1. CS790 – Bioinformatics A Gentle Introduction to (or review of) Fundamentals of Chemistry and Organic Chemistry Square one… CS 790 – Bioinformatics

2. Intro to biochemistry2 Fundamentals of Chemistry  Reading the periodic table  Neutrons and isotopes  Electron shells, subshells and orbitals Each orbital can hold at most 2 electrons In the ground state orbitals are filled from lower to higher energy 6 C Carbon 12.01 Isotopes of Chlorine AtomicNatural IsotopeProtonsNeutrons massabundance 35 Cl171834.9776% 37 Cl172036.9724%

3. CS790 – BioinformaticsIntro to biochemistry3 Electron shells and orbitals  Quantum numbers n = First quantum number = shell l = Second quantum number = orbital type Golden rule: l < n Know these two. Types of Orbitals SecondLetterNumberMaximum quantumdenotingofnumber of numberorbitalsorbitalselectrons 0s12 1p36 2d510 3f714

4. CS790 – BioinformaticsIntro to biochemistry4 Subshells and valence  All orbitals of the same type (same l and n) are called a subshell  Subshell notation: Electron shell # electrons in the subshell Type of orbitals 2p 5 Electron Subshells 1 st Quantum2 nd QuantumNotation for numbernumbersubshells 101s 20,12s,2p 30,1,23s,3p,3d 40,1,2,34s,4p,4d,4f …

5. CS790 – BioinformaticsIntro to biochemistry5 Electronic configurations  Since the subshells are filled from lowest to highest energy, we can specify only the outermost shell.  Atoms tend to lose or gain electrons such that the outermost subshell is full: valence

6. CS790 – BioinformaticsIntro to biochemistry6 Covalent Bonds  For almost all of the elements that we will deal with, 8 valence electrons is an electronically stable configuration.  Covalent bonds are formed when atoms share electrons to fill the valence shell

7. CS790 – BioinformaticsIntro to biochemistry7 Covalent bonds: Lewis diagrams  How many covalent bonds will an atom form?  Flourine:Atomic number = 9, Electron configuration: 1s 2,2s 2,2p 5  Oxygen:Atomic number = 8 Electron configuration: 1s 2,2s 2,2p 4 FFF or FF OOO OO

8. CS790 – BioinformaticsIntro to biochemistry8 How many covalent bonds?  Note the common valences for the elements most common in proteins and DNA: CarbonCarbon OxygenOxygen NitrogenNitrogen HydrogenHydrogen SulfurSulfur  Note the similarity between S and O.

9. CS790 – BioinformaticsIntro to biochemistry9 Ions and ionic bonds  Formation of ions Conflicting goals: neutral charge vs. stable electronic configuration Some atoms have a strong tendency to gain or lose electrons:  Sodium (Na): Atomic # = 11: 1s 2,2s 2,2p 6,3s 1  Na +  Chlorine (Cl): A# = 17: 1s 2,2s 2,2p 6,3s 2,3p 5  Cl – Complete electron transfer, no sharing  Coulombs law:  Ionic bond or salt bridge

10. CS790 – BioinformaticsIntro to biochemistry10 Polar Bonds  In reality, some atoms will attract shared electrons more strongly. That is, the shared electrons will be “off center”.  The tendency to attract electrons is called electronegativity.  There is a continuum between covalent bonds and ionic bonds. KIK+K+ I  –

11. CS790 – BioinformaticsIntro to biochemistry11 The Hydrogen Bond  When hydrogen forms a polar bond, the nucleus is left without any unshared electrons It can make a secondary bond with another negative ion, called a hydrogen bond Very common in water: Weaker than polar and covalent bonds Donor: covalent/polar bond to H Acceptor: ionic attraction to H OH+H+ H+H+ –– ON

12. CS790 – BioinformaticsIntro to biochemistry12 Van der Waals bonds  Nonspecific – when any two atoms at ~3 to 4 Å apart Å = angstrom units = 10  10 meters = 0.1 nm  Low energy interaction Significantly smaller than h-bonds or ionic attraction Adds up over many atoms When two atoms have very similar shapes, the Van der Waals contacts can become significant

13. CS790 – BioinformaticsIntro to biochemistry13 Energy of molecular interactions  1 calorie = the amount of energy to raise the temperature of 1g of water from 14.5 to 15.5°C  Molecules have about 0.6 kcal/mole of energy from heat/vibration  Molecular interactions: C–C : 83 kcal/mole Electrostatic and hydrogen bonds: ~3 – 7 kcal/mole Van der Walls interaction: ~1 kcal/mole

14. CS790 – BioinformaticsIntro to biochemistry14 Looking at chemical structures CH 3 H H HH HCC HHH C CH 2 CH 3 CCC Propane: C CC C CC H H HH HH Benzene:

15. CS790 – BioinformaticsIntro to biochemistry15 A hydrocarbon isomer  Carbon can make 4 covalent bonds There are more carbon-based compounds present on earth than the total of all compounds lacking carbon We could spend an entire course examining the properties of hydrocarbons: molecules made up only of carbon and hydrogen.  Example: Isomers of C 4 H 10 Butane: Isobutane: CH 3 CH 2 CH 3 CH CH 3

16. CS790 – BioinformaticsIntro to biochemistry16 Double Bonds  Double bonds can force a molecule or functional group to be planar:  Geometric isomers cis = on the same side trans = on the opposite side

17. CS790 – BioinformaticsIntro to biochemistry17 Some Common Functional Groups

18. CS790 – BioinformaticsIntro to biochemistry18 Concentration  1 mole of a substance = 6.02 × 10 23 atoms or molecules of that substance C – atomic weight = 12, one mole = 12 grams  We express concentration in molarity or moles/liter. Denoted [x]. Example – If we take 1 mole of sodium sulfate (142.1g of Na 2 SO 4 ) and add enough water to make 1 liter of solution: M = [Na 2 SO 4 ] = 1.0

19. CS790 – BioinformaticsIntro to biochemistry19 Acids and Bases  Acids give off protons in solution HCl  H + + Cl  In water, the H + ion often binds with water to form a hydronium ion H 3 O + Strong acids dissociate completely Weak acids do not dissociate completely  pH of a solution pH =  log[H + ]

20. CS790 – BioinformaticsIntro to biochemistry20 More on pH  A simple example: Suppose we add 0.001 moles of HCl to 1.0 L of H 2 0 [H + ] = 10  3 moles/liter, so pH = 3  0714  acidicbasic   Bases accept H + ions pOH =  log[OH  ]  pH + pOH = 14 Water: pH = 7, pOH = 7

21. CS790 – BioinformaticsIntro to biochemistry21 pKa  For a weak acid, the pKa is a measure of the tendency of the acid to dissociate (give of an H + ion)  Key rule: pH = pKa : protonated and unprotonated forms are at equilibrium pH < pKa : more protonated pH > pKa : less protonated  Biological pH varies but is generally close to neutral (7.0) or slightly acidic

22. CS790 – BioinformaticsIntro to biochemistry22 Properties of Water  The polarity of water makes it highly cohesive:  Water solvates & weakens ionic and hydrogen bonds:

23. CS790 – BioinformaticsIntro to biochemistry23 Hydrophobic Attraction  Nonpolar (hydrophobic atoms), are driven together Hydrophobic interactions Driven by water’s affinity for itself