1 / 57

Biochemistry Notes

Learn about elements, compounds, chemical bonds, and reactions in biology. Understand the periodic table, isotopes, and how energy affects chemical reactions. Dive into enzymes as catalysts for reactions.

parisp
Download Presentation

Biochemistry Notes

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript


  1. Biochemistry Notes

  2. Chemistry in Biology Chapter 6 6.1 Atoms, Elements, and Compounds Elements • An element is a pure substance that cannot be broken down • There are over 100 known elements, 92 of which occur naturally. • Each element has a unique name and symbol.

  3. Chemistry in Biology Chapter 6 6.1 Atoms, Elements, and Compounds The Periodic Table of Elements • Horizontal rows are called periods. • Vertical columns are called groups.

  4. Chemistry in Biology Chapter 6 6.1 Atoms, Elements, and Compounds • Chemistry = study of matter. • Atoms are the building blocks of matter. • Neutrons and protons are located at the nucleus of the atom. • Protons are positively charged particles. • Neutrons are particles that have no charge.

  5. Chemistry in Biology Chapter 6 6.1 Atoms, Elements, and Compounds • Electrons are negatively charged particles that are located outside the nucleus.

  6. 6.1 Atoms, Elements, and Compounds • Atomic Number: number of protons in the nucleus of an element (atom).

  7. 6.1 Atoms, Elements, and Compounds • Atomic Mass: the number of protons & neutrons in the nucleus of an element (atom). • Find the neutrons only: • Atomic mass-atomic number=neutrons • Ex: Carbon Picture

  8. Chemistry in Biology Chapter 6 6.1 Atoms, Elements, and Compounds Isotopes • Atoms of the same element that have the same number of protons and electrons but have a different number of neutrons

  9. Isotope Clip • http://glencoe.mcgraw-hill.com/sites/dl/free/0078695104/164155/00038306.html

  10. Chemistry in Biology Chapter 6 6.1 Atoms, Elements, and Compounds Radioactive Isotopes • When a nucleus breaks apart, it gives off radiation that can be detected and used for many applications.

  11. Chemistry in Biology Chapter 6 6.1 Atoms, Elements, and Compounds Compounds • A pure substance formed when two or more different elements combine • Compounds cannot be broken down into simpler compounds or elements by physical means, must be a chemical reaction

  12. Chemistry in Biology • A molecule is a compound in which the atoms are held together by covalent bonds. Chapter 6 6.1 Atoms, Elements, and Compounds Chemical Bonds • Covalent bonds • Chemical bond that forms when electrons are shared

  13. Chemistry in Biology Chapter 6 6.1 Atoms, Elements, and Compounds Ionic Bonds • Electrical attraction between two oppositely charged atoms or groups of atoms

  14. Chemistry in Biology Chapter 6

  15. Chemistry in Biology Chapter 6 6.1 Atoms, Elements, and Compounds • Some atoms donate or accept electrons easier than other atoms. • The elements identified as metals tend to donate electrons. • The elements identified as nonmetals tend to accept electrons.

  16. Chemistry in Biology Chapter 6 6.1 Atoms, Elements, and Compounds van der Waals Forces • When molecules come close together, the attractive forces between slightly positive and negative regions pull on the molecules and hold them together. • The strength of the attraction depends on the size of the molecule, its shape, and its ability to attract electrons.

  17. Chemistry in Biology Chapter 6 6.2 Chemical Reactions Reactants and Products • A chemical reaction is the process by which atoms or groups of atoms in substances are reorganized into different substances. Chemical reaction • Clues that a chemical reaction has taken place include the production of heat or light, and formation of a gas, liquid, or solid. Physical reaction

  18. Chemistry in Biology Chapter 6 6.2 Chemical Reactions Chemical Equations • Chemical formulas describe the substances in the reaction and arrows indicate the process of change. • Reactants are the starting substances, on the left side of the arrow. • Products are the substances formed during the reaction, on the right side of the arrow.

  19. Chemistry in Biology Chapter 6 6.2 Chemical Reactions • Glucose and oxygen react to form carbon dioxide and water.

  20. Chemistry in Biology Chapter 6 6.2 Chemical Reactions Balanced Equations • The law of conservation of mass states matter cannot be created or destroyed. • The number of atoms of each element on the reactant side must equal the number of atoms of the same element on the product side.

  21. Chemistry in Biology Chapter 6 6.2 Chemical Reactions Energy of Reactions • Theactivation energy is the minimum amount of energy needed for reactants to form products in a chemical reaction.

  22. Chemistry in Biology Chapter 6 6.2 Chemical Reactions • This reaction is exothermic and released heat energy. • The energy of the product is lower than the energy of the reactants.

  23. Chemistry in Biology Chapter 6 6.2 Chemical Reactions • This reaction is endothermic and absorbed heat energy. • The energy of the products is higher than the energy of the reactants.

  24. Chemistry in Biology • It does not increase how much product is made and it does not get used up in the reaction. Chapter 6 6.2 Chemical Reactions Enzymes • A catalyst is a substance that lowers the activation energy needed to start a chemical reaction. • Enzymes are biological catalysts.

  25. Chemistry in Biology Chapter 6 6.2 Chemical Reactions • The reactants that bind to the enzyme are called substrates. • The specific location where a substrate binds on an enzyme is called the active site. Fits together like a lock and key

  26. Chemistry in Biology Chapter 6 6.2 Chemical Reactions • The active site changes shape and forms the enzyme-substrate complex, which helps chemical bonds in the reactants to be broken and new bonds to form. • Factors such as pH, temperature, and the concentrations of substrate & enzyme affect enzyme activity.

  27. What role do enzymes play in chemical reactions within living organisms? • Chemical reaction – process that changes 1 set of chemicals into another set of different chemicals • Reactants – starting chemicals • Products – ending chemicals • Involves breaking of bonds and forming new ones • Energy • Either released or absorbed • Activation energy – energy needed to start a reaction

  28. Chemistry in Biology Chapter 6

  29. Enzyme Review • Enzymes are a form of ___. a. carbohydrate b. lipid c. protein • Enzymes can speed up a reaction, so they are called ___. a. catalysts b. reactants c. inhibitors • The area where the enzyme attaches to the substrate is called the ___. a. active site b. cohesion area c. vectors 4. If the enzyme is heated, it will change shape. This ______ affect the ability of the enzyme to work. a. will b. will not • Enzymes work because they lower the ___. a. chemical reactant rate b. active site location c. activation energy

  30. Chemistry in Biology Chapter 6 6.3 Water and Solutions Water’s Polarity • Molecules that have an unequal distribution of charges are called polar molecules. • Polarity is the property of having two opposite poles. (Think of North & South Pole) • A hydrogen bond is a weak interaction involving a hydrogen atom and a fluorine, oxygen, or nitrogen atom.

  31. Chemistry in Biology Chapter 6 6.3 Water and Solutions

  32. Water Polarity & Hydrogen Bond VideoClip • http://glencoe.mcgraw-hill.com/olcweb/cgi/pluginpop.cgi?it=swf::550::400::/sites/dl/free/0078695104/383915/CH06_Properties_of_Water_103006.swf::Visualizing Properties of Water

  33. Water properties: • Water is cohesive • Cohesion: attraction between same molecules, causes molecules to draw inward at surface • Ex: allows some insects & spiders can “walk” on the surface • Water is adhesive • Adhesion: attraction between different molecules, causes water to bend at the surface • Ex: capillary action-pulls column of water up to the top of a plant

  34. Water properties: • Water is called “Universal solvent”: dissolves many other substances due to polarity • Differences in charges pulls/pushes substances apart (Like a magnet attracts or repels other magnets) • Water exhibits evaporative cooling: removes heat when it evaporates from a surface • Ex: sweating cools skin • Water expands during freezing: expands into crystal formation releasing heat • Ex: rocks broken up by ice creating soil; ice layer protects fruit from freezing

  35. Chemistry in Biology Chapter 6 6.3 Water and Solutions Homogenous Mixtures • A mixture that has a uniform composition throughout • A solvent is a substance in which another substance is dissolved. • A solute is the substance that is dissolved in the solvent. Food coloring dissolved in water forms a homogenous mixture.

  36. Chemistry in Biology Chapter 6 6.3 Water and Solutions Heterogeneous Mixtures • In a heterogeneous mixture, the components remain distinct. A salad is a heterogeneous mixture.

  37. Chemistry in Biology Chapter 6 6.3 Water and Solutions Acids and Bases • Substances that release hydrogen ions (H+) when dissolved in water are called acids. • Substances that release hydroxide ions (OH–) when dissolved in water are called bases.

  38. Chemistry in Biology Chapter 6 6.3 Water and Solutions pH and Buffers • The measure of concentration of H+ in a solution is called pH. • Acidic solutions have pH values lower than 7. • Basic solutions have pH values higher than 7.

  39. Chemistry in Biology Chapter 6 6.3 Water and Solutions • Buffers are mixtures that can react with acids or bases to keep the pH within a particular range.

  40. Chemistry in Biology Chapter 6 6.4 The Building Blocks of Life Organic Chemistry • The study of all compounds containing the element CARBON

  41. Chemistry in Biology Chapter 6 6.4 The Building Blocks of Life • Carbon compounds can be in the shape of straight chains, branched chains, and rings.

  42. What is a macromolecule? • A giant molecule made up of 100’s or 1000’s or smaller units called MONOMERS • Monomers link together to form large POLYMERS • formed by polymerization

  43. Chemistry in Biology Chapter 6 6.4 The Building Blocks of Life Macromolecules • Carbon atoms can be joined to form carbon molecules. • Macromolecules are large molecules formed by joining smaller organic molecules together. • Polymers are molecules made from repeating units of identical or nearly identical compounds linked together by a series of covalent bonds.

  44. The 4 types of macromolecules: NUCLEIC ACIDS CARBOHYDRATES PROTEINS LIPIDS

  45. Chemistry in Biology Chapter 6 6.4 The Building Blocks of Life Carbohydrates • Made up of carbon, hydrogen, and oxygen

  46. Chemistry in Biology Chapter 6 6.4 The Building Blocks of Life • Values of n ranging from three to seven are called simple sugars, or monosaccharides. • Two monosaccharides joined together form a disaccharide. • Longer carbohydrate molecules are called polysaccharides.

  47. CARBOHYDRATES • Made up of C,H,O • Used as main source of energy • Sugars: quick source of energy • Monosaccharide-simple sugar, disaccharide-2, polysaccharide-many • Ex: glucose, lactose, fructose, sucrose • Starches: many sugars linked together, source of energy breaking down slower • Used by plants for energy storage • Ex: potatoes, pasta, bread, grains Two types:

  48. Figure 2-13 A Starch Section 2-3 Starch Glucose Go to Section:

  49. Chemistry in Biology Chapter 6 6.4 The Building Blocks of Life Lipids • Made mostly of carbon and hydrogen • A triglyceride is a fat if it is solid at room temperature and an oil if it is liquid at room temperature.

  50. Chemistry in Biology Chapter 6 6.4 The Building Blocks of Life • Lipids that have tail chains with only single bonds are called saturated fats. • Lipids that have at least one double bond in the tail chain are called unsaturated fats. • Fats with more than one double bond in the tail are called polyunsaturated fats.

More Related