ftfanri< Sfc^.*.trr- /,er)r
Since D"ln:s d"\
r e'I '
mode'n o,vn ic
( o, -t
ho^ Se \,-fal
Atomic Energy Levels and Spectrum of Atomic Hydrogen
Which variable determines the electron energy in hydrogen atom according to Bohr's
model? What is the name of this variable?
PI lnftl quantuvn nrirlr be
When photons come out of the hydr
ldentification of an Unknown Organic Compound
(This assiqnment is due at the end of the laboratorv period for this laboratarv.l
Look up "pentane" and "acetic acid" in your textbook or on-line. Provide for
x to -tl
L sg 4,5
c. rr.llt5 va '^o'&s fu
J. 3.ib x lor ro'r.s t"
Lab Sec: _
Density of Unknown Liquid
1. Give the definition of density. Give at least two different examples of different units for
What is the SI unit for density?
Using back of this page, list things to do and to avoid when using a la
Problem Set 12
Ch. 5, pp 193-204
VSEPR, Orbital Hybridization, and Molecular Shape
We are going to rely on a variation of VESPR referred to as the KXP notation to aid us in determining the
geometry (3-dimensional shape) of molecules. This t
Problem Set 6
Ch. 2, pp. 85-99
Aufbau Principle and Periodic Properties
Develop a mnemonic diagram for the Aufbau principle that you can use if you dont have a periodic table.
Define the Periodic Law.
Describe how the major divisio
Problem Set 8
Ch. 3, pp. 124-137
Chemical Formulas, Naming, and Chemical Equations
Describe the principle difference in the nature of the chemical bonding in compounds referred to as ionic versus
those termed molecular.
Problem Set 9
Ch 4, pp. 145-162
Models of Bonding: Coulombs Law, Electronegativity, Polarity and Dipoles
1. Qualitatively describe the terms ionic, covalent, and metallic bonding.
2. What are some of the important characteristics of materia
Problem Set 7
Ch. 3 pp. 111-123
Molecular Weight, Mass, and Moles
1. What is the difference between molecular weight and formula weight? Use the following species as
examples in providing an explanation. Determine the appropriate value for
Problem Set 5
Ch. 2, pp. 80-84
Electron Spin, Polyelectronic Atoms, and the Periodic Table
1. How many electrons can occupy each orbital? What are their ms quantum numbers?
2. What is the origin of the fourth quantum number ms, and how is i
Problem Set 1
Ch. R, pp. 1-23
Ch. 1, pp. 30-41
Introduction to the Scientific Method and Dimensional Analysis
1. Describe the application of a Law, a Hypothesis, and a Theory, in the context of the 'Scientific Method'.
2. Using the definiti
Problem Set 29
Ch. 10, pp. 458-470
Chem Reactions & Stoichiometry: Oxidation-Reduction reactions & Calorimetry
Define: oxidation, reduction, oxidizing agent and reducing agent.
What is the oxidation state of each element in the follow
Problem Set 2
Ch. 1, pp 41-51
The Structure of the Atom.
Describe Dalton's "Atomic Theory". What sorts of laws and hypotheses were likely to be behind its origin?
Why do some of the symbols for the elements in the periodic table corre
Problem Set 3
Ch.2, pp. 57-72
Light Waves, Photons and the Bohr Model of the Atom
At the turn of the century, when scientists were trying to understand the structure of the atom, what was
considered unique and inexplicable about the ligh
Problem Set 11
Ch 4, pp. 169-182
Lewis Structures, Exceptions to Octets, Resonance, and Formal charge
Using the method of Lewis, indicate the number of valence electrons around each of the following atoms.
Problem Set 20
Ch. 8, pp. 327-337
Liquids and Solids: Intermolecular Forces, liquid structure, and solid structure
In each of the following sentences circle the correct word in parenthesis.
Strong intermolecular forces cause a substa
Problem Set 16
Ch. 6, pp. 251-272
Enthalpy, Hesss Law, Std. Enthalpy of Formation / Sources of Energy, Fuel and food.
1. Define standard enthalpy of formation, !Hf!.
2. Write a balanced chemical equation to represent the standard enthalpy o
Problem Set 21
Ch. 8, pp. 337-349
Liquids and Solids: Types of solids, metal structure, & networks.
What structural units make up solids; atoms, molecules, ions, or all three ?
List the four types of solids. Define each and provide an
Problem Set 22
Liquids and Solids:
Ch. 8, pp. 349-370
Ceramics, Semi-conductors, Molecular Solids, Ionics
Vapor pressure and State changes
Take two sodium atoms and form a bound system. Plot the valence energy levels and fill them with t
Problem Set 27
Ch. 10, pp. 435-442
Chem Rxns & Stoich: Solution composition, molarity
1. Describe the terms molarity, solute, solution, and solvent, as they might apply to a quantity of sodium
chloride dissolved in water.
2. Determine the m
Problem Set 24
Ch. 9, pp. 392-406
Stoichiometry: Balancing Chemical Eqns, limiting reagents; theoretical, actual, and percent yield
Balance the following equations:
a) C5H12 + O2 -> CO2 + H2O
b) NaOH + H2SO4 -> Na2SO4 + H2O
c) V2O5 + H2
Problem Set 18
Ch. 7, pp. 299-308
Kinetic-molecular theory: gas laws, distribution of molecular velocities, diffusion and effusion
m ! speed " # RT
1. What is meant by an "ideal gas?"
2. State the postula
Problem Set 17
Ch. 7, pp 282-299
Units of pressure and gas laws, and Dalton's Law
1. List the physical characteristics one might measure in describing a sample of a gas.
2. A system containing a gas was connected to a closed-end manometer.
Problem Set 15
Ch. 6 pp 243-251
Chemical Energy: Internal, PV, Heat and Work
What name is given to the study of the quantity of heat absorbed or given off by a chemical reaction?
Define the terms energy, kinetic energy, potential ener
Problem Set 26
Ch. 10, pp. 429-435
Chemical Reactions & Stoichiometry: Water & Electrolytes
1. What feature(s) of acids, bases, and salts is (are) the same when discussing them as electrolytes?
2. Place solutions of non-electrolytes, strong
Problem Set 10
Ch 4, pp. 163-169
Models of bonding: covalent bonds, bond energies, localized electrons
Using the covalent radii of Figure 2.36, estimate the lengths of the single bonds in the following
Problem Set 4
Ch. 2, pp. 73-79
Quantum mechanics and quantum numbers
4. Describe how the uncertainty principle of Heisenberg puts Bohr's model of the atom in doubt.
5. How do the atomic orbitals of quantum mechanics differ from the circular
Problem Set 14
Ch 5, pp 217-231
Molecular Orbital Theory - Homonuclear & Heteronuclear Diatomic Molecules
1. Provide both a Lewis dot structure and valence bond description of the bonding for the molecule O2, and
comment on the ob