Exam 1 Review Sheet
Honors Biology
This is to be used for REVIEW. It is not all encompassing.
Exam 1 will cover:
ALL of Chapter 1
Chapter 2 – Introduction THROUGH 2.8
1. Quiz 1 Review Sheet
2. Quiz 2 Review Sheet
3. Quiz 3 Review Sheet
4. Read the intro of chapter 2, there will be one question.
5. Explain figure 2.1 in terms of structure-function relationships and emergent properties.
6. Compare the holistic to the reductionist approach to science.
7. What is matter?
8. Define what an atom is. What does “atom” mean in Greek and why is this appropriate.
9. What is an element? (Two similar definitions)
10. How many elements are known? How many occur naturally? How many are found in
organisms (are essential to life)?
11. Be familiar with the table in section 2.2. Identify the top four major elements of life.
Be familiar with the other seven elements below those.
12. What is meant by a trace element? Give an example that demonstrates the importance
of these elements even though we only need them in small amounts.
13. If you didn’t use the goiter as your example in #37, identify what a goiter is and how
one would develop such a disease.
14. What is a compound?
15. Compare an element to a compound and give examples of each.
16. Explain elements like oxygen and nitrogen exist in the atmosphere.
17. Explain how emergent properties apply when going from element to compound. Give
an example.
18. Study tip: When you think you know what you need to know, go through the assigned
book sections, cover the section with a piece of paper except for the heading and try to
explain to yourself what the section says. Make sure you hit all the bolds words and
figures/tables. Your are most likely ready if you can teach the material to someone else.
19. Atom drawing work sheet online under notes section. Be able to do every problem on
that sheet.
20. Molecule drawing worksheet online. Be able to do every problem on that sheet.
21. Identify the subatomic particles that make up all atoms. Make a chart showing the
charge of each particle and the mass of each particle in atomic mass units and kilograms.
22. How does one determine the mass of a given atom? Why are the electrons not
counted when they clearly have a mass?
23. Explain how the protons, neutrons and electrons are arranged in an atom according to
the Bohr model.
24. Draw a neutral oxygen atom with a mass of 16 in the lowest energy state (also called
the ground state because all the electrons are closest to the “ground” if you think of the
nucleus as the Earth). Now modify your atom so that it is not in the ground state.
25. Explain why the electrons in the inner most orbital (shell) have less energy than the
electrons in the outer orbitals (shells). Make an analogy using a basketball and planet
Earth.
26. Explain why electrons move around the nucleus if Isaac Newtons first law of motion
clearly states that an object will continue moving in a straight path unless acted upon by a
force. Describe the force. Explain how this concept is similar to the moon going around
the Earth or the Earth around the sun. Describe this force.
27. If gravity is the attraction of all matter to all matter then why don’t we say that
gravity is pulling the electrons to the nucleus like the Earth to the sun? Basically, why do
you think we completely ignore gravity on the atomic level? (Hint: why do we ignore
electrons when calculating mass?)
28. The nucleus of elements larger than hydrogen obviously has more than one proton in
close proximity. How can this be if the electromagnetic force is pushing these like
charges apart?
29. What determines the elemental identity of an atom? How does this relate to the
atomic number?
30. Make sure you have memorized the atomic numbers of H, C, N, O so that you can
draw the proper atoms and molecules when asked.
31. If I had a mole of pencils, how many pencils would I have?
32. What is the significance of a mole?
33. ***This question is above and beyond the scope of the course, but very
important to understand. Therefore, I will put a bonus question on the exam
pertaining to this mini-lesson. There will not be an exam question outside the bonus
question.
If I had a mole of hydrogen atoms, how many hydrogen atoms would I have? What mass
of hydrogen atoms would I have? What if I had one mole of helium atoms, what mass
would I have? Think about it…a helium atom has how many protons and neutrons? (2
protons and 2 neutrons) If I have have a mole of helium atoms then I have 6.023x1023
times 4 protons and neutrons. Each 6.023x1023 has a mass of 1 gram and therefore I
would have 4 grams of helium. What is the atomic mass of this helium? 4 amu. How
many grams is a mole of this helium? 4 grams (see the obvious pattern)
****The atomic mass of a given piece of matter equals the mass in grams of a mole of
that substance.
Matter
carbon atom
oxygen atom
water molecule
carbon dioxide
ethanol (C2H6O)
glucose C6H12O6
total atomic mass (amu)
12
16
18 (1 per hydrogen and 16
for water for a total of 18
protons and neutrons)
12+18+18= 48amu
12+12+1+1+1+1+1+1+18= 48
72+12+96 = 180
mass of 1 mole (grams)
12 grams
16 grams
18 grams
(density of water = 1g/ml)
therefore 18ml of water is
a mol of water molecules!!
48g
48g
180g
Therefore if I needed you to weigh out a mole of glucose for me in the lab, you would
weigh out 180g. 180g grams of glucose contains 6.023x1023 glucose molecules. The
bonus question will ask you to weigh out some amount of material. For example, I might
ask you to weigh out 2 moles of glucose for me. You would need to calculate the atomic
mass of glucose and then multiply it by two to get two moles.
34. What is the other name for the number that represents a mole?
35. Why if I were to stand in front of an x-ray laser, 99% of the x-rays would pass right
through me as if I were not even there (x-rays are a form of light like visible light, UV
and IR). How does this relate to the formation of super dense objects like black holes or
neutron stars (reminder: neutron stars form when a star 8 times or more larger than our
sun die resulting in a supernova and leaving behind a chunk of matter made entirely of
neutrons and about the size of a city like NYC. One thimble full of these neutrons would
weigh tons!!!*****
36. Describe the analogy we used in class to convey how much empty space is present in
matter.
37. Explain how matter like one of Georges Seurat’s most famous works A Sunday
Afternoon on the Island of La Grande Jatte, a remarkable example of pointillism. You
will need to read about the painting here
http://en.wikipedia.org/wiki/A_Sunday_Afternoon_on_the_Island_of_La_Grande_Jatte
and
http://www.art.com/products/p11745560-sa-i2326848/georges-seurat-sunday-afternoonon-the-island-of-la-grande-jatte-c1886.htm
38. Explain what I mean when I say that you have never actually touched anything in
your life. Why is it that I don’t just fall through the Earth?
39. Make sure you understand how to write and read the atom format:
40. How big is an average size nucleus (in parts of a millimeter)? How many could fit
across a millimeter. How large is an average sized atom (in parts of a millimeter)? How
many could fit across a millimeter. How many water molecules are in a mere 18ml of
water? What do these numbers tell you about atoms?
41. How large would an atom be inside a cell if the cell were scaled up to the size of
Madison Square Garden?
42. What happens in terms of mass, charge and elemental identity if the number of
neutrons in an atom change?
43. What is nuclear radioactivity and when does it occur? Give an example of an atom
undergoing radioactive decay.
44. How can radioactive decay be useful and harmful? Give examples of each.
45. Explain how you can use radioactive carbon (C-14) to determine the fate of CO2 after
entering the leaf of a plant.
46. How does one determine the charge of an atom? What happens to an atom if one
changes the number of electrons in terms of charge, elemental identity and mass? What if
one changed the number of protons?
47. Look over review questions in the powerpoint.
48. Look at all book sections and make sure you understand every bold word, figure and
table and can explain them without looking.
49. What determines how an atom reacts with other atoms (chemical reactivity)? When
are atoms most stable(happy)?
50. Explain why when sodium metal is added to chlorine gas a somewhat violent
explosion occurs. Be sure to include the word AFFINITY in your explanation. It is all
about affinity. What type of bond forms? Why does this type of bond form? What force is
involved?
51. Where does an ionic bond get its name? What is an ion? Describe the difference
between a cation and an anion. Which is sodium and which is chlorine after they react to
form sodium chloride?
52. Describe the structure of a salt crystal.
53. Compare a covalent bond to an ionic bond. Give an example of a covalent bond.
Show, using valence shell diagrams, how two oxygen atoms come together to form a
double bond.
54. Arrange the terms single, double and triple covalent bonds from strongest to weakest.
Which would require the most energy (would need to be hit the hardest) to break?
55. Define the word molecule.
56. If I give you a substance, you should be able to characterize it in terms of whether it
is a molecule, element and/or compound. There are examples in the PowerPoint for you
to try.
57. When does molecular motion stop (matter has zero kinetic energy)? How fast are
atoms/molecules moving on average at room temperature? What happens as temperature
increases?
58. Write out a chemical reaction. It can be any reaction you want. Indicate the reactants
and the products. What is a chemical reaction?
59. Find a periodic table now and look at it. Assuming the atoms are neutral, how many
valence shell electrons does sodium (Na) have? How many electrons are in the valence
shell of potassium (K), the element below Na? What about the element below potassium
(K)? Do you see a trend? The columns in a periodic table are called groups or families.
Know this. They are called families because they all react in a similar fashion. Why do
members of a family all react in a similar fashion?
60. Look at family or group II on your periodic table. How many valence electrons do
these elements all have? What could you tell me in terms of being similar or very
different the chemical reactivity of group II elements?
This is your first exam. Train Hard and Good Luck.