carbon compounds
DESCRIPTION
Carbon Compounds. Section 2.3. Carbon Compounds. Organic Compounds. All compounds are either organic , containing carbon bonded to hydrogen and oxygen, or inorganic . The chemistry of carbon is the chemistry of life. Carbon Bonding:. Carbon has four valence electrons - PowerPoint PPT PresentationTRANSCRIPT
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Carbon Compounds
Section 2.3
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Lipids Fats/Oils/Steroids/Wax
4 Categories of Organic Molecules
Molecules of Life
Biochemicals
(CHON)Proteins
Enzymes/Structure/ Movement/Protection
Nucleic Acids(DNA/RNA)
CarbohydratesGlucose/Fructose
Starch/Cellulose
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Carbon CompoundsOrganic Compounds
Carbohydrates
Monomer:Monosaccharide
Made up of:Carbon, Hydrogen,
Oxygen (H:O in 2:1 ratio)
Lipids
Monomer: Glycerol and Fatty Acids
Made up of: Carbon, Hydrogen,
Oxygen(H:O not in 2:1 ratio)
Proteins
Monomer: Amino Acid
Made up of: Carbon, Hydrogen, Oxygen, Nitrogen
Nucleic Acids
Monomer: Nucleotide
1) 5 Carbon sugar, 2) phosphate group 3)nitrogenous base
Made up of: Carbon, Hydrogen,
Oxygen, Nitrogen and Phosphorus
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All compounds are either ORGANIC, containing carbon bonded to hydrogen and oxygen, or INORGANIC.
The chemistry of carbon is the chemistry of life.
Organic Compounds
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Organic Compounds >11 million compounds Contain a C-C or C-H bond in combination with
N, O, S, P or halogens Simplest = CH4 Most complex = DNA
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Organic CompoundsAllotropes of carbon
Allotropes: Different forms of an element in same physical state
Catenation: ability of an element to form chains and/or rings of covalently bonded atoms
Carbon has high bond energiesC-C 346 kJ/molC-H 418 kJ/mol
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Diamond tetrahedral array of C
atoms o sp3 hybridized
high mp (>3500°C) hardest material known
to man brittle most dense (3.5x that of
H2O) Industrial uses: cutting,
drilling, grinding
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Graphite layers of hexagonal
arrays of C atoms o sp2 hybridized (planar)
high mp no covalent bonds
between layers – C atoms too far apart from each other (London Dispersion forces)
layers slip past one another
lubricant and pencil “lead”
Graphite fibers (stronger and less dense than steel)- sporting goods and aircraft
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Soot amorphous form of carbon (no structure)
impure carbon particles resulting from incomplete combustion
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How many protons does carbon have? Electrons?
Carbon has FOUR valence electronso Needs eight electrons to be stable
Carbon readily forms four covalent bonds with other atoms, including carbon
Carbon Bonding:
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Carbon Bonding Carbon can form straight chains, branched
chains, or ringso Leading to a great variety of organic
compounds
Isomers
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Arrangement of Atoms Isomers – compounds that have the same
molecular formula but different structures
More C atoms in formula, more isomerso 18 isomers for C8H18o 35 isomers for C9H20o 75 isomers for C10H22
Isomers of C6H14
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Ex #1) Butane, C4H10
Ex #2) Butene, C4H8
Ex #3) 2-Butene, C4H8
Ex #4) methyl propene, C4H8
ISO
MER
S
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Structural Formula Indicates the number and types of atoms
present in a molecule and also shows the bonding arrangement of the atoms
One possible isomer of C4H10
Does not show 3D shape
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Structural Isomers Isomers in which the atoms are bonded
together in different orders. C4H10 (note continuous chain of C atoms)
butane
methylpropane
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Physical Properties of Structural Isomers
Melting Point (°C)
Boiling Point (°C)
Density at 20°C
Butane-138.4 -0.5 0.5788
Methylpropane -159.4 -11.633 0.549
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Hydrocarbons Only have carbon and hydrogen Simplest organic compounds From petroleum (crude oil)
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Single Bond Sharing 2 electrons A single line
Double Bond Sharing 4 electrons Two parallel lines
Triple Bond Sharing 6 electrons Three parallel lines
Carbon Bonding
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Naming Carbon Compounds Organic PREFIXES Indicates the number of carbon atoms in the
hydrocarbon chain Hydrocarbon: any organic compound that
contains only the elements, hydrogen and carbon# of C prefix # of C prefix
1 Meth- 6 Hex-2 Eth- 7 Hept-3 Prop- 8 Oct-4 But- 9 Non-5 Pent- 10 Dec-
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Organic PREFIXES Prefixes for alkanes that have 1-4
carbons are rooted historically. o These are methane, ethane, propane,
and butane, respectively. o An easy way to remember the first four
names is the anagram Mary Eats Peanut Butter (methane, ethane, propane, butane)
Prefixes for 5 carbons and up are derived from the Greek language.
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Naming Carbon Compounds
Series Ending Formula determines the
# H atoms
Type of Bond(s)
Alkane -ane CnH2n+2 Single
Alkene -ene CnH2n Double
Alkyne -yne CnH2n-2 Triple
Organic SUFFIXES Indicates the types of covalent bonds that
are present in the hydrocarbon chaino Identifies the series to which it belongs
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Aliphatic Hydrocarbons- hydrocarbons without aromatic
ringsSaturated
Hydrocarbons: compounds that contain all SINGLE bonds
Alkanes: each carbon is bonded to 4 atoms– Only contain single
bonds– Skeleton: C-C Molecular formula:
CnH2n+2
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Unsaturated HydrocarbonsCompounds that contain at least one double bond or triple bond
1. Alkenes: compounds that contain a double bond
• Skeleton: C=C• Molecular formula = CnH2n
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2. Alkynes: compounds that contain a triple bond
– Skeleton: CC– Molecular formula = CnH2n-2
Unsaturated Hydrocarbons
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Naming Alkanes To give an alkane a name, a
prefix indicating the number of carbons in the molecule is added to the suffix aneo identifies both the kind of
molecule (an alkane) and how many carbons the molecule has (the prefix).
The name pentane tells you that the molecule is an alkane (-ane ending) and that it has 5 carbons (pent- indicates 5)
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Naming Alkenes1. Locate the carbon atoms in the longest carbon chain
that contains the double bond. Use the stem with the ending –ene.
2. Number the carbon atoms of this chain sequentially, beginning at the end nearer the double bond. If the parent chain has more than 3 carbons, insert the number describing the position of the double bond (indicated by its 1st carbon location) before the base name.
1-butene 2-butene
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http://wps.prenhall.com/wps/media/objects/476/488316/index.html
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Named just like the alkenes except the suffix –yne is added
Naming Alkynes
1-butyne
2-butyne
ethyne
propyne
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Write the names of the organic compounds
methane
propyne
1-pentene
2-pentene
nonane
3-hexene
2-butyne
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1. ethene2. heptane3. 3-
decyne4. butane5. 2-
octene
Give the structural formulas for the organic compounds
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Functional Groups An atom or group of atoms,
that replaces hydrogen in an organic compound and that defines the structure of a family of compounds and determines the properties of the family.
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Female lion
Estradiol(estrogen)
HO
OH
OH
O Testosterone
Male lion
Hydroxyl
Carbonyl(middle)
Carboxyl
Lactic Acid {Amino
Urea
Wohler1828
FUNCTIONAL GROUP - a cluster of atoms that influence the properties of the molecules that they compose, and determine the characteristics of the compound.
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Hydroxyl Group
Structure
Compound Name Alcohols
PropertiesPolar,
attracts water (good
solvent)
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Carbonyl Group
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Carbonyl (end):Structure
Compound Name Aldehydes
PropertiesStructural
isomers with different
properties
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Carbonyl (middle):Structure
Compound Name Ketones
PropertiesStructural
isomers with different
properties
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Carboxyl GroupStructu
re
Compound Name
Carboxylic acid
(organic acids)
Properties
Acidic properties
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Amino GroupStructu
re
Compound Name Amines
Properties
Basic properties
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Phosphate Group
Structure
Compound Name Phosphates
Properties
Makes the molecule and
anionTransfer energy
DNA
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Methyl Group
Structure
Compound Name
Methylated compounds
Properties
May affect gene expression
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Sulfhydryl GroupStructu
re
Compound Name Thiols
Properties
Stabilize proteins
Some can have a stinky odor –
skunk, rotten eggs, garlic
Methanethiol - It is a colorless gas with a distinctive putrid smell. It is a natural substance found in the blood and brain of humans and other animals as well as plant tissues. It occurs naturally in certain foods, such as some nuts and cheese. It is also one of the main compounds responsible for bad breath and the smell of flatus.
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In many carbon compounds, the molecules are built up from smaller, simpler molecules known as MONOMERS.
Monomers can bind to one another to form complex molecules known as POLYMERS. o Large polymers are also called MACROMOLECULES o The process of reacting monomer molecules together in a
chemical reaction to form polymer chains or three-dimensional networks - POLYMERIZATION
Large Carbon Molecules:
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WATER is the most important inorganic compound in the body and it participates in two biological reactions:o Hydrolysis o Dehydration Synthesis
Biological Reactions
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Breaking down polymers by adding a water molecule.
Hydrolysis
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Breaking down polymers by adding a water molecule.
C12H22O11 + H2O C6H12O6 + C6H12O6
Hydrolysis
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Build up large molecules by releasing a molecule of water.
Dehydration Synthesis
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Build up large molecules by releasing a molecule of water.
C6H12O6 + C6H12O6 C12H22O11 + H2O
Dehydration Synthesis
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Enzyme Catalytic Cycle
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The four main classes of organic compounds essential to all living things are made from CARBON, HYDROGEN, and OXYGEN atoms, but in different ratios giving them different properties.
Molecules of Life
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Made of carbon, hydrogen, and oxygen with H to O in a 2:1 ratio
Monosaccharides are a single sugar - MONOMER
Source of energy Can be in straight or ring form -ose ending for sugars
Carbohydrates:
Glucose (C6H12O6) Ribose (C5H10O5)
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Glucose, galactose, and fructose all have the same molecular formula but differ in the arrangement of atoms = ISOMERSo Molecular formula = C6H12O6 (hexoses)
C5H10O5 (pentoses)
Carbohydrates:
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Type of Sugar
Name of Sugar Description of Sugar
Pentose ribose Found in RNA
Pentose deoxyribose Found in DNA
Hexose glucose In blood; cell’s main energy source
Hexose fructose In fruit; sweetest of monomers
Hexose galactose In milk
Carbohydrates:
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Disaccharides are double sugars Two monosaccharides condense to form
disaccharideso Formed by dehydration synthesiso Molecular formula = C12H22O11
Carbohydrates
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Bond that joins monosaccharides (carbohydrates) = glycosidic bond
Carbohydrates:
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Carbohydrates
A disaccharide is produced by joining 2 monosaccharide (single sugar) units.
In this animation, 2 glucose molecules are combined using a condensation reaction, with the removal of water.
Glucose molecules joining to form a disaccharideCondensation of Monosaccharides
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Name of Disaccharide
2 single sugars that join to form the
disaccharide Description of Sugar
Sucrose Glucose + Fructose Table Sugar
Lactose Glucose + Galactose
In milk
Maltose Glucose + Glucose In malt
Common Disaccharides
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Carbohydrates Polysaccharides many sugars: General formula – (C6H10O5)n plus H2O (n = #
monomers) Formed by dehydration synthesis Long chains of glucose molecules
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Name of Polysacchari
deDescription of Sugar
Glycogen(animal starch)
• Animal polysaccharide - stores excess sugar
• Stored in liver and muscles • Muscle contraction & movement
• Broken down into glucose and released into blood for quick energy
Starch • Plant polysaccharide• Stores excess sugar
Cellulose
• Gives plants strength and rigidity• Major component of wood and paper
• Component of cell wall
Carbohydrates:
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Elements – carbon, hydrogen, and oxygen (NOT a 2:1 H:O ratio)
Do not dissolve in water Lipids contain a large number of C-H bonds which store
more energy than C-O bonds in carbohydrates Monomers: glycerol and fatty acid
Lipids: Fats, Oils, and Waxes
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Fatty Acids:o Fatty acids are unbranched C-chains (12-28 C) with
a carboxyl group (acid) at one end• The carboxyl end is POLAR and attracted to water –
HYDROPHILIC• The hydrocarbon end is NONPOLAR and does not interact with
water – HYDROPHOBIC
Lipids:
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Fatty AcidGeneral
Structure
Saturated (single bonds)
Unsaturated (double bonds)
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Three major roles of lipids in living organisms:o Lipids can be used to store energyo Lipids are important parts of biological membraneso Lipids are waterproof coverings
Lipids:
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Saturated Fatty Acids
• Carbon atoms with 4 atoms covalently bonded
• All single bonds
• High melting points• Solid @ room temperature• Ex.) animal fat, shortening
Unsaturated Fatty Acids
• Carbon not bonded to the maximum # of atoms
• There are double bond(s)• polyunsaturated
• Liquid @ room temperature• Primarily in plants• Energy storage in animals
Saturated & Unsaturated Fatty Acids
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Saturated and Unsaturated Fatty Acids:
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Lipids (fats, oils, and waxes) are formed by a glycerol molecule bonding to fatty acid(s) o formed by dehydration synthesis
Lipids
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Dehydration Synthesis:
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Three fatty acids attached to glycerol
Triglycerides
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Formation of a Triglyceride
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Two fatty acids joined to a glycerol Makes up cell membrane - PHOSPHOLIPID BILAYER
Phospholipids
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Elements: Carbon, Hydrogen, Oxygen, Nitrogen Monomer: AMINO ACID (20 different kinds) Each amino acid has a central carbon atom bonded
to 4 other atoms or functional groups
Proteins
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Proteins Bond that joins amino acids (protein) = PEPTIDE
BOND
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Formation of a peptide bond
amino acid 1 amino acid 2 dipeptide water
Peptide bondFormation of a peptide bond
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1. Control the rate of reactions2. Regulate cell processes3. Form important cellular structures4. Transport substances into or out of cells5. Help to fight disease
Functions of Proteins
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Enzyme + Substrate = ES complex EP complex = Enzyme + product(s)
Enzymes and Substrates:
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Enzyme Catalytic Cycle
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Protein that has lost its active conformation, or shape
Denaturing caused by:o Temperatureo Solute (salt) Concentrationo pH
Denaturing Proteins:
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Large, complex organic compounds that store information in cells, using a system of four compounds to store hereditary information, arranged in a certain order as a code for genetic instructions of the cell.
Elements: Carbon, Hydrogen, Oxygen, Nitrogen, Phosphorus Monomer: Nucleotide1. Phosphate group (Phosphoric Acid)2. 5-carbon (pentose) sugar (Deoxyribose or Ribose)3. Nitrogenous Base
Nucleic Acids
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Nitrogenous Bases There are FOUR Nitrogen bases
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Nucleic Acids Nucleotides combine, in DNA to form a double
helix, and in RNA a single helix The sides of the ladder are made up of the phosphate group and the sugar and the rungs of the ladder are nitrogen bases Examples of Nucleic Acids:
1. Deoxyribonucleic Acid (DNA)2. Ribonucleic Acid (RNA)
Nucleic Acids and Dehydration Synthesis