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AP Bio: Intro to Statistics & Ch 1-4 Review Name_______________________________

Based on 2012 redesign by the College Board Date ________ Period ____ and on a project designed by S. Phillips

The following assignments are due to the second day of class. They must be HAND written. In addition, there will be a test on the summer assignment that same day. Use youtube for the Bozeman videos.

INTRO TO STATISTICS: (for additional help, see Open Stax, Statistics)

A. Watch the following videos. Take notes in your composition notebook and answer the following

questions directly on this sheet. You must be able to APPLY and/or ANALYZE data on most EVERY

assignment throughout this course based on these principles, concepts and practices:

1. Bozeman- Types of Graphs (*MUST know when to use each type appropriately!)

a. What type of graph uses a ‘best fit’ line?

b. Explain the difference in a bar graph and a histogram.

c. What type of graph shows a change over time?

d. What type of graph displays a correlation of variables?

1. Distinguish between the independent variable and dependent variable and

where they are placed on a graph.

e. Which type of graph is best for comparing 2 or more different groups?

f. Which type of graph is better for showing distribution of data?

g. Explain when a pie graph should be used and give (draw) any example.

h. State at least 5 elements that any graph should always display.

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i. Watch ‘Graphing Data by Spreadsheet’. Bookmark it and take notes in your notebook

for reference. Also, watch ‘Graphing Data by Hand’, if needed.

2. Bozeman- Statistics for Science

a. What is n?

b. What is x (bar)?

c. What is M?

d. What was the range of the sample he gave?

e. Explain ‘Degrees of Freedom’ (with any example) and why the formula is n-1.

3. Bozeman- Standard Deviation

a. What is meant by normal distribution?

b. What does standard deviation (SD) measure?

c. Can 2 sets of data have the same mean but a different SD? Explain.

d. 1 SD means ______% of the population falls within this range; while 2 SD means

_____% falls in this range.

e. Pause the video and calculate the SD from the 2nd set of data given BY HAND. Show

your work.

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3. Bozeman- Standard Error and Kevin Piers Standard Deviation & Standard Error of Mean

a. From Bozeman: Explain the significance of standard error among 2 different sets of

data with different sample sizes that have the same Mean (in terms of precision).

b. From Piers (If you have Boswell, know that he does NOT agree with most of what

Piers says in this video. So just focus on whether or not the Confidence Intervals or SEM

bars overlap and whether that means there is a statistically significant difference

between the means)

1- What do SEM bars that have overlapping Means on a graph indicate?

2- Explain the significance if SEM bars overlap, but the Means do not overlap.

3- Explain the significance if there is no overlap between SEM bars.

c. From Bozeman-As stated earlier, make notes (notebook) for calculating & using Excel.

Use the example he gave and try it yourself!

4. Go to www.Bozemanscience.com/ap-biology/. Watch the videos on AP Biology Practices.

TAKE NOTES in space provided

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*SEE NEXT PAGE FOR PROBLEMS TO SOLVE

D. Solve the following problems IN PENCIL. You must show ALL WORK. Make sure graphs have Titles

and are properly labeled WITH UNITS: (Click here for AP Bio Formulas Sheet)

1. Graph the following sample data set showing the number of leaf disks that rise in a solution

over time as photosynthesis occurs.

2. A- Calculate the mean and standard deviation for the data set of annual monthly rainfall. B- Use the

data to sketch the appropriate type of graph.

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3. Below are 2 samples of data that were collected (*we will ignore Units & Graph Title for this one):

Sample A: 12, 13, 14, 15, 16, 17, 18

Sample B: 10, 15, 20

Calculate the mean for Sample A ________

Calculate the mean for Sample B ________

Are the calculated means sufficient in explaining the data? Why or why not? (*Be specific!)

Calculate:

SD for Sample A _________

SD for Sample B ___________

Explain the significance of the results.

Calculate the Standard Error of Mean for Sample A _______

Calculate the SEM for Sample B _______

Graph your results, showing error bars for each.

Do the bars overlap?

Do the means overlap?

Explain whether or not there are ‘significant’ differences between the 2 populations.

4. A student noticed that the ivy leaves growing on the shady side of a building were larger than ivy

leaves growing on the sunny side of the same building. The student collected and measured the

maximum width, in centimeters, of 30 leaves from each habitat. Use statistical analysis to determine if

it’s likely that there is a significant difference in leaf size between the shady and sunny ivy plants with

95% confidence (±2 SE). Graph the data and indicate error bars. (*see next page)

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Calculated Results (from collected data):

Using the data given and constructed graph, justify the significance between the two samples.

CHAPTERS 1-4 (Note: If you do not have access to a Campbell text book, please use

openstax.org to find your answers to the biology portion. https://openstax.org/details/biology) QUESTIONS: Answers MUST be handwritten, or NO CREDIT GIVEN! Pay attention to what

the prompt asks you to do (ex-describe). Prompt words have been underlined for many questions, below.

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1. Compare and contrast a prokaryotic and eukaryotic cell.

2. Define the term ‘genome’.

3. Distinguish between positive and negative feedback, including an example of each. *Relate these

concepts to homeostasis.

3. Identify the core theme of biology that accounts for the unity and diversity of life.

4. Compare/Contrast the 3 Domains of life.

5. Explain the process of natural selection, including the term adaptation in the response.

6. State what Darwin meant by “descent with modification”?

7. Differentiate: inductive reasoning vs deductive reasoning. Give an example of each.

8. Differentiate: invalid hypothesis vs falsified hypothesis.

9. Do the Review Questions at the end of Sections 1.1 & 1.2.

10. List the 4 elements make up > 95% of living organism.

11. Explain how table salt has emergent properties.

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12. Recall atomic structure, including proton, neutron, electron, mass number and orbital. Describe

what is meant by electrons in an "excited state" vs those in a "ground state", in terms of energy.

13. Define: isotope. Explain two important physical properties of radioactive isotopes that make

them useful in biological research.

14. Compare/contrast: C-12 and C-14.

15. Recall- ionic bond. Given: CaSO4. A- State which is the cation and which is the anion.

B- Describe why this bond is ionic, rather than covalent, in terms of electronegativity.

C- Would this substance disassociate in water? _____ If so, explain WHY and indicate how many

‘particles’ it would disassociate into.

D- If glucose (C6H12O6) was the solute, would it disassociate in water? Explain (and include if

disassociation means the same as solubility).

16. Does a valence e- in Carbon have higher or lower chemical (potential) bond energy than a val e-

of Sulfur?

17. Distinguish between a polar and nonpolar covalent bond. BE SPECIFIC! Give an example of each.

18. Diagram 2 water molecules and indicate the Hydrogen bond(s) with labeled dashed lines.

19. Give an example of any BIOLOGICAL (organic) molecule that forms H bonds with water.

Diagram your example, showing the positive and negative attractions, as were done above.

Predict at least one ‘consequence’ if the bond was either covalent or ionic.

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20. Does a chemical reaction in dynamic equilibrium mean that the concentration of reactants and

products is equal? Explain.

21. Do the Review Questions & Free Response Questions at the end of Section 2.1

22. A- Define what is meant by pH.

B-Describe how the pH scale works (in terms of H+ and OH-)

C- Explain how buffers resist changes in pH (refer to carbonic acid/bicarbonate for an example)

23. Water is essential for life on earth.

A- List at least 5 properties of water.

B- Explain why water is a good solvent (include the terms polar and hydrophilic)

C- Explain how the high surface tension of water affects evaporation.

D- Compare & contrast cohesion and adhesion. Give an example of each as it relates to a living

organism (ex- root uptake of a tree)

E- Explain water in terms of specific heat. Compare with a substance that has a ‘contrasting’

specific heat, such as a metal.

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24. A- Describe an example of how acid precipitation affects life on earth.

B- CO2 is the main product of fossil fuel combustion. Although the majority stays in the

atmosphere, contributing to the greenhouse effect, about 30% is absorbed in the oceans.

Explain what happens when CO2 dissolves in seawater.

25. *Review: Molarity/Concentration from chemistry. You must apply the formula C1V1 = C2V2 (or

M1V1 = M2V2). *Refer to AP Bio Formula Sheet. Given: Your teacher tells you to prepare 0.5L of

1X TAE solution for an electrophoresis experiment, but s/he gives you a bottle of 50X TAE.

Describe the procedure for doing this (*include showing your work, using the equation).

26. Do the Review Questions & Free Response Questions at the end of Section 2.2

27. Why is organic chemistry so important in the study of biology?

30. Why was the Urey-Miller experiment so important? 31. What is unique about carbon that makes it the central atom in the chemistry of life?

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32. Use the diagram below and label the three types of isomers (*both exp from ‘c’ are same type)

33. Be very familiar with the following functional groups, as their properties are most important in the processes of life. Create a table (below or on a separate sheet): after each functional group, draw the structure, name the compound, state an example & note the functional properties of each

a. Hydroxyl

b. Carbonyl- aldehyde

c. Carbonyl- ketone

d. Carboxyl

e. Amino

f. Sulfhydryl

g- Methyl

h. Phosphate

34. Do the Review Question & Free Response Questions at the end of Section 2.3.

35. Define the following:

a. condensation reaction (dehyration synthesis)

b. hydrolysis

36. What is an enzyme?

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37 Complete the chart below:

Monomer Polymer Example Function in your

body

Carbohydrate

Lipid

Protein

Nucleic Acid

38. List 3 monosaccharides with their molecular formulas.

39. Double sugars are called

What makes up maltose?

Sucrose?

Lactose?

40. How does alpha glucose differ from beta glucose and why is that significant to animals?

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41. Describe the STRUCTURE and FUNCTION of the following polysaccharides.

a. starch

b. glycogen

c. cellulose

d. chitin

42 Explain 2 ways that saturated fats are different than unsaturated fats.

43. Draw a phospholipid bilayer.

44. What are 3 different properties that side chains of amino acids have?

45. Sketch 2 amino acids, side by side, joined by a peptide bond. Label all important parts.

46. Describe the 4 levels of protein structure.

a. primary c. tertiary

b. secondary d. quaternary

47. What is DENATURATION?

48. Do the Review Questions at the end of Sections 3.1, 3.2, 3.3, 3.4, & 3.5.

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Module 2: pH Directions: There is not an appropriate video for this section, but the material is covered in the textbook,

pp. 52 – 54 or in the OpenStax Chemistry text(https://openstax.org/details/chemistry) in section “14.2 pH

and pOH”. Also, I suspect that you can find this information online.

NOTE: The pH formula will be provided to you on the AP Exam.

1. Write out each of the two (2) equations for the dissociation of water?

2. Describe how hydronium and hydroxide ions form from water.

3. In pure water, what is the concentration of hydronium ions? Hydroxide ions?

4. What does an acid do when placed into solution?

5. What does a base do when placed into solution?

6. When as acid is added to pure water, what happens to the concentration of hydronium ions relative

to hydroxide ions?

7. When as acid is added to pure water, what happens to the concentration of hydronium ions relative

to hydroxide ions?

8. Since the concentration of hydronium ions and hydroxide ions equal each other, what is the equation

for their product and numerically what is their product?

9. Since pH = - log [H+], what is the pH of pure water?

10. Since pOH = -log [OH-], what is the pOH of water?

11. When pH is less than 7, then what is true about the relative hydrogen ion concentration [H+] and

hydroxide concentration [OH-]?

12. When pH is less than 7, the solution is considered __________

13. When pH is greater than 7, then what is true about the relative hydrogen ion concentration [H+] and

hydroxide concentration [OH-]?

14. When pH is greater than 7, the solution is considered __________

15. Compared to a basic solution at a pH 8, the same volume of an acidic solution at pH of 6 has _________

times as many hydrogen ions (H+)?

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16. Compared to a basic solution at a pH 10, the same volume of an acidic solution at pH of 6 has _________

times as many hydrogen ions (H+)?

17. Compared to acidic solution at a pH 6, the same volume of an acidic solution at pH of 8 has _________

times as many hydronium ions (OH-)?

18. Compared to a basic solution at a pH 9, the same volume of an acidic solution at pH of 6 has _________

times as many hydronium ions (OH-)?

19. Complete the following table:

[H+]

[OH-] pH pOH Acidic, Basic, & Neutral

7

6

10-11

10-9

10

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Module 3: Covalent vs. Ionic Bonding Directions: Watch Bozeman Biology’s: “Chemical Bonds: Covalent vs. Ionic”

(http://www.youtube.com/watch?v=7DjsD7Hcd9U) AND

Crash Course’s: “That’s Why Carbon is A Tramp: Crash Course Biology #1”.

(http://www.youtube.com/watch?v=QnQe0xW_JY4)

(Optional) Dr. Eric Lander’s (MIT Professor) Videos: 1. Lecture 2.2: Molecular Composition of Cells

(https://www.youtube.com/watch?feature=player_embedded&v=Xx3aR4zwqQY)

2. Lecture 2.3: Covalent Bonds

(https://www.youtube.com/watch?feature=player_embedded&v=UfNOcb8eAiI)

2 NOTES:

1. You do not need to understand Lewis Dot Structures for AP Biology, but they are good to know. You will

become intimately familiar with them during your travels through Chemistry-land (it’s like Disneyland in

many ways).

2. Hydrogen bonds will not be considered in this module, they will instead be considered in the IMF module

(which just happens to be the next module, weird – I know).

Without further ado, use the information from the above videos as well as any other information you

gather from the internet or other sources to answer the following questions.

1. What is a chemical bond?

2. What happens to the electrons in a covalent bond?

3. What happens to the electrons in an ionic bond?

4. What is the difference in electron sharing between the two (2) types of covalent bonds?

5. When the electronegativity difference between two elements is basically zero, what does that tell us

about those elements?

6. When the electronegativity difference between two elements is zero, what does that tell us about the

elements? (This is not true for Honors Chemistry; they use a different, and preferable definition, but

this one suits our needs well.)

7. While the information in the Bozeman Biology video is helpful in college, your good friends at the

Cypress Bay Chemistry Teachers Co-op have a slightly different way to determine whether a bond is

polar/nonpolar covalent or ionic, and it is called BrINClSOF.

Each of the elements in that statement: Bromine (Br), Iodine (I), Nitrogen(N), Chlorine (Cl), Sulfur

(S), Oxygen (O), and Fluorine (F) are rather special for this method. Polar bonds ONLY form between

one member of BrINClSOF and one NON-member. Nonpolar bond – Two(2) BrINClSOFs OR Two (2)

non-BrINClSOFs Ionic bond – one metal and one nonmetal. However, you may not know which

elements are metals. So your rule-of-thumb is if two elements are on opposite sides of the periodic

table, then they form an ionic bond, easy. But I have even better news for you: except for protein

structure you will likely not encounter any ionic bonds in any meaningful form throughout AP Bio.

So let’s now do some practice in determining whether it is an ionic, nonpolar covalent, or polar

covalent bond. (ON THE NEXT PAGE)

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8.

Bond Type of Bond Why do you think this?

O – H

C – O

C – H

C – N

C – C

N – H

O – O

P – O

S – H

S – S

Na+ Cl-

9. Given what you know about ionic bonds, polar covalent bonds, and nonpolar covalent bonds, which

type of bond do you think is the most common in the world of Chemistry? Provide justification for

your answer.

10. Which is a stronger bond: ionic or covalent? Provide a justification for your answer.

11. Given your answer to the above question, you may be surprised to learn that the strongest bond in

biological systems is the polar covalent bond as biological systems are largely aqueous in nature.

Using the Internet and your knowledge of chemical bonds, describe your reasoning for why polar

covalent bonds are stronger than ionic bonds in biological systems.

12. How does a double (covalent) bond differ from a single (covalent) bond?

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13. Fill out the table below

14. There is a difference between polar bonds and polar molecules, and it is not truly relevant to

us. Indeed, whether a molecule is polar will be communicated to you, but you can assume a

biological molecule is polar unless told otherwise. However, the following is good to know:

a) If a molecule ONLY consists of nonpolar bonds, then it is a nonpolar molecule.

b) If a molecule consists of polar bonds, it is highly likely to be polar,

EXCEPT hydrocarbons (molecules that only contain hydrogen and carbon).

So let’s use this information to determine the polarity of some molecules

Molecule Polarity Justification O2

NH3

PO4

CH4

C2H6

CO2

Nonpolar (refer to line 3 of

the instructions)

No response is required for this one.

C6H12O6

DNA

You will have to look this one up on the Internet.

(Glycine) Amino Acid

You will have to look this one up on the Internet. This question will NOT count against you if

incorrect.

Property Single Bond Double Bond Triple Bond

Number of electrons involved in the bond

Relative Distance

between atoms

Relative Strength

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The questions #15 – 19 draw on information directly obtained from: “That’s Why Carbon is A Tramp: Crash

Course Biology #1”. (http://www.youtube.com/watch?v=QnQe0xW_JY4)

15. What one element is life based upon?

16. According to Hank, what are the 4 elements that commonly bond with carbon?

17. Use the video by They Might Be Giants: “Meet the Elements”

(http://www.youtube.com/watch?v=Uy0m7jnyv6U ) to answer the following question in the

table below. What are the 4 elements that comprise that vast majority of biological organisms,

ordered from largest (by total mass) to smallest? Also list the percentage of elements in an

animal by mole fraction as well (Dr. Lander gives you this OR you can find it on the Internet).

Element Percentage by Mass

Percentage by Mole Fraction

18. What explains the dramatic discrepancy between these two measures for oxygen and

hydrogen? (Hint: “Mole Fraction” basically is the number of atoms.)

19. Describe three (3) reasons why Hank considers carbon to be “a bit of a tramp”?

20. How many electrons does carbon need to have in its outer electron shell to be happy? How

many does it possess when it is by itself?

21. Which of the following results from a transfer of electron(s) between atoms?

a) nonpolar covalent bond b) polar covalent bond c) ionic bond

d) hydrogen bond e) hydrophobic interaction

22. Which of the following explains most specifically the attraction of water molecules to one

another?

a) nonpolar covalent bond b) polar covalent bond c) ionic bond

d) hydrogen bond e) hydrophobic interaction

23. The molecule shown here could be described in chemical symbols as (select ALL that are

correct). A) CH4 B) H2O C) C2H3 D) C4H4 E) CH2O

24. The molecule shown here is the simplest of organic compounds. It is called A) A carbohydrate. B) Carbon dioxide. C) Methane. D) Carbonic hydrate. E) Methyl carbonate.

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Module 4: Intermolecular Forces (IMFs) Directions: Watch Dr. Eric Lander’s: “NON-Covalent Bonds”

(https://www.youtube.com/watch?feature=player_embedded&v=bMd67kgm_gI )

AND Rob’s Deep Dive: “Intermolecular Bonding”

(https://www.youtube.com/watch?feature=player_embedded&v=yFq4EieGWF0)

READ THIS BEFORE YOU WATCH THESE VIDEOS: These videos are by a group from MIT. If the

molecules used as examples seem advanced for this stage, you are correct. Don’t freak out on me, just

listen to him and learn.

1. Fill out the table below about the four (4) IMFs discussed in the video.

Force or Bond

Relative Strength

Use “Strong” or “Weak”

Description

2. Covalent and ionic bonds (and a few other type of bonds are called intramolecular forces, but now

we are looking at intermolecular forces. Based on their names alone what do you think is the

difference between these two forces (bonds)?

3. Give one example of an intramolecular force, and one example of an intermolecular force for the

same substance or molecule. (ensure that you give the correct term for both the intramolecular force

as well as the intermolecular force.)

4. Hydrogen bonds (5 Kcal/mole) are really weak compared to covalent bonds (80 Kcal/mole), so how

do they become significant chemical forces?

5. Now you can provide a far richer explanation of surface tension. When a bug “walks” on water what

actual chemical structure is it walking upon?

6. Why is the gecko able to climb up glass and even hang upside down (not that dumbass one from the

online insurance company)?

7. Covalent bonds are approximately ________ times stronger than hydrogen bonds, and hydrogen bonds

are approximately ________ times stronger than van der Waals forces. (Your answer should come out

to an integer for each one.)

8. Each water molecule can hydrogen bond to _____ other water molecules.

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9. What allows sucrose to dissolve in water?

10. What prevents oil from dissolving in water?

11. What does it now mean for something to be hydrophilic? (Your answer will be in terms of molecules

of water and of the substance trying to dissolve)

12. What does it now mean for something to be hydrophobic? (Your answer will be in terms of molecules

of water and of the substance trying to dissolve)

13. In Chemistry, when determining the answer to the question: “will it dissolve?” the answer typically

appeals to the aphorism: “like dissolves like” as it pertains to polarity of the substances. Accordingly,

what type of molecules will dissolve in polar substances?

14. Similarly, what types of molecules will dissolve in nonpolar substances?

15. What is the hydrophobic effect?

16. Briefly describe how the hydrophobic effect might enable the plasma (cell) membrane to do its job?

17. Indicate which of the following molecules will feature Van der Waal forces (Select ALL that have Van

der Waal forces present – assume that ALL molecules are close enough for the forces to form):

a) H2O b) O2 c) NH3 d) CO2 e) C4H10

18. Using your knowledge of intermolecular forces (IMFs), place a check in each box if the molecule has

the indicated IMF, and then shade in the box for the strongest IMF each molecule possesses.

Molecule Ionic Bonds Hydrogen Bond Hydrophobic Effect

Van der Waals

Water

Fructose (sugar)

Glycine

(amine and carboxyl group)

Olive oil

(hydrocarbon)