Chemistry Semester 1 Final Review
A. Accuracy and Precision and Measurement
1. Write the measurement
2. Calculate the LOP next to each measurement. Show your work.
15
25
30
40
50
200
60
70
300
20
3
4
5
6
7
10
3. In the pictures above, you have mass and a volume. How would you calculated the density
of a substance? Write the equation and calculate the density with units.
4. Think about the density of solid lab and the density of carbon dioxide lab. How did we
determine the accuracy of our experiment? How did we determine the precision of our
experiment? Hint: These are calculation based….. not LOP.
5. Know how to identify if a property of matter is physical or chemical.
6. Know the similarities and differences between a chemical and physical change.
7. Specific Heat Questions: (This will be a short answer question on the final)
a. How much heat is absorbed when 62.5 g of water (specific heat 4.18 J/g˚C) is heated
from 25.7 ˚C to 98.7 ˚C?
b. How much heat is transferred from a hot chunk of metal to water (specific heat 4.18 J/g
˚C) when 25.4 g of water is raised from 37.4 ˚C to 45.3 ˚C?
c. What is the specific heat of an unknown metal weighing 47.5 g if 6384.2 J of energy
changes its temperature by 73.2 ˚C?
d. What was the initial temperature of 347.8 g of water after 26.8 g of copper, starting at
168.1 ˚C, raised the temperature of the water to 88.3 ˚C. The specific heat of copper is
0.385 J/g ˚C and the specific heat of water is 4.18 J/g ˚C.
e. What was the initial temperature of aluminum if 16.3 g of it heated 25.7 g of water from
30.5 ˚C to 55.7 ˚C? Given that the specific heat of aluminum is 0.900 J/g ˚C and the
specific heat of water is 4.18 J/g ˚C.
B. Basic Science Math Review:
1. Convert the following to scientific notation and then indicate the number of significant
figures.
a. 3427
d. 0.0000455
g. 0.00456
j. 2205.2
b. 172
e. 0.982 x 10-3
h. 0.000984
k. 0.0473
c. 3100.0 x 102
f. 3.03 x 10-1
i. 0.0114 x 104
l. 20.4 x 105
2. Round to 3 significant figures.
a. 468421
b. 80.49
c. 0.000486790
d. 1349.821
e. 0.0023978
f. 0.48927
3. Calculate the following answers and indicate the correct number of significant figures.
a. 3.95 x 102/1.5 x 106
e. (3.5 x 102)(6.45 x 1010)
b. 4.44 x 107 /2.25 x 105
f. (4.50 x 10-12)(3.67 x 10-12)
c. 1.05 x 10-26 / 4.2 x 1056
g. (2.5 x 109)(6.45 x 104)
d. 6.022 x 1023 / 3.011 x 10-56
h. (6.88 x 102)(3.45 x 10-10)
4. Using train tracks, convert the following numbers.
a. 1.98x1033 ps into centiyears
b. 6.27x1013 ng into kg
c. 7.49x10-7 km into pm
d. 6.84x10-2 cg into kg
e. 3.27x106 μL into ML
f. 8.43x103 kg/ML into lbs/cm3
(454 g = 1 lbs)
g. 4.58x102 ft into mm
(2.54 cm = 1 inch)
C. Atomic Structure and Periodic Trends
Average Atomic Mass = (% isotope 1 x amu isotope 1) + (% isotope 2 x amu isotope) + etc.
1. Atomic Mass Calculations
a. Oxygen has three isotopes, O-16 (15.994915 amu) at 99.757% abundance, O-17
(16.999132 amu) at 0.038% abundance, and O-18 (17.999160 amu) at 0.205%
abundance. Given these isotopes and percent abundances, what is the average atomic
weight of oxygen? Show your work!
b. Silver has two isotopes, Ag-107 (106.905093 amu) and Ag-109 (108.904756 amu).
Given the average atomic mass of silver from the periodic table, what are the isotopes’
percent abundances?
2. Complete the following chart.
3. What are the similarities and differences between a proton, neutron and electron?
4. What subatomic particles are need to find the atomic mass?
5. What subatomic particle changes in an isotope? An Ion?
6. Complete the following questions. (Makes sure you know the difference between an orbital
diagram, shorthand configuration, and longhand configuration.)
a. Write the abbreviated (shorthand) electron configuration for copper.
b. Write the un-abbreviated electron configuration for niobium.
c. Write the abbreviated electron configuration for chlorine.
d. Write the un-abbreviated electron configuration for technetium.
e. Complete the orbital notation for magnesium
f. Complete the orbital notation for sulfur
g. What is an orbital? How many electrons are found in an orbital?
h. How are the s, p, d, and f blocks different from each other? Hint: Think about their
orbitals and electron.
7. Write the Lewis Dot Diagram for a-f AND determine the charge for each element.
a. Barium
c. Rubidium
e. Germanium
b. Fluorine
d. Xenon
f. Selenium
8. Rank the following elements: potassium, sodium, and rubidium from lowest to highest
(smallest to largest) for each periodic trend:
a. Electronegativity
b. Ionization Energy
c. Atomic Radius
d. Ionic Radius
9. Complete the following Multiple Choice Questions
a. The plum pudding model was developed by:
i. Geoppert-Mayer
iii. Thomson
ii. Moseley
iv. Millikan
b. The oil-drop experiment is important because it helped to explain:
i. The positive charge of the proton
ii. The negative charge of the electron
iii. The existence of the nucleus
iv. The atomic number of different elements.
c. X-Ray diffraction was used to discover the atomic number of the elements by:
i. Moseley
iii. Millikan
ii. Chadwick
iv. Rutherford
d. James Chadwick discovered the _________.
i. Proton
ii. Neutron
iii. Electron
iv. Nucleus
e. Dmitry Mendeleev is often called the father of ______________.
i. The atom
ii. The electron
iii. The quark
iv. The periodic table
f. If an atom contains 26 electrons, how many energy levels will contain electrons?
i. 2
ii. 3
iii. 4
iv. 5
g. Electrons found in the same orbit must have
i. Opposite charge
iii. Opposite spins
ii. Different energy levels
iv. i, ii, and iii
h. What sublevels are occupied by electrons in the outer most energy level of argon atom?
i. 3s and 3d ii. 3s and 3p
iii. 2s and 3p
iv. 2p and 3d
i. Elements in period 3 are all alike in that they all have the same number of:
i. Protons
iii. Occupied Energy Levels
ii. Neutrons
iv. Electrons in their Valence Shell
C. Bonding and Naming
1. Molecules are fun!
a. Draw Lewis Structures for the following compounds:
SiCl4, CH3CH2CH2OH, PCl3, CO2, and BH3,
b. For the structures above,
i. What type (s) of intermolecular forces can be found in each of the molecules? .
ii. Identify if the molecules above are polar or nonpolar.
iii. What is the electron and molecular geometry of the Lewis Structures?
iv. Decide if the bonds within the molecules are nonpolar, polar covalent or ionic.
v. What is a dipole arrow and where does it point?
2. Please correct the chemical formulas in the box below by rewriting the formula.
a. NaSO4
b. K2NO2
c. Na(NO3)3
d. Mg2SO4
e. Mg(NO3)3
f. CaClO
g. NH4(C2H3O2)2
h. Ba(NO2)3
i. K2ClO4
j. BaClO3
k. NH4(ClO3)2
l. Ca2SO3
m. Na2ClO4
n. KO2
o. Al S3
p. BaCl
3. Describe what is happening in the graph above. Use your knowledge of intermolecular
forces to help you. Why does one molecule evaporate faster than another?
Butanol
4. For the following equations:
a. Write the chemical formula for the equation using subscripts.
b. Be able to balance the equation using coefficients
c. Be able to tell if the single and double displacements will react or not.
d. Be able to complete the total and net ionic equation.
e. Be able to decide which type of reaction is occurring (single
displacement, synthesis, decomposition, combustion, and double
displacement)
i.
ii.
iii.
iv.
v.
vi.
vii.
viii.
potassium carbonate + strontium sulfate
calcium hydroxide + magnesium chlorate
ammonium chromate + Copper (II) fluoride
barium + cobalt (II) carbonate 
silver chlorate + magnesium 
C12H22O11  C + H2O ( )
___C6H12O6  ___ CO2 + H2O ( )
FeCl2( ) + Na3PO4( )  Fe3(PO4)2(
)
+ ___ NaCl(
Methanol
Ethanol
Propanol
Hexane
Pentane
)