SEMESTER 1 FINAL REVIEW – CHEMISTRY
2015-16
Please ensure that you know how to answer these questions correctly, these are all good example problems for
your final exam. Study your notes, labs, homework assignments and use the PowerPoint presentations that are
online. Any of this information is fair game to be asked on the final exam. Good luck and ask questions in class
during the review times if you have them. Don’t wait to the last minute to start reviewing!
1.
2.
3.
4.
What is the number of significant figures in 1007000.0
What is the difference between accuracy and precision?
What is Avogadro’s number? Why is it useful?
Find the molecular weight of CO2, NH3, SF6 ?
5. Be able to use density to calculate mass and or volume for various objects. Also, understand that density
can be used at times with moles and particles through the D=m/v formula.
6. What is a mole? Be able to explain how the mole is a central connecting idea between mass, particles and
gases @STP
7. What is the molar volume of a gas at STP?
8. What are the seven diatomic elements?
9. Define: atom, molecule, diatomic gas, monoatomic gas, element, compound, STP
10. What elements form the following bonds: ionic, covalent
11. Give an example of the following (both name and formula)
a. an ionic compound
b. a covalent compound
c. a metal
d. a nonmetal
e. a diatomic gas
12. Name the following:
a) NaOH
b) SO2
c) C2SO4
d) HCl
e) Ca(NO3)2
f) NH4
g) N2O5
h) Al2(SO4)3 i) K3PO4
j) Na2O
k) CO
l) CO3
13. Write formulas for following
a) dinitrogen trioxide
b) potassium sulfate
c) hydrogen phosphate
d) sodium bromide
e) ammonium acetate
f) manganese IV nitrate
g) iron III hydroxide
h) aluminum carbonate
14 Write the following in correct scientific notation:
a) 476
b) 0.0000000002223
c) 324000000000000
d) 462.9 x 1023
e) 0.000000345 x1012
f) 5677.9 x 10-12
g) 0.000000223 x 10-6
15.
16.
17.
18.
How many oxygen atoms are there in 420 grams of carbon dioxide?
What is the mass of 1.2 x 1024 molecules of bromine?
What is the volume occupied by 243 grams of oxygen gas at STP?
How do you convert from:
a) moles grams
b) grams  moles
c) moles  molecules
d) moles  liters of gas at STP
e) moles  liters of solution
19.
20.
21.
22.
How many individual atoms of hydrogen are in the drop of water that weighs 0.05 grams?
How many oxygen atoms are in 0.5 moles of oxygen gas?
Find the mass in grams of one iron atom.
A piece of metal weighing 17.6 grams is placed in a graduated cylinder containing 10.0 ml of water. The
water rises to the 12.20 ml mark. What is the density of the metal?
23. A 3.78 gram sample of iron metal is reacted with sulfur to produce 5.95 grams of iron(II) sulfide. What is
the empirical formula of the iron(II) sulfide?
24. What is the concentration of a solution made by dissolving 20.0 grams of NaCl in enough water to make
2000 ml of solution?
25. Find the percent composition of silver nitrate.
26. If a compound is made of 4.99 grams of oxygen and 5.01 grams of sulfur find the empirical formula. If the
molecular mass is 128.2 grams per mole, find the molecular formula.
27. A wavelength of light in the infrared region is 4.257 x 10-5 meters. What is the frequency?
28. The distance from the Earth to the Moon is 3.84 x 105 kilometers. How long would it take a radio wave
with a frequency of 7.25 x 105 Hz to travel from the Earth to the Moon?
29. Be able to complete the following chart using a periodic table as a reference
Element
Protons
Neutrons
Electrons
Mass #
Charge
Symbol
Pt
Te
120
52
5
75
0
198
Pt
Te-2
54
12
+3
30. Be able to explain what valence electrons are and how they differ from other electrons. What are the
maximum number of valence electrons in any element and why?
31. Know the differences between the electron orbitals s, p, d, and f and how many electrons each orbital can
hold. Be able to write electron configurations for the elements in long form and Noble Gas short form.
32. Understand where the s-block, p-block, d-block and f-blocks are on the periodic table and how they are
filled with different numbers of electrons.
33. Understand how the periodic table is organized in a repeating or “periodic” manner. Be able to explain and
show the following trends in the periodic table.
 Ionization energy
 Atomic radii
 Electronegativity
 Valence Electrons
34. Define and provide the formula for Molarity. Understand how Molarity of a solution is another way to
determine or measure solution concentration.
35. You are in the lab. How would you make 10 mL of 0.3 M copper (II) sulfate solution? How many moles
of Copper (II) sulfate and liters of water are needed to do this?
36. Understand how to write and balance chemical equations.