Go to Section: What’s the Matter? All of the materials around you are made up of matter. You are made up of matter, as are the chair you sit on and the air you breathe. 1. Give an example of solid matter. 2. Give an example of liquid matter. 3. Give an example of gaseous matter. 4. Is all matter visible? 5. Does all matter take up space? Section 2-1 Interest Grabber

Go to Section: 2–1The Nature of Matter A.Atoms B.Elements and Isotopes 1.Isotopes 2.Radioactive Isotopes C.Chemical Compounds D.Chemical Bonds 1.Ionic Bonds 2.Covalent Bonds 3.Van der Waals Forces Section 2-1 Section Outline

Go to Section: Atoms At Atom is the basic unit of matter. There are 3 subatomic particles in an atom. They are called a proton, neutron and an electron. The Nucleus of an atoms is the center of an atom and is made up of protons and neutrons. 2-1 The Nature of Matter

Go to Section: Atoms 2-1 The Nature of Matter ParticleChargeLocation in Atom ProtonPositiveNucleus NeutronNeutralNucleus ElectronNegativeSurrounding nucleus

Go to Section: Atoms Protons + Neutrons 0 electrons The Nature of Matter Atoms have equal numbers of electrons and protons, and these subatomic particles have equal, but opposite charges

Go to Section: 6 C Carbon Section 2-1 An Element in the Periodic Table Atomic number Element name Element symbol Mass number A chemical element is a pure substance that consists entirely of one type of atom.

Go to Section: Elements and Isotopes An element’s atomic number represents the number of protons in an atom of the element. An element’s mass number represents the number of protons and neutrons in an atoms of the element. Isotopes are atoms of the same element that differ in the number of neutrons they contain. Isotopes are identified by their mass number. They have the same chemical properties because they have the same number of electrons. 2-1 The Nature of Matter

Go to Section: Nonradioactive carbon-12Nonradioactive carbon-13Radioactive carbon-14 6 electrons 6 protons 6 neutrons 6 electrons 6 protons 8 neutrons 6 electrons 6 protons 7 neutrons Section 2-1 Figure 2-2 Isotopes of Carbon

Go to Section: Elements and Isotopes A chemical compound is a substance formed by the chemical combination of 2 or more elements in definite proportions. H Hydrogen to 1 Oxygen CO Carbon to 2 Oxygen NaCl- 1 Sodium to 1 Chlroine C 6 H 12 O 6 -6 Carbon to 12 Hydrogen to 6 Oxygen 2-1 The Nature of Matter

Go to Section: Chemical Bonds Chemical bonds holds atoms in compounds together. The 2 types of chemicals bonds are ionic and covalent Ionic bonds form when one or more electrons are transferred from one atom to another. 2-1 The Nature of Matter

Go to Section: Sodium atom (Na)Chlorine atom (Cl)Sodium ion (Na + )Chloride ion (Cl - ) Transfer of electron Protons +11 Electrons -11 Charge 0 Protons +17 Electrons -17 Charge 0 Protons +11 Electrons -10 Charge +1 Protons +17 Electrons -18 Charge -1 Section 2-1 Figure 2-3 Ionic Bonding

Go to Section: Sodium atom (Na) Chlorine atom (Cl)Sodium ion (Na + ) Chloride ion (Cl - ) Transfer of electron Protons +11 Electrons -11 Charge 0 Protons +17 Electrons -17 Charge 0 Protons +11 Electrons -10 Charge +1 Protons +17 Electrons -18 Charge -1 Section 2-1 Figure 2-3 Ionic Bonding An ion is an atoms that is positively or negatively charged because it has lost or gained electrons. If it loses an electron it has a positive charge If it gains an electron it has a negative charge Show video 2B

Go to Section: Chemical Bonds Covalent bonds form when electrons are shared between atoms A single bond is when atoms share 2 electrons A double bond is when atoms share 4 electrons A triple bond is when atoms share 6 electrons A molecules is the structure that results when atoms are joined together by covalent bonds Van der Waals forces are the slight attractions that develop between oppositely charged regions of nearby molecules. Show video 2A and 2C 2-1 The Nature of Matter

Go to Section: Water, Water Everywhere If you have ever seen a photograph of Earth from space, you know that much of the planet is covered by water. Water makes life on Earth possible. If life as we know it exists on some other planet, water must be present to support that life. Section 2-2 Interest Grabber

Go to Section: 1. Working with a partner, make a list of ten things that have water in them. 2. Exchange your list for the list of another pair of students. Did your lists contain some of the same things? Did anything on the other list surprise you? 3. Did either list contain any living things? Section 2-2 Interest Grabber continued

Go to Section: 2–2 Properties of Water A.The Water Molecule 1.Polarity 2.Hydrogen Bonds B.Solutions and Suspensions 1.Solutions 2.Suspensions C.Acids, Bases, and pH 1.The pH Scale 2.Acids 3.Bases 4.Buffers Section 2-2 Section Outline

Go to Section: The water molecule Water is polar because there is an uneven distribution of electrons between the oxygen and hydrogen atoms. Hydrogen has a slightly positive charge Oxygen has a slightly negative charge. The attraction between the hydrogen atoms of one water molecule and the oxygen molecule of another water molecule is an example of a hydrogen bond 2-2 Properties of water

Go to Section: The water molecule The 3 properties of water are: 1.Cohesion: attraction between molecules of the same substance 2.Adhesion: attraction between molecules of different substances 3.Capillary action: movement through small spaces due to cohesion and adhesion 2-2 Properties of water

Go to Section: Solutions and suspensions A mixture is a material composed of 2 or more elements of compounds that are physically mixed together but not chemically combined. The 2 types are solutions and suspensions A solution is a mixture of 2 or more substances in which the molecules of the substances are evenly mixed An example of a solution is saltwater. 2-2 Properties of water

Go to Section: Cl - Water Cl - Na + Water Na + Section 2-2 Figure 2-9 NaCI Solution

Go to Section: Section 2-2 Figure 2-9 NaCI Solution Cl - Water Cl - Na + Water Na +

Go to Section: Substances in a solution 2-2 Properties of water SubstanceDefinitionExample in a saltwater solution SoluteSubstance that is dissolved Table salt SolventSubstance in which the solute dissolves water

Go to Section: Solutions and suspensions The greatest solvent in the world is water A suspension is a mixture of water and non- dissolved substances that are so small they do not settle out An example is blood 2-2 Properties of water

Go to Section: Acids, Bases and pH An acid is any compound that forms H+ (positive hydrogen) ions in a solution. A base is any compound that forms OH- (Negative hydroxide) ions in a solution. A compound is neutral if it produces equal number of H+ and OH- ions. Water is neutral H 2 O↔H+ + OH- H+ + H 2 O ↔ H 3 O+ 2-2 Properties of water

Go to Section: Acids, Bases and pH Acids have a pH less than 7 Bases have a pH greater than 7 A neutral compound has a pH of 7 Buffers are weak acids or bases that can react with strong acids and bases to prevent sharp, sudden changes in pH 2-2 Properties of water

Go to Section: Oven cleaner Bleach Ammonia solution Soap Sea water Human blood Pure water Milk Normal rainfall Acid rain Tomato juice Lemon juice Stomach acid Neutral Increasingly Basic Increasingly Acidic Section 2-2 pH Scale

Go to Section: Life’s Backbone Most of the compounds that make up living things contain carbon. In fact, carbon makes up the basic structure, or “backbone,” of these compounds. Each atom of carbon has four electrons in its outer energy level, which makes it possible for each carbon atom to form four bonds with other atoms. As a result, carbon atoms can form long chains. A huge number of different carbon compounds exist. Each compound has a different structure. For example, carbon chains can be straight or branching. Also, other kinds of atoms can be attached to the carbon chain. Section 2-3 Interest Grabber

Go to Section: 1. On a sheet of paper, make a list of at least ten things that contain carbon. 2. Working with a partner, review your list. If you think some things on your list contain only carbon, write “only carbon” next to them. 3. If you know other elements that are in any items on your list, write those elements next to them. Section 2-3 Interest Grabber continued

Go to Section: 2–3Carbon Compounds A.The Chemistry of Carbon B.Macromolecules C.Carbohydrates D.Lipids E.Nucleic Acids F.Proteins Section 2-3 Section Outline

Go to Section: The chemistry of carbon Carbon has 4 valence electrons A carbon atom can bond to other carbon atoms so they can forms chains that can be almost unlimited in length. 2-3 Carbon Compounds

Go to Section: MethaneAcetyleneButadieneBenzeneIsooctane Section 2-3 Figure 2-11 Carbon Compounds

Go to Section: Macromolecules Many of the molecules in living cells are so large that they are known as macromolecules A monomer is a small unit that can join with other small units to form a polymer Monomers join together to form polymers This process is called polymerization 2-3 Carbon Compounds

Go to Section: Carbon Compounds include that consist of which contain that consist of which contain Section 2-3 Concept Map CarbohydratesLipidsNucleic acidsProteins Sugars and starches Fats and oilsNucleotidesAmino Acids Carbon, hydrogen, oxygen Carbon, hydrogen, oxygen Carbon,hydrogen, oxygen, nitrogen, phosphorus Carbon, hydrogen,oxygen, nitrogen, 4 groups of organic compounds

Go to Section: Carbohydrates Made up of the element Carbon, Hydrogen and oxygen and are usually in a 1:2:1 ration They are a main source of energy and structural. The monomer is a monosaccharide The three types of monosaccharides are glucose, fructose and galactose Polysaccharides are large macromolecules formed from monosaccharides The three are starch-plant storage cellulose-plant structure gylcogen –animal storage 2-3 Carbon Compounds

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

Go to Section: Lipids Lipids are mostly made up of the elements carbon, hydrogen and oxygen The functions of lipids are store energy, serve as part of membranes, and waterproof covering. Lipids are formed when glycerol combines with fatty acids 3 examples: fats, oils and waxes 2-3 Carbon Compounds

Go to Section: Lipids 2-3 Carbon Compounds Kind of lipidDescriptionExample Saturated All fatty acid carbons are joined to another carbon by a single bond butter Unsaturated At least one carbon- carbon double bond in a fatty acid Olive oil Polyunsaturated More than one c-c double bond in fatty acid Corn oil

Go to Section: Nucleic Acids Made up of hydrogen, oxygen, nitrogen, carbon and phosphorus. Their function is to store and transmit genetic information They monomer is a nucleotide 3 parts to the nucleotide: nitrogenous base, phosphate group and 5-carbon sugar 2 types are : Ribonucleic Acid (RNA) and Deoxyribonucleic Acid (DNA) 2-3 Carbon Compounds

Go to Section: Proteins Proteins are made up of the elements: nitrogen, hydrogen, carbon and oxygen. Their functions are control rate of reactions, transport substances in or out of cells, fight disease, and form bones and muscles. Their monomer is the amino acid 2-3 Carbon Compounds

Go to Section: General structureAlanineSerine Section 2-3 Figure 2-16 Amino Acids Amino groupCarboxyl group

Go to Section: General structureAlanineSerine Section 2-3 Figure 2-16 Amino Acids Amino groupCarboxyl group

Go to Section: General structureAlanineSerine Section 2-3 Figure 2-16 Amino Acids Amino groupCarboxyl group

Go to Section: Amino acids Section 2-3 Figure 2-17 A Protein

Go to Section: Matter and Energy Have you ever sat around a campfire or watched flames flicker in a fireplace? The burning of wood is a chemical reaction—a process that changes one set of chemicals into another set of chemicals. A chemical reaction always involves changes in chemical bonds that join atoms in compounds. The elements or compounds that enter into a chemical reaction are called reactants. The elements or compounds produced by a chemical reaction are called products. As wood burns, molecules of cellulose are broken down and combine with oxygen to form carbon dioxide and water vapor, and energy is released. Section 2-4 Interest Grabber

Go to Section: 1. What are the reactants when wood burns? 2. What are the products when wood burns? 3. What kinds of energy are given off when wood burns? 4. Wood doesn’t burn all by itself. What must you do to start a fire? What does this mean in terms of energy? 5. Once the fire gets started, it keeps burning. Why don’t you need to keep restarting the fire? Section 2-4 Interest Grabber continued

Go to Section: 2–4Chemical Reactions and Enzymes A.Chemical Reactions B.Energy in Reactions 1.Energy Changes 2.Activation Energy C.Enzymes D.Enzyme Action 1.The Enzyme-Substrate Complex 2.Regulation of Enzyme Activity Section 2-4 Section Outline

Go to Section: Chemical reactions A chemical reaction is a process that changes one set of chemicals into another set of chemicals by changing chemical bonds. The reactants are the elements or compounds that enter into a chemical reaction The products are the elements or compounds produced by a chemical reaction. On notes label reactants and products 2-4 Chemical reactions and enzymes

Go to Section: Energy in reactions Energy is either released or absorbed when chemical bonds are formed or broken. Activation energy is the energy needed to get a reaction started. 2-4 Chemical reactions and enzymes

Go to Section: Energy-Absorbing Reaction Energy-Releasing Reaction Products Activation energy Activation energy Reactants Section 2-4 Figure 2-19 Chemical Reactions

Go to Section: Energy-Absorbing Reaction Energy-Releasing Reaction Products Activation energy Activation energy Reactants Section 2-4 Figure 2-19 Chemical Reactions

Go to Section: Enzymes A catalyst is a substance that speeds up the rate of a chemical reaction An enzyme is a protein that acts as a biological catalyst Enzymes speed up reaction by lowering the activation energy of the chemical reaction Show video 2D 2-4 Chemical reactions and enzymes

Go to Section: Reaction pathway without enzyme Activation energy without enzyme Activation energy with enzyme Reaction pathway with enzyme Reactants Products Section 2-4 Effect of Enzymes

Go to Section: Enzyme Action Substrates are the reactants of enzyme- catalyzed reactions An active site is the site on the enzyme where the substrate binds. The active site and substrates in an enzyme- catalyzed reaction are often compared to a lock and key because the active site and substrate have complementary shapes and the fit is precise. 2-4 Chemical reactions and enzymes

Go to Section: Glucose Substrates ATP Substrates bind to enzyme Substrates are converted into products Enzyme-substrate complex Enzyme (hexokinase) ADP Products Glucose-6- phosphate Products are released Section 2-4 Figure 2-21 Enzyme Action Active site

Go to Section: Glucose Substrates ATP Substrates bind to enzyme Substrates are converted into products Enzyme-substrate complex Enzyme (hexokinase) ADP Products Glucose-6- phosphate Products are released Section 2-4 Figure 2-21 Enzyme Action Active site

Go to Section: Glucose Substrates ATP Substrates bind to enzyme Substrates are converted into products Enzyme-substrate complex Enzyme (hexokinase) ADP Products Glucose-6- phosphate Products are released Section 2-4 Figure 2-21 Enzyme Action Active site

Go to Section: Glucose Substrates ATP Substrates bind to enzyme Substrates are converted into products Enzyme-substrate complex Enzyme (hexokinase) ADP Products Glucose-6- phosphate Products are released Section 2-4 Figure 2-21 Enzyme Action Active site

Video Contents Videos Click a hyperlink to choose a video. Atomic Structure Energy Levels and Ionic Bonding Covalent Bonding Enzymatic Reactions

Video 1 Click the image to play the video segment. Video 1 Atomic Structure

Video 2 Click the image to play the video segment. Video 2 Energy Levels and Ionic Bonding

Video 3 Click the image to play the video segment. Video 3 Covalent Bonding

Video 4 Click the image to play the video segment. Video 4 Enzymatic Reactions

Internet Career links on forensic scientists Interactive test Articles on organic chemistry For links on properties of water, go to and enter the Web Code as follows: cbn For links on enzymes, go to and enter the Web Code as follows: cbn Go Online

Section 1 Answers 1.Give an example of solid matter. Sample answers: books, desks, chairs 2. Give an example of liquid matter. Sample answers: water, milk 3. Give an example of gaseous matter. Sample answers: air, helium in a balloon 4. Is all matter visible? No 5. Does all matter take up space? Yes Interest Grabber Answers

Section 2 Answers Interest Grabber Answers 1. Working with a partner, make a list of ten things that have water in them. Possible answers: bodies of water, rain and snow, soft drinks and other beverages, juicy foods such as fruits, and so on. 2. Exchange your list for the list of another pair of students. Did your lists contain some of the same things? Did anything on the other list surprise you? Students’ answers will likely be similar, but not exactly alike. 3. Did either list contain any living things? Students’ lists may include plants, animals, or other living things.

Section 3 Answers Interest Grabber Answers 1. On a sheet of paper, make a list of at least ten things that contain carbon. Students will likely know that charcoal and coal contain carbon. They may also list carbohydrates (starches and sugars), oil, gasoline, wood, or carbon dioxide. 2. Working with a partner, review your list. If you think some things on your list contain only carbon, write “only carbon” next to them. Students will say that charcoal and coal contain only carbon. While these materials do contain small amounts of other elements, such as sulfur, they are composed mostly of carbon. 3. If you know other elements that are in any items on your list, write those elements next to them. Students may know that many carbon compounds also contain oxygen and/or hydrogen.

Section 4 Answers Interest Grabber Answers 1.What are the reactants when wood burns? Reactants are oxygen and cellulose. 2. What are the products when wood burns? Products are carbon dioxide and water. 3. What kinds of energy are given off when wood burns? Light and heat are given off. Some students may also mention sound (the crackling of a fire). 4. Wood doesn’t burn all by itself. What must you do to start a fire? What does this mean in terms of energy? To start a fire, you must light it with a match and kindling. You are giving the wood some energy in the form of heat. 5. Once the fire gets started, it keeps burning. Why don’t you need to keep restarting the fire? Once the fire gets going, it gives off enough heat to start more of the wood burning.

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