Chapter+Six

Definition Worksheet #8: Chapter 6 Define the following terms related to energy and metabolism.


 * 1) Activation Energy: is the minimum amount of energy required to start a chemical reaction. It is independent of any energy difference between reactants and products.
 * 2) Active Site: The sites are pockets where substrates bind and where reactions proceed. The active site is complementary in shape, size, polarity, and charge to the substrate.
 * 3) Anabolism: Referring to the metabolic pathway in which smaller molecules are built into larger molecules are called biosynthetic, or anabolic.
 * 4) Catabolism: A metabolic pathway reaction that breaks molecules apart are degradative, or catabolic.
 * 5) Co-enzymes: Organic cofactors are called co-enzymes and almost all vitamins are coenzymes or precursors of them.
 * 6) Co-factors: associate with enzymes and assist their function. Cofactors are atoms or molecules (other than proteins) that associate with enzymes and are necessary for their function.
 * 7) Competitive Inhibition: this occurs when a molecule that resembles the reactant (substrate) specific for an enzyme is present in solution and binds to the active site before the reactant has a chance to do so. The prevents the reactions from occurring. Increasing the concentration of the reactant will help speed up the reaction as it gives the substrate a better chance of getting to the active site before the inhibitor.
 * 8) Endothermic Reactions: “Energy in” Reactions in which the reactants have less free energy that the products require a net energy input to proceed. Cells store energy by running endergonic reactions. For example, the sunlight drives the overall reaction of photosynthesis, resulting in the glucose which is stored inside the cell.
 * 9) Exothermic Reactions: “Energy out” Reactions end with a net release of energy. Cells access free energy of molecules by running exergonic reactions. For example, the overall process of aerobic respiration which converts glucose and oxygen to carbon dioxide and water for a net energy output.
 * 10) First Law of Thermodynamics: Energy does not appear from nowhere, and it does not vanish into nothing.
 * 11) Kinetic Energy: the energy of motion. Generally there are three types: Light, Sound, and Temperature.
 * 12) Noncompetive Inhibition: this occurs when a molecule attaches to the enzyme molecule at some place other than the active site, but in doing so changes the “shape” of the active site so the reactant can no longer attach. This prevents the ration form occurring. In this case increasing the concentration of the reactant will NOT help speed up the reaction since it still will not be able to bond to the enzyme.
 * 13) Oxidation Reactions: Reaction in which one molecule accepts electrons (it becomes reduced) from another molecule (which becomes oxidized).
 * 14) Phosphorylation Reactions: A phosphate-group transfer.
 * 15) Potential Energy: the energy that is stored. This can also be seen as the capacity to do work due to an object’s location or arrangements of parts.
 * 16) Reduction Reactions: Involve the gain of electrons in a chemical reaction in which the release or absorption of energy does not require ATP, but the transfer of electrons.
 * 17) Second Law of Thermodynamics: when energy disperses, the system tends to change toward a state of maximum entropy; energy tends to disperse spontaneously.


 * __ CHAPTER 6 __**** : Ground Rules of Metabolism **

It is important to note that, even though we may not fully understand energy’s true nature (is it a wave or a particle?) we do understand that energy can be converted from one form to another. Often, this is how we HARNESS energy!
 * 1) Before learning about metabolism it is important to review some basic concepts regarding ENERGY. What is the definition of energy? The capacity to do work

There are two basic forms of energy: A. POTENTIAL ENERGY is defined as energy that is stored. This can also be seen as the capacity to do work due to an object’s location or arrangement of parts. 1. The higher an object is above the ground the more energy it possesses. Think of jumping off of a chair verses jumping out of a plane; which would have a greater potential to do you bodily harm? 2. Another definition relates this energy to the structure of molecules and the type of bonds connecting the atoms together; hydrogen bonds have less energy than covalent bonds, so are easier to break. This form of energy is also called CHEMICAL energy and is the type we will be discussing in this class. 1. LIGHT : The differrent colors of the rainbow ( R **O** Y G B **I** V ) have different levels of kinetic energy. “l**o**w” “h**i**gh” Red-orange-yellow light has low kinetic energy; blue-indigo-violet light has high kinetic energy. 2. SOUND: Different sounds both loudness and pitch (high or low) have different levels of kinetic energy. High volume or high pitched sounds with a high frequency have a high level of energy and can actually break glass 
 * 1) KINETIC ENERGY is defined as energy of motion. There are generally three types of kinetic energy:

** low energy ** ** low frequency **
 * long wavelength **


 * short wavelength **
 * high energy **
 * high frequency **

3. TEMPERATURE : Temperature is a number that is related to the average [|kinetic energy] of the molecules of a substance. If temperature is measured in Kelvin degrees, then this number is directly proportional to the average kinetic energy of the molecules. Heat is a measurement of the total energy in a substance. That total energy is made up of not only of the kinetic energies of the molecules of the substance, but total energy is also made up of the potential energies of the molecules.

More About Temperature So, temperature is not energy. It is, though, a number that relates to one type of energy possessed by the molecules of a substance. Temperature directly relates to the kinetic energy of the molecules. The molecules have another type of energy besides kinetic, however; they have potential energy, also. Temperature readings do not tell you anything directly about this potential energy. http://www.eia.doe.gov/kids/energyfacts/science/formsofenergy.html 2. THERMODYNAMICS is the study of energy transformations that occur in matter. A. There are several laws that govern energy conversions: 1. 1st LAW of THERMODYNAMICS (law of energy conservation) states that the total amount of energy in the universe is constant (can’t be created or destroyed). a. it can be __transferred__ or moved from one object or location to another, for example a cold metal chair gets warm after we sit on it for awhile. b. it can also be __transformed__ or changed from one form to another, for example the stored energy in wood is changed to light and heat as the wood burns 2. 2nd LAW of THERMODYNAMICS states that energy tends to flow from concentrated to less concentrated areas. a. In other words, chemical reactions are never 100% efficient; some energy will always be “lost” to the surroundings as heat when chemical bonds break. As chemical reactions occur in the human body, about 60% of the potential energy becomes heat.The molecules in the surrounding area are moving more rapidly and therefore are becoming less organized. b. _ Entropy is a measurement of how much and how far a concentrated form of energy has been dispersed after an energy change has occurred. c. It takes energy to stay organized (orderly). Without energy input any system will tend to become more disorganized; large polymers will ultimately break down to become monomers. 3. Answer the following True-False statements. If the statement is false, make it correct by changing the underlined word and writing the correct word in the answer blank. 1. False Energy that is stored in the bonds between atoms (chemical energy) is also called __kinetic__ (chemical) energy. 2. True __Energy__ is the capacity to accomplish work, or to move objects. 3. False The amount of low-quality (heat) energy in the universe is __decreasing__ remaining constant. 4. True The entropy of two atoms decreases when a bond forms between them. 5. True No energy conversion can ever be 100 percent efficient, some of the stored energy will always be converted to __heat__. 6. True The collective strength of chemical bonds resists the spontaneous direction of energy flow. 7. False The __second__ (1st) law of thermodynamics states that the total amount of energy in the universe is remaining constant. 4. Metabolism involves all the chemical reactions by which cells acquire and use energy as they synthesize (make), store, degrade (break down) and eliminate substances. There may be many molecules involved in an overall chemical reaction from start to finish. A. Reactants (substrates) are substances that enter a reaction or are present at the beginning of the reaction. B. Intermediates __are the substances that form before a reaction ends somewhere along the way from the beginning of the process to the end of the process.__ __C.__ ___ Products are the final substances that are produced by a chemical reaction, or are left at the end of a reaction pathway.__

__5. Chemical reactions in our bodies either store, release or transfer energy.__ __ A. ENDERGONIC REACTIONS are those__ __that require an input of energy. If the__ __energy input is in the form of heat it is__ __called an ENDOTHERMIC reaction.__ __These reactions generally start with many__ small __molecules with fewer bonds and__ __therefore with a lower energy and join__ __them together to form__ larger __molecules__ __that contain more bonds and therefore__ __have more energy. Energy must be__ added__ to create these additional bonds. 1. Photosynthesis is an example of an endergonic reaction; energy from the sun is used to combine CO2 and H2O to form glucose C6H12O6. 2. Joining together amino acids to form protein molecules is another example.

that release energy. If the energy released is in the form of heat it is called an EXOTHERMIC reaction. These reactions generally start with one __large__ molecule and break it apart to form many __smaller__ molecules that contain fewer bonds and therefore have less energy. Energy is __released__ to the surrounding area in the form of heat as the chemical bonds are broken. 1. Burning a candle or a piece of wood is an example of an exothermic reaction. All the stored energy in the cellulose (glucose molecules) is released __quickly__ in the form of heat and light. 2. Cellular Respiration is the chemical breakdown of glucose __slowly__, involving many steps to produce ATP and is also an example of an exothermic reaction. C. Endothermic and Exothermic reactions can be illustrated as an “energy hill” where the reactants of the chemical reaction either start at the bottom of the “hill” or at the top of the “hill”. Draw “energy hill” diagrams for an endothermic and exothermic reaction to illustrate whether energy is released when the reaction occurs or energy must be added for the reaction to occur. ENDOTHERMIC EXOTHERMIC  Energy Energy
 * 1) [[image:file:///C:/Users/family/AppData/Local/Temp/msohtmlclip1/01/clip_image006.gif width="259" height="189"]] EXERGONIC REACTIONS are those

  Time Time

Endo: Starts at bottom and goes up like a hill, Exo: Starts near top of and then goes down sharply and lands near bottom spikes and then reduces slightly to about middle

D. The molecule ATP __generally couples the energy input with the energy output in chemical reactions. Cells try to use the energy from EXERGONIC reactions to drive the ENDERGONIC reactions.__ __ 1. Covalent bonds are very strong, so as they are broken the stored, potential (chemical) energy is released.__ __2. ATP however has even more potential__ __energy than what is stored in the covalent__ __bonds. The three phosphate groups are__ __surrounded by negative charges due to the__ __electrons surrounding the oxygen atoms.__ __Remember that similar charges tend to repel__ __each other; therefore there is an added__ __potential energy that is released as each__ __of these phosphate groups is removed by a hydrolysis reaction. ATP (AdenosineTRIphosphate) becomes ADP (Adenosine DI phosphate) and stored potential energy is released.__ __[]__

__3.__ ___ Phosphorylation is the transfer of a phosphate group from one molecule (like ATP or ADP) to another molecule.__ __6. Classify each of the following reactions as either //endergonic// or //exergonic//.__

_ Exergonic 1. Burning of wood in a campfire. ___ Endergonic 2. The products of a chemical reaction have more energy than the reactants (starting materials) had originally.__ _ Exergonic 3. Glucose + oxygen → carbon dioxide + water + energy ___ Exergonic 4. The reactants (starting materials) of a chemical reaction have more energy than the products produced.__ _ Exergonic 5. The reaction releases energy in the form of heat to the surrounding area. ___ Endergonic 6. CO2 + H2O + solar (UV) energy → Glucose + oxygen__

__7. Many substances in a cell possess a large amount of stored energy, are quite reactive and break down easily; however, they also require an initial amount of energy to start the chemical reaction. What is ACTIVATION ENERGY? the minimum amount of energy that will get a chemical reaction started. It is independent of any energy difference between reactants and products. __

__8.__ Enzymes are catalysts that can  speed up chemical reactions hundreds to millions of times faster than without the help of the catalyst. Without them, most chemical reactions that occur in the body would not occur fast enough to satisfy the needs of the cell. A. Most enzymes are which type of organic molecule? Proteins, but some RNA. B. Each enzyme is very specific for a specific molecule (substrate) or type of molecule. C. Enzyzmes do NOT change the original amount of stored energy (potential energy) of the reactants of the reaction.

D. Enzymes work by changing the amount of activation energy needed by the reactants to overcome the activation energy barrier and enter a chemical reaction. In other words, enzymes Reduce/lower _ the activation barrier that normally prevents the reaction from occurring. The amount of original potential energy in the reactants, the potential energy in the products and the overall energy of the reaction does NOT change, only the speed (rate) of the reaction changes. E. The same enzyme works in both forward and reverse reactions. The direction of the reaction is determined by the concentration of the reactants and products and the amount of energy available NOT the enzyme itself. F. During chemical reactions, the enzymes are NOT chemically changed to a different molecule; they remain unchanged at the end of the reaction, unlike the reactants (substrates) which are broken down and can be used again and again.

G. Enzymes work on the __molecular__ level by following several different mechanisms, either alone or in combination. 1. Some enzymes help ___ substrate molecules (reactants) get together (match-maker). If left on their own it is unlikely the molecules will collide with each other, so the enzyme attracts the substrates.__ __2. Some enzymes hold substrate molecules in a correct__ ___ orientation (position) that favors a reaction. If left on their own, it is unlikely that the functional groups of the molecules will be in the correct positions to react with each other.__ __3. Some enzymes work by shutting out water ____. This often lowers the activation energy of a reaction. Remember that water tends to cause a “hydrolysis reaction” that causes bonds to break, not to form.__ __4. Some enzymes help the substrate by Inducing ___ a fit that helps to allow the substrate in to the active site, but then push it into place so the reaction can procede. 5. Some enzymes promote an acid-base environment which further encourages the loss of water and a dehydration synthesis reaction to occur so bonds can form between the substrate molecules. H. Most enzymes require assistance or help from other molecules including: 1. __Co-enzymes__ (also known as VITAMINS) are organic molecules that help enzymes speed up chemical reactions. Niacin (B3) for example helps in the metabolism of carbohydrates, lipids and proteins for energy. 2. __Co-factors__ (also known as MINERALS) are inorganic or metal ions that also help enzymes. Ca+2 for example is needed to help break peptide bonds during the digestion of protein molecules and helps to form blood clots.  I. As mentioned, enzymes are very specific for a specific reactant or group of reactants. Enzymes are generally very large protein molecules with a specific 3-dimensional shape. Part of the enzyme serves as the “attachment site”, the location where the substrate molecule or molecules attach to the enzyme. This area is commonly called the ___ Active SITE of the enzyme.__ __Describing enzyme function this way is often called the__ __“Lock and Key Model”. This means that the enzyme__ __and substrate work like a key in lock on a door, where__ __only a specific key will work on a specific lock.__ __J. In some cases, once the reactant or reactants attach__ __to the active site of an enzyme, the enzyme changes__ __its shape to better hold the substrate(s) in place while__ __the chemical reaction occurs. Describing enzyme__ __function this way is often called the__ __ Induced Fit _ MODEL.__ __K. Once the chemical reaction is completed, the enzyme releases the new molecule formed (product) and is free to be used over and over again.__ __L. Enzyme activity can change with changes in the cellular environment.__ __ 1. Changes in__ __: Temperature __ __a. For a reaction to occur quickly, the substrate molecules__ __(reactants) must come in direct contact with the active__ __site of the enzyme. Changing the speed that molecules__ __in solution move about may increase or decrease the__ __likelihood that the two molecules will “find” each other.__ __- increasing the temperature will generally cause the__ __molecules to move faster, increasing the reaction rate__ __- decreasing temperature will generally cause molecules to move slower, decreasing the reaction rate__ __b. Enzymes are protein molecules; any change in the__ __overall 3-D shape of the protein may change the__ __effectiveness of the enzyme. Increasing the temperature__ __weakens hydrogen bonds that help hold the 3-D shape,__ __thus alters the effectiveness of the enzyme.__ __c. Most human enzymes work best at normal body temperature of 35-40 oC.__ __ 2. Change in__ PH ___:__ __a. The presence of hydrogen ions may__ __interfere with the hydrogen bonds__ __stabilizing the protein 3-D structure,__ __thus may result in a change in the protein__ __structure and therefore its function.__ __b. Most human enzymes work best at a__ __pH of 6-8, however enzymes in the__ __stomach work best at a pH of 1-2.__ __3. Changes in__ IONS___concentrations (salinity):__ __a. Most enzymes stop working effectively when the solution is “saltier” or less salty than they can tolerate. Remember that a salt is a compound that when dissolved in water produces both positive (+) and negative (-) ions. Too much or too little salt can also interfere with the hydrogen bonds that hold the enzyme in the correct shape.__ __b. Most human enzymes work best at a salinity of 0.85%__ __4. When a protein molecule (or in this case an enzyme) has a change in the 3-D__ __structure causing it to lose its function, it is said to be__ _Denaturation.

M. Many factors influence what an enzyme molecule does at any given time or whether it is produced in the first place. Enzyme inhibitors are important regulators of chemical reactions in the cell. In some cases, the product of a chemical reaction acts as an inhibitor of the enzyme required to start the reaction. When enough product is produced, the cell can stop the production of any more product by binding a product molecule to the enzyme preventing the reaction from continuing. This is generally called Allosteric INHIBITION. 

 There are two methods whereby enymes by be inhibited or prevented from performing their actions. 1. COMPETITIVE INHIBITION: this occurs when molecule that resembles the reactant (substrate) specific for an enzyme is present in solution and binds to the active site before the reactant has a chance to do so. This prevents the reaction from occurring. Increasing the concentration of the reactant will help speed up the reaction as it gives the substrate a better chance of getting to the active site before the inhibitor. An example of this type of reaction is seen with the competative nature of carbon monoxide with oxygen for hemoglogin in the blood.  Both molecules have a very similar molecular structure. 2. NONCOMPETITIVE (ALLOSTERIC) INHIBITION: this occurs when a molecule attaches to the enzyme molecule at some place other than the active site, but in doing so changes the “shape” of the active site so the reactant can no longer attach. This also prevents the reaction from occurring. In this case increasing the concentration of the reactant will NOT help speed up the reaction since it still will not be able to bind to the enzyme.

9. CELLULAR METABOLISM is defined as the sum of all chemical reactions that build up larger molecules from smaller ones and those that break down larger molecules into smaller ones releasing energy in the process.
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 * || [[image:file:///C:/Users/family/AppData/Local/Temp/msohtmlclip1/01/clip_image027.gif width="575" height="262"]] ||

A.BioSynthesisPathways (also known as ANABOLISM) involve the “building up” of larger molecules from smaller ones and requires the input of energy (_THERMIC). B. Degraduative Catabolic___ Pathways (also known as CATABOLISM) involve the “breaking down” of larger molecules into smaller ones and__ __releases energy EXO(____THERMIC).__ __C. Many chemical reactions are “reversible” meaning the direction the reaction proceeds is based on the concentration of the reactants and products. If there are more reactants the reaction will move “forward”; if there are more products than reactants, then the reaction will tend to reverse and move “backward” breaking down the products and reforming the reactants. The reaction will continue until “equilibrium” (the rate of the forward and reverse reactions are equal) is reached.__ __10. Some chemical reactions that release or absorb energy do not use ATP as a__ __driving force; instead they involve the transfer of__ Electrons. These reactions are called Oxidation___ Reactions.__ __A. The removal or loss of electrons is called Oxidation__ __B. The addition or gain of electrons is called Reduction__ __

11. Match each of the following descriptions to the correct term.
2. G_ degradative pathways 3. _I chemical equilibrium 4. D_ cofactors 5.J _ transport proteins 6. A_ metabolic pathway 7. E_ reactants (substrates) 8. C_ energy carriers 9. B_ biosynthetic pathways 10. Henzymes || A. An orderly series of reactions catalyzed by enzymes B. Metabolic pathway where small organic molecules are assembled into larger organic molecules in a series of reactions C. Mainly ATP; donate(s) energy to reactions D. Small molecules and metal ions that assist enzymes or serve as carriers E. Substances able to enter into a reaction F. Compounds formed between the beginning and end of a metabolic pathway G. Metabolic pathway where organic compounds are broken down in a series of reactions H. Proteins (usually) that catalyze reactions I. Rate of the forward reaction equals the rate of the reverse reaction J. Membrane-bound substances that adjust concentration gradients in ways that influence the direction of metabolic reactions ||
 * 1. E_ intermediates

12. Which contains more potential energy, a large complex molecule like a protein, or the smaller amino acid subunits of which it is composed? Why? Large Complex Molecules hold more Potential energy in their many complex bonds.

13. Is the joining together of amino acids to form a protein an exothermic or endothermic reaction? Why?

Endothermic Reaction because the reactants have less energy than the products

14. Where does the cell obtain energy to carry out endothermic reactions? From ATP and from performing exothermic reactions which release energy. that energy is used to perform reactions that require energy


 * //Sample Test Questions for chapter 6://**

1. Kinetic energy differs from chemical energy in that a. kinetic energy is stored energy that has the potential to do work, and chemical energy is the energy of movement b. kinetic energy depends on the movement of atoms, whereas chemical energy depends on the movement of molecules c. kinetic energy can be converted into various forms of energy, whereas chemical energy can only be converted to heat e. chemical energy is a particular form of kinetic energy
 * d**. kinetic energy is the energy of a moving object, whereas chemical energy is the potential energy stored in chemical bonds.

2. TRUE or **FALSE**: According to the second law of thermodynamics, energy can neither be created nor destroyed.

3. What percent of energy obtained from food is lost as heat energy? a. 100% c. 40% d. 25%
 * b.** 60%

4. Where is energy stored in a molecule? a. in the nucleus b. in the mitochondria c. in glycogen
 * d**. in bonds

5. What are the three parts that make up an ATP molecule? b. adenine, thymine, 3 phosphate c. adenine, glucose, 3 potassium d. adenine, glucose, 3 phosphate
 * a**. adenine, ribose, 3 phosphate

6. During enzyme catalyzed reactions, a //substrate// is another word to mean a. end product b. enzyme d. all of the above
 * c**. reactant

7. The active site of an enzyme a. is where the coenzyme is attached b. is a specific bulge or protrusion on an enzyme d. is less active than other parts of the enzyme
 * c**. is a place on the enzyme where substrate molecules attach

8. TRUE or **FALSE**: Most of the cell’s enzymes are classified as carbohydrates.

9. Some enzymes involved in the hydrolysis of ATP cannot function without the help of inorganic molecules called minerals. In this case the minerals function as a. substrate molecules c. coenzymes d. non-competitive inhibitors e. competitive inhibitors
 * b**. cofactors

10. A substance that binds to a site other than the active site and in the process changes the shape of the active site on the enzyme is called a(n) a. competitive inhibitor c. enzyme deactivator d. co-enzyme
 * b**. non-competitive inhibitor

11. TRUE or **FALSE:** Reactions that are part of a “biosynthetic pathway” (anabolism) are generally described as being exothermic reactions.

12. **TRUE** or FALSE: Reduction reactions involve a gain in electrons.