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1st Semester Final Study Guide
2016-2017 Honors Chemistry Class
I have done my best to put together what I feel is a fair study guide that should help you to study for the final.
However, please do some extra studying on your own. Be sure to bring a scientific calculator (SHARING IS NOT
ALLOWED and we don’t have very many extras). Don’t be late!!! No cheat sheets/notecards allowed.
Major Units covered:
1. Math/Intro
2. Matter (structure of an atom)
3. Electron Configurations
4. Bonding and Formula Writing
Topics Covered:
 Lab safety
 Chemistry Math
o Dimensional analysis
o Density problems
o Significant figures
o Scientific notation
o Metric conversions
o mole conversions
 SI units used in science (mass, volume, temperature, density, etc)
 Matter – solids, liquids, gases
 Mixtures (homogeneous/heterogeneous) and pure substances (elements/compounds)
 physical vs. chemical changes/properties
 Atomic structure
o Protons, neutrons, electrons
o Models of the atom – Dalton, Rutherford, Bohr
o History of the atom: gold foil experiment, plumb pudding model, etc.
 Atomic number, mass number, # of protons, neutrons and electrons
 cations/anions and predicting charges on the periodic table
 Coulomb’s law (basic understanding)
 Isotopes (same number of protons, different number of neutrons)
 Calculating average atomic masses from % abundance and mass of isotopes
 Bohr models, Orbital notations, and electron dot structures
 Atomic orbitals and energy levels (s, p, d, f)
 Electron configurations (abbreviated, regular)
 Periodic table
o Families/groups and periods (alkali metals, alkaline earth, halogens, noble gasses, transition metals, etc)
o Metals/nonmetals/metalloids
o Periodic trends – atomic radius, electronegativity, ionization energy
 Ionic compounds
 Covalent compounds
o polar bonds
 Bond strength and characteristics
 Naming compounds (ionic, molecular, acids)
 Writing formulas (ionic, molecular, acids)
 % composition (MOE/MOC x 100)
 % yield, % error
Unit one review
Measuring: Determine the correct reading for the following examples:
1. see picture to the right:
2. See picture to the right:
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Scientific Notation
Put the following into scientific notation
3. 0.000000678
4. 574000000
Write the following as a decimal
5. 7.54 x 105
6. 8.259 x 10-4
Significant figures
How many sig figs in the following
7. 0.0045 L
8. 150
9. 16.070 mm
Round each of the following to 4 sig figs
10. 987954 mm
11. 15.999 cm
Find the answer with the correct number of sig figs and correct units
12. 6.7cm + 10.4cm + 1.953cm =
13. 6.58 x 10-5 ÷ 8.5 x 10-4
14. 1.45 cm x 2.487 cm x 5.6 cm =
Solve the following using dimensional analysis(remember units and sig figs. No credit for no DA work shown.)
15. What is the volume of a pure silver coin that has a mass of 14.9g? The density of silver is 10.5 g/cm 3.
16. An atom of gold has a mass of 3.271 x 10-22g. How many atoms of gold are in 5.00g of gold?
17.
In the lab, you find the density of aluminum to be 2.93 g/mL. The actual value is 2.70g/mL. What is your percent
error?
18. A copper penny has a mass of 3.1 g and a volume of 0.35cm 3. What is the density?
19. Convert 45.8 cm to μm.
20. Convert 89.4 nL to cL
21. The density of silver is 10.5g/cm 3. What is the volume of a 68 g bar of silver?
22. Identify at least 2 different separation techniques for separating homogeneous mixtures. Describe what physical
property it takes advantage of.
23. Identify at least 2 different separation techniques for separating heterogeneous mixtures. Describe what physical
property it takes advantage of.
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24. Label the following diagrams as either endothermic or exothermic.
DIAGRAM A
DIAGRAM B
25. Which diagram feels hot? _________ Which feels cold? ____________
26. Determine if the following depicts a chemical or physical change:
A
B
27. Look at the diagrams below and determine if they are a substance or mixture, then determine which TYPE of
substance or mixture they are INCLUDING what state of matter you believe the matter to be in. Justify your response
for each.
Unit two review
Periodic table
Be able to label the following: alkali metals, alkaline earth metals, transition metals, inner transition metals, halogens,
metalloids, groups/families, and periods.
Isotopes
28. What is an isotope?
29. What is the formula for average atomic mass?
30. Define mass number and atomic number.
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a) what is the mass number for the most common isotope of carbon? ___________________
b) what is the average atomic mass of carbon? _________________
c) what unit is atomic mass in (spell it out…don’t give the symbol)? _________________
31. Element Y has 4 isotopes. Calculate the average atomic mass.
a. 5.2%, 16.2165 amu
b. 6.4%, 12.5485 amu
c. 10.9%, 13.6852 amu
d. 77.5%, 15.384 amu
32. Draw and fill in a concept map with the following terms:
Homogeneous, heterogeneous, matter, substance, mixtures, element, compound
33. Fill in the following table
Chemical
Atomic #
Symbol
F
Mass #
# protons
14
25
47
55
# neutrons
# electrons
10
15
25
34. How many neutrons does gold-198 have?
35. Describe Rutherford’s experiment. What did he do? What did he conclude?
36. Describe Thomson’s experiment. What did he do? What did he conclude?
37. If you make 15.23 grams of magnesium oxide and you originally started with 6.85 grams of magnesium, how much
oxygen reacted with your magnesium? What law or principal confirms this?
38. 5.0 grams of hydrogen reacts completely with 19.0 grams of fluorine. What is the percent by mass of hydrogen in the compound
that is formed?
39. Copper sulfide is formed when copper and sulfur are heated together. In this reaction, 56.4 g of copper reacts with 34.5 g of
sulfur. After the reaction is complete, 9.5 g of sulfur remains unreacted. What is the mass of copper sulfide formed?
40. What is the atomic number and mass number of the most common isotope that each atom forms? Gold, Magnesium,
Helium, Krypton, and Sulfur
41. What is the average atomic mass given the following information: Copper has two isotopes: Cu-63 (abundance =
69.2%, mass = 62.930 amu) and Cu – 65 (abundance = 30.8%, mass 64.928 amu).
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Unit 3: electrons
42. Sketch out a periodic table and label in where the s, p, d, and f blocks are on the periodic table.
43. How many electrons does each orbital hold?
44. What is the maximum number of electrons that can fit in the 1st principle energy level? 2 nd? 3rd? 4th?
45. What is the full electron configuration of sulfur?
46. What is the abbreviated electron configuration of Calcium?
47. What is the electron orbital notation for Fluorine?
48. What is the Bohr model for silver?
49. Explain the Aufbau principle, the Pauli exclusion principle, and Hund’s rule.
50. When an electron absorbs energy, what will the electron do?
51. When an electron falls from the 4th ring to the 3rd ring, what happens?
Unit 4 – periodic table, compounds and bonding
52. Describe the trends for atomic size and electronegativity on the periodic table going across and down a family.
53. What is the largest atom on the periodic table?
54. Which atom on the periodic table has the highest electronegativity?
55. What is electronegativity?
56. Choose the atom that will be the most electronegative from the two choices.
a. K or Fr?
_______
b. Mg or S? _______
57. Choose the atom that will be the largest atom from the two choices.
a. Na or Cs? _______
b. Ca or Zn? _______
58. How is a positive ion formed? What type of elements form these ions?
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59. How is a negative ion formed? What type of elements form these ions?
60. What is a formula unit?
61.
62.
63.
64.
What is the formula for copper (II) sulfide? _________________________________
What is the formula for sulfurous acid? _____________________________
What is the formula for Nitrogen decaoxide? ___________________________
What are the rules for naming ionic compounds?
65. What are the rules for naming molecules?
66. What are the rules for naming acids?
67. Where are metals found on the periodic table? Nonmetals? Metalloids? Transition metals?
68. Name the following:
a. HClO3
b. Al2(CO3)3
c. NaHSO4
d. CuBr2
e. NO2
f. H2SO3
Write the formula for the following:
g. Nitrous acid
h. Tetracarbon octaoxide
i. Potassium chromate
j. Hydrophosphoric acid
k. Zinc hydroxide
l. Copper (II) phosphate
69. Draw an atomic model of ammonium sulfate.
70. Describe the bond strength of ionic vs. polar vs. covalent compounds.
71. Describe how covalent vs. ionic compounds are formed.
72. How do you determine whether a bond is ionic, polar, or non-polar?
73. List the electronegativity difference values for covalent, polar, and ionic bond types.
74. Under what conditions with a compound conduct electricity?
75. Describe metallic bonds.
76. Describe Coulomb’s law:
77. Draw a bond energy diagram. Label the x-axis as distance and the y-axis as potential energy. Be sure to label the
bond length and relative attractive force.
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