1. Your Roadmap for Success in Chapter 6
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1 1. Your Roadmap for Success in Chapter 6 Preview the chapter: 1. Read Summary (p. 171). 2. Skim the Assessment questions (p ). 3. Rewrite Learning Objectives for the chapter and each section in the form of possible test questions. (So, four sets of questions.) 4. Look at pictures.
2 2. Your Roadmap for Success in Chapter 6 You are expected to read all parts of each section (1, 2, 3) on your own. You are responsible for knowing this material. We will be covering most of the book content during class with slides, discussions, demos, and other activities. However, we can t possibly cover all chapter content during class.
3 3. Your Roadmap for Success in Chapter 6 Assignments will include (at minimum): 1. Reading the chapter 2. Questions from each Section Assessment 3. Questions from the Chapter Assessment 4. Chapter notes (more later) 5. Class activities or labs
4 4. Your Roadmap for Success in Chapter 6 Assessments will include (at minimum): 1. The assignments mentioned 2. Quiz for each section 3. Test at the end of the chapter 4. Behavior/positive participation There will be at least one extra credit opportunity offered per chapter.
5 Biology Chapter 6: The Chemistry of Life 1. Atoms and Their Interactions 2. Water and Diffusion 3. Life Substances
6 Biology Chapter 6: The Chemistry of Life What You ll Learn (p. 144) (Turn these statements into test questions; write them down.)
7 Chapter 6.1 Atoms & Their Interactions Learning Objectives (p. 145): (Turn these objectives into test questions.) Vocabulary:
8 Matter is anything that has mass and takes up space. Examples? Energy is anything that brings about change. can hold matter together or break it apart.
9 Atoms All matter (whether solid, liquid, or gas) is made of atoms. Center of atom is called the nucleus. The nucleus consists of: protons (have a + charge) neutrons (have no charge)
10 Matter vs. Energy Matter Energy Definition Examples atoms, electrons, protons, and neutrons;,,,, sunlight, electricity, heat, chemical energy
11 Atoms - Electrons Around the nucleus is a cloud of electrons (have a charge). Constantly moving VERY small mass compared to protons and neutrons! The mass of 1,837 electrons = the mass of 1 proton Involved in CHEMICAL REACTIONS
12 Parts of an Atom Protons Electrical Charge? Location in Atom? Relative Mass? Neutrons Electrons
13 Elements are made up of only one kind of atom. can t be broken down into simpler form by chemical reactions. are known by their own one- or two-letter symbol. make up everything in the Universe.
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15 How many of these elements can you identify? O C H N Ca P K S Na Cl Mg
16 Elements that make up the human body 0.4% 0.3% 0.2% 0.1% 1.5% 1.0% 0.2% 0.1% 3.2% 18.5% 9.5% 65.0% Percent in Human Body Oxygen Carbon Hydrogen Nitrogen Calcium Phosphorus Potassium Sulfur Sodium Chlorine
17 99% of living matter is made up of six (6) elements. That makes these elements pretty important! S P O N C H
18 Compounds and Molecules A Compound is a substance that is composed of atoms of two or more different elements that are chemically combined. Example: Water
19 Compounds and Molecules A Compound is a substance that is composed of atoms of two or more different elements that are chemically combined. These elements are in exact proportions. Example: Water is always made up of hydrogen atom(s) and oxygen atom(s), bonded together in exactly the same way, to form a water molecule.
20 Compounds and Bonding Most matter is in the form of compounds. Why and how do atoms combine? Atoms combine with other atoms: Only when conditions are right To become more stable When is an atom usually most stable? How does an atom become more stable?
21 Covalent Bonds vs. Ionic Bonds Covalent bonds form when two atoms share electrons in their outermost shell (energy level). Atoms are held together by the attraction between the positively-charged nuclei and the shared, negatively-charged electrons. Most compounds in organisms have covalent bonds (ex. sugars, fats, proteins, water). Molecule: Group of atoms held together by covalent bonds and having no overall charge.
22 Compounds and Molecules Molecular Compounds form when different atoms share their outermost electrons. Hydrogen atoms have 1 electron. How many electrons does an oxygen atom have? (see pg. 147) On Earth, oxygen and hydrogen normally exist as gases. But as a compound (water), they can be liquid, solid, or gas. **When a compound is formed, changes occur and a new substance forms.
23 Covalent Bonds vs. Ionic Bonds Most atoms have an equal # of electrons and protons; therefore, they have an electrical charge of. Ionic bonds form when atoms gain or lose an electron from their outer energy level. An ion is an atom (or group of atoms) that or electrons and has an. An ion is a charged particle.
24 Covalent Bonds vs. Ionic Bonds Ions are held together by a different kind of chemical bond than covalent bonds. An ionic bond is the attractive force between two ions of opposite charge. Example: NaCl Sodium atom (11e, 11p, 12n) Chlorine atom (17e, 17p, 18n)
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26 Ionic Bonds, cont d Ionic compounds are less abundant in living things than are covalent molecules. However, ions are very important in biological processes. Examples: Sodium and potassium ions are required for transmission of nerve impulses. Calcium ions are necessary for muscles to contract. Plant roots absorb essential minerals in the form of ions.
27 Chemical Reactions What is going on during a chemical reaction? Bonds between atoms are formed or broken, causing substances to combine and recombine as different molecules. Chemical reactions occur over and over again inside cells. Metabolism: All of the chemical reactions that occur within an organism. These chemical reactions are essential for the organism s function.
28 Chemical Reactions and Chemical Equations Chemical reactions are represented by chemical equations. Symbols and formulas are used to represent each element or substance. 2H 2 + O 2 2H 2 O (Reactants) (Products)
29 Chemical Reactions and Chemical Equations Reactants: Substances that undergo chemical reactions Products: Substances formed by chemical reactions Atoms are neither created nor destroyed by chemical reactions! Just rearranged. Same number of atoms should appear on both sides of the equation (if balanced).
30 Showing a Chemical Reactions With a Chemical Equation 2H 2 + O 2 2H 2 O How many molecules are involved with this chemical reaction? Number before each chemical formula indicates the # of molecules of each substance. Subscript numbers indicate the # of atoms of each element in a molecule of the substance. If no # before or under a symbol, then only one atom or molecule is present.
31 Showing a Chemical Reactions With a Chemical Equation 2H 2 + O 2 2H 2 O
32 Mixtures When substances combine, but DON T combine chemically (no chemical reaction) Mixture: A combination of substances in which the individual components retain their own properties. Solution: Type of mixture in which one or more substances (solutes) are distributed evenly in another substance.
33 Solution: Solutions Type of mixture in which one or more substances (solutes) are distributed evenly in another substance (solvent). Basically, one substance is completely dissolved in another and won t settle out of solution. Solvent means to loosen or dissolve. Water is known as the universal solvent.
34 Concentration of a Solution The more solute in a given amount of solvent, the HIGHER the concentration of the solution (i.e., stronger ). To dilute a solution means that you add more solvent. Ex. Adding more water to a pitcher of Kool-Aid makes it weaker.
35 What does this mean for living organisms? Organisms have very specific requirements for the concentrations of solutions in their bodies usually an extremely narrow range of tolerance. Ex. Blood sugar level, cellular contents
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