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Chapter 3

Chapter 3. Matter and Energy. Vocabulary. Acid activation energy Amino acid bond Carbohydrate chemical formula Coenzyme compound Covalent bond electron cloud Element energy level Enzyme ion Ionic bond isomer Kinetic energy lipid Molecule nucleic acid

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Chapter 3

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  1. Chapter 3 Matter and Energy

  2. Vocabulary • Acid activation energy • Amino acid bond • Carbohydrate chemical formula • Coenzyme compound • Covalent bond electron cloud • Element energy level • Enzyme ion • Ionic bond isomer • Kinetic energy lipid • Molecule nucleic acid • Polypeptide polysaccharide • Potential energy protein • solution

  3. Matter and Its Combinations • All matter is made up of atoms. • Protons (+ charge) and neutrons (no charge) are in the center. • Electrons ( - charge) are outside of the nucleus in an electron cloud. • Click here!

  4. Energy Levels • Electrons travel around the nucleus at different energy levels. The farther away from the nucleus an electron is, the more energy it has because it’s farther away from the pull of the positively charged protons.

  5. Atom Song (3:28) • The first energy level closest to the nucleus can hold up to 2 electrons. • 2nd level: up to 8 electrons. • 3rd level: 18 e- • 4th level: 32 e-

  6. Elements (2:05) • Elements are substances composed of only one kind of atom. • The number of neutrons in any given element are the same except in isotopes. • Isotopes have different numbers of neutrons and thus different masses then the most common form of any given element. Examples: C-12 and C-14 are isotopes of carbon. One has a mass of 12 amu and the other a mass of 14 amu because it has more neutrons.

  7. Elements vs. Compounds • Elements • Carbon: C • Hydrogen: H • Oxygen: O • Nitrogen: N • Phosphorous: P • Compounds • Methane: CH4 • Hydrogen molecule: H2 • Oxygen molecule: O2 • Nitrogen molecule: N2 • Phosphate ion: PO43-

  8. Covalent vs Ionic bonding • When atoms combine chemically by sharing electrons, they have formed a covalent bond. • Ions are atoms that have given up or taken electrons. Compounds that are formed by ions(2:12) are called ionic compounds.(17:38)

  9. Chemical equations • Chemical equations use formulas to describe chemical changes that take place. Numbers of atoms before the reaction and after the reaction must be the same. • Reactants  Products • Hydrogen + Oxygen produces water • H2 + O2  H2O (unbalanced equation) • Balanced, this equation is: • 2H2 + O2  2H2O

  10. Balance these equations: • Zn + HCl ZnCl2 + H2 • Mg + H2O  Mg(OH)2 • Mg(OH)2 + HCl  MgCl2 + H2O • NaClO3  NaCl + O2 • CH4 + O2  CO2 + H2O

  11. Solutions • Solutions are homogeneous mixtures that are the same throughout, although they can have varying amounts of dissolved substances in them. • So, why do some things dissolve in water and others don’t? • Potassium permanganate dissolution demo 1. (click here) (1:00) • Demo 2 (click here) (1:00)

  12. Acids and Bases Introduction to Acids/Bases (2:04) pH Scale (2:42) pH in the Chemistry of Nature (3:19)

  13. 3.2 Biological Chemistry • Carbon compounds • Structure • Isomers • Carbohydrates • Monosaccharides, Disaccharides and Polysaccharides • Lipids • Structure • Proteins • Structure • Nucleic Acids • Condensation Reactions • Hydrolysis

  14. Carbon Compounds • Living organisms as well as substances like fossil fuels are made up of carbon compounds. Carbon has 4 valence electrons that can form single, double and triple bonds.

  15. Isomers • Isomers are molecules that have identical formulas but different structural arrangements. • Both of the molecules → have the formula C6H14 but have different structures. • These different shapes do not constitute different compounds. To get a different compound the bonding pattern of the atoms would have to change. Branched chain isomers (4:36)

  16. Carbohydrates • Carbohydrates are organic compounds made up of 1 part carbon to 2 parts hydrogen and 1 part oxygen, or a 1:2:1 ratio. • Glucose, galactose and fructose are examples of simple sugars called monosaccharides. • Intro to carbohydrates (2:00)

  17. Two simple sugars can bond together to form disaccharides. Sucrose (table sugar), is made up of glucose and fructose bonded together. • Monosaccharides and disaccharides (click here) • (2:16)

  18. Complex Carbohydrates:Polysaccharides ( click) (4:32) Glycogen • Polysaccharides are formed from long chains of monosaccharides. • An example is glycogen which is made up of glucose. The body can store the glycogen and then convert it back to glucose when needed. • Others include cellulose and starch. Assignment: Using a Venn Diagram, compare and contrast simple and complex carbohydrates

  19. Fats, Lipids and Fatty Acids • Fats and oils belong to a class of organic compounds called lipids. • Are fats good? (3:07) • Lipids and cholesterol (1:12) • Fatty Acids (2:45)

  20. Proteins and Amino Acids (2:30) • What is protein? (3:05) • Proteins are built from chains of amino acids. They have a central carbon atom bonded to a carboxyl group, a hydrogen atom and an amino group. • The bonds that form proteins are called peptide bonds. (2: 23)

  21. Nucleic Acids • Molecules that control an organism’s basic appearance and behavior are called nucleic acids. • These include deoxyribonucleic acid (DNA) and ribonucleic acid (RNA). DNA Molecule

  22. Condensation Reaction • Maltose is a large disaccharide formed from the condensation (water producing) reaction between two glucose molecules. • Amino acids from the foods you eat form proteins with this type of reaction. Two glucose molecules react to form maltose and water

  23. Hydrolysis • Hydrolysis (2:10) occurs when the addition of a water molecule breaks up a larger molecule into smaller molecules. • A dipeptide + water can yield two amino acids such as glycine and alanine. Formation of glucose and fructose by adding a water molecule to sucrose

  24. ENERGY!!! • Potential and Kinetic Energy (2:07) • Law of Conservation of Energy (4:35) Potential and Kinetic Energy

  25. Activation energy/Enzymes • Activation energy is the smallest amount of energy it takes to start a chemical reaction. • Different reactions require different amounts of energy. Heat is a common form of energy used to start a chemical reaction, but is not practical when looking at biochemical reactions because too much heat would kill cells. • Enzymes are proteins that lower the activation energy needed for chemical reactions in cells. ↑ I am an enzyme, click on me! (1:37)

  26. Enzymes/Substrates • Enzymes are reusable and each has a unique shape that determines its chemical function. • Substrates work with enzymes in chemical reactions. • Most enzymes are named by adding the suffix –ase to the name of the substrate reaction the enzyme controls. ie: the enzyme that guides the conversion of maltose to glucose is called maltase.

  27. Substrates/Coenzymes • Substrates attach themselves to enzymes, which change shape slightly which lowers the activation energy needed because the active site of the enzyme will only fit together with a certain part of the substrate. • Coenzymes sometimes made from vitamin molecules, are reusable, and needed in small amounts. They are enzymes’ little helpers by helping substrates bind or transferring atoms from one substrate to another..

  28. Micro Elements (next 9 slides) • Iron (Fe) Contained in hemoglobin and myoglobin which are required for oxygen transport. • Anemia results from a lack of Fe. • Enlarged liver, diabetes and cardiac failure can be caused by too much iron. • Hemochromatosis is a genetic disease caused by excess iron absorption.

  29. Potassium (K) is a major electrolyte of blood and extracellular fluid. Maintains pH and osmotic balance. • Chlorine (Cl) Major electrolyte of the blood and intracellular/extracellular fluid. Maintains pH and osmotic balance. • Sulfur(S) Part of essential amino acids. Contained in vitamins, thiamin and biotin. Part of glutathione and required for detoxification.

  30. Copper (Cu) regulates Fe transport and release from storage. • Too much copper can cause liver disease and is associated with the genetic disorder, Wilson’s disease, where excess copper affects the brain, eyes and kidneys. • Manganese (Mn) Needed for bone formation and reproduction. Too much causes poor Fe absorption.

  31. Iodine: Produces thyroxine which controls metabolic rate and prevents goiter.

  32. Zinc (Zn) important for reproduction, required for DNA binding which regulate a variety of activities. An excess can cause anemia or reduced bone formation. • Selenium (Se) Deficiency esults in oxidative membrane damage. In humans it causes heart damage, known as Keshan’s Disease.

  33. Fluorine (F) Tooth development and protection. • Strengthens enamel to prevent decay. • Cobalt (Co) An excess may cause cardiac failure.

  34. Macro elements—essential for proteins and enzyme activity • Calcium: Ca Structure of bones and teeth • Phosphorous: P • Structure of bones and teeth, required for ATP production.

  35. Magnesium (Mg) Bone structure, too little results in muscle spasms and can lead to Ca deficiency. • Sodium (Na) Major electrolyte of blood and extracellular fluid. Maintains pH and osmotic balance.

  36. Molybdenum (Mo) An excess can cause diarrhea and growth reduction. • Chromium (Cr) Helps regulate sugar levels. Deficiency may cause hyperglycemia (elevated blood sugar) and glucosuria. (sugar in urine)

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