Name _____________________________________________
Period ______
Chemistry Midterm Review 2015-2016
Name______________________Pd___
Name _____________________________________________
Period ______
Mid-Term Exam Review
Unit 1: Chapter 3 – Measurement and Calculations
Complete the following questions.
Key Vocabulary
metric prefixes
scientific notation
significant figures
Key Concepts




write numbers in scientific notation
perform addition, subtraction, multiplication and division and round the answer to the proper number of
significant figures
o some problems involve numbers in scientific notation so you must know how to enter these
numbers properly in your calculator
calculating area
 calculations involving density
calculating percent error (page 65)
 dimensional analysis
Review Questions Note: There are a few review questions here, but if you need more assistance, please look in
your book in Appendix C (p. R56) for additional review, examples and practice problems.
1. How many significant figures are in each of the following numbers:
a. 12000 kg
c.
0.000234 cg
b. 360.0 g
d. 0.0550 m
2. Determine the number of significant figures in each calculated answer, without solving the problem.
a. 71.4 cm + 12.45 cm =
c.
6.070 m x 0.044 m =
b. 50. km – 2.44 km =
d. 0.0087 m2 / 0.0008 m =
3. Perform the following calculations and round your answers to the proper number of significant figures.
a. 12.450 g – 3.8000 g =
d. 50002 km2 / 123.0 km =
b. 5.69 x 103 m + 3.4 x 102 m =
e. [(11.45 – 11.08) / 11.08] x 100 =
c.
(0.00045 mm)(12.008 mm) =
4. A piece of tin is 1.098 cm long and 3.00 cm wide. What is the area of this piece of tin?
5. Perform the following density calculations, round your answers to the proper number of significant figures.
a. A piece of metal has a mass of 38.500 g and a volume of 10.2 mL. What is the density of the
metal?
b. A gas is found to have a density of 6.89 x 10–2 g/L and a mass of 5.2 x 10–3 g. What is the volume
of this sample of gas?
6. A student measures the boiling point of water to be 97.34 °C. The actual boiling point of water is
100.00 °C. What is the percent error for this measurement?
7. The mass of a weighing dish is 0.23 g. If the mass of lead and the weighing dish is 3.76 g, what is the
mass of the lead sample?
Name ____________________________________
Mid-Term Exam Review
Period _______
Unit 2: Chapter 7 and 9 – Ionic Compounds
Complete the following questions.
Key Vocabulary
ionic compound
ion
cation
anion
acid
Key Concepts






be able to tell an ionic compound from a molecular compound by looking at the formula or name
determine the charge on an ion based on the formula
understand how cations and anions are formed
write the name of an ionic compound given the formula (including acids)
write the formula of an ionic compound given the name (including acids)
recognize formulas for ionic compounds that are written incorrectly
Review Questions
1. What types of elements form cations? Is the charge on a cation positive or negative?
2. How does calcium go from the element Ca with no charge to the ion Ca2+ with a plus two charge?
3. Which statements are correct when magnesium and sulfur react to form an ionic compound?
a. Magnesium atoms lose 2 electrons and form cations.
b. Sulfur atoms form sulfide anions (S2-)
c. In the compound the ions are present in a one-to-one ratio.
4. What charge does copper have in the following compound: CuO?
5. Circle all of the following compounds that are ionic.
a. NaBr
c.
P4S2
b. N2O6
d. CaS
e. FeN
f.
g. BCl4
CuNO3
6. Name the following compounds based on their formulas.
a. Li2O
__________________________________________
b. Ca(OH)2
__________________________________________
c.
__________________________________________
FeF3
d. FePO4
__________________________________________
e. H2CO3
__________________________________________
7. Write the correct formulas for the following compounds.
a. zinc bromide
_____________________
b. copper(I) phosphide
_____________________
c.
iron(III) nitrate
_____________________
d. chromium(III) oxide
_____________________
e. nitrous acid
_____________________
8. Circle the formulas that are written incorrectly.
a. Fe3O2
c. MnP
e. CoCrO4
b. ZnCl
d. SnCN2
f. Pb3(PO4)2
Name _______________________________________
Period _________
Mid-Term Exam Review
Unit 3 Chapter 8 and 9 – Molecular Compounds
Complete the following questions.
Key Vocabulary
prefixes
molecular compound
valence electron
octet
Lewis dot formula
electron dot diagram
linear
trigonal planar
Bent
tetrahedral
polar molecule
Key Concepts
 know the seven diatomic elements
 recognizing molecular compounds
 writing names and formulas for molecular compounds
 understanding why atoms form covalent bonds
 recognizing exceptions to the octet rule
 drawing electron dot diagrams for individual elements
 drawing electron dot diagrams for compounds and predicting their shape
Review Questions
9. What are the seven diatomic elements?
10. What types of elements make up molecular compounds?
11. What is the octet rule? Why do atoms form octets?
12. Circle all of the following compounds that would be expected to have covalent bonds.
a. NaBr
c.
P4S2
b. N2O6
d. CaS
e. FeN
f.
g. BCl4
SiF
13. Name the following molecular compounds.
a. C2S3
___________________________________
b. SO3
___________________________________
c.
___________________________________
P6Br
14. Write the formulas for the following compounds.
a. phosphorus pentafluoride ________
c.
b. trisilicon mononitride
d. dinitrogen hexabromide _____
_________
15. What is a polar molecule? Give an example.
16. Draw the electron dot diagram for the following elements:
a. Mg
c.
Ga
b. Cl
d. Se
17. Draw the Lewis dot diagram for NH3.
18. Draw the Lewis dot diagram for CCl4 and predict its shape.
e. K
f.
Kr
boron disulfide
_____
Name _____________________________Date __________________Period __________
Midterm Review
Chapter 4 & 5 – Nuclear
Key Vocabulary
protons
electrons
atomic mass
neutrons
atomic number
mass number
isotope
Key Concepts





Rutherford – what did he discover and what did his model of the atom look like
properties of protons, neutrons and electrons
understand the two different types of isotope notation and what the different pieces tell you
how to determine the number of protons, neutrons and/or electrons based on given information
calculate the mass number based on given information
Review Questions – Answer the following questions on a separate piece of paper.
1. Review Rutherford’s Gold Foil Experiment & label all of the parts. Briefly summarize & draw a
sketch for his model of the atom. What were some of the problems with Rutherford’s model?
2. Review Bohr’s model of the atom. What evidence supported his model? What were some of
the problems with his model?
3. Write the symbol and determine the charge for an electron, proton and neutron.
4. Consider the following notation: 197
79 Au. What do the numbers stand for? How many protons,
neutrons and electrons are in an atom of this isotope?
5. Consider the following notation: iodine-126. What does the number represent? How many
protons, neutrons and electrons are in an atom of this isotope?
6. The element chromium has four naturally occurring isotopes. Use the relative abundance of
each to calculate the average atomic mass of chromium.
50
Cr  4.34%,
52
Cr  83.79%,
53
Cr  9.50%,
54
Cr  2.37%