Introduction to Biochemistrylibvolume2.xyz/biotechnology/semester4/biochemical...08/21/08...
Transcript of Introduction to Biochemistrylibvolume2.xyz/biotechnology/semester4/biochemical...08/21/08...
08/21/08 Biochemistry: Introduction 1
Introduction to Biochemistry
Andy Howard
Biochemistry, Fall 2008
IIT
08/21/08 Biochemistry: Introduction p. 2 of 62
What is biochemistry?
� By the end of this course you should
be able to construct your own
definition; but for now:
� Biochemistry is the study of
chemical reactions in living tissue.
08/21/08 Biochemistry: Introduction p. 3 of 62
Plans
� What is biochemistry?
� Cells
� Cell components
� Organic and biochemistry
� Concepts from organic chemistry to remember
� Small molecules and macromolecules
� Classes of small
molecules
� Classes of
macromolecules
� Water
� Catalysis
� Energetics
� Regulation
� Molecular biology
� Evolution
08/21/08 Biochemistry: Introduction p. 4 of 62
What will we study?
� Biochemistry is the study of chemical
reactions in living tissue, both within cells and
in intercellular media.
� As such, it concerns itself with a variety of
specific topics:
08/21/08 Biochemistry: Introduction p. 5 of 62
Topics in biochemistry
� What reactions occur;
� The equilibrium energetics and kinetics of those
reactions;
� How the reactions are controlled, at the chemical and
cellular or organellar levels;
� How the reactions are organized to enable biological function within the cell and in tissues and organisms.
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Organic and biological chemistry
� Most molecules in living things
(other than H2O, O2, and CO2)
contain C-C or C-H bonds, so
biochemistry depends heavily on
organic chemistry
� But the range of organic reactions
that occur in biological systems is
fairly limited compared to the full
range of organic reactions:
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Why we use only a subset of
organic chemistry in biochemistry
� Biochemical reactions arealmost always aqueous.
� They occur within a narrow temperature and pressure range.
� They occur within narrowly buffered pH ranges.
� Many of the complex reaction mechanisms discovered and exploited by organic chemists since the 1860's have no counterparts in the biochemical universe.
Frederich
Wöhler
08/21/08 Biochemistry: Introduction p. 8 of 62
Cells
� Most biochemical reactions (but not all!) take place within semi-independent biological entities known as cells
� Cells in general contain replicative and protein-synthetic machinery in order to reproduce and survive
� They often exchange nutrients and information with other cells
08/21/08 Biochemistry: Introduction p. 9 of 62
Cell components
� Cells are separated from their
environments via a selectively porous
membrane
� Individual components (often called
organelles) within the cell may also
have membranes separating them from
the bulk cytosol and from one another
08/21/08 Biochemistry: Introduction p. 10 of 62
Eukaryotes and prokaryotes
� The lowest-level distinction among organisms is on the basis of whether their cells have defined nuclei or not
� Cells with nuclei are eukaryotic
� Cells without nuclei are prokaryotic
� Eubacteria and archaea are prokaryotic
� Other organisms (including some unicellular ones!) are eukaryotic
08/21/08 Biochemistry: Introduction p. 11 of 62
Eukaryotic organelles I
� Nucleus: contains genetic information; site for replication and transcription
� Endoplasmic reticulum: site for protein synthesis and protein processing
� Ribosome: protein-synthetic machine
� Golgi apparatus: site for packaging proteins for secretion and delivery
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Eukaryotic organelles II
� Mitochondrion: site for most energy-producing reactions
� Lysosome: digests materials during endocytosis and cellular degradation
� Peroxisome: site for oxidation of some nutrients and detoxification of the H2O2
created thereby
� Cytoskeleton: network of filaments that define the shape and mobility of a cell
08/21/08 Biochemistry: Introduction p. 13 of 62
Eukaryotic organelles III
� Chloroplast: site for most photosynthetic reactions
� Vacuoles: sacs for water or other nutrients
� Cell wall: bacterial or plant component outside cell membrane that provides rigidity and protection against osmotic shock
08/21/08 Biochemistry: Introduction p. 14 of 62
Concepts from organic chemistry
� There are some elements of organic
chemistry that you should have clear in your
minds.
� All of these are concepts with significance
outside of biochemistry, but they do play
important roles in biochemistry.
� If any of these concepts is less than
thoroughly familiar, please review it:
08/21/08 Biochemistry: Introduction p. 15 of 62
Organic
concepts I
� Covalent bond: A strong attractive interaction between neighboring atoms in which a pair of electrons is roughly equally shared between the two atoms.– Covalent bonds may be single bonds, in which
one pair of electrons is shared; double bonds, which involve two pairs of electrons; or triple bonds, which involve three pairs (see above).
– Single bonds do not restrict the rotation of other substituents around the bond; double and triple bonds do.
Image courtesy Michigan State U.
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Organic concepts II
� Ionic bond: a strong
attractive interaction
between atoms in
which one atom or
group is positively charged, and another
is negatively charged.
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Organic concepts III
� Hydrogen bond: A weak attractive
interaction between neighboring atoms in
which a hydrogen atom carrying a slight,
partial positive charge shares that positive
charge with a neighboring electronegative atom.
– The non-hydrogen atom to which the hydrogen
is covalently bonded is called the hydrogen-
bond donor;
– the neighboring atom that takes on a bit of the
charge is called the hydrogen-bond acceptor
Cartoon
courtesy
CUNY
Brooklyn
08/21/08 Biochemistry: Introduction p. 18 of 62
Organic
concepts IV
� Van der Waals
interaction:
A weak attractive
interaction between
nonpolar atoms,
arising from
transient induced
dipoles in the two
atoms. Image courtesy
Columbia U. Biology Dept.
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Organic
Concepts V
� Chirality: The property of
a molecule under which it
cannot be superimposed
upon its mirror image.
Image courtesy DRECAM, France
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Organic
Concepts VI
� Tautomerization: The interconversion of two
covalently different forms of a molecule via a
unimolecular reaction that proceeds with a low
activation energy. The two forms of the molecule
are known as tautomers: because of the low activation barrier between the two forms, we will
typically find both species present.
acetonepropen-2-ol
08/21/08 Biochemistry: Introduction p. 21 of 62
Organic Concepts
VII
� Nucleophilic substitution: a reaction in which an electron-rich (nucleophilic) molecule attacks an electron-poor (electrophilic) molecule and replaces group or atom within the attacked species.
– The displaced group is known as a leaving group.
– This is one of several types of substitution reactions, and it occurs constantly in biological systems.
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Organic Concepts VIII
� Polymerization: creation of large
molecules by sequential addition of simple
building blocks
– often by dehydration, i.e., the elimination of
water from two species to form a larger one:
R1-O-H + HO-R2-X-H → R1-X-R2-OH + H2O
– The product here can then react with
HO-R3-X-H to form
R1-X-R2-X-R3-OH with elimination of another water molecule, and so on.
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Organic Concepts IX
� Equilibrium: in the context of a chemical reaction, the state in which the concentrations of reactants and products are no longer changing with time because the rate of reaction in one direction is equal to the rate in the opposite direction.
� Kinetics: the study of the rates at which reactions proceed.
� Conventionally, we use the term thermodynamics to describe our understanding of the energetics of equilibriumsystems
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Organic Concepts X
� Catalysis: the lowering of the energetic barrier
between substrates and products in a reaction by the
participation of a substance that ultimately is
unchanged by the reaction
– It is crucial to recognize that catalysts (chemical agents that
perform catalysis) do not change the equilibrium position of
the reactions in which they participate:
– they only change the rates (the kinetics) of the reactions they
catalyze.
� Zwitterion: a compound containing both a positive
and a negative charge
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Classes of small molecules
� Small molecules other than water make up a small percentage of a cell's mass, but small molecules have significant roles in the cell, both on their own and as building blocks of macromolecules. The classes of small molecules that play significant roles in biology are listed below. In this list, "soluble" means "water-soluble".
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iClicker quiz (for attendance)
� How many midterms will we have?
� (a) 1
� (b) 2
� (c ) 3
� (d) 4
� (e) I don’t care.
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Biological small molecules I
� Water: Hydrogen hydroxide. In liquid form in
biological systems. See below.
� Lipids: Hydrophobic molecules, containing
either alkyl chains or fused-ring structures. A
biological lipid usually contains at least one
highly hydrophobic moeity.
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Biological small molecules II
� Carbohydrates: Polyhydroxylated
compounds for which the building
blocks are highly soluble.
– The typical molecular formula for the
monomeric forms of these compounds is
(CH2O)n, where 3 < n < 9,
– but usually n = 5 or 6.
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Biological small molecules III
� Amino acids: Compounds containing an
amine (NH3+) group and a carboxyl (COO-)
group.
� The most important biological amino acids are α-amino acids, in which the amine
group and the carboxyl group are separated
by one carbon, and that intervening carbon
has a hydrogen attached to it. Thus the
general formula for an α-amino acid is
� H3N+ - CHR - COO-
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Biological small
molecules IV
� Nucleic acids: Soluble compounds that
include a nitrogen-containing ring system.
– The ring systems are derived either from purine or
pyrimidine.
– The most important biological nucleic acids are those in which the ring system is covalently
attached to a five-carbon sugar, ribose, usually
with a phosphate group attached to the same
ribose ring.
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Small molecules V
� Inorganic ions: Ionic species containing no carbon but containing one or more atoms and at least one net charge.
– Ions of biological significance includeCl-, Na+, K+, Mg+2, Mn+2, I-, Ca+2, PO4
-3, SO4-2,
NO3-, NO2
-, and NH4+.
– Phosphate (PO4-3) is often found in partially
protonated forms HPO4-2 and H2PO4
-
– Ammonium ions occasionally appear as neutral ammonia (NH3), particularly at higher pH values
08/21/08 Biochemistry: Introduction p. 32 of 62
Biological Small Molecules VI
� Cofactors: This is a catchall category for organic small molecules that serve in some functional role in biological organisms. Many are vitamins or are derived from vitamins; a vitamin is defined as an organic molecule that is necessary for metabolism but cannot be synthesized by the organism. Thus the same compound may be a vitamin for one organism and not for another.
� Ascorbate (vitamin C) is a vitamin for humans and guinea pigs but not for most other mammals.
� Cofactors often end up as prosthetic groups, covalently or noncovalently attached to proteins and involved in those proteins' functions.
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Biological
macromolecules
� Most big biological
molecules are polymers, i.e.
molecules made up of large
numbers of relatively simple
building blocks.
� Cobalamin is the biggest
nonpolymeric biomolecule I
can think of (MW 1356 Da)
Structure
courtesy
Wikimedia
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Categories of biological polymers
� Proteins
� Nucleic acids
� Polysaccharides
� Lipids (sort of):
– 2-3 chains of aliphatics attached to a
polar head group, often built on glycerol
– Aliphatic chains are usually 11-23 C’s
08/21/08 Biochemistry: Introduction p. 35 of 62
Polymers and oligomers
� These are distinguished only by the
number of building-blocks contained
within the multimer
� Oligomers: typically < 50 building
blocks
� Polymers ≥≥≥≥ 50 building blocks.
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Categories of biopolymers
Category # mono-
mers
<mol wt/
monomer>
# mono-
mers
Branch-
ing?
Protein 20 110 65-5000 no
RNA 4-10 220-400 50-15K no
DNA 4 200-400 50-106 no
Polysac-
charide
~10 180 2-105 Some-
times
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Water: a complex substance
� Oxygen atom is covalently bonded to 2
hydrogens
� Single bond character of these bonds means
the H-O-H bond angle is close to 109.5º =
acos(-1/3): actually more like 104.5º
� This contrasts with O=C=O (angle=180º) or
urea ((NH2)2-C=O) (angles=120º)
� Two lone pairs available per oxygen:
these are available as H-bond acceptors
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Water is polar
� Charge is somewhat unequally shared
� Small positive charge on H’s (δδδδ+); small
negative charge on O (2δδδδ-) (Why?)
� A water molecule will orient itself to align
partial negative charge on one molecule
close to partial positive charges on
another.
� Hydrogen bonds are involved in this.
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Liquid water is mobile
� The hydrogen-bond networks
created among water molecules
change constantly on a sub-
picosecond time scale
� At any moment the H-bonds look like
those in crystalline ice
� Solutes disrupt the H-bond networks
08/21/08 Biochemistry: Introduction p. 40 of 62
Water in reactions
� Water is a medium within which reactions occur;
� But it also participates in reactions
� Enzymes often function by making water oxygen atoms better nucleophiles or water H’s better electrophiles
� Therefore water is a direct participant in reactions that wouldn’t work in a nonenzymatic lab setting!
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Water’s physical properties
� High heat capacity:
stabilizes temperature in living
things
� High surface tension
� Nearly incompressible (density
almost independent of pressure)
� Density max at 3.98ºC
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Catalysis
� Catalysis is the lowering of the activation energy barrier between reactants and products
� How?
– Physical surface on which reactants can be exposed to one another
– Providing moieties that can temporarily participate in the reaction and be restored to their original state at the end
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Biological catalysts
� 1890’s: Fischer realized that there had to be catalysts in biological systems
� 1920’s: Sumner said they were proteins
� It took another 10 years forthe whole community to accept that
� It’s now known that RNA can be catalytic too:
– Can catalyze modifications in itself
– Catalyzes the key step in protein synthesis in the ribosome
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Energy in biological systems
� We distinguish between
thermodynamics and kinetics:
� Thermodynamics characterizes the
energy associated with equilibrium
conditions in reactions
� Kinetics describes the rate at which a
reaction moves toward equilibrium
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Thermodynamics
� Equilibrium constant is a measure of the ratio of product concentrations to reactant concentrations at equilibrium
� Free energy is a measure of the available energy in the products and reactants
� They’re related by ∆∆∆∆Go = -RT ln Keq
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Kinetics
� Rate of reaction is dependent on Kelvin temperature T and on activation barrier ∆G‡
preventing conversion from one site to the other
� Rate = Qexp(-∆G‡/RT)
� Job of an enzyme is to reduce ∆G‡
Svante Arrhenius
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Regulation
� Biological reactions are regulated in the
sense that they’re catalyzed by enzymes, so
the presence or absence of the enzyme
determines whether the reaction will proceed
� The enzymes themselves are subject to
extensive regulation so that the right
reactions occur in the right places and times
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Typical enzymatic regulation
� Suppose enzymes are involved in converting A to
B, B to C, C to D, and D to F. E is the enzyme that
converts A to B:
(E)
A →→→→ B →→→→ C →→→→ D →→→→ F
� In many instance F will inhibit (interfere) with the
reaction that converts A to B by binding to a site
on enzyme E so that it can’t bind A.
� This feedback inhibition helps to prevent
overproduction of F—homeostasis.
08/21/08 Biochemistry: Introduction p. 49 of 62
Molecular biology
� This phrase means something much more
specific than biochemistry:
� It’s the chemistry of replication, transcription,
and translation, i.e., the ways that genes are
reproduced and expressed.
� Most of you have taken biology 214 or its
equivalent; we’ll review some of the contents
of that course here, mostly near the end of the
semester.
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The molecules of
molecular biology
� Deoxyribonucleic acid: polymer; backbone is
deoxyribose-phosphate; side chains are
nitrogenous ring compounds
� RNA: polymer; backbone is ribose-
phosphate; side chains as above
� Protein: polymer: backbone is
NH-(CHR)-CO; side chains are 20
ribosomally encoded styles
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Steps in molecular biology:
the Central Dogma
� DNA replication (makes accurate copy of
existing double-stranded DNA prior to
mitosis)
� Transcription (RNA version of DNA message
is created)
� Translation (mRNA copy of gene serves as
template for making protein: 3 bases of RNA
per amino acid of synthesized protein)
08/21/08 Biochemistry: Introduction p. 52 of 62
Evolution and Taxonomy
� Traditional studies of interrelatedness of
organisms focused on functional similarities
� This enables production of phylogenetic trees
� Molecular biology provides an alternative,
possibly more quantitative, approach to
phylogenetic tree-building
� More rigorous hypothesis-testing possible
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Quantitation
� Biochemistry is a quantitative science.
� Results in biochemistry are rarely significant unless
they can be couched in quantifiable terms.
� Thermodynamic & kinetic behavior of biochemical
systems must be described quantitatively.
� Even the descriptive aspects of biochemistry, e.g. the compartmentalization of reactions and metabolites
into cells and into particular parts of cells, must be
characterized numerically.
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Mathematics in biochemistry
� Ooo: I went into biology rather than
physics because I don’t like math
� Too bad. You need some here:
but not much.
� Biggest problem in past years:
exponentials and logarithms
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Exponentials
� Many important biochemical equations are expressed in the formY = ef(x)
� O which can also be writtenY = exp(f(x))
� The number e is the base of the natural logarithm system and is, very roughly, 2.718281828459045
� I.e., it’s 2.7 1828 1828 45 90 45
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Logarithms
� First developed as computational tools because they convert multiplication problems into addition problems
� They have a fundamental connection with raising a value to a power:
� Y = xa ⇔ logx(Y) = a
� In particular, Y = exp(a) = ea⇔
lnY = loge(Y) = a
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Algebra of logarithms
� logv(A) = logu(A) / logu(v)
� logu(A/B) = logu(A) - logu(B)
� logu(AB) = Blogu(A)
� log10(A) = ln(A) / ln(10)= ln(A) / 2.30258509299= 0.4342944819 * ln(A)
� ln(A) = log10(A) / log10e= log10(A) / 0.4342944819= 2.30258509299 * log10(A)
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Course structure
� Two midterms plus a final
� All exams will be closed-book, closed-notes exams. Calculators are not allowed.
� Each exam will be accompanied by a help-sheet with many helpful facts
� Gauge your memorization with the help-sheet before you: what’s on the help sheet doesn’t need to be memorized
� My exams tend to be long but easy:budget your time carefully!
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Grading
� I’m a moderately tough grader, but I do curve this course
� The cutoff for an A is likely to be around an 82, but it’s uncertain
� Homework, literature assignments, iClicker quizzes, and discussion-board participation count
� Internet students will get a substitute assignment to replace iClicker quizzes
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Textbook and Lecture Notes
� Garrett & Grisham is a detail-rich and well-written text: read it!
� Many of my lectures are derived from Horton et al rather than from Garrett & Grisham, particularly in the version that I’ve already posted to the Internet
� Be prepared for the lecture notes themselves to evolve during the course
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Office Hours
� I should be available 3:30-5pm
Tuesdays and Thursdays in most cases
� If that doesn’t work, make an
appointment
� The discussion board is another good
way to reach me and the rest of the
class as well!
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Assignments
� Regular homeworks will be due weekly,
probably on Fridays
� But no assignment due tomorrow
� Literature assignments are due weekly,
probably on Tuesdays
� Specific readings already posted will be
augmented but not deleted