Chapter 2 Flashcards
What is the order of IMF’s from strongest to weakest?
Covalent bonds
Ionic bonds
H-bonds
Dipole-dipole
Dipole-induced dipole
Van Der Waals Forces
What is the dielectric constant? (D)
The measure of the ability to break ions apart
What is the hydrophobic effect and why is it important?
It drives the interaction between non-polar substances and water, and is critical for the folding of some proteins and the stability/structure of many macromolecules
What happens to lipids when they’re submerged in water?
The lipids force the water molecules to become highly ordered and form a cage around them. The water molecules don’t like this, so they push back as a way to increase their disorder
What happens when there are many lipids lined up in the water?
Only the outermost lipids will form the cage with the water, so the ones inside the line will not come into contact with it. This means fewer water molecules are ordered and the entropy is able to increase
What is the purpose of the hydrophobic patch on proteins?
It allows for the displacement of water so that enzymes can bind to the substrate
Amphipathic compounds have regions that are both ____ and _____
polar
non-polar
What is the equation for Ka and what is its importance?
Ka= [Products]/[reactants]
It tells the strength of an acid. Strong acids have a larger Ka because they dissociate more fully and trend towards the products. Weak acids have a smaller Ka because they dissociate less fully and trend towards the reactants
What is the equation for determining pH?
-log[H+]
What causes the electrical conductivity of water?
The charge (an extra proton) travels through the chain of waters from a hydronium ion at the end, to create another hydronium ion at the other end.
pH ____ be negative
Can
In a neutral solution [H+] is _____ to [OH-], and the resulting pH is _____
equal
7
______ is used as the buffer for blood because it keeps the pH around 7.2
Bicarbonate
(carbonic acid and bicarbonate)
The buffering range is where the pH is _____, and is essentially equal to the pKa
controlled
(it is the area where there isn’t much change in pH on the titration curve. So usually the middle of the curve)
What is the Henderson-Hasselbalch equation?
pH= pka + log ([A-]/[HA])
