = [H+][OH-]/[H2O]
KW = K[H2O] = [H+][OH-]
KW = 10-14 = [H+][OH-]
CO2 + H2O ↔ HCO3- + H+
Water Acidification
Acids to Buffer at Any pH
Chapter 2 Problems:
1-15, 21, 33, 35, 41, 53, 55 and 60