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PowerPoint® Lecture Slides Prepared by Patty Bostwick-Taylor, Florence-Darlington Technical College CHAPTER 2 Basic Chemistry © 2012 Pearson Education, Inc. Power Point Assignment For all the items marked with an * fill in the indicated information using Chapter 2 information. Do not look up these items in the glossary. The professor will not necessarily review these items so it is critical to your understanding of the material that you complete these notes on your power point. It is a good idea to download and print the powerpoint out and bring it to class. © 2012 Pearson Education, Inc. I. Introduction A. Matter and Energy 1. Matter:* Define 2. Energy:* Define a. Chemical b. Electrical c. Mechanical d. Radiant © 2012 Pearson Education, Inc. B. Composition of Matter 1. Elements:* Define •96 percent of the body = four elements •C * What does this letter stand for? •O * What does this letter stand for? •H * What does this letter stand for? •N * What does this letter stand for? 2. Atoms—building blocks of elements © 2012 Pearson Education, Inc. 3. Subatomic Particles a. Nucleus *Where is it and what does it contain Helium atom • Protons * Charge & location: e- • Neutrons * Charge & location: b. Electrons: Orbiting the nucleus • Electrons * Size, Charge & Location e- Proton Neutron c. Atomic Number = Number of protons (equals numbers of electrons) in an atom; different for each d. Atomic mass number: © 2012 Pearson Education, Inc. • How many protons, neutrons, and electrons does Hydrogen normally have? • Helium? • Lithium? © 2012 Pearson Education, Inc. Figure 2.2 4. Isotopes •Isotopes = Atoms of an element vary in the number of ______________ •Isotopes have the same number of? • Atomic Weight of Isotopes © 2012 Pearson Education, Inc. Radioactivity •Radioisotope = •Stability? •Decomposes: •Radioactivity: •Examples: Uranium, Iodine, … © 2012 Pearson Education, Inc. 5. IONS = • Positive & Negative Ions • Properties as compared to atoms: Na atom A Sodium Atom loses its outer electron to become a Sodium Ion Na+1 ion or Na+ ion + Table Salt © 2012 Pearson Education, Inc. Ions Examples… an Electron + Cl atom A Chlorine Atom gains an electron from another atom Cl ¯1 ion or Cl ¯ ion © 2012 Pearson Education, Inc. Properties of atoms compared to their ions … © 2012 Pearson Education, Inc. Figure 2.4 C. Making Larger Chemicals out of the Atoms or Elements 1. Chemical Formulas 2. Molecules and Compounds a. Molecule—two or more atoms, of the same or different elements, combined chemically H2O O2 NaCl b. Compound—two or more atoms of different elements combined chemically © 2012 Pearson Education, Inc. 3. Chemical Bonds • Bonding involves interactions between electrons in outer part of 2 atoms • One CHEMICAL BOND = ____ electrons a. Ionic Bonds (Electrovalent Bonds) • Bond Formed When: • Example: SALT Na atom © 2012 Pearson Education, Inc. Cl atom Na+ Cl ¯ b. Covalent Bonds i) Bonds occurs when: ii) Types Non Polar—electrons are: © 2012 Pearson Education, Inc. Polar Covalent Bonds • Bond– electrons are: • Example: WATER The Oxygen: -1/2 The Hydrogens: Oxygen • Polarity +1/2 +1/2 • Polar Molecule 2 Hydrogens -1/2 • Attraction between Polar Molecules +1/2 © 2012 Pearson Education, Inc. +1/2 Figure 2.8 Polar Molecules … Example: Attraction between Water Molecules -- creates surface tension Hydrogen Bonds Figure 2.9 © 2012 Pearson Education, Inc. D. Chemical Reactions 1. Chemical Reactions: a. Reactants = b. Products = c. Process of making Products • Bonds broken in ______________ • Atoms rearranged • New bonds in _______________ H2O + Reactants © 2012 Pearson Education, Inc. CO2 ---> ---> H2CO3 Products 2. Types of Chemical Reactions a. Synthesis reaction = •Example: Synthesis of Proteins © 2012 Pearson Education, Inc. b. Decomposition Reactions = •Example: Glycogen is broken down into ___ © 2012 Pearson Education, Inc. c. Exchange reaction: •Example: © 2012 Pearson Education, Inc. Parts moved around E. SOLUTIONS SOLUTION = a mixture of chemicals in a liquid - AQUEOUS SOLUTIONS = the liquid is WATER 1. Solvent: the liquid 2. Solute: the dissolved chemicals 3. The Concentration of a Solution: can use percentages % Solvent + % Solutes = 100% © 2012 Pearson Education, Inc. • 4. Movement of chemicals in Solutions a. Diffusion: b. Osmosis: water solute © 2012 Pearson Education, Inc. II. Biochemistry: Essentials for Life •TWO TYPES •Organic •Inorganic A. Inorganic compounds •No “C” framework •simpler •Examples © 2012 Pearson Education, Inc. Inorganic Compounds … 1. Water -- STUDENTS READ IN TEXT 2. Salts •ions •Vital • some conduct electrical currents •Examples: © 2012 Pearson Education, Inc. H – + O H + Water molecule Na+ Na+ Cl– © 2012 Pearson Education, Inc. Salt crystal Cl– Ions in solution Figure 2.11 Inorganic Compounds … 3. Acids •Release ______________ (H+) 4. Bases •Release hydroxyl ions (OH–) •Are ______________ acceptors •Neutralization reaction •Acids + bases - water + salt © 2012 Pearson Education, Inc. pH •concentration of hydrogen ions •Neutral = •Acidic = •Basic = •Buffers—regulate pH change © 2012 Pearson Education, Inc. B. ORGANIC CHEMICALS = framework of ____________ Types • Fossil Fuels • Biochemicals • Carbohydrates • Lipids • Proteins • Nucleic Acids © 2012 Pearson Education, Inc. Biochemicals 1. Carbohydrates •Elements: • Ratio of Hydrogen to Oxygen: •General Function: •Classification • Monosaccharides • Disaccharides • Polysaccharides © 2012 Pearson Education, Inc. Organic Compounds … 2. Lipids •Elements: •Ratio of H to C: •Solubility in water: •Types © 2012 Pearson Education, Inc. Lipids •Types •Neutral fats (triglycerides) •Location: •Function: •Composed of: Glycerol & 3 Fatty Acids © 2012 Pearson Education, Inc. Saturated Fats © 2012 Pearson Education, Inc. Figure 2.16a Un-Saturated Fat © 2012 Pearson Education, Inc. Figure 2.16b Lipids … • Types … •Phospholipids •Composition: •Function: •Important Characteristic: Glycerol + 2 Fatty Acids Phosphate (Charged) © 2012 Pearson Education, Inc. Lipids … •Steroids •Have rings •Cholesterol is the basis for all steroids made in the body • Function: © 2012 Pearson Education, Inc. Important Organic Compounds … 3. Proteins •Elements: •Subunit: •structure •R group © 2012 Pearson Education, Inc. Level of Complexity in Structure (a) Primary structure. sequence of amino acids. Amino acids Hydrogen bonds Amino acids (b) Secondary structure. Initial Folding into 2-D structure Alphahelix © 2012 Pearson Education, Inc. -pleated sheet Figure 2.18a-b Tertiary Structure 3-D Quaternary Structure Two or more polypetides © 2012 Pearson Education, Inc. Figure 2.18c-d Proteins– Structure & Function •Fibrous proteins, Structural proteins •Function •Stability •Examples: © 2012 Pearson Education, Inc. © 2012 Pearson Education, Inc. Figure 2.19a Proteins •3-D proteins have specific Functions •Stability– Denaturation •Functions: •Carriers •Long-distance transport •Hormones •Enzymes © 2012 Pearson Education, Inc. Heme group Globin protein (b) Hemoglobin molecule composed of the protein globin and attached heme groups. (Globin is a globular or functional protein.) © 2012 Pearson Education, Inc. Figure 2.19b Enzymes •Function: •How Function: • active site © 2012 Pearson Education, Inc. Energy is Water is absorbed; released. bond is H2O formed. Substrates (S) e.g., amino acids + Product (P) e.g., dipeptide Peptide bond Active site Enzyme-substrate complex (E-S) Enzyme (E) © 2012 Pearson Education, Inc. 1 Substrates bind to active site. Enzyme changes shape to hold substrates in proper position. 2 Structural changes occur, resulting in the product. Enzyme (E) 3 Product is released. Enzyme returns to original shape, ready to catalyze another reaction. Figure 2.20 Organic Compounds … 4. Nucleic Acids •Types: •Built from nucleotides •Pentose (5 carbon) sugar •A phosphate group •A nitrogenous base • A = Adenine • G = Guanine • C = Cytosine • T = Thymine • U = Uracil. © 2012 Pearson Education, Inc. Deoxyribose Phosphate sugar Adenine (A) (a) Adenine nucleotide (Chemical structure) KEY: © 2012 Pearson Education, Inc. Thymine (T) Cytosine (C) Adenine (A) Guanine (G) Figure 2.21a Nucleic Acids •DNA • Location •Structure: •Type sugar: deoxyribose • Bases: • Function: © 2012 Pearson Education, Inc. Hydrogen bond Deoxyribose sugar Phosphate (d) Diagram of a DNA molecule KEY: © 2012 Pearson Education, Inc. Thymine (T) Cytosine (C) Adenine (A) Guanine (G) Figure 2.21c-d Nucleic Acids •Ribonucleic acid (RNA) •Structure: •Sugar •Bases •Types •Function: © 2012 Pearson Education, Inc. Released mRNA Nucleic Acid Derivatives •Adenosine triphosphate (ATP) •Modified Nucleotide of adenine with three phosphate groups •Function: __________________________ •Examples © 2012 Pearson Education, Inc. (a) Adenosine triphosphate (ATP) Adenosine diphosphate (ADP) (b) Hydrolysis of ATP © 2012 Pearson Education, Inc. Figure 2.22a-b