Supplementary Material to accompany
A Final Exam Review Activity Based on the Jeopardy Format
Michael V. Keck
Division of Physical Sciences, Emporia State University, 1200 Commercial St., Emporia, KS 66801
Contents
1) Sample game board
2) Answers to questions on sample game board
3) Additional game questions
4) Answers to additional questions
1) Sample game board (point values to be assigned by instructor).
Electrochemistry
Kinetics
Equilibrium
Weak acids/bases
Transition Metals
The sign of G for a A homogeneous
solid solution of 2
spontaneous
or more different
reaction.
metals.
Type of reaction in
which electrons are
gained.
The kinetic
parameter
represented by the
symbol "lower case
k".
The equilibrium
constant expression
for the reaction
A(s) <===> B(g)
In the reaction
Fe(s) + Cu2+ ----->
Rate law for a
chemical reaction
that is first order in
A and zero order in
B.
The effect a catalyst What is the pKa of a
has on the
weak acid with a Ka
equilibrium
of 1.0 X 10-5 ?
constant.
The amount of
energy required to
raise the
temperature of 1 g
of material by one
Kelvin.
True or False: The One equivalent of
value of Keq
OH- is added to a
weak acid. The pH
depends on the
of the solution is:
temperature.
>7, <7, =7 ?
State the second law The d orbital
of thermodynamics. splitting pattern for
an octahedral
complex.
Fe2+ + Cu(s), which
is the oxidizing
agent?
The reaction that
The name given to
has been defined as the slowest step in a
having an E° of 0.00 multi-step reaction.
V.
The conjugate base
of H3O+.
Thermodynamics
The two common
geometries adopted
by 4 coordinate
metal complexes.
Sign of G if the net The energy required The sign of G° if
reaction potential is to attain the
Keq = 1000.
transition
state
in
a
-0.500 V.
reaction.
The easiest way to
Numerical value of Term given to a
calculate the pH of a G°f of H2 (g) at 25 metal complex with
buffered solution.
unpaired electrons.
°C and 1 atm
pressure.
The relationship
between standard
and non-standard
state EMFs.
During a titration,
you are at the point
at which pH = pKa.
How far through the
titration are you?
The order of a
The direction of
reaction for which a equilibrium shift for
plot of 1/[A] vs.
A(g) <==> 2B(g) if
time is linear.
the volume is
decreased.
An endothermic
reaction is
spontaneous. What
is the sign of S?
Give the complete
IUPAC name for the
compound
K3[Fe(CN)6].
2
3
2) Answers to questions on sample game board.
Electrochemistry
Kinetics
reduction
rate constant
Cu2+
Rate = k[A]
2H+(aq) + 2e- --->
H2 (g)
(+)
Nernst Equation
rate-determining
step
activation energy
Equilibrium
K = [B]
(or pressure of B)
none
True
(-)
2nd (wrt A)
Weak acids/bases
H2O
pKa = 5.00
>7
use the HendersonHasselbalch eqn.
Thermodynamics
(-)
specific heat
The entropy of the
universe is
increasing. (or
something along this
line
zero
Transition Metals
alloy
tetrahedral
square planar
_ _
_ _ _
paramagnetic
exactly half-way
left
(+)
potassium
tetracyanoferrate
(III)
4
3) Additional Questions
Units and measurements
100
What is the SI unit for mass?
200
What is the boiling point of water, stated in Kelvins?
300
What is the definition of density?
400
What is the prefix which means one millionth (10-6)?
500
How many significant figures are in the number 0.013070 ?
Ions and Formulas
+
100 Name NH4 .
200
What is the symbol for the oxide ion?
300
400
What is the formula for aluminum sulfate?
Name P4O10.
500
Go to the board and write the name for FeBr2.
Formulas and Stoichiometry
100
200
What is the numerical value for Avogadro's number, expressed to 4 significant figures?
What is the empirical formula for ethane, C2H6 ?
300
How many moles of water are formed when one mole of methane burns?
400
What is the mass of water formed upon combustion of one mole of hydrogen gas?
500
One mole of sodium metal reacts with one mole of chlorine gas to form NaCl. Which
reagent is limiting (if any)?
5
Intermolecular Forces
100
Name four major types of intermolecular forces.
200
Name 3 properties of condensed phases which depend upon intermolecular forces.
300
What is the strongest type of intermolecular force which can exist between neutral
molecules?
400
Which types of intermolecular forces are present in liquid carbon monoxide?
500
Which compound has a higher boiling point, HF or HCl?
Reactions in Aqueous Solution
100
Name the class of compound which binds to hydrogen ions in aqueous solution.
200
300
What is the name for the chemical process in which electrons are gained?
What products are formed in the reaction between Na2CO3 (aq) and CaCl2 (aq)?
400
What are the products formed when aqueous solutions of Ca(OH)2 and HClO4 are
mixed?
500
What is the oxidation state of nitrogen in the nitrite ion?
Gases and Gas Laws
100
State the ideal gas law, and define all symbols.
200
What happens to the pressure of a gas that is heated at constant volume?
300
One mole of gas has a volume of 20 L under a given set of conditions. Another 0.25
mole of gas is added. What is the new volume? (assume T and P remain constant)
400
20 g of He and 20 g of Ne are mixed under conditions in which the total pressure is 1
atm. What is the partial pressure of the helium?
500
What two physical properties of a gas are ignored in the ideal gas law but accounted for
in the van der Waals equation?
6
Thermochemistry
100
Define a formation reaction.
200
What is the sign of H for an endothermic reaction?
300
State Hess' Law.
400
If it takes 10 J to raise the temperature of a 10 g object by 1 °C, what is the specific heat
of the object?
Is the reaction H2 (g) -----> 2 H (g) exothermic or endothermic?
500
Atomic Structure
100
Name the three major particles that comprise an atom.
200
The observation of line spectra for atoms is a direct result of ?????????
300
Which quantum number defines the energy of the electron in a hydrogen atom?
400
Which orbitals are partially filled for the transition metals?
500
Name the quantum numbers required to completely specify an electron.
The Periodic Table
100
The first periodic tables were constructed on the basis of ????????
200
Which element in period 3 has the highest ionization energy?
300
Which group on the periodic table has an s2p5 valence electron cofiguration?
400
Which element has the larger second ionization energy, Na or Mg?
500
Which has the larger atomic radius:
S, Cl, F ?
7
Bonding
100
In one sentence, describe the difference between an ionic bond and a covalent bond.
200
Which is the most electronegative element on the periodic table?
300
The driving force which allows ionic solids to be stable is called ???
400
Jeopardy Challenge: Send one member of the team to the board to draw the Lewis dot
structure of PCl3.
500
What is the electron geometry about an atom that is sp3 hybridized?
Liquids and Solids
100 Which is larger, Hvap or Hfus?
200
Name two types of unit cell.
300
What property of a liquid is defined as a resistance to increase in surface area?
400
Define the boiling point of a substance.
500
Consider water and ammonia, both at 25 °C. Which has the greater vapor pressure?
Strong Acids and Bases
100
The algebraic definition of pH.
200
300
The pH of a 0.010 M hydrobromic acid solution.
Definition of the Kw , and its numerical value at 25 °C.
400
Concentration of hydroxide ion in a solution of pH 13.0.
500
The pH at the endpoint of a strong acid/strong base titration.
8
Nuclear
100
The highest atomic number possible for a stable nucleus.
200
The type of radioactive decay in which helium nuclei are emitted.
300
The general type of nuclear reaction which is energetically favorable for the smaller
elements.
400
Minimum amount of material required for a self-sustaining nuclear reaction.
500
The energy required to break a nucleus into its constituent protons and neutrons.
Basic Organic
100
Name the following molecule:
O
200
The type of functional group represented in the following structure: R
300
The hybridization of the carbon atoms in acetylene (ethyne).
400
The type of atomic orbital involved in a  bond.
500
A general term describing organic molecules containing delocalized  electrons in
"rings".
NH2
9
4) Answers to additional questions
Units and measurements
100
kilogram
200
373.15 K (373 is OK)
300
mass/volume
400
micro ()
500
5
Ions and Formulas
100
ammonium ion
200
300
O2Al2(SO4)3
400
tetraphosphorous decaoxide
500
iron (II) bromide (or ferrous bromide)
Stoichiometry
200
6.022 X 1023
CH3
300
2
400
18 g (H2 + 1/2 O2 ------> H2O, MW water = 18 g/mol)
500
sodium
100
(CH4 + 2 O2 -----> 2 H2O + CO2)
(Na + 1/2 Cl2 ------> NaCl (s) )
10
Intermolecular Forces
100
ionic, dipole-dipole, hydrogen bonds, London dispersion forces
200
boiling point, melting point, vapor pressure, viscocity, capillary action
300
hydrogen bonds
400
LDF, dipole-dipole
500
HF (because it is capable of hydrogen bonding)
Reactions in Aqueous Solution
100
base
200
300
reduction
solid calcium carbonate and aqueous sodium chloride (CaCO3 (s) + NaCl (aq)
400
calcium perchlorate and water
500
+3
Gases and Gas Laws
100
PV = nRT (pressure, volume, number of moles, gas constant, temperature)
200
increases
300
25 L (add 25% more gas, pressure increases by 25 %)
400
5/6 atm, or 0.84 atm (5 moles He, 1 mole Ne, for six moles total, 5/6 of which is He)
500
intermolecular forces, size of gas molecules
11
Thermochemistry
100
the formation of a compound from the elements in their standard states
200
positive (+)
300
For any reaction which can be considered as the sum of two or more other reactions, the
enthalpy change for the overall reaction is the sum of the enthalpy changes for each of
the individual steps.
400
1 J / g·K
500
endothermic
Atomic Structure
100
proton, neutron, electron
200
quantization of energy
300
principle quantum number (n)
400
d orbitals
principle (n), angular momentum (l), magnetic (ml), spin (ms)
500
The Periodic Table
100
trends in chemical reactivity
200
argon
300
halogens (also refered to as group 17 or group VII A)
400
Na
500
Sulfur
12
Bonding
100
covalent bond -- shared electrons; ionic bond -- electron transfer and electrostatic
attraction
200
Fluorine
300
Lattice energy
400
Cl
P
Cl
Cl
500
tetrahedral
Liquids and Solids
100 Hvap
200
simple cubic, body centered cubic, face centered cubic
300
surface tension
400
temperature at which vapor pressure equals atmospheric pressure
500
ammonia
(weaker intermolecular forces)
Strong Acids and Bases
100
-log[H+]
200
300
2.0
Kw=[H+][OH-] = 1.00 x 10-14 (could also be Kw = Ka x Kb)
400
0.10 M
500
7.00
13
Nuclear
100
83
200
alpha
300
fusion
400
critical mass
500
nuclear binding energy
Basic Organic
100
propene
200
amide
300
sp
400
atomic p orbital
500
aromatic
14