AP Chemistry First Week Homework—This is the only time I’m going to type out your homework (our
textbooks will be assigned on Friday).
Monday 8/25/2014
1) A measurement is a quantitative observation involving both a number and a unit.
a) What is a qualitative observation? ____________________________________________________
b) What are the SI units for mass, length, and volume? ______________________________________
2) To determine the volume of a cube, a student measured one of the dimensions of the cube several times.
If the true dimension of the cube is 10.62 cm, give an example of four sets of measurements that would
illustrate the following.
a) imprecise and inaccurate data
_______________________________________________
b) precise but inaccurate data
_______________________________________________
c) precise and accurate data
_______________________________________________
3) How many significant figures are there in each of the following values?
a) 6.07 x 10-15
d) 300
b) 17.00
e) 301
c) 8 x 108
f) 300.
4) How many significant figures are in each of the following?
a) 100
d) 0.00480
2
b) 1.0 x 10
e) 4.80 x 10-3
c) 0.0048
f) 4.800 x 10-3
5) Round off each of the following numbers to the indicated number of significant digits, and write the
answer in standard scientific notation.
a) 0.00034159 to three digits
_______________________
2
b) 103.351 x 10 to four digits
_______________________
6) Use exponential notation to express the number 385,500 to
a) one significant figure
_______________________
b) three significant figures
_______________________
7) Evaluate each of the following, and write the answer to the appropriate number of significant figures.
a) 212.2 + 26.7 + 402.09 = ______________
b) 1.0028 + 0.221 + 0.10337 = ___________
c) 52.331 + 26.01 – 0.9981= ____________
8) Perform the following mathematical operations, and express each result to the correct number of
significant figures.
0.102 x 0.0821 x 273
a)
= ______________________
1.01
b) 0.14 x 6.022 x 1023 = ______________________
2.00 x 106
c)
= ______________________
3.00 x 10−7
Tuesday 8/26/2014 (also prepare for safety “test” on Wednesday)
1) When a marble is dropped into a beaker of water, it sinks to the bottom. Which of the following is the
best explanation?
a) The surface area of the marble is not large enough to be held up by the surface tension of the water.
b) The mass of the marble is greater than the mass of the water.
c) The marble weighs more than an equivalent volume of water.
d) The force from dropping the marble breaks the surface tension of the water.
e) The marble has greater mass and volume than the water.
Justify your choice.
2) Perform the following unit conversions.
a) 908 oz = ______________ kilograms
b) 12.8 L = ______________ gallons
c) 4.48 lb = ______________ grams
3) Mercury poisoning is a debilitating disease that is often fatal. In the human body, mercury reacts with
essential enzymes leading to irreversible inactivity of these enzymes. If the amount of mercury in a polluted
lake is 0.4 μg Hg/mL, what is the total mass in kilograms of mercury in the lake? (The lake has a surface
area of 100 mi2 and an average depth of 20 ft.) Show your work for credit.
4) Convert the following Kelvin temperatures to Celsius and Fahrenheit degrees.
a) 233 K = _______ C = _______ F
b) 4 K = _______ C = _______ F
5) The density of pure silver is 10.5 g/cm3 at 20°C. If 5.25 g of pure silver pellets is added to a graduated
cylinder containing 11.2 mL of water, to what volume level will the water in the cylinder rise?
6) Classify each of the following mixtures as homogeneous or heterogeneous.
a) Potting soil
b) Window glass
c) Granite
7) Classify each of the following as a mixture or a pure substance.
a) Blood
d) Brass
b) The oceans
e) Uranium
c) Iron
f) Leather
g) Table salt
Wednesday 8/27/2014
1) Dalton assumed that all atoms of the same element were identical in all their properties. Explain
why this assumption is not valid.
2) What happens to the ratio of the mass number to the atomic number of a stable isotope, as stable
isotopes become heavier?
3) What is the trend in metallic character (increasing/decreasing) as you go down group 4A?
4) What is the trend in metallic character (increasing/decreasing) as you move from left to right
across a period in the periodic table?
5) Now, what do you think “metallic character” means? ______________________________________
6) What is the difference between ionic and covalent bonding?
7) What is the difference between an anion and a cation?
8) Do salts (ionic compounds) form molecules? Explain. ____________________________________
9) If 1 L of H2 reacts with 1 L of Cl2 at the same temperature and pressure, what volume of HCl is
formed?
10) A sample of sulfuric acid contains 2.02 g hydrogen, 32.07 g sulfur, and 64.00 g oxygen. How many
grams of sulfur would be present in a second sample of sulfuric acid if it contained 7.27 g of
hydrogen?
11) In a combustion reaction, 46.0 g of ethanol reacts with 96.0 g of oxygen to produce water and
carbon dioxide. If 54.0 g of water is produced, what mass of carbon dioxide is produced?
12) What are the symbols of the following elements?
a. Sodium
___________
b. Radium
___________
c. Iron
___________
d. Manganese ___________
e.
f.
g.
h.
Chlorine
___________
Sulfur
___________
Oxygen
___________
Phosphorous___________
13) Classify the following as metals, metalloids, or nonmetals.
a. Mg
_____________________
f. Br
b. Bi
_____________________
g. Element #17
c. B
_____________________
h. Element # 63
d. Ge
_____________________
i. Element #2
e. Am
_____________________
j. Element #55
_____________________
_____________________
_____________________
_____________________
_____________________
14) Color the periodic table to the right, giving
each group its own color according to the
list below. Use the list as a key by
circling/shading/highlighting each group
with the color you used.
a. Alkali metals
b. Alkali earth metals
c. Halogens
d. Noble gases
e. Transition metals
f. Inner transition metals
g. Other metals
h. Other nonmetals
15) Write the atomic symbol for an isotope where Z = 20 and the number of neutrons = 27. __________
16) How many protons and neutrons are in the nucleus of one atom of…
a. Cesium-133? p = ______
n = ______
b. Iron-57?
p = ______
n = ______
17) How many protons and electrons (total and valence) are in each of the following ions?
a. Ba2+
p = ______
total e= _______
valence e = ______
3b. N
p = ______
total e= _______
valence e = ______
3+
c. Co
p = ______
total e= _______
valence e = ______
18) Which groups of elements typically gain electrons when they become ions? _____________ Which
groups typically lose electrons when they become ions? ___________
Thursday 8/28/2014 Pg. 72-80
Fill out the following table.
Name
Formula
NaBr
Strontium fluoride
CaS
Potassium nitride
Hg2O
Tin (II) nitride
CoS
Mercury (II) oxide
CsF
Ag2S
TiO2
Zinc Chloride
Tin (IV) bromide
Calcium phosphide
KMnO4
K2Cr2O7
Chromium (III) hydroxide
Magnesium cyanide
Diboron trioxide
Arsenic Pentafluoride
CuI
NaOCl
NH4NO3
HC2H3O2
Pb3(PO4)2
KClO3
SnO2
HClO
SO42SeO42H2TeO4
HClO3
HIO3
Sulfur difluoride
Sodium dihydrogen phosphate
Ammonium acetate
Disulfur dichloride
Ammonia
Sodium oxide
Sodium peroxide
Nitrous acid
Iodous acid
Zinc sulfide
Silicon dioxide
Perbromic acid
Each of the following compounds is incorrectly named. Circle the part that makes it incorrect, and write the
correct name for each formula. There may be more than one error in some of the names.
FeCl3
Iron chloride
Correct name: _____________________________________
NO2
Nitrogen (IV) oxide
Correct name: _____________________________________
Mg(C2H3O2)2 Magnesium diacetate
Correct name: _____________________________________
H2S
Sulfuric acid
Correct name: _____________________________________
FePO4
Iron (II) phosphide
Correct name: _____________________________________
Friday 8/29: Go over any questions from this homework set that you may have had trouble with. The
answers are online and our Ch 1/2 Exam is on W 9/3. We will review T 9/2.