ABI 102 Exam 1

Acidemia

decreased pH in blood

Alkalemia

increased pH in blood

Acidosis

a condition characterized by an increased concentration of hydrogen ions, leading to a decrease in blood pH. (acidemia)

Alkalosis

a conditioncharacterized by a decreased concentration of hydrogen ions, leading to an increase in blood pH. (alkalemia)

hypercapnia

excess CO2 in blood

hypocapnia

deficiency of CO2 in blood

pH

a measure of the acidity or alkalinity of a solution, -log[H+]

Large Ka

products of dissociation are favored; acid is largely dissociated (strong acid)

Small Ka

undissociated acid favored, very little acid dissociated (weak acid)

good buffering capacity

Ability to resist pH changes or addition of acid or base, max when pKa = pH

good’s buffer

• pKa between 6 and 8

• should not absorb wavelengths >230

• Soluble in water

• membrane impermeability

• minimal effects from salt, changes in temperature and concentrations

polyprotic acids

acids capable of losing more than one proton per molecule in an acid base reation

acid

compound that can donate a proton, [H+]>10^-7M, [OH]<10^-7M

base

compound that can accept a proton

Henderson Hasselbalch Equation

pH=pKA-log[A-/HA], relates the pH of a solution of a weak acid to the pKa and te concentrations of the acid and its conjugate base

peptide bonds

covalent bonds formed between amino acids, rigid and planar, partial double-bond character

gene duplication

genetic recombination event leads to a second copy of the gene, a duplicate, in the genome

paralogous genes

genes evolved independently and one gains a new function

tertiary structure

the three-dimensional form of an entire polypeptide, including its side chains

secondary structure

local spacial arrangement of a polypeptides backbone atoms

thermodynamics

a study of the relationships among the various forms of energy and how energy affects matter

open system

can exchange matter and energy with surroundings

closed system

can exchange energy with surroundings but not matter

isolated system

cannot exchange matter and energy with surroundings

isolated system

doesn’t exchange energy or matter with surroundings

open system

exchanges energy and matter with surroundings

first law of thermodynamics

energy can neither be created nor destroyed

q

heat absorbed by the system from the surroundings

w

work done on the system by the surroundings

exothermic

system releases heat -q

endothermic

system gains heat +q

enthapy

heat generated or used by the system, depends only upon the state of the system and not on the way in which the system acquired the state

Hess’s Law

regardless of the multiple stages of steps of a reaction, the total enthalpy change for the reaction is the sum of all changes

second law of thermodynamics

the total entropy or disorder of an isolated system can never decrease over time; it can only increase or remain constant.

essential amino acids

Phe, Val, Thr, Trp, Ile, Met, His, Leu, Lys

nonessential amino acids

G=H-tS

the Gibbs free energy equation, which relates enthalpy (H), temperature (T), and entropy (S) to predict spontaneity of reactions.

Isoelectric Point

The pH at which a molecule carries no net electric charge
pI = 1/2 (pKi + pKj)