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
Game3 Questions
Game3 Answers
Game3 Questions
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
500
of the object?
Is the reaction H2 (g) -----> 2 H (g) exothermic or endothermic?
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 ?
2
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.
3
Answers to Game3 Questions
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
4
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
5