-AP Biology Biochemistry/Chemistry Review
Name ____________________________
Chapter 2 - The Nature of Molecules
Sections 2.1 - 2.3
Chapter 3 – The Chemical building blocks of life
1.
What occurrence 12.5 billion years ago is proposed to have begun the process that lead to the formation of the
earth? _______________________ When did the earth form? _________________
When did life form and begin to diversify? ________________
2. Define matter:
3. All matter is composed of extremely small particles called ________________, the smallest particles of an
element.
4. Identify and compare the three subatomic particles:
Particle
Location
a.
Mass (daltons or amu’s)
Charge
b.
c.
5. Define:
a. atomic number –
b. atomic mass –
6. What determines the chemical behavior of an atom?
7. What characteristic do all the atoms of the same element have in common?
8. Give the atomic number ________________and average atomic mass ____________(round to 3 sig.figs) for
K. What is the mass number for the most common isotope of potassium? __________
9. Atoms have the same number of protons and electrons and are thus electrically _______________.
10. An atom which has gained one or more electrons is called an _________________ and has a net
______________ charge. An atom which has lost one or more electrons is called an ___________________
and has a net __________________ charge.
11. Compare and contrast carbon-12 with its isotope carbon-14 as to abundance, number of p, e, and n and stability.
12. Give two uses of radioactivity related to biology:
a.
b.
13. Complete the following chart for the most common isotope of each atom/ion.
Symbol
Number of
Number of
Number of
Number of
Protons
Electrons
Neutrons
Outermost or
Valence e-‘s
O
Predicted oxidation
State(s)/# of electrons it
tends to gain, lose, or share
P
Li
F-1
Na
+1
14. The key to the chemical behavior of an atom lies in the arrangement of its __________________. The area
around the nucleus where an electron is most likely to be found is called an ____________, which represents a
_______________________ distribution for an electron. The first energy level, K, is occupied by a single
spherical shaped _______ orbital. The second energy level, L, is occupied by one spherical _______ orbital
and 3 dumbbell shaped _________ orbitals. Regardless of its shape, no orbital can contain more than
__________ electrons.
15. Circle the two correct terms: Electrons that are found in more distant orbitals have (more or less)
(kinetic or potential) energy.
16. Electrons within an atom have discrete _____________ ______________ due to their position or distance
from the nucleus.
17. The loss of electrons from an atom in a chemical reaction is called _______________________. The gain of
electrons is called ___________________________.
18. Write the complete electron configuration for the following atoms: (Do not use noble gas shorthand.)
Atom
Electron Configuration
Number of Valence eK
19
26Fe
92U
19. The interactions of outermost or ____________________electrons is the basis for differing chemical
properties.
20. The noble gases are nonreactive or _______________. Group VII elements, the halogens such as F, Cl, and Br
tend to _____________an electron. Group I elements, the alkali metals such as Li, Na, and K tend to
_____________ an electron.
21. State the octet rule.
22. Explain why iron atoms tend to form +2 Ferrous as well as +3 Ferric ions.
23. Identify the 6 major elements found in living things.
24. Describe the role of carbon in molecular diversity, its characteristics, and its forms of organization structures.
25. Two or more different elements chemically combined in definite proportions make up a
___________________. A group of covalently bound atoms with an overall neutral charge is called a
________________.
26. Recognize the importance of molecular bonding and distinguish among strong and weak bonds, giving biological
examples of each. (polar covalent, nonpolar covalent, ionic and hydrogen bonds)
27. Which molecule has a stronger covalent bond, O2 or H2? __________Explain.
28. How many covalent bonds does a C atom form? _____________ Explain.
29. Distinguish among the three types of isomers: structural, geometric, and enantiomers.
30. Recognize the major functional groups and describe the traits they give their macromolecule.
31. Define monomer, polymer, hydrolysis, and dehydration synthesis and be able to give specific examples from
each of 4 macromolecule groups.
32. Complete the chart in order to compare the four groups of macromolecules:
monomers
Bond types
structures
functions
carbohydrates
lipids
proteins
nucleic acids
33. The affinity of an atom for electrons in a bond is called _______________________. Where are the
elements located with highest electonegativity? ____________________________ Which element has the
highest electronegativity? ______________
34. What type of bonds result when atoms share electrons unequally? __________ _______________
35. Is the bond between 2 oxygen atoms polar or nonpolar? _____________
36. Is the bond between a C and a H atom, polar or nonpolar? ______________
37. Is the bond between an O and a H atom, considered polar or nonpolar? _____________
38. The formation and breaking of chemical bonds is termed a chemical ________________ which is represented
by a chemical ____________________.
39. Why must chemical equations be balanced?
40. State three factors that influence the extent to which a chemical reaction occurs/influence rates of reactions
a.
b.
c.
41. What information can be communicated around the four corners of an element’s symbol?
upper left? ______________ lower left? ____________
upper right? ______________ lower right? ____________
42. Name the following compounds:
a. C55H98O6
b. C6H12O6
c.
C55H72O5N4Mg
43. Give the formulas for the following elements/compounds.
a. nitrogen gas
b. sodium chloride
c.
magnesium sulfate
d. calcium hydroxide
e.
iron(III) oxide
f.
hydrochloric acid
g.
carbon dioxide
h. sodium thiosulfate
i.
carbonic acid
44. Give the: molecular formula, structural formula and Lewis dot diagram for water.
45. Calculate the molecular mass of 1 molecule of glucose, C6H12O6. (Give proper units.)
46. What many molecules are in a mole of glucose molecules?
47. What is the mass of one mole of glucose molecules?
48. Balance the following equation for photosynthesis. b. Circle the reactants and underline the products.
CO2 +
H2O → C6H12O6 +
O2
49. How many moles of CO2 are required to produce 24.0 grams of glucose? (Show work with appropriate
conversion factors and units, i.e. use dimensional analysis to solve.)