Presentation is loading. Please wait.

Presentation is loading. Please wait.

Ch. 8 An Introduction to Metabolism. I.Introduction A.The cell has thousands of chemical reactions occurring within a microscopic space. -Example: Cellular.

Similar presentations

Presentation on theme: "Ch. 8 An Introduction to Metabolism. I.Introduction A.The cell has thousands of chemical reactions occurring within a microscopic space. -Example: Cellular."— Presentation transcript:

1 Ch. 8 An Introduction to Metabolism

2 I.Introduction A.The cell has thousands of chemical reactions occurring within a microscopic space. -Example: Cellular respiration - energy from sugar is extracted. II.Metabolism, Energy, and Life A.Metabolic pathways 1.Metabolism is the sum of all chemical reactions in an organism. 2.Enzymes accelerate chemical rxns. 3. Catabolic pathways release energy by breaking down complex molecules to simpler compounds. Ex. Cellular respiration

3 4.Anabolic pathways consume energy to build complicated molecules from simpler compounds. Ex. Synthesis of proteins from amino acids B.Energy coupling: Energy from catabolic pathways is used for anabolic pathways. C.Bioenergetics is the study of how organisms manage their energy resources. D.How organism transform energy 1.Energy: 2.Kinetic energy: 3.Potential energy: 4.Chemical energy:  Organisms can convert one type of energy to another (Ex. Slide)


5 E.The two laws of thermodynamics (the study of energy transformations) in regards to an open system: 1.The first law of thermodynamics: energy can be transferred and transformed, but it cannot be created or destroyed. 2.The second law of thermodynamics: entropy increases with every energy transformation or transfer. The universe is becoming more random. -much of the energy transformed in the universe is transformed into heat energy.  Combining the two laws, the quantity of energy is constant, but the quality is not.

6 F.Organisms live at the expense of free energy 1.Spontaneous processes are those that can occur without outside help. Spontaneous processes occur so that a system may become more stable.


8 2.The free energy (G) in a system is related to the total energy (H) and its entropy (S) by this relationship: G = H – TS, where T is temperature in Kelvin units. a.Free energy can also be a measure of stability in a system. Systems high in free energy are unstable. They will lose free energy in spontaneous processes. delta G = G final state - G starting state Delta G is negative in spontaneous processes.

9 3.Systems that are stable and are at equilibrium have no change in free energy.  Systems at equilibrium means that it can do no work.  Systems at equilibrium must receive energy from an outside source in order to do work; it is nonspontaneous. G.Exergonic and Endergonic reactions in metabolism 1.In an exergonic reaction, there is a release of energy. -delta G is negative. It is a spontaneous reaction.

10 For the overall reaction of cellular respiration: C 6 H 12 O 6 + 6O 2 -> 6CO 2 + 6H 2 O delta G = -686 kcal/mol

11 2.In an endergonic reaction, energy is absorbed. -delta G is positive and free energy is stored. -it is nonspontaneous.

12 Photosynthesis is steeply endergonic, powered by the absorption of light energy. Delta G = + 686 kcal / mol. H.Metabolic Disequilibrium: reactions in a closed system will eventually reach equilibrium and do no work.

13 1.Cells maintain disequilibrium because there is a constant flow of energy in and out of a cell.

14 2.Sunlight is a source of free energy for photosynthetic organisms. Nonphotosynthetic organisms depend on photosynthetic organisms for energy in the form of organic molecules. I.ATP powers cellular work 1. A cell does three main kinds of work: Mechanical work Transport work Chemical work 2.In most cases, ATP is the immediate source of energy.

15 3.ATP (adenosine triphosphate) is a type of nucleotide consisting of: -nitrogenous base adenine -ribose sugar and a chain of -three phosphate groups

16 4.The bonds between phosphate groups can be broken by hydrolysis. Hydrolysis of the end phosphate group forms adenosine diphosphate [ATP  ADP + P i ] and releases 7.3 kcal of energy per mole of ATP under standard conditions. In the cell delta G is about -13 kcal/mol.

17 5.The bonds between the phosphate groups are referred to as high-energy. However, these bonds are weak and unstable. ADP + P i is more stable. ATP is more unstable than ADP because each phosphate group has a negative charge. These negative charges repel one another. 6.When ATP is hydrolyzed, the P i bonds to another molecule. This molecule is now phosphorylated, and energized.

18 7.ATP is a renewable resource that is continually regenerated by adding a phosphate group to ADP. III.Enzymes B. Enzymes speed up metabolic reactions by lowering energy barriers. A.Enzymes are catalysts. Catalysts change the rate of reaction without being destroyed.

19 Activation energy is the amount of energy necessary to push the reactants over an energy barrier.

20 Enzymes work by lowering the activation energy.

21 C.Enzymes are substrate specific 1.A substrate is a reactant that binds to the enzyme. The enzyme catalyzes the conversion of substrate to product. 2.The substrate binds to the active site on the enzyme. 3.When the substrate binds to the active site, the enzyme fits tighter around the substrate. This is called induced fit.


23 4.The substrate is held to the active site by weak bonds such as hydrogen and ionic bonds. 5.R-groups of amino acids in the active site catalyze of substrate to product. 6.Once the product is made, it leaves the active site and the enzyme is free to take another substrate. 7.Enzymes can catalyze reactions in both forward and reverse directions.

24 D.A cell’s physical and chemical environment can affect enzyme activity 1.Temperature Each enzyme has an optimal temperature.

25 2.pH: Most enzymes have an optimal pH between 6-8. However, digestive enzymes in the stomach (pepsin) have an optimal pH of 2, and intestinal enzymes (trypsin) have an optimal pH of 8.

26 E.Cofactors: many enzymes require non- protein helpers. These helpers are called cofactors. 1.These cofactors may be attached to the active site on enzymes, or they may bind to the substrate. 2. Inorganic examples: zinc, iron, copper. 3.Organic example (called a coenzyme): vitamins F.Enzyme Inhibitors: 1.Competitive inhibitors: 2.Noncompetitive inhibitors: 3.Examples: DDT, penicillin


28 IV.The control of Metabolism A.Molecules regulate enzyme activity: Allosteric regulation An activator will bind and change the shape of the enzyme to its active form. An inhibitor will bind and cause the enzyme to maintain its inactive form.

29 B.Feedback inhibition: a metabolic pathway is turned off by its end product, which acts as an inhibitor of an enzyme within the pathway.

30 C.Cooperativity: a substrate binds to the enzyme, causing the enzyme to take the active form. The enzyme’s multiple subunits are primed to accept its substrates.


Download ppt "Ch. 8 An Introduction to Metabolism. I.Introduction A.The cell has thousands of chemical reactions occurring within a microscopic space. -Example: Cellular."

Similar presentations

Ads by Google