
James, Joe, and Paul:

We will move onto chemistry tomorrow! Today, you will write the following 3 essays on energy. The next slide is a sample grid-in question on energy.
The essays and grid-in question are due at the end of the class. Directions are on each slide.

Write the following essay on a lined sheet of paper. Be sure to label your essay as #1.
Time: 20 minutes

1. All living things require a constant input of energy for their metabolic functions. Special structures within cells have evolved to produce this energy. Discuss the process of cellular respiration in aerobic organisms.
Include a discussion of each of the following (8 pts.):
 a. The structure of a mitochondrion and relate the structure to the particular respiration processes.
 b. The general process of glycolysis and fermentation and why these processes are important.
 c. The general description of the citric acid cycle and its importance in producing energy.
 d. A description of oxidative phosphorylation and the importance of the proton motive force.





2. All living things depend on producers to harness the energy form the sun and make it available for all living things on Earth. The essence of what green plants do it photosynthesis. Here is the simplified equation for photosynthesis (8 pts.):
 a. Describe and explain the structure of the chloroplast. You may sketch and label a drawing of it, but you must also explain the function of each part. b. Describe the process of light harvesting in the chloroplast. c. The making of sugar uses a great deal of energy in the form of ATP. Explain how ATP is made in chloroplasts.
 d. Plants take in water and carbon dioxide and give off water and oxygen, Explain where these chemicals fit into a discussion of photosynthesis. Include a brief explanation of the Calvin Cycle.



This is a short answer question. This question should take you no more than 6 minutes to answer.

3. ATP and GTP are primary sources of energy for biochemical reactions (4 pts.)
 a. Describe the structure of the ATP or GTP molecule.
 b. Explain how chemiosmosis produces ATP.


The grid-in questions are answered in the same section as the multiple choice section. You will have 90 minutes to answer 63 m.c.
questions and 6 grid-in questions. (~ 4 minutes to answer this question)


Read about CAM, C3, and C4 plants in your textbook in chapter 10.

AP test is moving away from plant physiology, but it may be a good idea to know about photorespiration and the evolutionary significance of it.

Do not forget to turn in your sub packet to the basket!


1. List the elements essential to life.

2. Where is the hydrophobic and the hydrophilic nature of water seen in the cell?

3. Give an example of matter in our classroom.

1.
List the elements essential to life.

Carbon, nitrogen, oxygen, hydrogen, phosphorus, sulfur, sodium, calcium, chlorine, magnesium, and potassium

2. Where is the hydrophobic and the hydrophilic nature of water seen in the cell?

The cell membrane is hydrophobic and does not allow polar molecules through without the help of transport proteins or channels. This allows a “barrier” between the intracellular and extracellular fluid of cells.

3. Give an example of matter in our classroom.

Desks, pencils, chair, table, projector, files, ceiling tiles, etc.

• 3 rd - nine week grades are due Friday
• Quiz #23 on Friday!
• See me for tutoring
• Check infinite campus for grade updates!


Daily Catalyst

Class Business

Chemistry vocab

Chemistry practice problems



They fall in the same year every year, New Year's Day just arrives very early in the year and Christmas arrives very late in the same year.


We will review basic chemistry and vocabulary to be able to apply these basic chemistry principles to advanced biology concepts.

 https://www.youtube.com/watch?v=izeuGr0lbN0


Key Concepts:
• Matter consists of chemical elements in pure form and in combinations called compounds
• An element’s properties depend on the structure of its atoms
• The formation and function of molecules depend on chemical bonding between atoms
• Chemical reactions make and break chemical bonds

Example Picture Vocab word Definition
Matter
Elements
Compounds
Atoms
Subatomic particles
Atomic numbers
Isotopes
Covalent
Bonds
Ionic Bonds
Hydrogen bonds

• Anything that takes up space and has mass

• Substances that cannot be broken down

Na, C, and Cl

Basic units

• Consists of 2 or more different elements

Salt, sugar, water, and baking soda

(C12H22O11, H2O, and NaCO3)

• Atom is the basic unit of a chemical element
• Atoms have neutrons, protons, and electrons
• Make up an atom

• Atomic Number

# of protons (and electrons to be =)
• Atomic Mass

# of protons and neutrons

• Same elements, same behavior, and same # of protons, but different number of neutrons (different mass)

Useful in radioactive dating for fossils

Radioactive isotopes decay

• Sharing of a pair of valence electrons

Strong bond

Valence bonds are the outer most electrons available for sharing or reactions

Where have we seen covalent bonds?

• Transfer of 1 electron to another element

Commonly between a + and - ion

• Hydrogen atom covalently bonds to H, F, O, or N

H20 or NH3

Weak bonds

H-FON!


Blue Book

# 2, 6, and 10

Homework: read 3.1 (water) and 3.3 (pH)


The grid-in questions are answered in the same section as the multiple choice section. You will have 90 minutes to answer 63 m.c.
questions and 6 grid-in questions. (~ 4 minutes to answer this question)


1. Why is C
2 and H
6 not an example of a compound?

2. Which subatomic particle gives atoms their identity?

3. How are isotopes related to evolution?

1.
Why is C 2 and H
6 not an example of a compound?

A compound is two or more elements in a fixed ratio

2. Which subatomic particle gives atoms their identity?

Protons

3. How are isotopes related to evolution?

Some isotopes are radioactive and will decay
(breakdown) over time. We can measure the amount of decay and figure out the number of years.

• 3 rd - nine week grades are due Friday
• Quiz #23 on Friday!
• See me for tutoring
• Check infinite campus for grade updates!

3/12 Brain Teaser
 A woman from New York married ten different men from that city, yet she did not break any laws. None of these men died and she never divorced. How was this possible?
 The lady was a Justice of the Peace.


Daily Catalyst

Class Business

Chemistry vocab

Chemistry practice problems


We will review basic chemistry and vocabulary to be able to apply these basic chemistry principles to advanced biology concepts.

Which of the following is the criterion upon which the modern periodic table is organized?
A.
Number of protons
B.
Number of neutrons
C.
Atomic mass number
D.
All of the above

Which of the following is the criterion upon which the modern periodic table is organized?
A.
Number of protons
B.
Number of neutrons
C.
Atomic mass number
D.
All of the above

• Key Point #1: Valence electrons
• Electrons in the outermost energy level
• The chemical behavior of an atom is mostly determined by the valence electrons
• Used in bonding
37

Why might scientists be interested in the "atomic mass" of an atom?
A.
It tells how it will behave in a chemical reaction.
B.
It lets us know the valence of the atom if we know the atomic number.
C.
If we know the atomic number, we can determine the number of neutrons.
D.
We can use it to know if the atom is radioactive or not.

Why might scientists be interested in the "atomic mass" of an atom?
A.
It tells how it will behave in a chemical reaction.
B.
It lets us know the valence of the atom if we know the atomic number.
C.
If we know the atomic number, we can determine the number of neutrons.
D.
We can use it to know if the atom is radioactive or not.

• Sharing of a pair of valence electrons

Strong bond

Valence bonds are the outer most electrons available for sharing or reactions

Where have we seen covalent bonds?

• Key Point #2: Covalent bonds-
• Sharing valence electrons
• STRONG bond
• 1 pair of e’s—a single bond
• 2 pairs of e’s—a double bond
• 3 pairs of e’s—a triple bond
41


Key Point #3: Polar-

Unequal distribution of charged electrons

May lead to + and - poles

• Key Point #4: In a nonpolar covalent bond, the atoms share the electron equally.
• No poles
43

Net dipole moment
 –
• Key Point #5: In a polar covalent bond, the atoms do not share the electrons equally.
• The electronegative atom hogs the electrons!
O

+
H H

+
H
2
O
44

KP #5 continued:
• Unequal sharing of electrons causes a partial positive or negative charge for each atom
45

Which of the following statements best describes the difference between an element and a molecule?
A.
An element is composed of atoms; a molecule is not.
B.
An element is composed of only one kind of atom; molecules can be composed of more than one kind of atom.
C.
Elements always have lower atomic weights than molecules.
D.
Elements exist in nature only as parts of molecules.
46

Which of the following statements best describes the difference between an element and a molecule?
A.
An element is composed of atoms; a molecule is not.
B.
An element is composed of only one kind of atom; molecules can be composed of more than one kind of atom .
C.
Elements always have lower atomic weights than molecules.
D.
Elements exist in nature only as parts of molecules.
47

For a covalent bond to be polar, the two atoms that form the bond must have
A.
different atomic weights.
B.
the same number of electrons.
C.
different electronegativities.
D.
similar electronegativities.
48

For a covalent bond to be polar, the two atoms that form the bond must have
A.
different atomic weights.
B.
the same number of electrons.
C.
different electronegativities.
D.
similar electronegativities.
49

• Transfer of 1 electron to another element

Commonly between a + and - ion

• Key Point #6: Ionic Bond
• A cation is a positively charged ion
• An anion is a negatively charged ion
• An ionic bond is an attraction between an anion and a cation
• Compounds formed by ionic bonds are called ionic compounds, or salts
• Salts, such as sodium chloride (table salt), are often found in nature as crystals
51

Why are covalent bonds more prevalent among biological molecules than ionic bonds?
A.
Ionic bonds only occur between metals and non-metals, and therefore aren't usually present in biological systems.
B.
You can have double covalent bonds, but not double ionic bonds, so covalent bonds provide more variety consistent with the structural demands required in biological systems.
C.
Biological conditions are often aqueous, and the water would cause ionic bonds to dissociate.
D.
Ions only form under extreme conditions not compatible with the cell's environment.

Why are covalent bonds more prevalent among biological molecules than ionic bonds?
A.
Ionic bonds only occur between metals and non-metals, and therefore aren't usually present in biological systems.
B.
You can have double covalent bonds, but not double ionic bonds, so covalent bonds provide more variety consistent with the structural demands required in biological systems.
C.
Biological conditions are often aqueous, and the water would cause ionic bonds to dissociate.
D.
Ions only form under extreme conditions not compatible with the cell's environment.

• Hydrogen atom covalently bonds to H, F, O, or N

H20 or NH3

Weak bonds

Whether an atom will be able to interact with other atoms can be determined by
A. Looking at the ratio of protons to neutrons in the nucleus.
B. Whether it has an even or odd number of electrons.
C. Determining the stability of the electrons in their valence orbitals around the nucleus.
D. Identifying the atom as a metal or non-metal.

Whether an atom will be able to interact with other atoms can be determined by
A. Looking at the ratio of protons to neutrons in the nucleus.
B. Whether it has an even or odd number of electrons.
C. Determining the stability of the electrons in their valence orbitals around the nucleus .
D. Identifying the atom as a metal or non-metal.


Blue Book

# 2, 6, and 10

Homework: read 3.2

Cohesion

Heat and temperature

Waters specific heat

Evaporative cooling

Insulation of bodies of water

The solvent of life

Hydrophobic and hydrophilic substances

Solute concentration in aqueous solutions

Concept check 3.2 question 1

Concept check 3.2 question 2

Concept check 3.2 question 3

Concept check 3.2 question 4