Biology. Chapter 2 Notes
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1 Biology Chapter 2 Notes
2 Section 1: Nature of Matter Objectives: 1) Differentiate between atoms and elements 2) Analyze how compounds are formed 3) Distinguish between covalent bonds, hydrogen bonds and ionic bonds.
3 Atoms & Elements Atom: smallest unit of matter that cannot be broken down by chemical means. Element: pure substance made of only one kind of atom. 3
4 Compounds Formed through chemical bonding. Compounds are made of two or more different kinds of atoms. Common compounds: NaCl NaHCO 3 C 12 H 22 O 11 4
5 Bonding Bonds are most stable when an atom s outer electron level is full. (Need 8 electrons to be full) If it is not full, it will either share, give, or take electrons from another atom. Share: Covalent bond Weakly attract: Hydrogen bond Give/Take: Ionic bond 5
6 Bonding Covalent bonds: when two or more atoms share electrons to form a molecule. 6
7 Bonding Polar: one positive end and one negative end. Hydrogen bonds: Weak chemical attractions between polar molecules Seen in water. 7
8 Bonding Ionic Bonds: when an atom or molecule gains or loses one or more electrons to form the bond. Seen in table salt One Electron Seven Electrons 8
9 Chemicals in Your Food 9
10 Chemicals in Your Food Question #2 Niacin: Vitamin B Riboflavin: Vitamin B2 Sodium Bicarbonate: Baking Soda 10
11 Question #4 Can you guess what it is? 11
12 Section 2: Water and Solutions Objectives: 4) Analyze the properties of water. 5) Describe how water dissolves substances. 6) Distinguish between acids and bases.
13 Storage of Energy Water absorbs and retains heat better than most other substances. Allows us to maintain constant body temperature. Evaporation: When we sweat, the water evaporates and makes us cooler. What is the term for maintaining stable internal conditions despite external changes?
14 Cohesion and Adhesion Cohesion: attraction between substances that are the same. Surface tension: attraction between molecules that prevents the surface from stretching and breaking. Adhesion: attraction between substances that are different. Capillary action: water moving because of it s attraction to the surface on which it has contact with.
15 Water: The Master Dissolver Water is important to life because of it s ability to dissolve many substances which living things need to survive. Substances dissolved in water: Aqueous solutions Examples of aqueous solutions in our body: Blood: moves nutrients around your body. Mucus: filters dirt out of mouth and nose. Urine: moves wastes from bloodstream out of body.
16 Polarity Water is a polar molecule - positive and negative end like a magnet. Polarity gives water it s ability to dissolve most substances. almost. Oil is non-polar and does not mix with water. This is also helpful for living things: Cell membranes, oil as protection for skin
17 Ingredient for Life: Water
18 Acids and Bases: - Substances that release ions in water are called electrolytes. - The concentrations of H + and OH - in the body is very important to physiology. - ph represents the concentration of hydrogen ions [H + ] in solution.
19 -Electrolytes that release hydrogen ions in water are called acids. -Electrolytes that release ions that combine with hydrogen ions in water are called bases.
20 6. A ph of 7 indicates a neutral solution with equal numbers of hydrogen ions and hydroxyl (OH - ) ions. a. A ph of zero to less than 7 indicates the presence of more hydrogen ions, and thus the solution is more acidic; a ph greater than 7 to 14 indicates more hydroxyl ions, or a basic solution. b. Between each whole number of the ph scale there is a tenfold difference in hydrogen ion concentration.
21 7. Buffers are chemicals that combine with excess acids or bases to help minimize ph changes in body fluids.
22 Section 3: Chemistry of Cells Objectives: 7) Summarize the characteristics of organic compounds. 8) Compare the structures and function of different types of biomolecules. 9) Describe the components of DNA and RNA. 10) State the main role of ATP in cells.
23 Organic Compounds Organic = contains carbon Most of the matter in your body that is not water is made of organic compounds. Four classes of organic compounds: Carbohydrates Lipids Proteins Nucleic Acids
24 Carbohydrates Made of carbon, hydrogen and oxygen atoms Always a 1:2:1 ratio Monosaccharides: single sugars Polysaccharides: many sugars together Sugars serve as a storehouse for energy until the organism can use it. Plants: Starch Animals: Glycogen
25 Lipids Non-polar molecules, will not dissolve in water. Fats are lipids that store energy. Composed of long chains of hydrogen and carbon with oxygen. Can be saturated or unsaturated Solid at room temperature Liquid at room temperature
26 Proteins Large molecules formed by linking Amino Acids Function: Enzymes: speed up chemical reactions Structural role: Collagen, Muscles, Bones, Hair Body needs protein to break down into amino acids and build new proteins Made in the cell by DNA transcription
27 Nucleic Acid Long chains of nucleotides: sugar, phosphate and base groups. Two types of nucleic acids: DNA: Deoxyribonucleic Acid RNA: Ribonucleic Acid DNA and RNA code for proteins in our cells.
28 ATP ATP or Adenosine Triphosphate is energy for the cell. Produced when food molecules are broken down. Many of our biological functions rely on ATP as an energy source.
29 Food as Fuel Food is used: Energy Source Build New Structures Energy is measured in kilocalories (calories) Carbohydrates: 4 calories/1 gram Proteins: 4 calories/ 1 gram Fats: 9 calories/ 1 gram If calories consumed are not used for energy, they will be stored as fat.
30 Section 4: Energy and Chemical Reactions Objectives: 11) Evaluate the importance of energy to living things. 12) Relate energy and chemical reactions. 13) Describe the role of enzymes in chemical reactions. 14) Identify the effect of enzymes on food molecules.
31 Energy for Life Process Energy: ability to move or change matter. Many forms: Light, heat, chemical, mechanical and electrical. Energy is converted from one form to another. What is the term for all chemical reactions within a living organism? Metabolism Chemical reactions are written in equations Reactants Products Example: NaCl Na + + Cl -
32 Energy in Chemical Reactions Energy is absorbed and released when bonds are broken and new ones are formed. Ice melting: Heat is transferred Heat is released as the water freezes Heat is absorbed when water melts Muscles moving Mechanical energy is transferred to heat energy when muscles/body is moving
33 Activation Energy Activation energy: Energy needed to start a chemical reaction. Examples: match, spark plugs in a car Activation energy needed to start a chemical reaction can be high or low depending on the process.
34 Enzymes Most enzymes are proteins. Enzymes are catalysts: Substances that increase the speed of a chemical reaction. Enzymes also decrease the activation energy needed to start a chemical reaction. Chemical reactions without enzymes are like a sailboat without wind.
35 Activation energy and enzymes
36 Enzyme Specificity Substrate: specific substances that react with the enzyme. Active sites: folds in the enzyme that only fit the substrates. Like a key in a lock. Enzyme changes substrates into a new product.
37 Factors in Enzyme Activity There are factors that change the shape of an enzyme and change how it functions. Factors: Temperature ph Other enzymes Other substrates that mimic the intended substrate Example: Prozac / Serotonin
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AP Biology Exam 1: The Chemistry of Life Name MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) Matter A) has mass. B) All of the choices are correct.