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Chemistry

Chemistry. Notes. Ch. 22 & 24 -. Organic and BioChemistry. BIOCHEMISTRY. The chemistry of living matter Polymer: Large molecule formed by the covalent bonding of repeating smaller molecules . Monomer: Small molecules that combine to form polymers.

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Chemistry

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  1. Chemistry Notes Ch. 22 & 24 - Organic and BioChemistry

  2. BIOCHEMISTRY The chemistry of living matter Polymer: • Large molecule formed by the covalent bonding of repeating smaller molecules. Monomer: • Small molecules that combine to form polymers.

  3. Large molecules (polymers) are formed by repetitive combinations of simple subunits (monomers). • Some types of polymers (monomers): • Proteins (amino acids) • Lipids (Triglycerides) • Nucleic Acids (nucleotides) • Polysaccharides (monosaccharides)

  4. Amino Acids – Proteins

  5. Fatty Acids – Triglycerides

  6. Nucleotides – Nucleic Acids

  7. Monosaccharides – Polysaccharides

  8. Organic Chemistry • Study of CARBON containing compounds. • Studies substances found only in living organisms • Why would there be an entire branch of chemistry that focuses on Carbon? What makes carbon so special compared to all of the other elements?

  9. Valence Electrons and the Octet Rule • What are Valence Electrons? • Electrons available for bonding (Outer shell electrons) • What is the octet rule? • Atoms want to have 8 valence electrons (with 2 exceptions) • Bonding patterns of atoms can be explained by an atom’s valence electrons and its desire to complete octet rule.

  10. Why is Carbon so Special? • It has four valence electrons, therefore it always forms four covalent bonds. • They can link together to form chains, branches, and rings.

  11. Bonding Review • List the types of bonds atoms can make and describe the difference between them? • Evaluate which types of bonds would be strongest? • Bio and Organic Chemistry focuses on Covalent Bonds. • Molecules tend to be large, and are composed of mostly non-metals

  12. Bonding Characteristics Use the HONC 1234 rule to explain the number of covalent bonds an atom will make. H – Hydrogen 1 covalent bond O – Oxygen 2 covalent bonds N – Nitrogen 3 covalent bonds C – Carbon 4 covalent bonds

  13. Amino Acids – Proteins

  14. Fatty Acids – Triglycerides

  15. Nucleotides – Nucleic Acids

  16. Monosaccharides – Polysaccharides

  17. HYDROCARBONS • Compounds that contain only Hydrogen and Carbon • Types of Hydrocarbons: • Alkanes = single covalent bond • Alkenes = double covalent bond • Alkynes = triple covalent bond

  18. The First Ten Alkanes: Methane CH4 Ethane C2H6 Propane C3H8 Butane C4H10 Pentane C5H12 Hexane C6H14 Heptane C7H16 Octane C8H18 Nonane C9H20 Decane C10H22

  19. Structural Formulas H Line represents a covalent bond (shared electron pair). H H C H Methane Molecule

  20. Exit Slip FRONT: • List the four main polymers and include the monomer that makes them up in (parenthesis) • Name the type of bond that holds monomers together to form polymers. BACK: • Write a “Tweet” (about 25 words) describing something you learned today (include a hash tag if you want)

  21. Branched-Chain Alkanes C C C C C C C C Dash between carbons is a covalent bond. Dash on the outside represents a hydrogen.

  22. Naming Hydrocarbons C C C C C C C C 1. Count the longest chain. (You may bend corners!) This is hexane since it has six carbons.

  23. C C C C C C 6 5 4 3 2 1 C C 2. Now number the chain from the end closest to a side branch. 3. Name the side branches and assign numbers to them. Names for branches end in –yl.

  24. C C C C C C 6 5 4 3 2 1 C C 4. If multiple branches of the same thing, then use prefixes di, tri, tetra, etc. This is 2,4 - dimethylhexane

  25. Saturated vs. Unsaturated • Saturated: • Organic compounds that contain the maximum number of hydrogen atoms per carbon. (All Single Bonds) – Alkanes. • Unsaturated: • Organic compounds that contain less than the maximum number of hydrogen atoms per carbon. (Double and Triple Bonds) – Alkenes and Alkynes.

  26. Unsaturated Hydrocarbons Alkenes These are hydrocarbons containing double bonds somewhere in the main chain. These are hydrocarbons containing triple bonds somewhere in the main chain. Alkynes

  27. Naming Alkenes 1. Find the longest chain in the molecule that contains the double bond. 2. The chain is numbered so that the carbon atoms of the double bond get the lowest possible number. 3. The root name is followed by the suffix –ene (or –yne) 4. Name the branches the same.

  28. C C C C C 1 2 3 4 5 This is 2-Pentene. Notice some of the hydrogen atoms appear to be “missing”. Each carbon atom may only have four bonds.

  29. Structural Isomers Compounds having the same molecular formula but different structures. C C C C C C C C Butane 2 - Methylpropane

  30. Geometric Isomers Structures differ in geometry. Trans configuration is when the substituted groups are on opposite sides of the double bond. Cis configuration is when the substituted groups are on the same side as the double bond.

  31. Geometric Isomers CH3 H trans-2-Pentene C=C H CH2CH3 CH3 CH2CH3 C=C cis-2- Pentene H H

  32. Stereoisomers Atoms of the same molecular structure that differ only in the arrangement of the atoms in space. They are mirror images.

  33. Hydrocarbon Rings • Cyclic Hydrocarbons • Aromatic Hydrocarbons

  34. Cyclic Hydrocarbons Compounds that contain a hydrocarbon ring. Hydrocarbon compounds that do not contain a ring are known as aliphatic compounds.

  35. C C C cyclopropane cyclobutane C C C C C C C C C C C cyclohexane cyclopentane C C C C

  36. Aromatic Hydrocarbons Any organic compound containing a benzene ring. Each corner contains a carbon atom. There are alternating double bonds between carbons. One hydrogen is attached to each carbon.

  37. Hydrocarbons from the Earth Natural Gas Petroleum Coal

  38. Functional Groups A specific arrangement of atoms in an organic compound that is capable of characteristic chemical reactions. Functional groups are attached to hydrocarbon chains.

  39. Substitution Reactions A common type of organic reaction in which an atom or group of atoms replaces another atom or group of atoms. CH4 + Cl2 CH3Cl + HCl Methane Chlorine Chloromethane Hydrogen chloride

  40. Alcohols The –OH functional group in alcohols is called a hydroxyl group. CH3 – CH2 – OH Ethyl alcohol or ethanol

  41. Addition Reactions A substance is added at the double or triple bond of an alkene or alkyne. OH C C C=C + H OH Ethene Water Ethanol

  42. Ethers Compounds in which oxygen is bonded to two carbon groups. The general structure of an ether is R-O-R. (Where “R” represents a carbon chain of any length.) Ethylmethyl ether CH3 – CH2 – O – CH3

  43. Aldehydes A carbonyl group consists of a carbon atom and an oxygen atom joined by a double bond. (C=O) Aldehydes are organic compounds in which the carbon of the carbonyl group is always joined to at least one hydrogen. The general formula for an aldehyde is RCHO.

  44. Ketones organic compounds in which the carbon of the carbonyl group is joined to two other carbons. The general formula for a ketone is RCOR.

  45. O O R-C-H R-C-R Aldehyde Ketone The name for an aldehyde ends in –anal. The name for a ketone ends in –anone.

  46. Carboxylic Acids Compounds with a carboxyl group. (a carbonyl group attached to a hydroxyl group.) O The general formula is RCOOH. The name ends in –oic acid. R-C-OH

  47. Esters Derivatives of carboxylic acids in which the –OH of the carboxyl group has been replaced by an –OR from an alcohol. The general formula is RCOOR. O R-C O - R

  48. Many esters have pleasant fruity odors. They are also responsible for giving some perfumes their fragrances.

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