Transcript Organic Chemistry

Inorganic Chemistry
• Atoms – Smallest unit of matter
• Elements – Different types of matter
– 92 in nature, 15 in life, 4 major elements in life
• Molecules – 2 or more atoms ex) H2, O2, N2
• Compounds – 2 or more elements ex) H2O
Atomic Structure
• Particles – protons +, electrons -, neutrons n
• Nucleus – contains protons & neutrons
• Energy levels – electrons orbit nucleus
– 1st – 2 electrons max
– 2nd – 8 electrons max
– 3rd – 8 electrons max
Characteristics of atoms
• Atomic Number - # of Protons = # of Electrons
• Atomic Mass - # Protons + # Neutrons
What atoms like to be…..
1) Neutral
2) Full outer energy level
Elements of Life
• Hydrogen – 1 proton, 0 neutrons, 1 electron
– 1 outer electron (1 needed)
• Carbon – 6 protons, 6 neutrons, 6 electrons
– 4 outer electrons (4 needed)
• Nitrogen – 7 protons, 7 neutrons, 7 electrons
– 5 outer electrons (3 needed)
• Oxygen – 8 protons, 8 neutrons, 8 electrons
– 6 outer electrons (2 needed)
Electron Configuration
Chapter 2: Small Molecules: Structure and Behavior
2.5
Figure 2.5
figure 02-05.jpg
Isotopes
• Different forms or the same element
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Carbon 14 vs. Carbon 12
Hydrogen 2 or 3 vs. Hydrogen 1
Nitrogen 15 vs. Nitrogen 14
Oxygen 18 vs. Oxygen 16
• Tracers – use of radioisotopes to trace
chemical pathways in living things.
Isotopes
Chapter 2: Small Molecules: Structure and Behavior
2.2
Figure 2.2
figure 02-02.jpg
Chemical Bonding
• Covalent Bonds
• Ionic Bonds
• Hydrogen Bonds
Covalent Bonding
• Covalent bonding – sharing electron pairs
• Single – share 1 pr. of electrons (H2)
• Double – share 2 prs. of electrons (O2)
• Triple – share 3 prs. of electrons (N2)
Methane
Chapter 2: Small Molecules: Structure and Behavior
2.7
Figure 2.7
figure 02-07.jpg
Polar Covalent Bonds
• Unequal sharing of the electrons creates
partial charges on the molecule
– Ex) Water
• Hydrogen bonds form between partial
positive and negative charges on atoms
Ionic Bonding
• Ionic bonding – transfer of electrons from
one atom to another atom.
– Ex) NaCl - Na+ & Cl-
• Ions – charged atoms or groups of atoms
Ionic Bonds
Chapter 2: Small Molecules: Structure and Behavior
2.10
Figure 2.10
figure 02-10.jpg
Salt dissolves in water
Chapter 2: Small Molecules: Structure and Behavior
2.11
Figure 2.11
figure 02-11.jpg
Organic Chemistry
Compounds found in living things.
Contain C,H,O, but based on carbon.
Form long chains, branched chains, rings.
4 Types:
Carbohydrates
Proteins
Lipids
Nucleic Acids
Carbohydrates
Characteristics
• Contain C, H, O & H:O ratio = 2:1
• Primary energy source for living things.
• Form ring structures
• Names end in –ose.
Carbohydrates
Building Blocks
• Monosaccharide ex) Glucose – C6H12O6
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Galactose, Fructose
Isomers – Different forms of the same molecule
Disaccharide ex) Maltose, Lactose, Sucrose
C12H22O11
Dehydration Synthesis – Remove water to make a
larger molecule.
Polysaccharide ex) Starch, Cellulose, Glycogen
Monosaccharides
Chapter 3: Macromolecules: Their Chemistry and Biology
3.12 –
Part 2
Figure 3.12 – Part 2
figure 03-12b.jpg
Dehydration Synthesis
Chapter 3: Macromolecules: Their Chemistry and Biology
3.2
Figure 3.2
figure 03-02.jpg
Lipids
Characteristics
• Contain C,H,O, but much less oxygen
• Cell membranes, secondary energy source
• Lipids are NOT soluble in water
• Common examples: Fats, oils, waxes
Lipids
Building Blocks
• Glycerol + 3 Fatty Acids
• Glycerol has 3 –OH groups
• Fatty Acids have –COOH group
• Dehydration Synthesis removes 3 waters.
Lipid formation
Chapter 3: Macromolecules: Their Chemistry and Biology
3.19
Figure 3.19
figure 03-19.jpg
Fatty Acid Chains
• Saturated
– Maximum # of hydrogen atoms
• Unsaturated
– 1 double bond, 2 less hydrogens
• Polyunsaturated
– Many double bonds, much fewer hydrogens
• Cholesterol – forms from saturated F.A.’s
Fatty Acid Chains
Chapter 3: Macromolecules: Their Chemistry and Biology
3.20
Figure 3.20
figure 03-20.jpg
Proteins
Characteristics
• Contain C,H,O,N (S)
• Cell structures, pigments, hormones,
antibodies, contractile materials, enzymes.
• Forms: helixes, folded chains, globular.
• Names end in _______.
Proteins
Building Blocks
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Amino Acids – 20 different types
Central carbon atom
Amino group –NH2
Acid Group –COOH
Single Hydrogen
20 different ® groups
Charged Amino Acids
Chapter 3: Macromolecules: Their Chemistry and Biology
Table 3.2 –
Part 1
Table 3.2 – Part 1
table 03-02a.jpg
Polar & Special Amino Acids
Chapter 3: Macromolecules: Their Chemistry and Biology
Table 3.2 –
Part 2
Table 3.2 – Part 2
table 03-02bc.jpg
Hydrophobic Amino Acids
Chapter 3: Macromolecules: Their Chemistry and Biology
Table 3.2 –
Part 3
Table 3.2 – Part 3
table 03-02d.jpg
Proteins
• Dipeptide – 2 Amino acids
• Dehydration synthesis forms peptide bond.
• Polypeptide – many amino acids.
Dehydration Sysnthesis
Chapter 3: Macromolecules: Their Chemistry and Biology
3.4
Figure 3.4
figure 03-04.jpg
4 levels of structural organization
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1) Order of amino acids
2) Initial folding (helix, sheets)
3) Folding of folds (globular)
4) Multiple polypeptide chains together
• 3-D shape determines protein function
• Hydrogen bonds hold molecule in it’s shape
figure 03-05a.jpg
3.5 –
Part 1
Figure 3.5 – Part 1
figure 03-05b.jpg
3.5 –
Part 2
Figure 3.5 – Part 2
Enzymes
• Proteins that act as catalysts to speed up
chemical reactions in a cell.
• Active Site – reaction part of enzyme.
• Substrate – substance enzyme acts on.
• Lock & key theory – substrate exactly fits
into enzyme active site to perform reaction.
• Enzyme is not affected by the reaction.
Characteristics of Enzymes
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Enzymes are Reusable. Only need a little.
Work best at an Optimal Temperature.
Work best at an Optimal pH.
Rate depends on concentration of both the
enzyme and the substrate.
• Co-enzymes assist enzyme action.
• Most work inside cells, some outside.