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Cellular and Molecular Biology > Exam 1: Ch 2 > Flashcards

Exam 1: Ch 2 Flashcards

(65 cards)

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1
Q

water constitutes what % by weight of cells

A

70-80%

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2
Q

amphipathic

A

molecules with hydrophilic and hydrophobic regions

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3
Q

covalent bond

A

strongest bond

when 2 atoms share electrons

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4
Q

types on noncovalent interaction

A

ionic bonds

hydrogen bonds

van der waals forces

hydrophobic effect

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5
Q

most abundant elements in biological molecules

A

carbon, hydrogen, oxygen, nitrogen, sulfur, phosphorus

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6
Q

chirality

A

asymmetric carbon with 4 different groups around it

makes stereoisomers

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7
Q

biochemistry stereoisomers

A

different arrangement = different molecule

different biological functions b/c arrangement differences cause them to interact with the body differently

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8
Q

dipole moment

A

measure of the strength or extent of charge separation

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9
Q

molecular complementarity

A

lock and key fit of shapes, charges, or other physical properties of molecules

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10
Q

3 main types of biological macromolecules

A

protein

nucleic acids

polysacharides

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11
Q

phosphodiester bonds

A

link nucleotides together

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12
Q

purines

A

adenine

guanine

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13
Q

pyrimidines

A

cytosine

thymine

uracil

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14
Q

nucleoside

A

combination of a base/sugar without a phosphate

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15
Q

carbohydrate

A

covalently bonded combinations of carbon and water in a one to one ratio

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16
Q

glycogen

A

storage of carbohydrate in animal cells

very long highly branched polymer of glucose

10% of liver

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17
Q

what is starch, and its 2 forms

A

storage form of carbohydrate in plants

amylose - unbranched

amylopectin - branched

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18
Q

cullulose

A

major consituent of plant cell walls

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19
Q

peptidoglycan

A

polysaccharide chain cross linked by peptide bridges

rigidity and cell shape

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20
Q

glycosaminoglycans

A

major polysaccharide components of ECM

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21
Q

enthalpy and entropy

A

enthalpy: bond energy
entropy: measure of randomness or disorder

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22
Q

carbon fixation

A

ATP is hydrolyzed to provide energy for conversion of CO2 to hexoses

these sugars are food sources for the plants

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23
Q

oxidation of glucose rxn

A

C6H12O6 + 6 O2 –> 6CO2 + 6H2O

-686 kcal/mol

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24
Q

purpose of coenzymes NAD+ and FAD

A

electron carrying

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25
electronegativity
how well an atom can attract an electron
26
van der waals interactions
nonspecific interactions resulting from the momentary random fluctuations in the distribution of the elections of any atom strength of interaction decreases rapidly with distance
27
acetylation
most common chemical modification of a protein 80% play an important role in controlling the life span of proteins nonacetylated proteins are rapidly degraded
28
fatty acid
hydrocarbon chain attached to a carboxyl group important energy source esterified with phosphates to form phospholipids
29
microscopic reversibility
ability of a reaction to go backwards slow at first, but speeds up as concentration of product increases
30
chemical equilibrium
rates of forward and reverse reactions are equal so concentrations of reactants and products stop changing
31
equilibrium constant
Keq is a fixed value that measures the extent to which a rxn occurs by the time it reaches equilibrium
32
standard biological conditions
1atm, 25 celcius
33
steady state
system of linked reactions where production and consumption of products is steady helps prevent accumulation of potentially toxic intermediates
34
dissociation constant
the reciprocal of the equilibrium constant that describes binding reactions when half the protein molecules are bound, the concentration of protein is equal to the Kd
35
what do high and low Kds mean
lower Kd means tighter binding: less protein is needed to bind half of its ligand higher Kd is less tight binding: more protein is needed to bind half of its ligand
36
what is Kd measured in
molarity moles/L
37
pH
concentration of hydrogen ions in solution negative log of hydrogen ion concentration pure H2O is 7
38
1 unit difference in pH represents how many fold difference in proton concentration?
tenfold
39
zwitterion
a molecule that has an equal number of positive and negative charge they are neutral amino acids are zwitterions (amino end and carboxyl end cancel each other out)
40
Ka
equilibrium constant for acid dissociation HA --> H+ + A- Ka = [H+][A-] / [HA] high Ka = low pKa (stronger acid)
41
Henderson Hasselbach
pKa of any acid is equal to the pH when half the molecules are dissociated and half are not pH = pKa + log [A-] / [HA] because when [A-] = [HA], log [A-] / [HA] is 0 and then pH = pKa
42
buffer
a reservoir of weak acids and bases that maintain a stable pH by soaking up excess H+ or OH- must be within 1 pH unit
43
buffering capacity
ability of a buffer to minimize changes in pH depends on the concentration of the buffer and the relationship between its pKa and pH
44
if pH > pKa
A- dominates disassociation occurs
45
if pH < pKa
HA dominates no disassociation occurs
46
kinetic energy
energy of movement
47
potential energy
stored energy ex. covalent bonds
48
thermal energy
form of kinetic energy: the energy of the motion of molecules to perform work flows from higher temp to lower temp
49
radient energy
kinetic energy of photons converted to thermal energy when light is absorbed and moves molecules change electronic structure of a molecule by moving an electron into a higher energy orbital (photosynthesis)
50
mechanical energy
form of kinetic energy can result from the conversion of chemical energy
51
electric energy
form of kinetic energy energy of moving electrons
52
chemical potential energy
energy stored in bonds connecting atoms in molecules harnessed to do work ex. ATP
53
concentration gradient and electric potential
ex. ions of different sides of the membrane form [ ] gradient energy of charge separation occurs on diff sides of membrane too
54
unit of energy
joule or calorie 1 joule = 0.239 calorie
55
calorie
energy required to raise temp of 1 gram of water by 1 celcius
56
exergonic
energy releasing rxn products contain less energy than reactants
57
endergonic
energy absorbing rxn products contain more energy than reactants
58
gibbs free energy
all systems change to minimize free energy describes whether or not the products contain more or less energy than reactants enthalpy is bond energy entropy is a measure of disorder or randomness
59
units of gibbs free energy
kilocalorie/mol
60
delta g from standard free energy (delta g not prime)
delta g = standard delta g + RTlnKeq
61
delta g not prime from Keq
delta g not prime = -2.3RTlogKeq
62
transition state
time when system in rxn is at its highest energy level activation energy is E needed to overcome t.s
63
reduction potential (E) vs. oxidation potential
reduction potential: ease an atom or molecule gains an electron oxidation potential: ease an atom or molecule loses an electron both measured in volts
64
in redox rxns electrons move spontaneously toward atoms or molecules with a more _____ reduction portential
positive
65
electric potential delta E
delta G = -n delta E measured in volts

Cellular and Molecular Biology (34 decks)

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