© Dr. E. Neeland. Not to be copied, used, or revised without express written permission from the copyright owner
Chemistry 121
Professor:
Dr. E. Neeland, Fipke Building, Office F-354, e.neeland@ubc.ca
Course Title:
Atomic and Molecular Chemistry
Prerequisites:
CHEM 12 and a MATH 12 (Principles of Mathematics or Pre-Calculus)
Lectures:
Clickers:
Section 002 – 8:00-9:20 M, W
8:30-9:20 F
No
Extra Help:
My office, student learning, Chemistry Course Union (CCU) Sci-233b
Laboratory:
Week of September 17
Useful Stuff:
1.
2.
3.
4.
Evaluation:
Quizzes.......................................... 10%
Midterm 1, Sept. 28........................ 10%
Midterm 2, Oct. 29*........................ 10%
Midterm 3, Nov. 19* ...................... 10%
Laboratory Work.............................20%
Final Exam..................................... 40%
100%
ASC-140
ASC-140
th
th
Petrucci et al., General Chemistry, Principles and Modern Applications, 10 Ed., (2011)
UBC Okanagan Chemistry 121/123 Lab Manual
Blackboard Learning website (connect.ubc.ca)
Inexpensive scientific calculator (not programmable) for tests
N.B.
Failure to attend a lab or the handing in
of work after a prescribed deadline will
result in no marks for that lab or work.
*Carrot Rule: For example, increase your MT3 % over that of MT2 % by y% (y≥10)
[y - 3.75]
= x (new MT2 : MT3 ratio as 1:x)
3.75
To receive credit for Chemistry 121 – Failure to obtain at least 50% in BOTH the lecture
and lab sections of the course separately will result in a maximum mark of 48%.
Absences:
Invalid reasons for missing a test/lab: bus was late, concert, a wedding, slept in, broke up with
boy/girlfriend, headache, hockey game on TV and other assorted trivial non-reasons.
Valid reasons for missing a test/lab: verifiable sickness, death, car accident, etc...
Disabilities:
If you require disability related accommodations to meet the course objectives please contact the
Coordinator of Disability Resources. For more information about Disability Resources or about
academic accommodations: http://web.ubc.ca/okanagan/students/disres/welcome.html
Academic Integrity: Students are expected to know, understand, and follow the codes of conduct regarding academic
integrity. This means submitting only original work done by you and acknowledging all sources of
information or ideas and attributing them to others as required. This also means you should not
cheat, copy, or mislead others about what is your work. Violations of academic integrity will lead to
harsh sanctions like a failing grade or mark of zero on the assignment or even in the course.
More details: http://web.ubc.ca/okanagan/faculties/resources/academicintegrity.html
: http://okanagan.students.ubc.ca/calendar/index.cfm?tree=3,54,111,0
© Dr. E. Neeland. Not to be copied, used, or revised without express written permission from the copyright owner
Tentative Course Outline
Topic 1
Review (0.0167 hour)
1.0
1.1
1.2
1.3
1.4
1.5
1.6
Topic 2
Topic 3
Topic 5
Topic 6
Chapter 6
Empirical approach to the gas laws, Boyle, Charles.
The kinetic-molecular theory of gases (qualitatively).
Ideal vs. real gases.
Graham's Law of Effusion, Dalton's Law of Partial Pressures.
Solids and Liquids (8-9 hours)
6.0
6.1
6.2
6.3
6.4
Chapters 10,11
The ionic and covalent bond types; properties of covalent and ionic cmpds.
Lewis structures, octet rule (and exceptions), formal charges, resonance
Molecular geometry: the VSEPR approach
Bonding: valence bond theory, hybridization, geometry, σ/π bonds, bond energies/lengths
Bonding: molecular orbital theory – diatomic molecules (H to Ne), bond order
The Gaseous State (4-5 hours)
5.0
5.1
5.2
5.3
Chapters 2,8,9
Nature of light, elementary spectroscopy.
The quantum theory and the Bohr atom.
Quantum mechanics; the orbital concept.
Electron configurations of atoms; the Aufbau process; electronic structures to Ca.
The periodic table: its historical development.
The periodic table as a reflection of atomic structure; periodic trends.
Chemical Bonding (13-14 hours)
4.0
4.1
4.2
4.3
4.4
Chapters 3-4
The weight laws.
Atomic/molecular masses, isotopes, mass spectroscopy, nuclear chemistry
The mole
Inorganic formulae and nomenclature
% Composition, combustion analysis
Empirical and molecular formulae.
Mole and mass relationships from balanced chemical equations.
Yields; % yields; limiting reagents.
Volumetric and gravimetric analyses
Analysis of mixtures.
Atomic Structure and Periodicity (13-14 hours)
3.0
3.1
3.2
3.3
3.4
3.5
Topic 4
Introduction
Scientific method
Physical quantities: measurement, units, sig. figs., unit conversion
Chemistry and the nature of matter
Symbols: elements, compounds
Atoms, molecules and ions
Empirical and molecular formulae
From Atoms to Stoichiometry (5-6 hours)
2.0
2.1
2.2
2.3
2.4
2.5
2.6
2.7
2.8
2.9
Chapters 1-3
Four types of crystalline solids. Their properties using bond types.
Solid, liquid and vapour equilibria; the phase diagram.
Solubility: saturation, unsaturation, supersaturation; concentration units
Effects of temperature and pressure.
Colligative properties, vapour pressure, BP, FP, osmotic pressure.
Chapters 12,13
© Dr. E. Neeland. Not to be copied, used, or revised without express written permission from the copyright owner