Organic and Biochemistry Narrated

Organic and Biochemistry: 

Organic and Biochemistry

Organic Chemistry: 

Organic Chemistry Inorganic Chemistry Study of compounds that do not contain carbon as the principal element Study of organic compounds Contain carbon as the principle element May or may not be formed by living things Most known compounds are organic

Why is CARBON so special? : 

Why is CARBON so special? 2 nd row of periodic table Atomic number = 6 6 protons, 6 electrons 1s 2 2s 2 2p 2 electron structure Valence of 4 electrons Need 8 electrons to fill valence shell Form 4 bonds with other atoms Can combine with 1, 2, 3 or 4 other C atoms Single, double, triple bonds Each bond consists of 1 electron from carbon & 1 electron from bonding atom

Hydrocarbons: 

Hydrocarbons Consist of only two elements Hydrogen and Carbon Carbon atoms can combine with each other Thousands of possible structures and arrangements Simplest hydrocarbon Methane CH 4 1 C atom, 4 H atoms

Carbon-Carbon Bond: 

Carbon-Carbon Bond Non polar covalent Can be: Double -C=C- Triple -C C- Single -C-C- Line stands for 1 electron pair (1 bond) To satisfy octet rule, each C atom must have 4 bonds (lines)

Hydrocarbons: 

Hydrocarbons 4 groups of hydrocarbons Alkanes (all single bonded carbons) Alkenes (at least 1 double bonded carbon) Alkynes (at least 1 triple bonded carbon) Aromatics (ring structures) Saturated hydrocarbon - all single bonds present, all possible sites are filled with hydrogen atoms Unsaturated hydrocarbon - double or triple bonds present, less hydrogen atoms are needed

NAMING OF ORGANICS: 

NAMING OF ORGANICS Prefix tells number of carbons in chain Suffix tells if alkane, alkene, alkyne pentane # of Carbons (5) Type of hydrocarbon (alkane)

Isomers: 

Isomers Same molecular formula Different structure Different physical and chemical properties Frequently many different isomers of a compound Number of carbon atoms in compound increases, so does number of isomers IUPAC rules for naming Compound with straight continuous chain identified with term normal (n) Compound with branching indicated by iso in front of name Iso butane

Alkanes: 

Alkanes Single carbon to carbon bonds covalent bonds between carbon atoms Paraffin series each successive molecule higher in molecular weight Petroleum and petroleum products Not as chemically reactive as other hydrocarbons Straight chains, branched chains or ring structure General formula C n H 2n+2 Simplest alkane: methane CH 4

Slide 10: 

Alkane # C atoms Molecular formula Meth ane 1 CH 4 Eth ane 2 C 2 H 6 Prop ane 3 C 3 H 8 But ane 4 C 4 H 10 Pent ane 5 C 5 H 12 Hex ane 6 C 6 H 14 Hept ane 7 C 7 H 16 Oct ane 8 C 8 H 18 Non ane 9 C 9 H 20 Dec ane 10 C 10 H 22

Alkenes: 

Alkenes Double covalent carbon-to-carbon bonds covalent bonds between carbon atoms Can form straight chains, branched chains or ring structure General formula C n H 2n Room for two fewer hydrogen atoms around the double bond Simplest alkene: ethene (ethylene) C 2 H 4

Alkynes: 

Alkynes Triple carbon to carbon bonds covalent bonds between carbon atoms Can form straight chains, branched chains or ring Highly reactive General formula C n H 2n-2 Simplest alkyne: ethyne (acetylene) C 2 H 2

Ring Structures: 

Ring Structures Cycloalkanes All single carbon-carbon bonds Aromatics Single and double carbon-carbon bond Electrons delocalized Based on benzene

Hydrocarbon Mixtures: 

Hydrocarbon Mixtures Natural Gas (95% methane) 1 to 4 carbon atoms/molecule Gasoline 5-12 Carbon atoms/molecule Kerosene (lamp, fuel, heating oil #1) 12-15 carbon atoms/molecule Diesel Fuel (heating oil #2) 15-18 carbon atoms/molecule Motor oil 16-18 carbon atoms/molecule Petroleum Jelly/Paraffin wax 20 or more carbon atoms/molecule Asphalt/Asphaltenes 36 or more carbon atoms/molecule Increasing molecular mass Solid Gas

Gasoline: 

Gasoline Mixture of hydrocarbons Each hydrocarbon may have 5 to 12 carbon atoms per molecule Need combination of straight and branched chain hydrocarbon molecules Straight chain molecules not suitable to burn alone Burn too rapidly More explosive than smooth burning Ignite spontaneously under compression not with spark plug ignition Engines knock and ping Can damage engine

Polymers: 

Polymers Macromolecules Very large chain-like organic molecules Formed from many smaller molecules called “monomers” Poly = many Mono = one or single Mer = units or segments Monomers in the chain can be identical or different Polymer has different properties than monomers from which it was formed Polymers can take many different shapes Chains, lattices, helices, sheets

Alcohols: 

Alcohols Contains hydroxyl functional group (-OH) Thousands of unique alcohols some of the most common and useful compounds in nature and industry Simple Alcohols Methanol (CH 3 OH) Ethanol (C 2 H 5 OH) Proponal (C 3 H 7 OH) n-proponal isopropanol -OH group at end -OH group in middle

Organic Acids and Esters: 

Organic Acids and Esters Organic Acids Sometimes called carboxylic or fatty acids Contain the carboxyl functional group -COOH Examples Formic Acid – simplest one Acetic Acid - vinegar Citric Acid – citrus fruit Lactic Acid - milk Esters Give fruits and flowers characteristic odor and taste Used in flavoring and perfume industries

Carbohydrates: 

Carbohydrates Contains carbon, hydrogen, oxygen linked together to form monosaccharides (simple sugars) Empirical formula CH 2 O (1 carbon for each water) Simple sugars combined to form complex carbohydrates Attached to each other by the removal of water from between the sugar molecules Used for: main energy source (food) structure and protection essential part of genes Includes sugars, starches, cellulose

Saccharides: 

Saccharides Describes sugars 1 sugar molecule = monosaccharide 2 sugar molecules= disaccharide 3 sugar molecules= trisaccharide Larger molecules are called polysaccharides (complex carbohydrates)

Combination of Sugars: 

Combination of Sugars Different monosaccharides can be combined to form disaccharides or polysaccharides C 6 H 12 O 6 + C 6 H 12 O 6  C 12 H 22 O 11 + H 2 O glucose fructose sucrose Glucose and fructose are isomers same molecular formula; different structure

Proteins and Amino Acids: 

Proteins and Amino Acids Proteins Polymers made up of amino acids Include enzymes, hemoglobin, hormones, antibodies Amino Acids Short carbon skeleton with amino group (nitrogen + 2 hydrogens) on one end; carboxylic acid group at the other end Can have side chains Vary in composition Designated as R-group 20 common amino acids Different side chains Amino acids link together Form polypeptides

Four Levels (Degrees) of Protein Structure: 

Four Levels (Degrees) of Protein Structure Primary Specific sequence of amino acids in polypeptide Genetically controlled Secondary Amino acid chain twists and folds into various shapes (helixes, pleated sheets) Important in protein function Tertiary Amino acid chain forms complex 3-D globular structures Quaternary Several polypeptides twist around each other and chemically combine

Nucleic Acids: An overview: 

Nucleic Acids: An overview Complex polymers constructed of nucleotide monomers Nucleotide composed of three parts 5-carbon simple sugar molecule (either ribose or deoxyribose) Phosphate group Nitrogenous base (5 types) Adenine (A), Guanine (G), Thymine (T), Cytosine (C), Uracil (U) Nucleotide monomers linked together Sugar and phosphate groups form backbone Nitrogenous bases stick out Two types of nucleic acids DNA (Deoxyribose sugar; bases A, T, G, C) RNA (Ribose sugar; bases A, U, G, C) DNA Single Strand RNA

Deoxyribonucleic Acid (DNA): 

D eoxyribo n ucleic A cid (DNA) Composed of two strands of nucleotide bases Double helix Attached between bases according to base pair rule Human cells contain 46 strands of DNA (chromosomes) Each strand contains thousands of genes Base Pair Rule For both DNA and RNA Guanine always pairs with Cytosine (G C) In DNA: Adenine always pairs with Thymine (A T) In RNA: Adenine always pairs with Uracil (A U)

Ribonucleic Acid (RNA): 

R ibo n ucleic A cid (RNA) Messenger RNA (mRNA) Single strand copy of portion of DNA coding strand Formed on the surface of DNA using base pair rule Uses U-A pairing instead of T-A pairing After formation, associates with ribosome where genetic message is translated into protein molecule Ribosomal RNA (rRNA) Also a RNA copy of DNA After formation, forms a ribosome Transfer RNA (tRNA) Made from different segments of DNA Responsible for transferring specific amino acids to ribosome for protein manufacture

Formation of Proteins: 

Formation of Proteins

Lipids (fats): 

Lipids (fats) Large non-polar molecules Three types True fats; used for energy Phospholipids; major component of cell membranes Steroids; some hormones, cholesterol Saturated and Unsaturated Fats Unsaturated fats at least one carbon-carbon double bond in one of the fatty acids. usually liquid at room temperature Some vegetable oils (olive, safflower sunflower, soybean, peanut) Saturated fats no C-C double bonds usually solid or almost solid at room temperature animal fats (meat, poultry, dairy products)

True Fats: 

True Fats Composed of Glycerol molecule Carbon skeleton with 3 alcohol groups Carboxylic functional group Saturated fatty acid Unsaturated fatty acid Fatty acid Long chain carbon skeleton with a carboxylic acid functional group

Synthetic Polymers: 

Synthetic Polymers Celluloid - first synthetic polymer (1862) Chemically modified cellulose Bakelite - first completely synthetic polymer (early 1900s) Thermosetting material Cross-links formed between chains Permanently hardened when heated at high temperatures Other Synthetic Polymers