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Biochemistry

Biochemistry. Chapter 4 Functional Groups Chapter 5 Macromolecules. Carbon—The Backbone of Biological Molecules All living organisms Are made up of chemicals based mostly on carbon due to its bonding ability All life considered “carbon based life-forms”. Biochemistry Part 1

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Biochemistry

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  1. Biochemistry Chapter 4 Functional Groups Chapter 5 Macromolecules

  2. Carbon—The Backbone of Biological Molecules • All living organisms • Are made up of chemicals based mostly on carbon due to its bonding ability • All life considered “carbon based life-forms”

  3. Biochemistry Part 1 Chapter 4: Functional Groups

  4. Chapter 4 • Organic chemistry • the study of carbon compounds • Organic compoundshave carbon in them (& usually H) • Exception: CO2 is considered INORGANIC • Range from simple to big molecules

  5. Stanley Miller’s Experiment • The concept ofvitalism • idea that organic compounds arise only within living organisms • disproved when chemists synthesized carbon compounds in lab • Ex: Miller • Thoughts shifted from vitalism to mechanism • the view that all natural phenomena are governed by physical and chemical laws.

  6. Stanley Miller’s Experiment Gases CH4, NH3, H2O, H2

  7. Formation of Bonds w/ Carbon • Carbon atoms • forms diverse molecules • b/c carbon has 4valence electrons bind to to 4 other atoms • can form 4 covalent bonds with itself or other atoms  very important in living things! • Carbon has bonding versatility • allows it to form many diverse molecules, including carbon skeletons (carbon “chains”)

  8. Hydrogen (valence = 1) Oxygen (valence = 2) Nitrogen (valence = 3) Carbon (valence = 4) H O N C Figure 4.4 The electron configuration of carbon • Gives it covalent compatibilitywith many different elements

  9. Molecular Diversity Arising from Carbon Skeleton Variation • Carbon chains • Form skeletons of most organic molecules • Vary in length and shape • Straight • Branched • Rings

  10. Hydrocarbons • Organic molecules consisting of only C and • Ex: petroleum; lipid ‘tails’ • Found in many of cell’s organic molecules • Ex: fat molecules • Covalent bonding btw C-H nonpolar (hydrophoic) • High energy storage

  11. Fat droplets (stained red) 100 µm (b) Mammalian adipose cells (a) A fat molecule Figure 4.6 A, B Example of a Hydrocarbon

  12. ISOMERS Isomers • same molecular formula, but different structure & properties • Have same # of atoms arranged differently 3 types of isomers • structural~ differ in covalent bonding arrangement • geometric~ differ in spatial arrangement • Arise from inflexibility of double C bond • cis (same side) vs. trans (opposite sides) • enantiomers~ mirror images of each other • Ex: used in pharmacological industry

  13. Example of Isomers Straight vs. branched Cis vs. trans 1 usually active; other inactive Asymmetrical Carbon

  14. L-Dopa (effective against Parkinson’s disease) D-Dopa (biologically inactive) Figure 4.8 Enantiomers • Are important in the pharmaceutical industry

  15. Functional Groups • Functional groups • parts of organic molecules involved in chemical rxns (i.e.-chemically reactive groups) • each functional group behaves in a consistentfashion from 1 organic molecule to the next • # & arrangement of groups helps give molecules unique, distinctive chemical properties

  16. 6 functional groups important in chemistry of life • Hydroxyl • Carbonyl • Carboxyl • Amino • Sulfhydryl • Phosphate • Methyl (yes…another one)

  17. Functional Groups • Attachments replace 1+ of H’s bonded to C skeleton of the hydrocarbon • Each GROUP are HYDROPHILIC  increase organic molecule solubility in water 1. Hydroxyl Group (-OH) • H bonded to O • Make alcohols, sugars • polar (b/c of oxygen electronegivity) • soluble in water (attracts H20)

  18. Functional Groups 2. Carbonyl Group (C=O) • C double bond to O • Aldehyde(at the end of C skeleton) • Ketone (INSIDE Carbon skeleton) • Ex: Acetone, Propanal

  19. Ketone • Aldehyde • **Think: all the way at the end!

  20. Functional Groups cont’d 3. Carboxyl Group (-COOH) • O double bonded to C to hydroxyl • Carboxylic acids (organic acids) • Covalent bond between O and H • Polar • Dissociation  H ion source (Acidic properties) • **Think: Carboxyl has a hydroxyl!

  21. Functional Groups cont’d 4. Amino Group (-NH2) • N to 2 H atoms • Makes Amines • Acts as a base (+1) • Also makes AMINO ACIDS Have both amino and carboxyl groups

  22. Functional Groups cont’d 5. Sulfhydral Group (-SH) • sulfur bonded to H • Makes disulfide bridges • 2 sulfhydral groups can interact to stabilize protein structure

  23. Functional Groups cont’d 6. Phosphate Group (-OPO3-) • Organic phosphates • Forms phosphate ion • Covalently attached by 1 of its O to the C skeleton • Can transfer energy btw organic molecules • Ex: ATP

  24. Functional Groups cont’d 7. Methyl Group (-CH3) • Usually not as reactive as other groups • Used in gene expression

  25. Male or Female!! • Only one little itty bitty difference that separates the sexes

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