Name:______
Chemistry 20 – Final Exam
January 25th, 2011
Part A - Matching
Match each of the statements from the first column with a term in the second column. Each statement is worth one mark.
Name:______
_____ explains that the volume of a gas decreases as
pressure increases.
_____ a compound with a charge.
_____ the central part of the atom.
_____ a chemical reaction that produces heat.
_____ holds compounds together by sharing electrons.
_____ a reactant that gets completely used up during a
reaction.
_____ substances that form during a chemical reaction.
_____ explains how an increase in the amount of a gas
produces an increase in volume.
_____ a negatively charged particle that is part of the
atom.
_____ substances that get used up during a chemical
reaction.
_____ the process of using a chemical equation to
predict the amount of products forming or
reactants being used up.
_____ a structure made up of more than one atom.
_____ describes how an increase in the temperature of a
gas increases its volume.
_____ a summary of the substances involved in a
chemical reaction.
_____ a formula that contains the simplest whole
number ratio of atoms for a compound
_____ a neutral particle within the nucleus.
_____ a solid that forms when two solutions are mixed.
_____ atoms of the same element with differing
numbers of neutrons.
_____ substance that consists of two or more elements.
_____ the mass of 6.02 x 1023 atoms or molecules.
A. Avagadro’s law
B. Boyle’s law
C. Charles’ law
D. chemical equation
E. compound
F. covalent bond
G. Dalton’s law of Partial Pressure
H. electron
I. empirical formula
J. endothermic
K. exothermic
L. Ideal Gas law
M. ionic bond
N. isotopes
O. limiting reagent
P. molar mass
Q. mole
R. molecule
S. neutron
T. nucleus
U. polyatomic ion
V. precipitate
W. products
X. proton
Y. reactants
Z. stoichiometry
Name:______
Name:______
Part B – Problems
Answer each of the following problems. Be sure to show all formulas, significant figures, and units where necessary.
1. Silver is found in two isotopes. 51.8 % of silver on earth is 47107Ag while 48.2 % is 47109Ag. Calculate the average atomic mass of silver from these values? Put to 2 decimal places.
2. Write the full electron configuration for:
a) Al
b) Ca2+
3. Write the electron configuration in noble gas notation for:
a) Br
b) Co
4. Show the full electron configuration in orbital notation for:
a) O2-
b) Ti
5. List one atom, one cation, and one anion that could have the electron configuration 1s22s22p63s23p6?
6. Write the names of the following compounds. If naming an acid, use acid rules.
a) K2O ______
b) SnS2 ______
c) Ag2SO4 ______
d) P2S3 ______
e) HI ______
f) NH4NO2 ______
g) Ca(OH)2 ______
h) S4N2 ______
i) FePO4 ______
j) HNO2 ______
7. Write the formulas for the following:
a) calcium phosphide ______
b) gold (III) nitrate ______
c) dinitrogen pentoxide ______
d) acetic acid ______
e) copper (II) iodide ______
f) calcium carbonate ______
g) ammonium phosphate ______
h) copper (I) fluoride ______
i) sodium bromide ______
j) sulfurous acid ______
8. Draw the lewis structures for the following:
a) AlCl3 b) CF4
c) Li2S d) C2H2
9. Balance the following equations.
a) BaCl2 + (NH4)2CO3 à BaCO3 + NH4Cl
b) CuSO4 + Fe à Fe2(SO4)3 + Cu
c) Al + NaOH + H2O à NaAl(OH)4 + H2
10. Classify each equation below (even if no reaction takes place), predict the products, and balance them.
a) Ni + FeSO4 à
b) H3PO4 + Al(OH)3 à
c) CoBr à
11. Will mixing a barium nitrate solution and a lithium sulfate solution produce any precipitates? Write the balanced chemical equation and the balanced net ionic equation to solve this problem. Show your states! (1 mark for reactants, 2 for products and states, 1 for balancing, 1 for balanced net ionic equation)
12. Consider the reaction:
3 FeCl2 + KNO3 + 4HCl à 3 FeCl3 + NO + 2H2O + KCl
a) If 0.750 moles of FeCl2 react with excess KNO3 and HCl, how many moles of H2O will form?
b) If 20.0 g of FeCl3 are produced, what mass of NO will be produced?
c) If 50.0 g of FeCl2 and 14.0 g of KNO3 are mixed with excess HCl, which is the limiting reagent? What mass of the excess substance will remain after the reaction takes place (hint – not HCl)?
13. What is the percent composition of the elements in lead (II) oxide? Put percents to 2 decimal places.
14. What is the empirical formula of a compound with 70.0% Fe and 30.0 % O.
15. A sample of gas has a volume of 235 mL when the pressure is
133 kPa. What will be the volume if the pressure is increases by 50.0 kPa?
16. 2.35 g of chlorine gas are collected over water at 30.0°C. If the volume of the gas is 10.0L, what is the total pressure?
17. Choose 4 of the following notable chemists and explain their contributions to chemistry. Each description is worth 1 mark.
Name:______
a) Aristotle
b) Democritus
c) John Dalton
d) JJ Thomson
e) Demitri Mendeleev
f) Earnest Rutherford
g) Robert Millikan
h) Amedeo Avogadro
Name:______