Introduction to Biochemistry Andy Howard Biochemistry Lectures Fall
Introduction to Biochemistry Andy Howard Biochemistry Lectures, Fall 2010 IIT 01/11/10 Biochemistry: Introduction 1
What is biochemistry? l By the end of this course you should be able to construct your own definition; but for now: l Biochemistry is the study of chemical reactions in living tissue. 01/11/10 Biochemistry: Introduction 2
Plans l l l What is biochemistry? Cells Cell components Organic and biochemistry Concepts from organic chemistry to remember Small molecules and macromolecules 01/11/10 l l l l Biochemistry: Introduction Classes of small molecules Classes of macromolecules Water Catalysis Energetics Regulation Molecular biology Evolution 3
What will we study? Biochemistry is the study of chemical reactions in living tissue, both within cells and in intercellular media. l As such, it concerns itself with a variety of specific topics: l 01/11/10 Biochemistry: Introduction 4
Topics in biochemistry What reactions occur; l The equilibrium energetics and kinetics of those reactions; l How the reactions are controlled, at the chemical and cellular or organellar levels; l How the reactions are organized to enable biological function within the cell and in tissues and organisms. l 01/11/10 Biochemistry: Introduction 5
Organic and biological chemistry Most molecules in living things (other than H 2 O, O 2, and CO 2) contain C-C or C-H bonds, so biochemistry depends heavily on organic chemistry l But the range of organic reactions that occur in biological systems is fairly limited compared to the full range of organic reactions: l 01/11/10 Biochemistry: Introduction 6
Why we use only a subset of organic chemistry in biochemistry Biochemical reactions are almost always aqueous. Frederich l They occur within a narrow temperature and Wöhler pressure range. l They occur within narrowly buffered p. H ranges. l Many of the complex reaction mechanisms discovered and exploited by organic chemists since the 1860's have no counterparts in the biochemical universe. l 01/11/10 Biochemistry: Introduction 7
Cells l Most biochemical reactions (but not all!) take place within semi-independent biological entities known as cells l Cells in general contain replicative and protein-synthetic machinery in order to reproduce and survive l They often exchange nutrients and information with other cells 01/11/10 Biochemistry: Introduction 8
Cell components l Cells are separated from their environments via a selectively porous membrane l Individual components (often called organelles) within the cell may also have membranes separating them from the bulk cytosol and from one another 01/11/10 Biochemistry: Introduction 9
Eukaryotes and prokaryotes l The lowest-level distinction among organisms is on the basis of whether their cells have defined nuclei or not l Cells with nuclei are eukaryotic l Cells without nuclei are prokaryotic l Eubacteria and archaea are prokaryotic l Other organisms (including some unicellular ones!) are eukaryotic 01/11/10 Biochemistry: Introduction 10
Eukaryotic organelles I l Nucleus: contains genetic information; site for replication and transcription l Endoplasmic reticulum: site for protein synthesis and protein processing l Ribosome: protein-synthetic machine l Golgi apparatus: site for packaging proteins for secretion and delivery 01/11/10 Biochemistry: Introduction 11
Eukaryotic organelles II Mitochondrion: site for most energyproducing reactions l Lysosome: digests materials during endocytosis and cellular degradation l Peroxisome: site for oxidation of some nutrients and detoxification of the H 2 O 2 created thereby l Cytoskeleton: network of filaments that define the shape and mobility of a cell l 01/11/10 Biochemistry: Introduction 12
Eukaryotic organelles III l Chloroplast: site for most photosynthetic reactions l Vacuoles: sacs for water or other nutrients l Cell wall: bacterial or plant component outside cell membrane that provides rigidity and protection against osmotic shock 01/11/10 Biochemistry: Introduction 13
Concepts from organic chemistry There are some elements of organic chemistry that you should have clear in your minds. l All of these are concepts with significance outside of biochemistry, but they do play important roles in biochemistry. l If any of these concepts is less than thoroughly familiar, please review it: l 01/11/10 Biochemistry: Introduction 14
Organic concepts I Image courtesy Michigan State U. l 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. 01/11/10 Biochemistry: Introduction 15
Organic concepts II l Ionic bond: a strong attractive interaction between atoms in which one atom or group is positively charged, and another is negatively charged. 01/11/10 Biochemistry: Introduction 16
Organic concepts III l 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. Cartoon courtesy CUNY Brooklyn – The non-hydrogen atom to which the hydrogen is covalently bonded is called the hydrogenbond donor; – the neighboring atom that takes on a bit of the charge is called the hydrogen-bond acceptor 01/11/10 Biochemistry: Introduction 17
Organic concepts IV l Van der Waals interaction: A weak attractive interaction between nonpolar atoms, arising from transient induced dipoles in the two atoms. 01/11/10 Image courtesy Columbia U. Biology Dept. Biochemistry: Introduction 18
Organic Concepts V l Chirality: The property of a molecule under which it cannot be superimposed upon its mirror image. Image courtesy DRECAM, France 01/11/10 Biochemistry: Introduction 19
Organic Concepts VI l acetone propen-2 -ol 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. 01/11/10 Biochemistry: Introduction 20
Organic Concepts VII l 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. 01/11/10 Biochemistry: Introduction 21
Organic Concepts VIII l 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: R 1 -O-H + HO-R 2 -X-H R 1 -X-R 2 -OH + H 2 O – The product here can then react with HO-R 3 -X-H to form R 1 -X-R 2 -X-R 3 -OH with elimination of another water molecule, and so on. 01/11/10 Biochemistry: Introduction 22
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. l Kinetics: the study of the rates at which reactions proceed. l Conventionally, we use the term thermodynamics to describe our understanding of the energetics of equilibrium systems l 01/11/10 Biochemistry: Introduction 23
Organic Concepts X l 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. l Zwitterion: a compound containing both a positive and a negative charge 01/11/10 Biochemistry: Introduction 24
Classes of small molecules l 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". 01/11/10 Biochemistry: Introduction 25
i. Clicker quiz (for attendance) How many midterms will we have? l (a) 1 l (b) 2 l (c) 3 l (d) 4 l (e) I don’t care. 01/11/10 Biochemistry: Introduction 26
Biological small molecules I Water: Hydrogen hydroxide. In liquid form in biological systems. See below. l Lipids: Hydrophobic molecules, containing either alkyl chains or fused-ring structures. A biological lipid usually contains at least one highly hydrophobic moeity. l 01/11/10 Biochemistry: Introduction 27
Biological small molecules II l Carbohydrates: Polyhydroxylated compounds for which the building blocks are highly soluble. – The typical molecular formula for the monomeric forms of these compounds is (CH 2 O)n, where 3 < n < 9, – but usually n = 5 or 6 (or 3). 01/11/10 Biochemistry: Introduction 28
Biological small molecules III Amino acids: Compounds containing an amine (NH 3+) group and a carboxyl (COO-) group. l The most important biological amino acids are a-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 a-amino acid is l H 3 N+ - CHR - COOl 01/11/10 Biochemistry: Introduction 29
Biological small molecules IV l 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. 01/11/10 Biochemistry: Introduction 30
Small molecules V l Inorganic ions: Ionic species containing no carbon but containing one or more atoms and at least one net charge. – Ions of biological significance include Cl-, Na+, K+, Mg+2, Mn+2, I-, Ca+2, PO 4 -3, SO 4 -2, NO 3 -, NO -, and NH +. 2 4 – Phosphate (PO 4 -3) is often found in partially protonated forms HPO 4 -2 and H 2 PO 4– Ammonium ions occasionally appear as neutral ammonia (NH 3), particularly at higher p. H values 01/11/10 Biochemistry: Introduction 31
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. l Ascorbate (vitamin C) is a vitamin for humans and guinea pigs but not for most other mammals. l Cofactors often end up as prosthetic groups, covalently or noncovalently attached to proteins and involved in those proteins' functions. l 01/11/10 Biochemistry: Introduction 32
Biological macromolecules l Most big biological molecules are polymers, i. e. molecules made up of large numbers of relatively simple building blocks. l Cobalamin is the biggest nonpolymeric biomolecule I can think of (MW 1356 Da) 01/11/10 Biochemistry: Introduction Structure courtesy Wikimedia 33
Categories of biological polymers l Proteins l Nucleic acids l Polysaccharides l 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 01/11/10 Biochemistry: Introduction 34
Polymers and oligomers l These are distinguished only by the number of building-blocks contained within the multimer l Oligomers: typically < 50 building blocks l Polymers 50 building blocks. 01/11/10 Biochemistry: Introduction 35
Categories of biopolymers Category <mol wt/ monomer> Protein Types of monomers 20 110 # mono- Branchmers per ing? polymer 65 -5000 no RNA 4 -10 220 -400 20 -15 K no DNA 4 200 -400 50 -106 no Polysaccharide ~10 162 2 -105 Sometimes 01/11/10 Biochemistry: Introduction 36
Water: a complex substance Oxygen atom is covalently bonded to 2 hydrogens l 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 l This contrasts with O=C=O (angle=180º) or urea ((NH 2)2 -C=O) (angles=120º) l Two lone pairs available per oxygen: these are available as H-bond acceptors l 01/11/10 Biochemistry: Introduction 37
Water is polar l Charge is somewhat unequally shared l Small positive charge on H’s (d+); small negative charge on O (2 d-) (Why? ) l A water molecule will orient itself to align partial negative charge on one molecule close to partial positive charges on another. l Hydrogen bonds are involved in this. 01/11/10 Biochemistry: Introduction 38
Liquid water is mobile l The hydrogen-bond networks created among water molecules change constantly on a sub-picosecond time scale l At any moment the H-bonds look like those in crystalline ice l Solutes disrupt the H-bond networks 01/11/10 Biochemistry: Introduction 39
Water in reactions Water is a medium within which reactions occur; l But it also participates in reactions l Enzymes often function by making water oxygen atoms better nucleophiles or water H’s better electrophiles l Therefore water is a direct participant in reactions that wouldn’t work in a nonenzymatic lab setting! l 01/11/10 Biochemistry: Introduction 40
Water’s physical properties l High heat capacity: stabilizes temperature in living things l High surface tension l Nearly incompressible (density almost independent of pressure) l Density max at 3. 98ºC 01/11/10 Biochemistry: Introduction 41
Catalysis l Catalysis is the lowering of the activation energy barrier between reactants and products l 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 01/11/10 Biochemistry: Introduction 42
Biological catalysts 1890’s: Fischer realized that there had to be catalysts in biological systems l 1920’s: Sumner said they were proteins l It took another 10 years for the whole community to accept that l It’s now known that RNA can be catalytic too: l – Can catalyze modifications in itself – Catalyzes the key step in protein synthesis in the ribosome 01/11/10 Biochemistry: Introduction 43
Energy in biological systems l We distinguish between thermodynamics and kinetics: l Thermodynamics characterizes the energy associated with equilibrium conditions in reactions l Kinetics describes the rate at which a reaction moves toward equilibrium 01/11/10 Biochemistry: Introduction 44
Thermodynamics l Equilibrium constant is a measure of the ratio of product concentrations to reactant concentrations at equilibrium l Free energy is a measure of the available energy in the products and reactants l They’re related by DGo = -RT ln Keq 01/11/10 Biochemistry: Introduction 45
Kinetics l Rate of reaction is dependent on Kelvin temperature T and on activation barrier DG‡ preventing conversion from one site to the other l Rate = Qexp(-DG‡/RT) l Job of an enzyme is to reduce DG‡ 01/11/10 Biochemistry: Introduction Svante Arrhenius 46
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 l The enzymes themselves are subject to extensive regulation so that the right reactions occur in the right places and times l 01/11/10 Biochemistry: Introduction 47
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 l 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. l This feedback inhibition helps to prevent overproduction of F—homeostasis. l 01/11/10 Biochemistry: Introduction 48
Molecular biology This phrase means something much more specific than biochemistry: l It’s the chemistry of replication, transcription, and translation, i. e. , the ways that genes are reproduced and expressed. l 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. l 01/11/10 Biochemistry: Introduction 49
The molecules of molecular biology Deoxyribonucleic acid: polymer; backbone is deoxyribose-phosphate; side chains are nitrogenous ring compounds l RNA: polymer; backbone is ribose-phosphate; side chains as above l Protein: polymer: backbone is NH-(CHR)-CO; side chains are 20 ribosomally encoded styles l 01/11/10 Biochemistry: Introduction 50
Steps in molecular biology: the Central Dogma DNA replication (makes accurate copy of existing double-stranded DNA prior to mitosis) l Transcription (RNA version of DNA message is created) l Translation (m. RNA copy of gene serves as template for making protein: 3 bases of RNA per amino acid of synthesized protein) l 01/11/10 Biochemistry: Introduction 51
Evolution and Taxonomy Traditional studies of interrelatedness of organisms focused on functional similarities l This enables production of phylogenetic trees l Molecular biology provides an alternative, possibly more quantitative, approach to phylogenetic tree-building l More rigorous hypothesis-testing possible l 01/11/10 Biochemistry: Introduction 52
Quantitation Biochemistry is a quantitative science. l Results in biochemistry are rarely significant unless they can be couched in quantifiable terms. l Thermodynamic & kinetic behavior of biochemical systems must be described quantitatively. l 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. l 01/11/10 Biochemistry: Introduction 53
Mathematics in biochemistry l Ooo: I went into biology rather than physics because I don’t like math l Too bad. You need some here: but not much. l Biggest problem in past years: exponentials and logarithms 01/11/10 Biochemistry: Introduction 54
Exponentials Many important biochemical equations are expressed in the form Y = ef(x) l … which can also be written Y = exp(f(x)) l The number e is the base of the natural logarithm system and is, very roughly, 2. 71828459045 l I. e. , it’s 2. 7 1828 45 90 45 l 01/11/10 Biochemistry: Introduction 55
Logarithms l First developed as computational tools because they convert multiplication problems into addition problems l They have a fundamental connection with raising a value to a power: l Y = xa logx(Y) = a l In particular, Y = exp(a) = ea ln. Y = loge(Y) = a 01/11/10 Biochemistry: Introduction 56
Algebra of logarithms l l logv(A) = logu(A) / logu(v) logu(A/B) = logu(A) - logu(B) logu(AB) = Blogu(A) log 10(A) = ln(A) / ln(10) = ln(A) / 2. 30258509299 = 0. 4342944819 * ln(A) = log 10(A) / log 10 e = log 10(A) / 0. 4342944819 = 2. 30258509299 * log 10(A) 01/11/10 Biochemistry: Introduction 57
Course structure l Three midterms plus a final – My exams will be closed-book, closed-notes exams. Calculators are not allowed. – You’ll have a help-sheet for each of my exams – 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! 01/11/10 Biochemistry: Introduction 58
Grading I’m a moderately tough grader, but I do curve this course l The cutoff for an A is likely to be around an 84, but it’s uncertain l Homework, literature assignments, i. Clicker quizzes, and discussionboard participation count l 01/11/10 Biochemistry: Introduction 59
Textbook and Lecture Notes Our textbook: Horton et al, Principles of Biochemistry, 4 th Ed. It’s clear and concise. l Garrett & Grisham is a detail-rich and wellwritten text: you’re welcome to try it too. l Most of my lectures are derived from Horton, but I’ll often give cross references to G&G l Be prepared for the lecture notes themselves to evolve during the course l 01/11/10 Biochemistry: Introduction 60
Office Hours l. I should be available 4: 15 -6 pm Wednesdays and 5 -6 pm Mondays, plus some late-mornings l If that doesn’t work, make an appointment l The discussion board is another good way to reach me and the rest of the class as well! 01/11/10 Biochemistry: Introduction 61
Assignments l Regular homeworks will be due weekly, generally on Thursdays l But no assignment due this week l Literature assignments are due weekly on Tuesdays except in midterm weeks l Specific readings already posted may be augmented but not deleted 01/11/10 Biochemistry: Introduction 62
Lateness? l Regular homework: – No penalty if turned in by 24 h of deadline – Modest penalties if 1 -7 days late – After 7 days the answer key will be posted, so no credit given after that l Literature assignments: – No penalty if turned in by 24 h of deadline – Half credit if turned in 1 -7 days late – No credit later than that 01/11/10 Biochemistry: Introduction 63
Arrangements for exams l Midterms: – Monday 1 February – Monday 1 March – Monday 5 April l Final exam date is uncertain because it’s set by the Registrar 01/11/10 Biochemistry: Introduction 64
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