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.

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:

Answers to What’s the Matter? 1. Sample answers: books, desks, chairs 2. Sample answers: water, milk 3. Sample answers: air, helium in a balloon 4. No 5. Yes

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:

The Atom An atom is the basic unit of matter. It is made up of protons, electrons, and neutrons. An atom has no charge.

An Atom’s Subatomic Particles Mass (amu) LocationCharge PROTON1 (1.0073) Inside the nucleus1+ Positive P and P NEUTRON1 (1.0087) Inside the nucleusNone (Neutral) ELECTRON1/1840 (5.486 x 10 -4 ) Outside of the nucleus (Electron cloud) 1- Negative

Vocabulary Words Element – pure substance that consists entirely of one type of atom Isotopes – atoms of the same element that differ in the number of neutrons; all isotopes of an element have the same chemical properties because they have the same number of electrons Radioactive Isotopes (radioisotopes)– isotopes with unstable nuclei that break down at a constant rate over time; the radiation they give off can be dangerous, but radioactive isotopes can also have scientific and practical uses Examples: 1.Determine the ages of rocks and fossils by analyzing the isotopes found in them 2.Treat cancer 3.Kill bacteria that cause food to spoil 4.Tracers (tagged atoms) to follow the movements of substances within organisms

Radioisotopes 1.Tracers (tagged atoms)-cancer and kidney disorders 2.Tracers with imaging instruments – positron emission tomography (PET scan) 3.Carbon-14 has been used as a tracer to determine how plants use carbon dioxide to make sugar (photosynthesis); archaeological carbon dating Note: Oxygen-18, a stable isotope, has also been used to study photosynthesis. Americium-241 is used in smoke alarms.

Look at the Periodic Table 1.Names and Symbols of the Elements (Note: New elements are assigned three-letter symbols until they are officially named.) 2.Atomic number – the number of protons (PAN) 3.Atomic mass – the number of protons and neutrons 4.How are the elements arranged in the table? In order of increasing atomic number 5.What else does the atomic number equal? The number of electrons because atoms have no charge 6.Which element has seven protons? Nitrogen

6 C Carbon 12.011 Section 2-1 An Element in the Periodic Table 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:

Isotopes of Hydrogen Common hydrogen – one proton and no neutron Deuterium – one proton and one neutron Tritium – one proton and two neutrons

Energy Levels Level and Maximum Number of Electrons Level 1 2 electrons Level 2 8 electrons Level 3 8 electrons Draw the carbon atom.

The General Rule Valence electrons are the electrons that are available to form bonds. Valence Electrons and Action 1Lose electrons 2Lose electrons 3Lose electrons 4Share 5Gain electrons 6Gain electrons 7Gain electrons 8HAPPY!

Chemical Compounds Chemical compound – substance formed by the chemical combination of two or more elements in definite proportions; physical and chemical properties are usually very different from those of the elements from which it is formed (Example: Hydrogen and oxygen are very different from H 2 O) Chemical Formula – a kind of shorthand that shows the composition of compounds (Note: The number 1 is not written; it is understood.) Examples: C 6 H 12 O 6 - glucose 1. Name the elements in glucose? Carbon, hydrogen, and oxygen 2. How many atoms of each element are in the compound? 6 carbon, 12 hydrogen, and 6 oxygen Structural formula – shows elements and bonding sites in the compound; see picture (Figure 2-14 on page 46 in text)

Facts to Know about Chemical Bonds 1.Atoms in compounds are held together by chemical bonds. 2.Bond formation involves the electrons that surround each atomic nucleus. 3.An ionic bond is formed when one or more electrons are transferred from one atom to another. Since atoms are electrically neutral, an atom that loses electrons has a positive charge. An atom that gains electrons, has a negative charge. 4.Charged atoms are called ions. Cations have a positive charge and anions have a negative charge. (Note: Circle the top of the t in cation and it looks like a positive sign.) 5.A covalent bond is formed when electrons are shared between atoms. The smallest unit of this compound is called a molecule.

Covalent Bonds 1.Increases stability of the atom 2.Found in a molecule of water 3.Results in the formation of a molecule 4. Found in most compounds making up living things

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:

Ions are more stable than the neutral atoms because their outermost levels are filled with electrons.

Van der Waals Forces When molecules are close together, a slight attraction can develop between the oppositely charged regions of nearby molecules. Chemists call such intermolecular forces Van der Waals forces. They are not as strong as covalent bonds or ionic bonds, but they can hold molecules together, especially when the molecules are large. (Example: geckos can climb up a vertical wall.) Why can’t a similar technique work for humans? Even if human toes and fingers had hairlike projections, the surface area would not be sufficient to generate a combined force that could support a human’s weight.

Answers to Questions 1-6 on Page 39 in Text 1.Atoms have a nucleus made of protons and neutrons. Electrons are in constant motion in the space around the nucleus. 2.They have the same number of electrons, but differ in the number of neutrons. 3.A covalent bond forms when electrons are shared. An ionic bond forms when electrons are transferred. 4.A compound is a substance formed by the combination of two or more elements in definite proportions. A molecule is the smallest unit of most compounds.

5.When the sharing of electrons is unequal, a molecule has regions that are charged. An attraction can occur between oppositely charged regions of nearby molecules. 6.In both cases, particles are held together by attractions between opposite charges, but the attractions are stronger between the ions than they are between the molecules. (Study Hint: This will be a test question!)

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:

Interest Grabber Possible Answers to Water, Water Everywhere 1.Possible answers: bodies of water, rain and snow, soft drinks and other beverages, juicy foods such as fruits, and so on. 2. Students’ answers will likely be similar, but not exactly alike. 3. Students’ lists may include plants, animals, or other living things.

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

Properties of Water Polar – a molecule in which the charges are unevenly distributed Water is a polar molecule because there is an uneven distribution of electrons between the hydrogen and oxygen atoms. The negative pole is near the oxygen atom and the positive pole is between the hydrogen atoms. The charges on a polar molecule are written in parenthesis (-) or (+) to show that they are weaker than the charges on ions.

Hydrogen Bonds The attraction between the hydrogen atom on one water molecule and the oxygen atom on another water molecule is an example of a hydrogen bond. (Oxygen is negative and the two hydrogen atoms are positive.) See Figure 2-7 on page 41 in the text. Hydrogen bonds are not as strong as ionic or covalent bonds, but they are the strongest of the bonds that can form between molecules. A single water molecule can be involved in as many as four hydrogen bonds at the same time.

Vocabulary Words Cohesion – an attraction between molecules of the same substance (Because of hydrogen, water is extremely cohesive) Adhesion – an attraction between molecules of different substances (The surface of the water in a graduated cylinder dips slightly in the center because the adhesion between water molecules and glass molecules is stronger than the cohesion of water molecules.Adhesion between water and glass also causes water to rise in a narrow tube against the force of gravity)

Think! (Study Hint: Test Questions) 1. Why are water molecules attracted to one another? Water molecules are polar, meaning that they have regions with partial positive and negative charges. 2.How are cohesion and adhesion similar? Different? Cohesion and adhesion are similar because they are attractions between molecules, but cohesion occurs between molecules of the same substance and adhesion occurs between molecules of different substances. 3.How does the tarantula’s physical structure help it to stay afloat? Because of its multiple legs, a tarantula’s mass is distributed over a large area on the water, which means that the pull of gravity is limited at any one location on the surface.

Vocabulary Words Mixture – material composed of two are more elements or compounds that are physically mixed together but not chemically combined (Salt and pepper, nut and fruit mix, alphabet grain and marshmallow cereal) Solutions and suspensions are two types of mixtures. Solution - all the components are evenly distributed (Example: If a crystal of table salt is placed in a glass of warm water, sodium and chloride ions on the surface of the crystal are attracted to the polar water molecules. Ions break away from the crystal and are surrounded by the water molecules. The ions gradually become dispersed in the water. ) Solute – substance that is dissolved (salt) Solvent substance in which the solute dissolves (Water) (Memory device: V and W are at the end of the alphabet.)

Suspension – some materials do not dissolve but separate into pieces so small that they do not settle out (The movement of water molecules keep the particles suspended.) Blood is both a solution and a suspension. It is mostly water that contains many dissolved substances. But it also contains particles that remain in suspension.

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 Go to Section: Cl - Water Cl - Na + Water Na +

Acids and Bases H + OH - Acid Neutral Base ___________________________________________________________ 0 7 14 Strong Weak Strong Know the examples in the next slide. See Figure 2-10 in the text.

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:

Vocabulary Acid – Any compound that forms hydrogen ions (H + ) in solution Hydrochloric acid produced by the stomach to help digest food is a strong acid (pH 1.5) Base (Alkaline) – A compound that produces hydroxide ions (OH - ) in solution pH scale - a measurement system that indicates the concentration of hydrogen ions in solution; each step represents a factor of 10. Example: A liter of a solution with a pH of 4 has ten times as many hydrogen ions as a liter of a solution with a pH of 5. Know the chemical equation on the bottom of page 42 in the text.

pH Indicators pH paper – match color with pH chart Electronic pH meter – insert probe and read pH Litmus paper – turns red in the presence of acid and blue in the presence of bases Phenolphthalein – pH range of 8-10; colorless for an acid and pink to red in a base Bromthymol blue – turns yellow in an acid and blue in a base

Buffers Buffers are weak acids or bases that can react with strong acids or bases to prevent sharp, sudden changes in pH. They are dissolved compounds in the human body. The pH of the fluids within most cells in the human body must generally be kept between 6.5 and 7.5 Human blood has a pH of 7.4 If the pH is lower or higher, it affects the chemical reactions that take place in the cell Buffers help maintain homeostasis. Carbonic acid-bicarbonate buffering system is an example.

Answers to Questions 1-5 on page 43 in the Text 1.The hydrogen atoms form covalent bonds with the oxygen atom. Because of oxygen’s greater attraction for electrons, there is an unequal distribution of electrons. The oxygen end of the bent water molecule is negative and the hydrogen end is positive. 2.Per volume, there are more hydrogen ions than hydroxide ions in an acidic solution and more hydroxide ions than hydrogen ions in a basic solution. 3.In a solution, all components are easily distributed. In a suspension, undissolved particles are suspended in the mixture and can settle out over time. 4.The pH scale measures concentrations of hydrogen ions in a solution. 5.The pH will be less than 7. (Strong acid and neutral water: still acidic)

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:

Answers to Life’s Backbone 1.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. 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. Students may know that many carbon compounds also contain oxygen and/or hydrogen.

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:

Carbon 1.Has four valence electrons, so can form four covalent bonds at one time 2.Carbon atoms bond together in straight chains, branched chains, or rings 3. Since there are four valence electrons, carbon can form single bonds, double bonds, and triple bonds.

Vocabulary Organic compounds – contain carbon and hydrogen, as well as other elements Examples: carbohydrates, lipids, proteins, nucleic acids Inorganic – contains no carbon Examples – water, mineral elements, acids and bases Organic chemistry – the study of all compounds that contain bonds between carbon atoms Answer to observing (Figure 2-11 on page 44 in text): There are three covalent bonds between the carbon atoms in acetylene.

MethaneAcetyleneButadieneBenzeneIsooctane Section 2-3 Figure 2-11 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, Go to Section:

Organic Compound ElementsBuilding BlocksShape/Significant Groups CarbohydrateC,H,OMonosaccharidesRing H and O present in same ration as water 2:1 LipidC,H,O3 Fatty acids and glycerolLong chains ProteinC,H,O,NAmino acidsAmino group and a carboxyl group Nucleic AcidC,H,O,N,PNucleotides5-carbon sugar, a phosphate group, and a nitrogenous base

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

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

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

Vocabulary Macromolecule – giant molecules made up of thousands or even hundreds of thousands of smaller molecules Polymerization – large compounds are build by joining smaller ones together; the process in which monomers are joined to form larger units called polymers Monomer – each subunit that acts as a building block for a polymer; can be identical like links on a watch or different like the beads in a multicolored necklace Polymer – similar, repeating units; a large compound formed from combinations of many monomers

Carbohydrates *Main source of energy for living things *Plants and some animals also use carbohydrates for structural purposes *Sugars are stored as starches *Monomers in starch molecules are sugar molecules

Monosaccharides One sugar carbohydrate C 6 H 12 O 6 Examples: galactose, glucose. fructose Disaccharides Two sugars C 12 H 22 O 11 Examples: Sucrose (table sugar composed of glucose and fructose), lactose (milk sugar), maltose Polysaccharides More than two Can be thousands Starch (storage form of sugar) Cellulose (forms cell wall, supporting material in plants,wood and paper) Glycogen (animal starch) *When the level of glucose in your blood runs low, glycogen is released from your liver. The glycogen stored in your muscles supplies energy for contraction and, thus, for movement. Isomers- same molecular formula but different structural formula Example: glucose and fructose

Lipids 1.Part of cell structures and reserve energy supply: membranes, waterproof coverings 2.Fats, oils, and waxes (found in fur, skin, leaves, exoskeleton of some insects) 3.Less O in relation to H 4.Relatively small, NOT polymers 5.Long-term energy storage, insulation, protective coating 6.Furnish about twice as much energy as the same amount of carbohydrates 7. Fats and oils are chemically similar. Unlike fats, however, oils remain liquid at room temperature *Note: Steroids (some are chemical messengers) are also lipids.

Vocabulary Saturated – only single bonds; has the maximum number of hydrogen atoms (fats with animal origins-milk, beef, butter) Unsaturated – has at least one carbon-carbon double bond Has double and triple bonds ( fats with plant origins) Examples – olive oil, corn oil, fish oil, sunflower oil Polyunsaturated – more than one double bond Fats and cholesterol: LDL- low density lipoproteins HDL – high density lipoproteins (H – Happy, good ) Lipid derivatives Phospholipids : Lecithin (part of cell membrane) Cephalin (brain nerves, neural tissue)

Nucleic Acids Store and transmit hereditary, or genetic information Largest organic molecules Nucleic Acids – DNA and RNA Deoxyribonucleic acid (DNA) contains the sugar deoxyribose. Ribonucleic acid (RNA) contains the sugar ribose. Know Figure 2-15 on page 47 in text. (Be able to draw and label)

Proteins 1.Found throughout living organisms - make life possible 2.Structures are very complex 3.More than 20 different types of amino acids represent the R (variable) group 4.There can be more than 3,000 amino acids in a protein 5.Carbon atoms bond in four places: A. Amino group (NH 2 ) B. Carboxyl group (COOH) C. Hydrogen atom D. Variable group (R) This group is a side chain that is different in each amino acid GLYCINE is the simplest amino acid. Its R group is hydrogen (H).

Proteins form peptide bonds- a bond between C in the carboxyl group of one amino acid and N in the amino group of the next amino acid dipeptide bond – two amino acids linked together by a peptide bond polypeptide chain – a large number of amino acids linked by peptide bonds Polypeptides combine to form proteins. Some proteins control the rate of reactions and regulate cell processes. Some are used to form bones and muscles. Other proteins transport substances into and out of the cells or help to fight disease.

Types of Proteins TypeFunctionExamples HormonalChemical messengersGlucagon, insulin TransportTransport of other substances Hemoglobin, carrier proteins StructuralPhysical supportCollagen ContractileMovementActin, myosin AntibodiesDefenseImmunoglobulins, Interferons EnzymesBiological catalystsAmylase, lipase, ATPase

Glucagon- secreted by pancreas, helps change glycogen (a polysaccharide that is a major storage product in animals) to glucose (a sugar) Insulin – secreted by pancreas, helps convert glucose to glycogen Hemoglobin – an iron-containing protein compound that helps transport O and CO 2 (gives blood red color) Collagen – part of connective tissue (supports, binds tissue and organs together) Actin – thin filaments found in microfilaments used for cell movement and contraction of muscle cells Myosin – thick filaments found in muscles Interferons – produced by living cells that have been entered by a virus

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:

Answers to Matter and Energy 1.Reactants are oxygen and cellulose. 2.Products are carbon dioxide and water. 3.Light and heat are given off. Some students may also mention sound (the crackling of a fire). 4.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 going, it gives off enough heat to start more of the wood burning.

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:

Vocabulary Chemical reactions – process that changes one set of chemicals into another set of chemicals They always involve the breaking of bonds in reactants and the formation of new bonds in products. Example: oxygen and iron form rust Reactants – elements or compounds that enter into a chemical reaction Products – elements or compounds produced by a chemical reaction Example: Carbon dioxide, which is not very soluble in water, reacts with water in your blood to form a soluble compound called carbonic acid. This enables the bloodstream to carry carbon dioxide into your lungs. In the lungs, the reaction is reversed. This produces carbon dioxide gas, which is released as you exhale. (Equations on bottom of page 49 in text.)

Energy in Reactions Chemical reactions that release energy often occur spontaneously. Example: Hydrogen gas burning, or reacting with oxygen to produce water vapor..Energy is released in the form of heat…and when hydrogen gas explodes – light and sound Chemical reactions that absorb energy will not occur without a source of energy. Example: Water generally doesn’t change into hydrogen and oxygen gas without requiring energy, such as an electric current. Cellulose (paper) burns in the presence of oxygen, but only if you apply a lit match. Activation energy – the energy that is needed for a reaction to begin

Answers to Analyzing Data on Page 51 in Text 1.Time is plotted on the x-axis and pressure of oxygen on the y-axis. 2.The rate was very rapid at first and then dropped off dramatically after about 40 seconds. 3.Hydrogen peroxide was used up OR the reaction is reversible. 4.With added base, the rate of reaction slowed down. With added acid, there is almost no reaction. 5.A base inhibits the enzyme so that it is less effective. An acid may deactivate the enzyme so that the reaction cannot take place. 6. Because vinegar is an acid, it would inhibit and possible destroy the catalyst

Enzymes Catalyst-substance that speeds up the rate of a chemical reaction (lowers the activation energy Enzymes – proteins that act as catalysts Cells use enzymes to speed up chemical reactions that take place in cells. A reaction can take place as much as ten billion times faster. Very specific Name derived from the reaction it catalyzes Lock and key fit (perfect fit)

Enzymes at Work Carbonic anhydrase – catalyzes the reaction that removes water from carbonic acid Hexokinase – converts glucose and ATP into glucose-6-phosphate and ADP (stored energy and released energy) Catalase – one of the fastest acting enzymes; breaks down hydrogen peroxide (poisonous byproduct of most chemical reactions in human cells) into water and oxygen

Commercial Uses of Enzymes Some enzymes split proteins so they are used in laundry detergents. Papain, found in papaya, is used in meat tenderizer.

Vocabulary Substrate – material acted upon by an enzyme; the reactants Active site – where enzyme and substrate join Products – substances liberated during the reaction Coenzyme – non-protein molecule that assists enzyme; vitamins Denaturation – active sites of enzymes altered; life-threatening Inhibitor-disables enzyme by joining with it without itself being changed Competitive inhibitor – fake substances (antibiotics) Non-competitive inhibitor – attaches to OR changes the shape of an active site (lead, mercury, cyanide)

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:

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

Factors Affecting Enzyme Action 1.pH – Pepsin (stomach) works best at a pH of 1.5-2.2 Trypsin (small intestine) works best at a pH of 7.9-9.0 2. Temperature – most at body temperature (37

Factors Affecting Enzyme Action 1.pH – Pepsin (stomach) works best at a pH of 1.5-2.2 Trypsin (small intestine) works best at a pH of 7.9-9.0 2.Temperature – most at body temperature (37 degrees Celsius) 3.Relative amounts of enzyme and substrate 4.Most cells contain proteins that turn key enzymes “on and off” during critical stages in the life of the cell.

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.

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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.

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Presentation on theme: "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."— Presentation transcript:

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