Name ______________________________________
AP Chem Final Exam Review
Date _________________ Period _____
1. Classification of Matter
1. Draw a picture of the particles representing that description.
a. A sample of solid copper (which consists of copper atoms).
b. A sample of liquid ethanol (which consists of C2H5OH).
c. A homogeneous mixture of water vapor and helium gas (which consists of helium atoms).
d. A heterogeneous mixture consisting of liquid water and solid aluminum; show a region of the sample
that includes both substances..
Picture ____
Picture ____
Picture ____
Picture ____
2. Changes in Matter
2. What is the difference between a physical and a chemical change?
3. What are some of the words you can look for in a problem to help you tell the difference?
4. Why is know the difference important?
3. Separation of Matter
2. What are different ways you can separate a mixture?
3. What type of technique would you use if you had two liquids? Why?
4. What type of technique would you use if you had a polar solid and a nonpolar solid? Why?
4. Laws of Matter
5. Describe what each law is about.
a. Law of conservation of Mass
b. Law of Definite Proportions
c. Law of Multiple Proportions
d. Dalton’s Theory
6. How can you illustrate the law of multiple proportions?
7. Draw a pictorial representation of the law of conservation of matter.
5. Chemical Nomenclature
8.
9.
10.
11.
How do you name an ionic compound?
How do you name a covalent compound?
How do you name an acid?
Name the following compounds.
a. NaClO2
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b. Li2O
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c. HBr
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d. IF5
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e. HBrO3
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f. SF6
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g. Fe(NO3)2
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h. XeP3
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i. Ca(CH3COO)2 ________________________________________________
j. K2CrO4
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k. Ag2Cr2O7
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l. HClO4
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m. H2CO3
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6. Chemical Formulas
12. Write the formula for the following chemicals.
a. Potassium sulfate
_________
b. Hydrofluoric acid
_________
c. Tetraphosphorus hexasulfide _______
d. Copper (I) oxide
_________
e. Iodic acid
_________
f. Iron (III) carbonate
_________
g.
h.
i.
j.
k.
l.
Zinc nitrate
Dinitrogen tetroxide
Iron (II) perchlorate
Sulfurous acid
Hypochlorous acid
Chloric acid
_________
_________
_________
_________
_________
_________
7. Molar Mass & % Composition
13. What is the % by mass of nitrogen in the following compounds?
a. N2O
b. N2O5
14. Which compound has the highest percentage of hydrogen?
a. Caffeine, C8H10N4O2
b. Sucrose, C12H22O11
c. Ethanol, C2H5OH
8. The Mole & Compounds
15. How many grams of calcium nitrate, Ca(NO3)2, contains 56 grams of N?
16. Ascorbic acid, or vitamin C (C6H8O6), is an essential vitamin.
a. how many moles of vitamin C are contained in 2000 mg?
b. how many molecules of vitamin C does 5 grams contain?
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9. Molecular & Empirical Formula
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17. What is the difference between an empirical and molecular formula?
18.
19.
20.
21.
If given the molecular formula, how do find the empirical formula?
If given the empirical formula and the molar mass, how do find the molecular formula?
If given the % composition, how do you find the empirical formula?
When hafnium metal is heated in an atmosphere of chlorine gas, the product of the reaction is found
to contain 62.2 % Hf by mass and 37.4 % Cl by mass. What is the empirical formula for this compound?
10. Atomic Structure and History
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22. What information did we learn about the atom through the following experiments:
a. Gold foil
b. Quantum mechanical mathematics
c. Cathode ray
d. Mass spectrometry
e. Ionization energy measurements
f. Experiments with light
23. Radioactive americium-241 is used in household smoke detector and in bone mineral analysis. Give the
number of protons, neutrons, and electrons in an atom of americium-241 (Am-241).
p+ _______
n0 _______
e- _______
24. Dalton assumed that all atoms of the same element were identical in all their properties. Explain why
this assumption is not valid.
25. Galium (average atomic mass = 69.723) has two naturally occurring isotopes, 69𝐺𝑎 and 71𝐺𝑎, with
masses of 68.9257 amu and 70.9249 amu, respectively. Calculate the percent abundance of these
isotopes of gallium.
11. Light
𝑬𝒏 =
−𝟐.𝟏𝟕𝟖 𝒙 𝟏𝟎−𝟏𝟖
𝒏𝟐
∆𝑬 = 𝑬𝒇 − 𝑬𝒊
26. Three of sources of radiation have the following wavelengths: 350 nm, 495 nm, 718 nm.
a. What is the energy of each radiation?
b. What is the relationship between energy and wavelength?
c. What is the relationship between energy and frequency?
27. Calculate the frequency of light emitted when an electron changes from n = 2 to n = 5 in the H atom.
12. Coulomb’s Law/ IE Data/ PES data
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28. Use the data above to answer the following questions.
a. Identify the element. How do you know this from the data?
b. How many energy levels does the element have? How do you know this from the data?
c. How many electrons does it have in an s orbital? How do you know this from the data?
d. How many electrons does it have in the p orbital? How do you know this from the data?
e. How many valence electrons does it have? How do you know this from the data?
29. Use the data to answer the following questions:
a. Identify the element. How do you know this from
the data?
b. How many energy levels does the element have?
How you know this from the data?
30. Explain how Coulomb’s law effects ionization energy.
13. Electron Configuration
31. What is the electron configuration for the following elements or ions?
a. Na
b. V
c. Fe
d. Fe3+
e. V5+
f. V2+
g. Kr
32. How can you tell if an element is paramagnetic or diamagnetic?
14. Periodic Trends
33.
34.
35.
36.
37.
38.
39.
Why does the atomic radius decrease going across the periodic table?
Why does the atomic radius increase going down the periodic table?
Why are anions larger than their atoms?
What are cations smaller than their atoms?
Why does ionization energy increase across the periods?
What does the ionization energy decrease down a group?
What are some of the exceptions to ionization energy? Why do they occur?
15. Ionic Bonds
40. How can you tell if a bond is ionic?
41. Draw the ionic bond that occurs between sodium and nitrogen.
42. What makes an ionic bond be the strongest? Have the highest lattice energy?
16. Covalent Bonds
43. Draw the Lewis structure for the following molecules. Draw resonance structures when appropriate.
a. SeF2
b. SCN44. How many sigma and pi bonds do the following molecules have?
a. CO2
b. C2H4
c. CCl2H2
d. CN¯
17. Bond Properties
45.
46.
47.
48.
49.
What are the factors that influence bond length?
How do you calculate bond order?
What is the connection between bond order and bond length?
What is the connection between bond length and bond strength?
Know how to calculate a bond energy.
18. Molecular Geometry
and 19. Molecular Polarity
For the following molecules, determine their geometry, bond angle, hybridization and polarity.
50.
51.
52.
53.
54.
55.
SiCl4
IF3
PCl3
XeF5+
NO3–
SO42–
56.
57.
58.
59.
SF6
BrF2–
PBr5
SO2
17. Intermolecular Forces
50. How do you know which types of intermolecular forces (hydrogen bonding, dipole-dipole, dispersion)
will be present in covalent compounds?
51. What influence do intermolecular forces have on compounds?
52. How can you determine if the melting point will be higher or lower?