Chemistry
Lab Safety and Common Lab Tools
1. There are 3 things in the classroom used for our safety. What are they and describe
how they are used.
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2. True or False? If it is false, tell which tool it is describing and what is the true
definition of a beaker.
The beaker is used to store, run rxns, and estimate a volume. It is not used for
specifically measuring liquids because it is not accurate.
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3. What tool is used to store or run rxns and is neither accurate nor precise?
____________________
4. What tool is used to measure solids and not liquids? It can range from very accurate to
sort of accurate. _________________
5. True or False? If it is false, tell which tool it is describing and what is the true
definition of a pipette.
Pipettes are used to measure liquids and can be very accurate or very inaccurate.
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7. What is a volumetric flask?
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8. What tool is used to measure volumes or liquids and is very accurate when read
correctly? ____________________________________
Accuracy, Precision, and Sig Figs
1. How many sig figs do the following have?
0.000000006 ___________
35645
_____________
360000
_____________
8.0000000009 ___________
360000.
______________
46.456 + 8.9
___________
35.73 x 745.5457
___________
2. What is the difference between accuracy and precision?
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3. You have 5 numbers: 0.234, 350. , 0.89, 0.9999, 0.78. What is your correct number of
sig figs? ____
Physical vs. Chemical Changes and Properties
1. Give the 10 physical properties and their definitions.
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
2. What is a physical change? Give examples.
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3. What is a chemical change? Give examples.
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The Periodic Table and Periodic Trends
1. Name all groups of the periodic table.
Group 1:
Group 2:
Groups 3-13:
Group 17:
Group 18:
2. What are the 3 trends? Draw their directions. BONUS: Definitions?
3. Rank the following from greatest to least by first ionization energy: C, F, Ag, Li
__________>___________>__________>_____________
Ba, Ba2+
F, F –
4. Rank the following from least to greatest by electronegativity: C, F, Ag, Li
__________<___________<__________<_____________
Ba, Ba2+
F, F –
5. Rank the following from greatest to least by atomic radius: C, F, Ag, Li
__________>___________>__________>_____________
Ba, Ba2+
F, F
-
6. Ions are: ______________________________________________________________
Isotopes are: ___________________________________________________________
Nomenclature
Name
Formula
1.
CH3CO2
2.
ClO3.
ClO24.
ClO35.
ClO46.
CN7.
HCO28.
OH9.
NO210.
NO311.
MnO412.
SCN13.
NH4+
14.
C2O4215.
CO3216.
CrO4217.
SO4218.
SO3219.
C4H4O6220.
O2221.
PO3322.
PO4323.
HPO4224.
H2PO425.
HSO426.
NH3
27.
H2O2
Cyanide
28.
Phosphite
29.
Permanganate
30.
Oxalate
31.
Hydroxide
32.
Nitrate
33.
Hydrogen Phosphate
34.
Hydrogen Peroxide
35.
Chlorate
36.
Acetate
37.
Ammonium
38.
Hypochlorite
39.
Ammonia
40.
Hydrogen sulfate
41.
Peroxide
42.
Tartrate
43.
Sulfite
44.
Carbonate
45.
Nitrite
46.
Formate
47.
Perchlorate
48.
Sulfate
49.
Phosphate
50.
Chromate
51.
Thiocyanate
52.
Chlorite
53.
Hydrogen phosphite
54.
VSEPR and Polarity and Lewis Structures
1. Draw the Lewis structure, NOT LEWIS DOT STRUCTURE, for the following
a. CH3COOH
b. CH3F
c. BCl3
d. PBr5
e. CH3NH2
2. VSPER and Polarity: draw the VSPER structures and determine if they are polar or
nonpolar.
-always related to ________________
-intermolecular forces:
-_______________ bonds
-H + F, H + O, H + N
-circle: real or not real
-intramolecular forces:
a. nitrogen trifluoride
b. CH2F
c. boron trichloride
d. PBr5
e. water
Empirical and Molecular Formulas
.1 round _____
.9 round _____
.5 round _____
Practice:
1. Molecular and Empirical Formulas? Molecular molar mass of 294.30 g/mol.
57.14% C
6.16% H
9.52% N
27.18% O
2. Molecular and Empirical Formulas? Molecular molar mass of 78.12 g/mol.
92.2% C
7.8% H
3. Determine the molecular formulas to which the following empirical formulas and
molar masses pertain.
a. SNH 188.35 g/mol
b. NPCl2 347.64 g/mol
c. CoC4O4 341.94 g/mol
d. SN 184.32 g/mol
4. Give the empirical formula for each of the compounds represented below:
a. N2O4
b. C3H6
c. P4O10
d. C6H12O6
5. There are two binary compounds of mercury and oxygen. Heating either of them
results in the decomposition of the compound, with oxygen gas escaping into the
atmosphere while leaving a residue of pure mercury. Heating 0.6498 g of one of the
compounds leaves a residue of 0.6018 g. Heating 0.4172 g of the other compound results
in a mass loss of 0.016 g. Determine the empirical formula of each compound.
6. A sample of urea contains 1.121 g N, 0.161 g H, 0.480 g C, and 0.640 g O. What is the
empirical formula of urea?
7. A compound that contains only nitrogen and oxygen is 30.4% N by mass; the molar
mass of the compound is 92 g/mol. What is the empirical formula of the compound?
What is the molecular formula of the compound?
8. A compound containing only sulfur and nitrogen is 69.6% S by mass; the molar mass
is 184 g/mol. What are the empirical and molecular formulas of the compound?
9. Adipic acid is an organic compound of 49.31% C, 43.79% O, and the rest hydrogen. If
the molar mass of Adipic acid is 146.1 g/mol, what are the empirical and molecular
formulas for adipic acid?
10. Maleic acid is an organic compound composed of 41.39% C, 3.47% H, and the rest
oxygen. If 0.129 mol of maleic acid has a mass of 15.0 g, what are the empirical and
molecular formulas for maleic acid?
11. Many homes in the rural America are heated by propane gas, a compound that
contains only carbon and hydrogen. Complete combustion of a sample of propane
produced 2.641 g of carbon dioxide and 1.442 g of water as the only products. Find the
empirical formula of propane.
12. A compound contains only C, H, and N. Combustion of 35.0 mg of the
compound produces 33.5 mg CO2 and 41.1 mg H2O. What is the empirical
formula of the compound?
13. Cumene is a compound containing only carbon and hydrogen that is used in the
production of acetone and phenol in the chemical industry. Combustion of 47.6 mg
cumene produces some CO2 and 42.8 mg water. The molar mass of cumene is
between 115 g/mol and 125 g/mol. Determine the empirical and molecular formulas.
14. A compound contains only carbon, hydrogen, and oxygen. Combustion of the
compound yields 16.01 mg CO2 and 4.37 mg H2O. The molar mass of the compound
is 176.1 g/mol. Empirical and molecular formulas?
Predicting Products, Redox, and the Activity Series: Predict the products given the reactants. Tell
me what type of reaction it is, and if it’s a molecular, complete ionic(if possible), and net ionic(if
possible) equation. If there is no equation, write N/A. Balance. Show the states. If it’s a redox,
tell me the active metal, the oxidized and reduced elements, and use the lines when balancing. If
there is no reaction made, don’t do the above. Just show me there’s no reaction and explain why.
1. Ca(NO3)2(aq) + Na3PO4(aq)
?+?
2. lead(II) nitrate + potassium iodide
3. Pb(s) + H3PO4(aq)
4. C5H9O + O2
?+?
H2(g) + Pb3(PO4)2(s)
CO2 + H2O
5. C2H6 + O2
?+?
6. MnO 4-(aq) + CH3OH(l)
7. Cr2O72-(aq) + Fe2+(aq)
HCO2H(l) + Mn2+(aq)
Cr3+(aq) + Fe3+(aq) + H2O(l)
8. Magnesium is reacted with hydrochloric acid to form magnesium chloride(aq) and
hydrogen gas. Balance.
9. I have two beakers. Beaker 1 has a zinc nitrate solution. Beaker 2 has an iron(II) nitrate
solution. I put a strip of iron into B1 and zinc strip into B2. Rxn?
10. Sodium hydroxide and sulfuric acid are placed in a beaker. Rxn?
11. K2S(aq) + N2(NO3)2(aq)
KNO3(aq) + NiS(s)
12. Ca(s) + Na2SO4(aq)
rxn?
Stoichiometry
1. If you have 100. g of sodium and 50.0 g of water to perform the following reaction,
how many grams of sodium hydroxide will you produce?
Na(s) + H2O(l) -> NaOH(aq) + H2(g)
2. You are a chemist performing an oxidation reduction reaction in which 20.4 mL of a
0.5 M solution of copper(II) nitrate is added to a 1.3 g sample of zinc metal. Find the
molecular formula, the balanced chemical reaction, the limiting reagent, the theoretical
yield in grams of the solid product, the grams of the excess reagent left over after the
reaction occurs, and the percent yield if in the reaction you actually produced 0.8 g of the
solid product.
Gas Laws
1. What are the diatomic elements?
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2. Consider the rxn between 50.0 mL of CH3OH(l) (d=0.850 g/mL) and 22.8 L of O2 at
27oC and a pressure of 2.00 atm. The products are CO2(g) and H2O(g). How many moles
of H2O are formed?
3. A person accidentally swallows a drop of liquid oxygen, which has a density of 1.149
g/mL. Assuming the drop has a volume of 0.050 mL, what volume of gas will be
produced in the person’s stomach at body temperature?