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Lecture Notes 3: Biochemistry

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Lecture Notes 3: Biochemistry

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    1. Lecture Notes 3: Biochemistry Biology A Eaton Rapids High School K.Coppins

    2. I. Basics of Chemistry A. The Atom 1. ______________________________ 2. Made of a __________________ surrounded by a cloud of negative particles called ____________. 3. All elements are listed on the _____________.

    3. I. Basics of Chemistry A. The Atom 4. Elements in the body: Oxygen (65%) Carbon (18%) Hydrogen (10%) Nitrogen (3%) Calcium (1.5%) Phosphorus (1.0%) Potassium (0.35%) Sulfur (0.25%) Sodium (0.15%) Magnesium (0.05%) Copper, Zinc, Selenium, Molybdenum, Fluorine, Chlorine, Iodine, Manganese, Cobalt, Iron (0.70%) Lithium, Strontium, Aluminum, Silicon, Lead, Vanadium, Arsenic, Bromine (trace amounts) Reference: H. A. Harper, V. W. Rodwell, P. A. Mayes, Review of Physiological Chemistry, 16th ed., Lange Medical Publications, Los Altos, California 1977.

    4. I. Basics of Chemistry B. Molecules 1. When two or more atoms join together, they form a ___________. 2. These are called _______________, and are based on interactions between the _________. 3. If a bond joins different elements, the new substance is a __________.

    5. I. Basics of Chemistry C. Types of Bonds 1. _____________ a. Electrons move from one atom to the other. b. Atoms become positively or negatively charged; called ____. c. Charges attract or repel. d. Good for __________________.

    6. I. Basics of Chemistry C. Types of Bonds 2. _______________ a. Electrons are shared between two atoms. b. Atoms must remain together c. Bonds are flexible d. Good for ________________.

    7. I. Basics of Chemistry C. Types of Bonds 3. _______________ a. Hydrogen holds electrons weakly b. Has a slightly positive charge, attracted to anything negative. c. Creates weak bonds that help hold structures but can be broken easily. d. Examples: _________________

    8. I. Basics of Chemistry D. Molecules and Energy 1. Energy is stored in the bonds between atoms. Energy is required to ______________ bonds. 2. The amount of energy varies with the type of bond. Some bonds (hydrogen) are easily broken while others (triple covalent) are very hard.

    9. II. Water Chemistry A. ________ is the most abundant chemical in the body. B. Water has many characteristics that make it vital to our bodies. 1. _____water is a very small molecule, so it moves fast and can squeeze into tiny crevasses between other molecules.

    10. II. Water Chemistry B. Water has many characteristics that make it vital to our bodies. 2. _________--Hydrogen has a slightly positive charge while oxygen has a slightly negative charge. This makes it easy for water to pry apart other charged molecules, dissolving them. Called a __________________.

    11. II. Water Chemistry B. Water has many characteristics that make it vital to our bodies. 3. _______________--Due to polarity, water forms a crystal structure that is less dense than liquid water.

    12. II. Water Chemistry B. Water has many characteristics that make it vital to our bodies. 4. _____________--water absorbs and releases heat energy slowly, and can hold a great deal of heat energy. This helps organisms maintain their body temperature in the safe range.

    13. II. Water Chemistry B. Water has many characteristics that make it vital to our bodies. 5. __________________--Polarity allows water to stick to itself (cohesion) and to any charged material (adhesion). Water can glue materials together.

    14. II. Water Chemistry B. Water has many characteristics that make it vital to our bodies. 6. _______--Water can act as either an acid or a base, maintaining a stable pH in our bodies.

    15. III. Macromolecules A. What are they? 1. __________________________________ _______________________________________ 2. Made of smaller pieces called __________ that can be assembled like legos to form a variety of structures. A large chain of monomers is called a _________.

    16. III. Macromolecules B. Carbohydrates 1. Monomer: ____________________ 2. Polymer: _____________________ 3. Structure:______________________ ________________________________ 4. Uses: ___________________ 5. Examples: ________________

    17. Examples of Carbohydrates

    18. III. Macromolecules C. Lipids 1. Monomer: __________ 2. Polymer: ___________ 3. Structure:______________________ ________________________________ 4. Uses: ________________________ 5. Examples: ____________________

    19. Examples of Lipids

    20. III. Macromolecules D. Protein 1. Monomer: _______________ 2. Polymer: _____________________ 3. Structure:______________________ ________________________________ 4. Uses: ________________________ 5. Examples: ____________________

    21. Examples of Proteins

    22. III. Macromolecules E. Nucleic Acids 1. Monomer: _______________ 2. Polymer: ___________ 3. Structure:______________________ ________________________________ 4. Uses: ___________________ 5. Examples: _______________

    23. Examples of Nucleic Acids

    24. IV. ATP A. ATP stands for _____________________ B. Cells use ATP as a __________________ C. Made of adenine with ___ phosphates D. Lots of energy is stored in the bond between _____________________________ E. When this bond is broken, tremendous energy is released. F. The pieces are then reassembled, storing more energy for another use.

    25. Examples of ATP

    26. V. Enzymes A. Special proteins that speed chemical reactions 1. Chemical reactions require a certain _______________ to get started. 2. Enzymes decrease this energy, making reactions occur faster.

    27. V. Enzymes B. Lock-and-Key Model 1. Enzymes are not used up by the reaction, but each can only work on one reaction (________________). 2. This is called the lock-and-key model of enzymes. An enzyme is like a _____ which can open exactly one _____. If you want to unlock another reaction, you need a different enzyme.

    28. V. Enzymes

    29. V. Enzymes C. Factors which affect enzymes 1. _____________--enzymes, like all proteins, change shape when exposed to heat or cold. Each has an optimal temperature range. 2. ____--all enzymes have an optimal range of pH. Example: stomach 3. _____________--having more enzymes makes the reaction faster.

    30. Images used in this presentation were obtained from: Atom: PowerPoint clipart Water molecule and Water attraction: stainsfile.info/StainsFile/jindex.html Bohr water molecule: ghs.gresham.k12.or.us Spoon on nose: statweb.calpoly.edu pH scale: bcn.boulder.co.us Glucose and Cellulose: www.greenspirit.org.uk Sucrose: encarta.msn.com

    31. Images, continued Saturated and unsaturated fatty acids, cis and trans fat, and lipid molecule: biology.clc.uc.edu Generic Amino acid: ffden-2.phys.uaf.edu Peptide bond: www.rothamsted.bbsrc.ac.uk Nucleotide: faculty.uca.edu DNA helix: www.biologycorner.com ATP: textbookofbacteriology.net Activation energy: faculty.clintocc.suny.edu Enzyme lock-and-key: www.celltech.com

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