FINAL EXAM Biochem Flashcards
Classify animals, plants, protists, fungi, archaea and bacteria as prokaryotes or eukaryotes and identify the distingushing features of prokaryotic and eukaryotic cells.
Prokaryotes: bacteria and archea; features: unicellular organisms without a nucleus, few proteins associated with genome due to simplicity of the cell, replicate + adapt over small scale periods of time.
Eukaryotes: Animals, plants, and fungi (Kingdoms of eukarya); features: have more complex cellular organization with membrane enclosed organells that have specialized fxn’s.
Identify the domaines of life that include unicellular or multicellular organisms.
bacteria and archaea = unicellular
eukarya = multicellular organisms.
Recognise/ label biologically relevant organic conpounds and functional groups and identify the polarity and geometry of molecule
amine: RNH2 or RNH3+; R2NH or R2NH2+; R3N or R3NH+ (amino group is functional group)
alcohol: ROH fxnal group is hydroxyl group
thiol : RSH fxnal group is sulfhydryl group
ether: ROR fxnal group is ether linkage.
aldehyde: R-C=O-R(H) fxnal group (carbonyl group, acyl group)
ketone: R-C=O-R fxnal group (carbonyl group, acyl group)
Carboxylic acid R-C=O-OH or R-C=O-O(-),fxnal group: carboxyl or carboxylate groups.
Ester: R-C=O-OR fxnal groups: ester linkage.
Amide: R-C=O-HN2, R-C=O-NHR, R-C=O-NR2, fxnal group : amido group
Imine: R=NH or R=NH2+, R=NR or R=NHR+, fxnal group: imino group.
Phosphoric acid ester: fxnal group phosphoester linkage
Diphosphoric acid ester: fxnal group diphosphoryl group, pyrophosphoryl group.
recognize and describe the classes of biologcal monomer and related polymers
Bio monomers: amino acids, monosaccharides, nucleotides, lipids.
Bio polymers: polypeptides, polysaccharides, nucleic acids, lipids have no true polymer they just aggregate via non covalent interactions
AA’s: typically has N atom, generically has carboxylate group, side chain, amino group. Ex: Asparagrine, Cysteine
Monosaccharaides: have 1:1 ratio of carbon:oxygen ex: C6 H12O6 or C6 H13NO5
Nucleotides: Nitrogenous base and sugar. ex: ATP, DNA, RNA
Lipids: high ratio of carbon to oxygen/nitrogen/ phosphorus ex: C16H31O2 or C27H46O. anthropathic contain polar and nonpolar region that define behavior in solution.
Define polypeptide
protein
and residue
Polypeptide: polymers of amino acids linked together by peptide bonds.
Protein: functional unit consisting of one or more polypeptides.
Residue: a monomer that has been incorporated into a polymer. Monomers are covalently linked together to form different macromolecules. (typically via covalent bonds)
Describe the major and minor roles of biopolymers
major roles: proteins: carry out metabolic reactions & support cellular structures ; Nucleic acids: encode information, polysaccharides: store energy and support cellular structures.
minor roles: proteins: store energy : if emergent situation due to starvation body reverts to elastrophoric methods.; nucleic acids: carry out metabolic rxns & support cellular structures. polysaccharides: encode information (fxn used when cells have unique identifiers on the cell surface.
Distinguish open systems, isolated systems and closed systems
open systems: one in which energy can be transferred between the system and its surroundings.
isolated systems: a thermodynamic system that cannot exchange either energy or matter outside the boundaries of the system
closed systems: one that cannot transfer energy to its surroundings
Define Gibbs Free energy, enthalpy, and entropy and solve equations involving these values
Gibbs: Change in entropy + enthalpy, unfavorable reactions may be coupled with favorable reactions so that the overall process is spontaneous. Pi is inorganic phosphate, Glucose to glucosr 6 phosphate rxn coupled with ATP break down rxn –> net favorable rxn
Enthalpy: a measure of the heat energy of a reaction
Entropy: thermodynamic measure of randomness throughout a system.
Define endergonic, exergoinc, endothermic and exothermic.
endergonic: energy is conserved and used within the reaction (energy is necessary for the reaction to occur, non spontaneous process, positive delta G)
exergonic: energy is produced by the reaction, delta G is negative and reaction is spontaneous
endothermic: heat energy is used by the system, non spontaneous
exothermic: heat energy is released by the system, spontaneous.
Solve for the delta G of a coupled reaction given the delta G of individual reactions
practice
Determine if a process is spontaneous ( favorable/exergonic) based on its delta G
If delta G < 0, then a process is ‘spontaneous’, ‘favorable’ or ‘exergonic’
If delta G > 0, the a process is ‘nonspontaneous’, ‘unfavorable’ or ‘endergonic’
Identify whether a molecule is being oxidized or reduced in a reaction.
oxidation: loss of electrons, qualitatively look at whether the molecule gains oxygen, loses hydrogen, or goes from a single bond to a double bond. more favorable and can drive the synthesis of monomers and macromolecules.
reduction: gain of electrons, qualitatively look at whether the molecule loses oxygen, gains hydrogen, or goes from a double bond to a single bond.
ex: CO 2 least reduced most oxidized, Methane most reduced/ least oxidized.
Define catabolism and describe how the free energy of catabolic reactions may be conserved.
catabolism: breaking down larger molecules, involves oxidation steps (favorable), free energy may be conserved in the formation of NTPs (eg ATP or GTP) or reduction of cofactors.
ex: NADP+ + H+ 2e - –> NADPH / Q + 2H+ + 2e- –> QH2
Define anabolism and describe how the celll makes anabolic reactions thermodynamically favorable.
anabiolism: building complex molecules at the expense of energy. ex: ATP , NADPH
Describe how the molecular structure of water affects its physical properties as well as its interactions with other molecules.
Water’s bent structure results in a polar molecule that is strongly attracted to neighboring water molecules.
Hydrogen bonds ( dipole dipole IMF) occur when an H atom in a molecule, bound to a small highly electronegative atom with lone pairs of electrons, is attracted to the lone pair in another molecule
dipole allows water to interact w/ charged hydrophilic groups due to favorable electrostatic interactions
Describe and order by strength covalent bonds, ionic interactions, hydrogen bonds and van der waals interactions (dipole-dipole, dipole induced dipole, and london dispersion forces).
Strength order: Covalent bonds > ionic interaction > hydrogen bonding > Van der Waals : dipole-dipole > dipole induced dipole > London dispersion (london dispersion forces are surface area dependent (more important with larger molecules and atoms – > the larger the surface area, the higher the boiling point.
Define amphipathic (amphiphilic) molecules and describe how they behave in aqueous solutions.
amphipathic molecules: aggregate (stick together) in water with the charged heads interacting with water and the hydrophobic nonpolar tails staying away from water
Define bronsted lowry acids, bases, conjugate acids, conjuate bases and neutral pH.
B-L acid : a proton donor
B-L base : a proton acceptor
CA : the acid that results from the B-L base
CB : the base that results from the B-L acid
neutral pH : has a value of 7 on 0-14 acid scale.
explain the hydrophobic effect
a process where nonpolar regions clusters together to maximize the entropy of the surrounding water molecules.
driving force in hydrophobic molecules: the more disordered lipid molecules the more favorable the reaction, there is an increase in entropy w/in the system.
intrepret and draw titration curves
at the flat curve, the acid and base are at equilirium
Describe a buffered solution and discuss its effective range
Buffered solutions need to be enough of both weak acid and congjugate base present to be effective. A buffer is a weak acid/base solution that resists changes in pH. useful when there is a +/- 1 pH/pKa value.
Describe the equilibrium of bicarbonate buffering system in the blood and explain how it maintians the blood pH close to 7.40
acidosis: a condition where blood pH is too low
Alkalosis: a condition where blood pH is too high.
Normal conditions; H+ + HCO3- = H2CO3 = H2O + CO2
Excess acid: H+ + HCO3- –> H2CO3 = H2O + CO2 ; H+ + HCO3- = H2CO3 –> H20 + CO2 ; H+ + HCO3 = H2CO3 = H2O + CO2
Insufficent acid: H+ + HCO3- = H2CO3 <– H2O +CO2 ; H+ + HCO3- <– H2CO3 = H2O + CO2 ; H+ + HCO3- = H2CO3 = H2O + CO2
Define acidosis and alkalosis and eplain how kidney and lung function can affect blood pH
Acidosis: a condition where blood pH is too low
Alkalosis: a condition where blood pH is too high.
Metabolic processes generate H+ , Kidney and lung fxn helps maintin a blood pH of 7.4.
Kidneys ususally retain HCO3- while eliminating H+ to prevent acidosis
Lungs breathe faster to raise blood pH and slow breathing to lower blood pH.
Carbonoic anhydrase speeds up the interconversion of HCO3- + H+ with H2O + CO2.
Label given structes as purine or pyrimidine nitrogenous bases
purine: Adenine, Guanine
pyrimidine: Cytosine, Thymine, Uracil