Category: 1st Semester

Chapter 8 Membrane Structure Objectives

 

 

Chapter 8   Introduction to Metabolism
Objectives
Metabolism, Energy, and Life

1.        Explain the role of catabolic and anabolic pathways in cellular metabolism.

2.        Distinguish between kinetic and potential energy.

3.        Explain why an organism is considered an open system.

4.        Explain the first and second laws of thermodynamics in your own words.

5.        Explain why highly ordered living organisms do not violate the second law of thermodynamics.

6.        Write and define each component of the equation for free-energy change.

7.        Distinguish between exergonic and endergonic reactions in terms of free energy change.

8.        Explain why metabolic disequilibrium is one of the defining features of life.

9.        List the three main kinds of cellular work. Explain in general terms how cells obtain the energy to do cellular work.

10.       Describe the structure of ATP and identify the major class of macromolecules to which ATP belongs.

11.       Explain how ATP performs cellular work.

Enzymes Are Catalytic Proteins

12. Describe the function of enzymes in biological systems.

13. Explain why an investment of activation energy is necessary to initiate a spontaneous reaction.

14. Explain how enzyme structure determines enzyme specificity.

15. Explain the induced-fit model of enzyme function.

16. Describe the mechanisms by which enzymes lower activation energy.

17. Explain how substrate concentration affects the rate of an enzyme-catalyzed reaction.

18. Explain how temperature, pH, cofactors, and enzyme inhibitors can affect enzyme activity.

The Control of Metabolism

19. Explain how metabolic pathways are regulated.

20. Explain how the location of enzymes in a cell may help order metabolism

 
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Chapter 51 AP Obj Behavior

 

 

Chapter 51    Behavioral Biology
Objectives
Introduction to Behavior and Behavioral Ecology
1. Define behavior.
2. Distinguish between proximate and ultimate questions about behavior. Ask a proximate question and an ultimate question about bird song.
3. Explain how the classical discipline of ethology led to the modern study of behavioral ecology.
4. Define fixed action patterns and give an example.
5. Define imprinting. Suggest a proximate cause and an ultimate cause for imprinting in young geese.
Many Behaviors Have a Genetic Component
6. Explain how genes and environment contribute to behavior. Explain what is unique about innate behavior.
7. Distinguish between kinesis and taxis.
8. Distinguish between signal and pheromone.
9. Explain how Berthold’s research demonstrated a genetic basis for blackcap migration.
10. Describe Insel’s research on the genetic and physiological controls on parental behavior of prairie voles. Describe Bester-Meredith and Marler’s research on the influence of social behavior on parental behavior of California mice.
Learning
11. Explain how habituation may influence behavior.
12. Describe Tinbergen’s classic experiment on spatial learning in digger wasps.
13. Distinguish between landmarks and cognitive maps.
14. Describe how associative learning might help a predator to avoid toxic prey.
15. Distinguish between classical conditioning and operant conditioning.
16. Describe an experiment that demonstrates problem solving in nonhuman animals.
Behavioral Traits Can Evolve by Natural Selection
17. Explain how Hedrick and Riechert’s experiments demonstrated that behavioral differences between populations might be the product of natural selection.
18. Use an example to show how researchers can demonstrate the evolution of behavior in laboratory experiments.
19. Explain optimal foraging theory.
20. Explain how behavioral ecologists carry out cost-benefit analyses to determine how an animal should forage optimally. Explain how Zach demonstrated that crows feed optimally on whelks.
21. Explain how predation risk may affect the foraging behavior of a prey species.
22. Define and distinguish among promiscuous, monogamous, and polygamous mating relationships. Define and distinguish between polygyny and polyandry.
23. Describe how the certainty of paternity influences the development of mating systems.
24. Explain why males are more likely than females to provide parental care in fishes.
25. Suggest an ultimate explanation for a female stalk-eyed fly’s preference for mates with relatively long eyestalks.
26. Agonistic behavior in males is often a ritualized contest rather than combat. Suggest an ultimate explanation for this.
27. Explain how game theory may be used to evaluate alternative behavioral strategies.
28. Define inclusive fitness and reciprocal altruism. Discuss conditions that would favor the evolution of altruistic behavior.
29. Relate the coefficient of relatedness to the concept of altruism.
30. Define Hamilton’s rule and the concept of kin selection.
Social Learning and Sociobiology
31. Define social learning and culture.
32. Explain why mate choice copying by a female may increase her fitness.
33. State the main premise of sociology.
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Chapter 9 – Cellular Respiration Objectives

 

 

Chapter 9    Cellular Respiration
Objectives
The Principles of Energy Harvest

1.  In general terms, distinguish between fermentation and cellular respiration.

2.  Write the summary equation for cellular respiration. Write the specific chemical equation for the degradation of glucose.

3.  Define oxidation and reduction.

4.  Explain in general terms how redox reactions are involved in energy exchanges.

5.  Describe the role of NAD+ in cellular respiration.

6.  In general terms, explain the role of the electron transport chain in cellular respiration.

The Process of Cellular Respiration

7.  Name the three stages of cellular respiration and state the region of the eukaryotic cell where each stage occurs.

8.  Describe how the carbon skeleton of glucose changes as it proceeds through glycolysis.

9.  Explain why ATP is required for the preparatory steps of glycolysis.

10. Identify where substrate-level phosphorylation and the reduction of NAD+ occur in glycolysis.

11. Describe where pyruvate is oxidized to acetyl CoA, what molecules are produced, and how this process links glycolysis to the citric acid cycle.

12. List the products of the citric acid cycle. Explain why it is called a cycle.

13. Describe the point at which glucose is completely oxidized during cellular respiration.

14. Distinguish between substrate-level phosphorylation and oxidative phosphorylation.

15. In general terms, explain how the exergonic “slide” of electrons down the electron transport chain is coupled to the endergonic production of ATP by chemiosmosis.

16. Explain where and how the respiratory electron transport chain creates a proton gradient.

17. Describe the structure and function of the four subunits of ATP synthase.

18. Summarize the net ATP yield from the oxidation of a glucose molecule by constructing an ATP ledger.

19. Explain why it is not possible to state an exact number of ATP molecules generated by the oxidation of glucose.

Related Metabolic Processes

20. State the basic function of fermentation.

21. Compare the fate of pyruvate in alcohol fermentation and in lactic acid fermentation.

22. Compare the processes of fermentation and cellular respiration.

23. Describe the evidence that suggests that glycolysis is an ancient metabolic pathway.

24. Describe how food molecules other than glucose can be oxidized to make ATP.

25. Explain how glycolysis and the citric acid cycle can contribute to anabolic pathways.

26. Explain how ATP production is controlled by the cell, and describe the role that the allosteric enzyme phosphofructokinase plays in the process.

 
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Chapter 52 AP Obj Pop Ecol

 

 

Chapter 52    Population Ecology
Objectives
Characteristics of Populations
1. Distinguish between density and dispersion of a population.
2. Explain how ecologists may estimate the density of a species.
3. Describe conditions that may result in clumped dispersion, uniform dispersion, and random dispersion of individuals in a population.
4. Explain how a life table is constructed.
5. Distinguish between a life table and a reproductive table.
6. Describe the characteristics of populations that exhibit Type I, Type II, and Type III survivorship curves.
Life Histories
7. Define and distinguish between semelparity and iteroparity. Explain what factors may favor the evolution of each life history strategy.
8. Explain, with examples, how limited resources and trade-offs may affect life histories.
Population Growth
9. Compare the exponential model of population growth with the logistic model.
10. Explain how an environment’s carrying capacity affects the per capita rate of increase of a population.
11. Explain the meaning of each of the following terms in the logistic model of population growth:
a. rmax
b. K 2 N
c. (K 2 N)/K
12. Distinguish between r-selected populations and K-selected populations.
Population-Limiting Factors
13. Explain how density-dependent factors affect population growth.
14. Explain, with examples, how biotic and abiotic factors may work together to control a population’s growth.
15. Describe boom-and-bust population cycles, explaining possible causes of lynx/hare fluctuations.
Human Population Growth
16. Describe the history of human population growth.
17. Define the demographic transition.
18. Compare the age structures of Italy, Afghanistan, and the United States. Describe the possible consequences for each country.
19. Describe the problems associated with estimating Earth’s carrying capacity for the human species.
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Chemistry of Organisms

Chemistry
All Materials © Cmassengale

Composition of Matter

Ø  Everything in the universe is made of matter

Ø  Matter takes up space & has mass

Ø  Mass is a measure of the amount of matter in the substance

Ø  Mass & weight are NOT the same

Ø  Weight is a measure of the pull of gravity on an object

Question: Is the mass of an object the same on the moon as it is on the Earth? Is its weight the same? (Hint: Gravitational pull on the moon is 1/6 of that on the Earth.)

Ø  Matter exists in 4 states – solid, liquid, gas, & plasma

Ø  Solids have both a definite volume & definite shape (rock)

Ø  Liquids have a definite volume but no definite shape; they can be    poured (water)

Ø  Gases do not have a definite volume or definite shape, but they take the  volume & shape of their container

Ø  Plasmas have no definite volume, no definite shape, and only exist at extremely high temperatures such as the sun

Ø  Chemical Changes in matter are essential to all life processes

Ø  Biologists study chemistry because all living things are made of the same kinds of matter that make up nonliving things

Elements

Ø     Elements are pure substances which cannot be chemically broken down into simpler kinds of matter

Ø     More than 100 elements have been identified, but only about 30 are important in living things

Ø     All of the Elements are arranged on a chart known as the Periodic Table

Ø     Periodic charts tell the atomic number, atomic mass, & chemical symbol for every element

Ø     Four elements, Carbon – C, Hydrogen – H, Oxygen – O, and Nitrogen – N make up almost 90% of the mass of living things

Ø     Every element has a different chemical symbol composed of one to two letters

Ø     Chemical symbols usually come from the first letter or letters of an element like C for Carbon and Cl for Chlorine

Ø     Some chemical symbols come form their Latin or Greek name such as  Na for Sodium (natrium) or K for Potassium (Kalium)

Ø      Elements in the same horizontal period on the periodic table have the same number of energy levels (e.g. H & He in period 1 have only a K energy level)

[Periodic Table]
All Period 2 elements have 2 energy levels
(K & L)

Ø      Elements in the same vertical Family on the periodic table have the same number of electrons in their outermost energy level & react similar (e.g. Family IV, the Carbon family all have 4 electrons in their outermost energy level)

Atoms

Ø     Atoms are the simplest part of an element that keeps all of the element’s properties

Ø     Atoms are too small to be seen so scientists have developed models that show their structure & properties

Ø     Atoms consist of 3 kinds of subatomic particles – protons & neutrons in the center or nucleus, and electrons spinning in energy levels around the center

Ø     The nucleus is the center of an atom where most of the mass is concentrated

Ø     Protons are positively charged ( p+ ),  have a mass of 1 amu (atomic mass unit) , are found in the nucleus, and determine the atomic number of the element

Example:  Carbon has 6 protons so its atomic number is 6

Ø     Neutrons are neutral or have no electrical charge (n), have a mass of 1 amu, are found in the nucleus, and when added to the number of protons, determine the atomic mass of the element

Example:  Sodium has 11 protons and 12 neutrons so its atomic mass is 11+12=23 amu

Ø     Electrons (e-) are negatively charged, high energy particles with little mass that spin around the nucleus in energy levels

Ø     Seven energy levels (K, L, M, N, O, P, & Q) exist around the nucleus and each holds a certain number of electrons

Ø     The K energy level is closest to the nucleus & only holds 2 electrons, while the  L – Q energy levels can hold 8 electrons  

Ø     Electrons in outer energy level are traveling faster & contain more energy than electrons in inner levels  

Ø     The number of protons (positive charges) and electrons (negative charges in an atom are equal so the net electrical charge on a atom is zero making it electrically neutral

Ø     Stable or non-reactive atoms have an outer energy level that is filled with electrons  

Compounds

Ø     Most elements do not exist by themselves; Most elements combine with other elements

Ø      Compounds are made of atoms of two or more elements chemically combined

Ø      Chemical Formulas represent a compound & show the kind & number of atoms of each element  (e.g. H2O has 2 hydrogen & 1 oxygen)

Ø      Compounds have different physical & chemical properties than the atoms that compose them  (e.g. hydrogen & oxygen are gases but H2O is a liquid)

Ø      The number & arrangement of electrons in an atom determines if it will combine to form compounds

Ø      Chemical reactions occur whenever unstable atoms (outer energy level not filled) combine to form more stable compounds

Ø      Chemical bonds form between atoms during chemical reactions

Types of Chemical Bonds

Ø     Covalent bonds form between atoms whenever they share 1 or more pairs of electrons (e.g. H2O)  

Ø     Molecules form from covalent bonding & are the simplest part of a compound (e.g. NaCl, H2O, O2)  

Ø     Ionic bonding occurs between a positively & negatively charged atom or ion  

Ø     Positively charged ions have more electrons (-) than protons (+); negatively charged ions have more protons than electrons

Ø     Table salt (NaCl) forms when the 1 outer electron of Na is transferred to the outer energy level of chlorine that has 7 electrons (e-)

Ø     Sodium (Na) with 1 less e- becomes positively charged, while Chlorine (Cl) with 1 more e- becomes negatively charged; the + and – charges attract & form the ionic bond holding NaCl together

Ø     Other types of chemical bonding include hydrogen bonding

Energy

Ø     Energy is the ability to do work

Ø     Energy occurs in several forms & may be converted from one form to another

Ø     Sunlight is the ultimate energy for all life on earth

Ø     Forms of energy include chemical, electrical, mechanical, thermal, light, & sound

Ø     Free energy is the energy available for work (e.g. cells have energy to carry out cell processes)

Ø     Cells convert the chemical energy stored in food into other types of energy such as thermal & mechanical

Ø     Energy is used to change matter form one state into another (e.g. liquid into a gas)

Chemical Reactions

Ø     Living things undergo thousands of chemical reactions

Ø     Chemical equations represent chemical reactions

Ø     CO2 + H20—–goes to—–H2CO3  (carbonic acid) is a sample Chemical Reaction in living things

Ø     Reactants are on the left side of the equation, while products are on the right side

Ø Activation energy is required to start many reactions

Ø     Chemical bonds are broken, atoms rearranged, and new bonds form in chemical reaction

Ø     Plants use sunlight to produce sugars such as C6H12O6 glucose; the chemical energy from the sun is stored in the chemical bonds of glucose

Ø      Organisms eat plants, break down the sugars, and release energy along with CO2 & H2O

Ø      Exergonic reactions involve a net release of energy; while endergonic reactions involve a net absorption of energy

Ø      Energy must be added to the reactants for most chemical reactions to occur; called activation energy

Ø      Enzymes are chemical substances in living things that act as catalysts & reduce the amount of activation energy needed

Ø      Organisms contain thousands of different enzymes

Ø      Most enzymes end with –ase (e.g. lipase is the enzyme that acts on lipids)

Reduction-Oxidation (Redox) reactions

Ø     Reactions in which e- are transferred between atoms is a redox or reduction-oxidation reaction (e.g. formation of table salt NaCl)

Ø     In oxidation reactions, a reactant loses 1 or more e- & becomes positively (+) charged (e.g. Sodium atom becomes a Na+ ion)

Ø     In a reduction reaction, a reactant gains 1 or more e- and becomes negatively (-) charged (e.g. Chlorine atom becomes a Cl- ion)

Ø     REDOX reactions always occur together; the electron(s) from the oxidation reaction are then accepted by another substance in the reduction reaction

Solutions

Ø     A large percentage of the mass of organisms is water & many of the chemical reactions of life occur in water

Ø     A solution  is a uniform mixture of one substance in anther

Ø     Solutions may be mixtures of solids, liquids, or gases

Ø     The solute is the substance uniformly dissolved in the solution & may be ions, molecules, or atoms

Ø     The solvent is the substance in which the solute is dissolved

Ø     Water is known as the universal solvent 

Ø     Dissolving one substance in another does not alter their chemical properties

Ø     The concentration of a solution is a measure of the amount of solute dissolved in a given volume of solvent

Ø     Increasing the amount of solute increases the solution’s concentration

Ø     Aqueous solutions are solutions in which water is the solvent; these are important in living things (e.g. blood, cytoplasm of cell…)

Acids and Bases

Ø     The degree of acidity or alkalinity (basic) is important in organisms

Ø     The force of attraction between molecules is so strong that the oxygen atom of one molecule can actually remove the hydrogen from other water molecules; called Dissociation

Ø      H20—–GOES TO—– H+  +  OH-

Ø     OH- called hydroxide ion; H+ called hydrogen ion

Ø     Free H+ ion can react with another water molecule to form H3O+  (hydronium ion)

Ø     Acidity or alkalinity is a measure of the relative amount of H+ and OH- ions dissolved in a solution

Ø     Neutral solutions have an equal number of H+ and OH- ions

Ø     Acids have more H3O+ ions than OH- ions; taste sour; and can be corrosive

Ø     Bases contain more OH- ions than H3O+ ions; taste bitter; & feel slippery  

 

Examples of Common Acids

  • citric acid (from certain fruits and veggies, notably citrus fruits)
  • ascorbic acid (vitamin C, as from certain fruits)
  • vinegar (5% acetic acid)
  • carbonic acid (for carbonation of soft drinks)
  • lactic acid (in buttermilk)
 Examples of Common Bases

  • detergents
  • soap
  • lye (NaOH)
  • household ammonia

PH Scale

Ø     Compares the relative concentration of H3O+ ions and OH- ions

Ø     Scale ranges from 0 to 14; 0-3 is very acidic; 7 is neutral; 11-14 is very basic or alkaline

 

Ø    Litmus paper, phenolphthalein, pH paper, & other indicators that change color can be used to measure pH

Buffers

Ø     Control of pH is important to organisms

Ø     Enzymes function only within a narrow pH range; usually neutral

Ø     Buffers neutral acids or bases in organisms to help control pH

Chemistry Study Guide Chemistry On-line

 

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