AP Biology Summer Assignment 14-15

8/10/2019 AP Biology Summer Assignment 14-15

http://slidepdf.com/reader/full/ap-biology-summer-assignment-14-15 1/27

AP Biology 2014-2015

Summer Assignment

Mrs. Pamela Griffin

[email protected]

!"y is t"ere a summer assignment#The first topics of the year are chemistry and biochemistry. If you are a junior or senior, you were taught the majority of

this content in chemistry and biology. If you are a sophomore, then you may have learned some of these concepts inmiddle school. The goal of the summer assignment is to review and/or learn these concepts prior to the first week of

school.

Reviewing this material over the summer will:

. !llow us to spend more time on the content with which students are less familiar and did not e"perience in

introductory biology.

#. Re$uire you to practice reading and interpreting the te"tbook.

%. !llow you to become familiar with the difficulty and design of !& 'iology tests.

!"en is t"e summer assignment $ue#The summer assignment is due the first $ay of school, (eptember #, #)*. %o late &or &ill 'e a((epte$.

!"at is t"e a(tual assignment#The summer assignment covers chapters #+ of the te"t and consists of learning objectives, review assignments, and practice tests.

-or hapters #+:

. )evie& the attached objectives. These are %*+ $uestions for you to answer, but you should use these to guide

your reading and use them as a checklist for self assessment.

#. )ea$ each chapter thoroughly.

%. )evie& the key terms for each chapter.

a. It is recommended that you review the terms and their definitions. There is %* specific assignment for

the terms this summer. Recommended formats to learn the terms:

i. -lash cards using colored paper/markers and adding pictures or diagrams to your cards can behelpful0

ii. Two columns place concepts on one side and definitions on the other so that the page can be

folded over for self $ui11ing.0

iii. reate practice matching tests for the vocabulary words break the lists into groups of +2 termsat once and make sure to answer the tests as well0

*. ,omplete the attached assignments specific to each chapter.

. ,omplete the attached practice tests you will write on the tests but make sure to also bubble in the scantron

sheets provided 3 make certain each scantron is labeled correctly with the test name0.

44 The te"tbook covers greater detail than is necessary for you to know at this point. Therefore it is important for you to

focus mainly on the objectives and vocabulary specified by the summer assignment.

ust to $ou'le ("e( &"en is t"e summer assignment $ue#

The summer assignment is due the first $ay of school, (eptember #, #)*. %o late &or &ill 'e a((epte$.

,an / get "elp over t"e summer if / $o not un$erstan$ some of t"e material#I can be contacted through email which I will check appro"imately once a week: pgriffin5spotsylvania.k#.va.us

mailto:[email protected]

mailto:[email protected]



,AP+) 2 +"e ,"emi(al ,onte3t of ife

Learning Objectiveslements an$ ,ompoun$s

. 6istinguish between an element and a compound.

#. Identify the four elements that make up 789 of living matter.

%. 6efine the term tra(e element and give an e"ample.Atoms an$ Mole(ules

*. 6raw and label a simplified model of an atom.

. 6istinguish between each of the following pairs of terms:

a. neutron and proton

b. atomic number and mass number 8. "plain how the atomic number and mass number of an atom can be used to determine the number of neutrons.

2. "plain how two isotopes of an element are similar. "plain how they are different.

;. 6escribe two biological applications that use radioactive isotopes.

7. 6efine the terms energy and potential energy. "plain why electrons in the first electron shell have less potential energythan electrons in higher electron shells.

). 6istinguish among nonpolar covalent, polar covalent and ionic bonds.

. "plain why strong covalent bonds and weak bonds are both essential in living organisms.#. 6istinguish between hydrogen bonds and van der <aals interactions.

%. =ive an e"ample that illustrates how a molecule>s shape can determine its biological function.

*. "plain what is meant by a chemical e$uilibrium.

,ommon Stu$ent Mis(on(eptions

. The simplified models of the atom -igure #.*0, electron shells -igure #.;0, and covalent bonding -igure #.0 can confuse

students who take them too literally. It is important to make sure that you understand that:

• !toms do not have defined surfaces.

• lectrons do not travel in planetary orbits around the nucleus of the atom.

• (hared electron pairs are not paired spatially in covalent bonds.

• lectron shells represent energy levels rather than the position of electrons.

#. (tudents have difficulty fully grasping the concept of energy, and especially the concept of potential energy. &otential energy

can be misunderstood as a substance or fuel that is somehow stored in matter. ?nderstand that potential energy is associated

with an object>s ability to move to a lower+energy state, thus releasing some of the potential energy. Return to the concept of potential energy in discussing electron shells, understand that electrons in different electron shells differ in potential energy

rather than in position.

%. (tudents should recogni1e that weak bonds play important roles in the chemistry of life, despite the transient nature of eachindividual bond. &age *# gives the e"ample of the gecko, able to walk on ceilings because of the van der <aals interactions

between the ceiling and the hairs on the gecko>s toes. @now that strong and weak bonds are both important in the chemistry

of life, and be able to provide e"amples illustrating this.

Stems

an- A not anion: a negatively charged ion0

(o- A togetherB -valent A strength covalent bond: an attraction between atoms that share one or more pairs of outer+shell electrons0

ele(tro- A electricity electronegativity: the tendency for an atom to pull electrons towards itself0

iso- A e$ual isotope: an element having the same number of protons and electrons but a different number of neutrons0

neutr- A neither neutron: a subatomic particle with a neutral electrical charge0

pro- A before proton: a subatomic particle with a single positive electrical charge0



ey +erms for ,"apter 2

anion

atom

atomic mass

atomic nucleus

atomic number

cationchemical bond

chemical e$uilibrium

chemical reaction

compound

covalent bond

dalton

electron

electron shell

electronegativity

elementenergy

energy level

hydrogen bond

ion

ionic bond

ionic compound

isotope

mass number

matter

molecular formula

molecule

neutron

nonpolar covalent bond

orbital

periodic table of theelements

polar covalent bond

potential energy

product

proton

radioactive isotopereactant

salt

structural formula

trace element

valence

valence electron

valence shell

van der <aals interactions



Chapter 2 Worksheet

1. Fill out the following chart for the major subatomic particles of an atom.

Particle

Charge Mass Location

Proton

Neutron

Electron

2. Distinguish between valence # and valence electrons. Also, explain the concept of theoctet rule in relation to valence electrons.

. Diagram each of the following atoms!

Atom# o

Protons

# o Neutro

ns

# o Electro

ns

!alence #

"iagram

Carbon

"



$%rogen

O&$gen

Nitrogen

". Distinguish between the following bonds!

Covalent 'onic $%rogen

polar covalent!

nonpolar covalent!



,". 2 ,"emi(al ,onte3t of ife Pra(ti(e +est

. !bout # of the 7# natural elements are known to be

essential to life. <hich four of these # elements make upappro"imately 789 of living matterC

a. carbon, sodium, chlorine, nitrogen

b. carbon, sulfur, phosphorus, hydrogen

c. o"ygen, hydrogen, calcium, sodiumd. carbon, hydrogen, nitrogen, o"ygen

e. carbon, o"ygen, sulfur, calcium

#. Trace elements are those re$uired by an organism inonly minute $uantities. <hich of the following is a trace

element that is re$uired by humans and other vertebratesC

a. nitrogen

b. calcium

c. iodined. sodium

e. phosphorus

%. <hat is the appro"imate atomic mass of an atom with

8 neutrons, protons, and electronsC

a. daltons

b. 8 daltonsc. %) daltons

d. % daltons

e. *8 daltons

*. D"ygen has an atomic number of ; and a mass

number of 8. Thus, the atomic mass of an o"ygen atom isa. e"actly ; grams.

b. e"actly ; daltons.c. appro"imately 8 grams.

d. appro"imately 8 daltons.

e. #* amu atomic mass units0.

. alcium has an atomic number of #) and an atomic

mass of *). Therefore, a calcium atom must have

a. #) protons.

b. *) electrons.

c. *) neutrons.

d. ! and ' onlye. !, ', and

8. 6ifferent atomic forms of an element contain the

same number of protons but a different number of neutrons.<hat are these different atomic forms calledC

a. ions

b. isotopes

c. neutronic atomsd. isomers

e. radioactive atoms

2. Dne difference between carbon+# and

carbon+* is that carbon+* has

a. two more protons than carbon+#.

b. two more electrons than carbon+#.

c. two more neutrons than carbon+#.d. ! and only

e. ' and only

;. lectrons e"ist only at fi"ed levels of potentialenergy. Eowever, if an atom absorbs sufficient energy, a

possible result is that

a. an electron may move to an electron shell farther out from

the nucleus. b. an electron may move to an electron shell closer to the

nucleus.

c. the atom may become a radioactive isotope.

d. the atom would become a positively charged ion, or cation

$



e. the atom would become a negatively charged ion, or anion.

Use the figure below to answer the following questions.

7. <hich drawing depicts the electron configuration of

o"ygen D0C

). <hich drawing depicts the electron configuration of

nitrogen F0C

. <hich drawing is of an atom with the atomic number of 8C

#. <hich drawing depicts an atom that is inert or

chemically unreactiveC

%. <hat does the reactivity of an atom depend onC

a. number of valence shells in the atom

b. number of orbitals found in the atomc. number of electrons in each orbital in the atom

d. presence of unpaired electrons in the outer valence shell of the

atom

e. presence of hybridi1ed orbitals in the atom

*. <hat are the chemical properties of atoms whose

valence shells are filled with electronsC

a. They form ionic bonds in a$ueous solutions. b. They form covalent bonds in a$ueous solutions.

c. They are stable and chemically unreactive or inert.

d. They e"hibit similar chemical behaviors.

e. and 6 only

Use the information extracted from the periodic table in the

figure below to answer the following questions.

. Eow many electrons does nitrogen have in itsvalence shellC

8. 'ased on electron configuration, which of these

elements would e"hibit chemical behavior most like that of

o"ygenCa. carbon

b. hydrogen

c. nitrogen

d. sulfur

e. phosphorus

Use the figure below to answer the following questions. .

2. <hat results from the chemical reactionC

a. a cation with a net charge of G

b. a cation with a net charge of +c. an anion with a net charge of G

d. an anion with a net charge of +

e. ! and 6

;. <hat is the difference between covalent bonds and

ionic bondsC

a. ovalent bonds involve the sharing of protons between

atoms, and ionic bonds involve the sharing of electrons between atoms.

b. ovalent bonds involve the sharing of neutrons between

atoms, and ionic bonds involve the sharing of electrons between atoms.

c. ovalent bonds involve the sharing of electrons between

atoms, and ionic bonds involve the electrical attraction

between atoms.d. ovalent bonds involve the sharing of protons between

atoms, and ionic bonds involve the sharing of neutrons

between atoms.

e. ovalent bonds involve the transfer of electrons betweenatoms, and ionic bonds involve the sharing of neutrons

between atoms.

7. <hich of the following is not considered to be aweak molecular interactionC

a. a covalent bond

b. a van der <aals interaction

c. an ionic bond in the presence of water d. a hydrogen bond

e. ! and ' only

#). <hich of the following describes any reaction thathas attained chemical e$uilibriumC

a. The concentration of the reactants e$uals the concentratio

the products.

b. The rate of the forward reaction is e$ual to the rate of thereverse reaction.

c. !ll of the reactants have been converted to the products o

reaction.

d. !ll of the products have been converted to the reactants oreaction.

e. 'oth the forward and the reverse reactions have stopped w

no net effect on the concentration of the reactants and the

products.

%



,". 6 !ater an$ t"e 7itness of ife*'8e(tives

+"e Properties of !ater

1. <ith the use of a diagram or diagrams, e"plain why water molecules are:a. polar

b. capable of hydrogen bonding with four neighboring water molecules

2. Hist four characteristics of water that are emergent properties resulting from hydrogen bonding.6. 6efine (o"esion and a$"esion. "plain how water>s cohesion and adhesion contribute to the movement of water from the

roots to the leaves of a tree.4. 6istinguish between heat and temperature, using e"amples to clarify your definitions.5. "plain the following observations by referring to the properties of water:

• oastal areas have milder climates than adjacent inland areas.

• Dcean temperatures fluctuate much less than air temperatures on land.

• Insects like water striders can walk on the surface of a pond without breaking the surface.

• If you slightly overfill a water glass, the water will form a conve" surface above the top of the glass.

• If you place a paper towel so that it touches spilled water, the towel will draw in the water.

• Ice floats on water.

• Eumans sweat and dogs pant to cool themselves on hot days.

9. 6istinguish among a solute, a solvent, and a solution.:. 6istinguish between hydrophobic and hydrophilic substances.

+"e ;isso(iation of !ater Mole(ules

<. Fame the products of the dissociation of water and give their concentration in pure water.=. 6efine a(i$ 'ase and p.

10. "plain how acids and bases may directly or indirectly alter the hydrogen ion concentration of a solution.11. ?sing the bicarbonate buffer system of human blood as an e"ample, e"plain how buffers work.12. 'riefly e"plain the causes and effects of acid precipitation.

Stu$ent Mis(on(eptions

. To understand the emergent properties of water and the importance of these properties to living things, you must fully

understand the structure of water and its ability to form hydrogen bonds with neighboring molecules.

#. (ome students think that water forms hydrogen bonds only in the li$uid state. Recogni1e that fro1en water molecules form a

crystalline lattice, with each water molecule forming four hydrogen bondsB E+bonds form in solid states of matter as well.%. Recall the difference between physical and chemical changes. !n ability to distinguish between these is important in

understanding many of the key properties of water, such as its role as a solute and its dissociation to form hydro"ide and

hydronium ions.*. any students do not fully understand the e"change of protons between water molecules. !n appreciation of water>s

dissociation to form hydro"ide and hydronium ions is crucial to understanding acid+base relationships, the effects of e"cess

DE+ and E%DG ions in solution, and the role of buffers.

Stems

-"y$ro - waterB

&



-p"ilos + lovingB

-p"o'os +fearing hydrophilic: having an affinity for waterB hydrophobic: having an aversion to water0-ilo - a thousand kilocalorie: a thousand calories0

ey +erms

acid

acid precipitation

adhesion

a$ueous solution

base

buffer

calorie cal0

elsius scale

cohesion

evaporative cooling

heat

heat of vapori1ation

hydration shell

hydrogen ion

hydrophilichydrophobic

hydro"ide ion

joule J0

kilocalorie kcal0

kinetic energy

molarity

mole mol0

pE

polar molecule

solutesolution

solvent

specific heat

surface tension

temperature

'



(hapter 1. (omplete the following chart for the properties of water.

Propert$ E&planation o Propert$ E&ample o (ene)t to Lie

)*drogen bonds holdmolecules together and

adhere them to h*drophilicsurfaces

)igh +pecic)eat

-emperature changes inenvironment and organismsare moderated

)*drogen bonds must bebroen for water toevaporate

/ater molecules with highinetic energ* evaporate0

remaining molecules arecooler

ce oats

3ost chemical reactions in lifeinvolve solute dissolved inwater



2. Draw a collection of ve 45 water molecules and label the diagram with the followingterms! h*drogen, ox*gen, polar covalent bond, and h*drogen bond.

. (omplete the following table on p) 4the rst one is completed as an example5.

*+, *O-, PAci%ic. basic.or neutral/

01-2 01-02 2 aci%ic

01 00 3

01-4 4

01-02

01-5

". 6xplain how the bicarbonate bu7er s*stem wors to regulate the p) of human blood.

. Describe the causes and e7ects of acid precipitation.

," 6. !ater an$ t"e 7itness of ife Pra(ti(e +est



. The slight negative charge at one end of one water

molecule is attracted to the slight positive charge of another

water molecule. <hat is this attraction calledCa. a covalent bond

b. a hydrogen bond

c. an ionic bond

d. a hydrophilic bond

e. a hydrophobic bond

#. <ater is able to form hydrogen bonds because

a. o"ygen has a valence of #. b. the water molecule is shaped like a tetrahedron.

c. the bonds that hold together the atoms in a water molecule

are polar covalent bonds.d. the o"ygen atom in a water molecule has a weak positive

charge.

e. each of the hydrogen atoms in a water molecule is weakly

negative in charge.

%. <hat do cohesion, surface tension, and adhesion

have in common with reference to waterC

a. !ll increase when temperature increases. b. !ll are produced by ionic bonding.

c. !ll are properties related to hydrogen bonding.

d. !ll have to do with nonpolar covalent bonds.

e. and 6 only

*. <hich of the following is possible due to the high

surface tension of waterC

a. Hakes donKt free1e solid in winter, despite low temperatures. b. ! water strider can walk across the surface of a small pond.

c. Drganisms resist temperature changes, although they give off

heat due to chemical reactions.

d. <ater can act as a solvent.

e. The pE of water remains e"actly neutral.

. <aterKs high specific heat is mainly a conse$uence of

thea. small si1e of the water molecules.

b. high specific heat of o"ygen and hydrogen atoms.

c. absorption and release of heat when hydrogen bonds break

and form.d. fact that water is a poor heat conductor.

e. inability of water to dissipate heat into dry air.

8. <hich bonds must be broken for water to vapori1eCa. ionic bonds

b. nonpolar covalent bondsc. polar covalent bonds

d. hydrogen bondse. covalent bonds

2. 6esert rabbits are adapted to the warm climate because their large ears aid in the removal of heat due to the

a. high surface tension of water.

b. high heat of vapori1ation of water.

c. high specific heat of water.d. buffering capacity of water.

e. dissociation of water molecules.

;. !t what temperature is water at its densestC

a. )L

b. *Lc. %#L

d. ))L

e. ##L

7. <hy does ice float in li$uid waterC

a. The li$uid water molecules have more kinetic energy and support the ice.

b. The ionic bonds between the molecules in ice prevent the

from sinking.

c. Ice always has air bubbles that keep it afloat.d. Eydrogen bonds stabili1e and keep the molecules of ice

farther apart than the water molecules of li$uid water.

e. The crystalline lattice of ice causes it to be denser than li$

water.

The picture below illustrates a solute molecule surrounded by

a hydration shell of water. Use it to answer the following

question.

). 'ased on your knowledge of the polarity of water

molecules, the solute molecule is most likely

a. positively charged. b. negatively charged.

c. without charge.

d. hydrophobic.

e. nonpolar.

. <hich of the following solutions has the greatest

concentration of hydrogen ions MEGNCa. gastric juice at pE #

b. vinegar at pE %

c. tomato juice at pE *

d. black coffee at pE

e. household bleach at pE #

#. <hich of the following solutions has the greatest

concentration of hydro"ide ions MDE+NC

a. lemon juice at pE # b. vinegar at pE %



," 4 ,ar'on an$ t"e Mole(ular ;iversity of ife*'8e(tives

+"e /mportan(e of ,ar'on

. "plain how carbon>s electron configuration accounts for its ability to form large, comple", and diverse organic molecules.

#. 6escribe how carbon skeletons may vary, and e"plain how this variation contributes to the diversity and comple"ity of organic

molecules.

%. 6escribe the basic structure of a hydrocarbon and e"plain why these molecules are hydrophobic.

7un(tional Groups

*. Fame the major functional groups found in organic molecules. 6escribe the basic structure of each functional group and outline

the chemical properties of the organic molecules in which they occur.

Stems

(ar'- coal carboxyl group: a functional group present in organic acids, consisting of a carbon atom double+bonded to an o"ygen

atom and a hydro"yl group0

"y$ro- water hydrocarbon: an organic molecule consisting only of carbon and hydrogen0

iso- e$ual isomer: one of several organic compounds with the same molecular formula but different structures and, therefore,

different properties0

sulf- sulfur sulfhydryl group: a functional group that consists of a sulfur atom bonded to an atom of hydrogen0

t"io- sulfur thiol: organic compounds containing sulfhydryl groups0

ey +erms

adenosine triphosphate !T&0

amino group

carbonyl group

carbo"yl group

functional group

hydrocarbon

hydro"yl group

organic chemistry

phosphate group

sulfhydryl group



(hapter " /orsheet1. Describe the structure of carbon atoms and explain wh* the* are able to function as

8bacbones9 for some man* di7erent molecules.

2. Fill in the following table on the functional groups.

6unctional7roup

Molecular6ormula 89tructural6ormula

Names an% characteristics o organic compoun%s containing the

group:

-O

Aldeh*de or etone0 polar group, watersoluble, often found in sugars4carboh*drates5

(arbox*l

-N2

-hiols0 cross:lins stabili;e proteinstructure, often 8smell*9 compounds



<hosphate

," 4 ,ar'on an$ t"e Mole(ular ;iversity of ife Pra(ti(e +est

. Drganic chemistry is a science based on the study of

a. functional groups.

b. vital forces interacting with matter.c. carbon compounds.

d. water and its interaction with other kinds of

molecules.

e. inorganic compounds.

#. <hich property of the carbon atom gives it

compatibility with a greater number of different elements than

any other type of atomCa. arbon has 8 to ; neutrons.

b. arbon has a valence of *.

c. arbon forms ionic bonds.d. ! and onlye. !, ', and

%. <hat types0 of bonds0 does carbon have a tendency

to formCa. ionic

b. hydrogen

c. covalent

d. ! and ' onlye. !, ', and

*. <hat is the reason why hydrocarbons are not soluble

in waterCa. The majority of their bonds are polar covalent carbon to

hydrogen linkages.

b. The majority of their bonds are nonpolar covalent carbon+to+

hydrogen linkages.c. They are hydrophilic.

d. They e"hibit considerable molecular comple"ity and diversity.

e. They are lighter than water.

Use the figure below to answer the following questions.

. <hich is a hydro"yl functional groupC

8. <hich is an amino functional groupC

2. <hich is a carbonyl functional groupC

;. <hich is a functional group that helps stabili1e

proteins by forming covalent cross+links within or between

protein moleculesC

7. <hich is a carbo"yl functional groupC

). <hich is an acidic functional group that candissociate and release EG into a solutionC

. <hich is a basic functional group that can accept EG

and become positively chargedC

Use the molecules shown in the figure below to answer the

following questions.

#. <hich molecule is water+soluble because it has ahydro"yl functional groupC

%. <hich molecule is an alcoholC

*. <hich molecules contain a carbonyl groupC

. <hich molecule has a carbonyl functional group in

the form of a ketoneC

8. <hich molecule has a carbonyl functional group in

the form of an aldehydeC

2. <hich molecule contains a carbo"yl groupC

;. <hich molecule can increase the concentration of

hydrogen ions in a solution and is therefore an organic acidC

Use the molecules shown in the figure below to answer the

following questions..



7. <hich molecule functions to transfer energy between

organic moleculesC

#). <hich molecule contains an amino functional group,

but is not an amino acidC

,". 5 +"e Stru(ture an$ 7un(tion of Ma(romole(ules

*'8e(tives

+"e Prin(iples of Polymers

. Hist the four major classes of macromolecules.

#. 6istinguish between monomers and polymers.

%. 6raw diagrams to illustrate condensation and hydrolysis reactions.

,ar'o"y$rates Serve as 7uel an$ Buil$ing Material *. 6istinguish among monosaccharides, disaccharides, and polysaccharides.

. Identify the elements that compose carbohydrates.

8. Identify e"amples of carbohydrates and describe their functions.

2. 6escribe the role of symbiosis in cellulose digestion.

ipi$s Are a ;iverse Group of y$rop"o'i( Mole(ules

;. 6escribe the building+block molecules, structure, and biological importance of fats, phospholipids, and steroids.

7. Identify the elements that compose lipids.

). 6istinguish between saturated and unsaturated fats.

. Identify e"amples of lipids and describe their functions.

Proteins ave Many Stru(tures an$ Many 7un(tions

#. 6istinguish between a protein and a polypeptide.

%. "plain how a peptide bond forms between two amino acids.

*. Hist and describe the four major components of an amino acid. "plain how amino acids may be grouped according to the physical and chemical properties of the R group.

. "plain what determines protein conformation and why it is important.

8. "plain how the primary structure of a protein is determined.

2. Fame two types of secondary protein structure. "plain the role of hydrogen bonds in maintaining secondary structure.

;. "plain how weak interactions and disulfide bridges contribute to tertiary protein structure.

7. Hist four conditions under which proteins may be denatured.

%u(lei( A(i$s Store an$ +ransmit ere$itary /nformation#). Hist the major components of a nucleotide, and describe how these monomers are linked to form a nucleic acid.

#. 6istinguish between:

a. pyrimidine and purine

b. nucleotide and nucleoside

c. ribose and deo"yribose

d. > end and %> end of a nucleotide

##. 'riefly describe the three+dimensional structure of 6F!.

Stu$ent Mis(on(eption



. (tudents may think that two+dimensional representations of organic molecules are accurate. These molecules are less

static than you imagine. onveniently drawn as linear, monosaccharides usually form rings in a$ueous solutions. There

may be considerable rotation around single bonds within organic molecules, unless their conformation is stabili1ed by

interactions between regions of the molecule. ?nderstand that #6 drawings of organic molecules are convenient butgreatly oversimplified representations of molecular structure.

#. (tudents may not reali1e that every protein has primary, secondary, and tertiary structures and may think that any

particular protein is characteri1ed only by one level of structure. ach level contributes to protein conformation.

%. The majority of students have difficulty visuali1ing the different levels of protein structure and the interaction of the

regions of the protein molecule. To fully understand levels of protein structure, you must be able to mentally constructthree+dimensional images of proteins. This can be very challenging. Try to construct your own %+6 models or look at

models online.

*. (tudents tend to define nucleic acids by the most familiar e"amples, 6F! and RF!, rather than understanding thestructure of nucleotide monomers. This causes confusion when students encounter important molecules such as !T& and

c!& and fail to recogni1e them as nucleotides. Take the time to understand the monomers 3 building blocks+ of nucleic

acids

Stems

(on- together condensation reaction: a reaction in which two molecules become covalently bonded to each other through the loss of

a small molecule, usually water0$i- two disaccharide: two monosaccharides joined together0gly(o- sweet glycogen: a polysaccharide sugar used to store energy in animals0

"y$ro- waterB -lyse break hydrolysis: breaking chemical bonds by adding water0ma(ro- large macromolecule: a large molecule0meros- part polymer: a chain made from smaller organic molecules0mono- singleB -sa(("ar sugar monosaccharide: simplest type of sugar0poly- many polysaccharide: many monosaccharides joined together0tri- three triacylglycerol: three fatty acids linked to one glycerol molecule0

ey +erms

alpha O0 heli"

amino acid

antiparallel

beta P0 pleated sheet

carbohydrate

catalyst

cellulose

chaperonin

chitin

cholesterol

condensation reaction

dehydration reaction

denaturation

deo"yribonucleic acid 6F!0

deo"yribosedisaccharide

disulfide bridge

double heli"

en1yme

fat

fatty acid

gene

glycogen

glycosidic linkage

hydrolysis

hydrophobic interaction

lipid

macromolecule

monomer

monosaccharide

nucleic acid

nucleotide

peptide bond

phospholipid

polymer

polynucleotide

polypeptide

polysaccharide primary structure

protein

purine

pyrimidine

$uaternary structure

ribonucleic acid RF!0

ribose

saturated fatty acid

secondary structure

starch

steroid

tertiary structure

triacylglycerol

unsaturated fatty acid

Q+ray crystallography



Ch ; Macromolecules Worksheet6or each o the macromolecules belo<= list the major unctions. list an% %escribe >or %ra<? thmonomers an% pol$mers:

Macromolecule

List o Major6unctions

Monomers orcommonsubunits

9tructure o subunits

CommonPol$mers or

large molecules

9tructure o Pol$mers

Carboh$%rates

C==O0=2=0

Lipi%s

C. . O

Nucleic

Aci%s

C. . O. N.P



(hapter " and Applications!=elow are structural formulas for several organic molecules. For each one, circle andlabel each functional group present and identif* the molecule as a carboh*drate, lipid,nucleic acid or protein.

E@AMPLE

POBE'N

carbo&$l

carbon$l

h$%ro

&$l

amino



," 5 +"e Stru(ture an$ 7un(tion of Ma(romole(ules Pra(ti(e +est

. <hich of the following is not one of the four major groups

of macromolecules found in living organismsCa. glucose

b. carbohydrates

c. lipids

d. proteinse. nucleic acids

#. &olymers of polysaccharides, fats, and proteins are all

synthesi1ed from monomers by which processCa. connecting monosaccharides together condensation

reactions0

b. the addition of water to each monomer hydrolysis0

c. the removal of water dehydration reactions0d. ionic bonding of the monomers

e. the formation of disulfide bridges between monomers

%. <hich of the following best summari1es the relationship between dehydration reactions and hydrolysisC

a. 6ehydration reactions assemble polymers, and hydrolysis

breaks down polymers. b. Eydrolysis only occurs in the urinary system, and

dehydration reactions only occur in the digestive tract.

c. 6ehydration reactions can occur only after hydrolysis.

d. Eydrolysis creates monomers, and dehydration reactions

break down polymers.e. ! and are correct.

*. ! molecule with the chemical formula 8E%#D8 is

probably aa. carbohydrate.

b. lipid.

c. protein.

d. nucleic acid.e. hydrocarbon.

. If #; molecules of the general type shown in the figure

below were covalently joined together in se$uence, thesingle molecule that would result would be a

a. polysaccharide.

b. polypeptide.c. polyunsaturated lipid.

d. monosaccharide.

e. disaccharide.

8. Hactose, a sugar in milk, is composed of one glucose

molecule joined by a glycosidic linkage to one galactose

molecule. Eow is lactose classifiedC

a. as a pentose

b. as a he"osec. as a monosaccharide

d. as a disaccharide

e. as a polysaccharide

2. <hich of the following is true of both starch and

celluloseC

a. They are both polymers of glucose. b. They are geometric isomers of each other.

c. They can both be digested by humans.

d. They are both used for energy storage in plants.

e. They are both structural components of the plant cell w

;. Eumans can digest starch but not cellulose becausea. the monomer of starch is glucose, while the monomer

cellulose is galactose. b. humans have en1ymes that can hydroly1e the beta

glycosidic linkages of starch but not the alpha

glycosidic linkages of cellulose.

c. humans have en1ymes that can hydroly1e the alpha

glycosidic linkages of starch but not the beta

glycosidic linkages of cellulose.

d. humans harbor starch+digesting bacteria in the digestiv



tract.

e. the monomer of starch is glucose, while the monomer of

cellulose is maltose.

7. ! molecule with the formula ;E%8D# is probably a

a. carbohydrate.

b. lipid.

c. protein.

d. nucleic acid.e. hydrocarbon.

). Triacylglycerol is aa. protein with tertiary structure.

b. lipid made with three fatty acids and glycerol.

c. lipid that makes up much of the plasma membrane.d. molecule formed from three alcohols by dehydration

reactions.

e. carbohydrate with three sugars joined together by

glycosidic linkages.

. (aturated fatty acids

a. are the predominant fatty acid in corn oil.

b. have double bonds between carbon atoms of the fattyacids.

c. have a higher ratio of hydrogen to carbon than do

unsaturated fatty acids.

d. are usually li$uid at room temperature.e. are usually produced by plants.

#. The molecule shown in the figure below is a

a. polysaccharide. b. polypeptide.

c. saturated fatty acid.

d. triacylglycerol.

e. unsaturated fatty acid.

%. The hydrogenation of vegetable oil would result in which

of the followingCa. a decrease in the number of carbon+carbon double bonds

in the oil fat. molecules

b. an increase in the number of hydrogen atoms in the oil

fat. moleculec. the oil fat. being a solid at room temperature

d. ! and only

e. !, ', and

*. <hat is the structure shown in the figure belowC

a. starch molecule

b. protein moleculec. steroid molecule

d. cellulose molecule

e. phospholipid molecule

. The #) different amino acids found in polypeptides e"hibit

different chemical and physical properties because of

different

a. carbo"yl groups attached to an alpha carbon

b. amino groups attached to an alpha carbon

c. side chains R groups0.d. alpha carbons.

e. asymmetric carbons.

8. The chemical reaction illustrated in the figure below

results in the formation of a an0

a. ionic bond.

b. peptide bond.

c. glycosidic linkage.

d. ester linkage.e. phosphodiester linkage.

2. <hich bonds are created during the formation of the

primary structure of a proteinCa. peptide bonds

b. hydrogen bonds

c. disulfide bonds

d. phosphodiester bondse. !, ', and



;. <hich type of interaction stabili1es the alpha heli"

and the beta pleated sheet structures of proteinsC

a. hydrophobic interactions

b. nonpolar covalent bondsc. ionic bonds

d. hydrogen bonds

e. peptide bonds

7. ! strong covalent bond between amino acids that functions

in maintaining a polypeptideKs specific three+dimensional

shape is a an0

a. ionic bond. b. hydrophobic interaction.

c. van der <aals interaction.

d. disulfide bond.

e. hydrogen bond.

). !t which level of protein structure are interactions between

the side chains R groups. most importantC

a. primary

b. secondaryc. tertiary

d. $uaternary

e. all of the above

. <hat would be an une"pected conse$uence of changing one

amino acid in a protein consisting of %# amino acidsC

a. The primary structure of the protein would be changed.

b. The tertiary structure of the protein might be changed.

c. The biological activity or function of the protein might be

altered.

d. Dnly ! and are correct.

e. !, ', and are correct.

#. !ll of the following molecules are proteins except a. hemoglobin.

b. transthyretin.

c. collagen.

d. lyso1yme.

e. glycogen.

%. <hat is the term used for a change in a proteinKs three+

dimensional shape or conformation due to disruption of

hydrogen bonds, disulfide bridges, or ionic bondsCa. hydrolysis

b. stabili1ation

c. destabili1ation

d. renaturatione. denaturation

*. <hat is the term used for a protein molecule that assists in

the proper folding of other proteinsCa. tertiary protein

b. chaperonin

c. en1yme protein

d. renaturing proteine. denaturing protein

. Df the following functions, the major purpose of RF! is to

a. transmit genetic information to offspring.

b. function in the synthesis of protein.

c. make a copy of itself, thus ensuring genetic continuity

d. act as a pattern or blueprint to form 6F!.e. form the genes of higher organisms.

#8. <hich of the following descriptions best fits the class of

molecules known as nucleotidesC

a. a nitrogenous base and a phosphate group b. a nitrogenous base and a pentose sugar

c. a nitrogenous base, a phosphate group, and a pentose

sugar d. a phosphate group and an adenine or uracil

e. a pentose sugar and a purine or pyrimidine

#2. <hich of the following are nitrogenous bases of the

pyrimidine typeC

a. guanine and adenine

b. cytosine and uracilc. thymine and guanine

d. ribose and deo"yribose

e. adenine and thymine

#;. <hich of the following statements best summari1es the

structural differences between 6F! and RF!C

a. RF! is a protein, whereas 6F! is a nucleic acid.

b. 6F! is a protein, whereas RF! is a nucleic acid.c. 6F! nucleotides contain a different sugar than RF!

nucleotides.

d. RF! is a double heli", but 6F! is single+stranded.

e. ! and 6 are correct.

#7. If one strand of a 6F! molecule has the se$uence of bases

K!TT=!%K, the other complementary strand would havethe se$uence

a. KT!!=T%K.

b. %KT!!=TK.c. K?!!=?%K.

d. %K?!!=?K.

e. K?=!!?%K.

%). The element nitrogen is present in all of the following

except

a. proteins.

b. nucleic acids.c. amino acids.

d. 6F!.e. monosaccharides.



The following questions are based on the 15 molecules illustrated below. ach molecule may be used once! more than once! or not at

all.

<hich of the following combinations could be linked together to

form a nucleotideC

a. , #, and

b. %, 2, and ;

c. , 7, and )

d. , #, and %

e. #, *, and

%#. <hich of the following molecules contains0 an aldehyde type

of carbonyl functional groupC

AP Biology Summer Assignment 14-15

Documents

Transcript of AP Biology Summer Assignment 14-15