Term
| the bonds that stabilize biomolecules (lipids, carbohydrates, proteins, and nucleic acids) |
|
Definition
|
|
Term
|
Definition
| allow for dynamic interactions and transmission of energy and information |
|
|
Term
| this forms the basis for biochem and life itself |
|
Definition
| transient chemical interactions |
|
|
Term
|
Definition
| random movement of particles due to fluctuations in temperature |
|
|
Term
|
Definition
| random fluctuation of the energy content of the environment |
|
|
Term
| what initiates biochemical interactions? |
|
Definition
|
|
Term
| the medium for Brownian motion |
|
Definition
|
|
Term
| something water does for living organisms |
|
Definition
| dissolving important molecules to render them mobile and available |
|
|
Term
| the type of covalent molecule water is |
|
Definition
|
|
Term
| why the polarity of water is important for biochemistry |
|
Definition
| because the polarity enables water to dissolve polar and charged molecules |
|
|
Term
| the type of bonding that occurs between water molecules |
|
Definition
|
|
Term
| molecules water can't dissolve |
|
Definition
|
|
Term
| the 3 fundamental noncovalent bonds |
|
Definition
1: ionic bonds / electrostatic interactions
2: H bonds
3: van der Waals interactions |
|
|
Term
|
Definition
| electrostatic interaction / ionic bond |
|
|
Term
|
Definition
| E = (kq1q2) / Dr
E = force
k = proportionality constant
q1 and q2 = charges on the 2 atoms
r = distance between 2 atoms (in Angstroms)
D = dielectric constant |
|
|
Term
| why NaCl dissolves in water |
|
Definition
| because the individual ions bind to the water instead of each other |
|
|
Term
| how to calculate the energy of an electrostatic interaction |
|
Definition
| Coulomb's law
E = (kq1q2) / Dr
E = force
k = proportionality constant
q1 and q2 = charges on the 2 atoms
r = distance between 2 atoms (in Angstroms)
D = dielectric constant |
|
|
Term
|
Definition
| between H and electronegative element |
|
|
Term
| the basis for van der Waals interactions |
|
Definition
| the distribution of electronic charge around an atom changes with time, and, at any instant, the charge distribution will not be perfectly symmetric; this creates momentary positive and negative |
|
|
Term
| why geckos can defy gravity |
|
Definition
| van der Waals interactions |
|
|
Term
| the second law of termodynamics |
|
Definition
| the total entropy of a system and its surroundings always increases in a spontaneous process |
|
|
Term
|
Definition
|
|
Term
|
Definition
| the aggregation of nonpolar groups in water increases the entropy in the water |
|
|
Term
| why nonpolar molecules congregate in water |
|
Definition
| because when they come into contact with each other, they release water molecules |
|
|
Term
|
Definition
| interactions driven by the hydrophobic effect |
|
|
Term
| depiction of how congregation of nonpolar molecules in water increases entropy |
|
Definition
|
|
Term
| membrane formation is powered by... |
|
Definition
|
|
Term
|
Definition
| molecule that has both a hydrophilic side and a hydrophobic side |
|
|
Term
|
Definition
| molecule that has both a hydrophilic side and a hydrophobic side |
|
|
Term
| the hydrophobic interior of the bilayer is stabilized by... |
|
Definition
| van der Waals interactions between the tails |
|
|
Term
| protein folding is powered by... |
|
Definition
|
|
Term
| why proteins can do so many things in living things |
|
Definition
| because they can form complex 3D structures that allow specific interactions with other biomolecules |
|
|
Term
|
Definition
| groups of atoms with distinct chemical properties |
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
| the hydroxyl functional group is found in... |
|
Definition
|
|
Term
| the aldehyde functional group is found in... |
|
Definition
|
|
Term
| the keto functional group is found in... |
|
Definition
|
|
Term
| the carboxyl functional group is found in... |
|
Definition
|
|
Term
| the amino functional group is found in... |
|
Definition
|
|
Term
| the phosphate functional group is found in... |
|
Definition
|
|
Term
| the sulfhydryl functional group is found in... |
|
Definition
|
|
Term
| why it's important for living things to maintain constant pH |
|
Definition
| because alterations in pH can drastically affect the internal electrostatic environment, of an organism, which can alter the weak bonds that maintain the structure of biomolecules; altered structure messes with function |
|
|
Term
| what water will ionize into |
|
Definition
|
|
Term
| the e'librium equation of water |
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
| Keq = [H+][OH-]/[H2O]
the brackets denote c'tration in molarity (M) |
|
|
Term
|
Definition
|
|
Term
|
Definition
| Kw = Keq X [H2O]
simplifies to...
Kw = [H+][OH-] |
|
|
Term
|
Definition
| pH = -log[H+]
or
pH = log(1/[H+]) |
|
|
Term
| acid is proton (donor or acceptor) |
|
Definition
|
|
Term
| base is proton (donor or acceptor) |
|
Definition
|
|
Term
| what happens to acid in solution? |
|
Definition
| ionizes to produce a proton and a base
acid <---> H+ + base |
|
|
Term
|
Definition
| the base that results when an acid dissociates in solution |
|
|
Term
|
Definition
| the acid that results when a base dissociates in solution |
|
|
Term
| ionization e'librium of a weak acid (HA) |
|
Definition
|
|
Term
| the e'librium constant (Ka) for HA |
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
| pH = pKa + log([A-]/[HA])
A- = ionized acid
HA = unionized acid
this is the Henderson-Hasselbach equation |
|
|
Term
| the Henderson-Hasselbach equation |
|
Definition
| pH = pKa + log([A-]/[HA])
A- = ionized acid
HA = unionized acid |
|
|
Term
|
Definition
| the pH at which the acid is half dissociated |
|
|
Term
| what's dominant above pKa? |
|
Definition
|
|
Term
| what's dominant below pKa? |
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
| in the vicinity of their pKa |
|
|
Term
| why knowledge of buffers is important |
|
Definition
1: biomolecules are sensitive to pH, so a good buffer is needed for a successful experiment
2: to understand how an organism controls its own pH |
|
|
Term
| compensatory respiratory alkalosis |
|
Definition
| mechanism by which the amount of carbonic acid and bicarbonate is adjusted in the blood in response to carbon dioxide |
|
|
