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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 – – – – 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 • • • • 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 • • • • • • 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 • • • • 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 • • • • 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.