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Chemistry
Central Campus
CHEM 1411 (10355)– General Chemistry I
Summer I 2014
Mon,Wed 12:45PM - 5:30 PM, in classroom 416
Tue,Thurs 12:45PM - 5:30 PM, in Labroom 414
We will meet for the first time on Mon, June 2, 2014, in Rm 416.
Instructor: Zhen (Jenny) Fu, Ph.D.
Instructor Contact Information:
E-mail: [email protected]
Learning Web: http://learning.hccs.edu/faculty/zhen.fu
Office hours: Before or after class or by appointment.
Course Description and Goals : 4-credit course. Core curriculum course.
This course is designed for science and engineering majors to study atomic
structure, the periodic table, chemical nomenclature, chemical reactions,
thermodynamics, electronic configuration, chemical bonding, molecular structure,
states of matter, and properties of solutions.
Prerequisites: One year of high school chemistry.
Must be placed into:
• Math 0312 (intermediate algebra) or higher
• College-level reading (or take GUST 0342 as a co-requisite)
• College-level writing (or take ENGL 0310/0349 as a co-requisite)
Important: Strong general math and algebra skills are needed for this course!
Students with disabilities: HCCS Disability Support Service states: Any student
with a documented disability (e.g. physical, learning, psychiatric, vision, hearing, etc)
who needs to arrange reasonable accommodations must contact the appropriate
Disability Support Service (DSS) Counselor at the beginning of each semester.
Faculty are authorized to provide only the accommodations requested by the
Disability Support Services Office. Students who are requesting special testing
1 CHEM 1411, Summer 2014, June 2 – July 6, 2014
CHEM 1411 – page 2
accommodations must first contact John Reno at [email protected] or call him at
713/718-6165.
Academic Honesty: Zero tolerance for any type of academic dishonesty. Student
who is caught cheating will receive a grade of zero for that exam or lab report with no
exceptions and may be administratively withdrawn from the class. The student will
be reported to the College for discipline action.
Attendance/Withdrawal/Grade: Keep perfect attendance is essential for any science
class. Attendance will be recorded in each lecture and lab. Students are responsible
by themselves for catching up the course works due to absence, tardiness or any other
forms of missing the class. Student may be dropped from a course after the student
has accumulated absences in excess of 12.5% of the hours of instruction.
Academic performance is the responsibility of each student. Failure to meet the
requirements for the course will result in an “F” on your transcript. If you are having
difficulty, please see the instructor for additional assistance. If you are unable to
improve your grade you may consider withdrawing from the course. A withdrawal
slip must be submitted on or before June 23 by 4:30 pm. REMEMBER, an “F” on
your transcript NEVER goes away. An incomplete (“I”) will only be given for
extraordinary circumstances (death in the family, severe illness, military duty, jury
selection, etc).
Instructional Materials:
textbook, lab manual, safety goggles, calculator(scientific), scantron(form No.
882-E)
1. Textbook: Chang, Raymond (2012) Chemistry, CHEM1411 (11th Edition),
Boston, MA: McGraw Hill. ISBN 978-0-07-775853-0 part of 978-0-07-775854-7
2. Lab Manual: “Laboratory Manual for Chem 1411: General Chemistry I ”
by Gholam H. Pahlavan, Yiyan Bai, William Askew and Houston Community
College (2011). ISBN 978-1-59984-380-3
3. Safety Goggles (Note: safety glasses are not adequate – you must have goggles)
4. Calculator: must have scientific notation, exponent, and logarithm (log and ln)
functions. For tests, you must have an actual calculator - you are not permitted to
use a calculator application on a cell phone, I-Touch, or other such device.
5. Scantron (Form No. 882-E): (plus #2 pencil) Must have. For quizzes and tests.
6. Periodic Table: will be provided at the time of each exam.
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CHEM 1411 – page 3
Instructional Methods
Lectures, problem-solving sessions, demonstrations, hands-on laboratory activities,
and active student participation exercises will be used to teach the concepts and
practice the skills essential to this chemistry course.
Assignment Policy
Students are responsible for all information covered in the course. It is your
responsibility to complete and submit all assignments and tests by their respective
due dates. Late work is not accepted in this course.
Class Quiz/Attendance (15%)
Quizzes will be given at the very beginning of class (to encourage punctuality) and
are designed to check that the students are keeping up with the textbook reading and
are able to utilize the material in the textbook (text, tables, figures, sample problems).
Missed quizzes can not be made up. The two lowest quiz grades will be dropped.
The scores on your quizzes will be totaled and then divided by the total number of
possible points on the quizzes and converted to a percentage. This quiz grades will
count as 15% of your final course grade.
Testing (40%): Three tests will be given during the semester. The worst score will be
dropped. Each test will be concentrated with specific chapters. The test date and the
exact content will be pre-announced. Sample/practice problems or exam review will
be posted. No make-up tests are allowed for any excuses.
Final Exam (25%): A system wide final exam will be given. It is comprehensive.
System Final Exam is mandatory and can not be dropped. Thus missing the Final
or inadequate preparation for it will have adverse consequence affecting your grade.
Lab (20%): the lab takes 20 points of the total grade. Each lab grade is based on your
attendance, participation and performance. Safety is the most important issue in the
lab. You must follow the safety procedure all the time.
No food or drink is allowed in the laboratory at any time.
Any student who does not follow the safety procedures will not be allowed to do
the lab experiments and will receive a grade of zero (0) for the laboratory portion of
the course grade.
A student arriving 20 minutes after the start of lab will not be allowed to perform the
lab.
See syllabus for schedule of experiments.
The Lab Report should be turned in on time, please see the schedule on syllabus.
Credit will be deducted for late report. (2 points per day).
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CHEM 1411 – page 4
Lab Report = prelab questions + data + data analysis + post lab questions
You will be allowed to drop one (1) lab grade during the semester so it is possible to
miss one lab experiment due to illness or personal situation without decreasing your
grade.
Make-up Policy: No make-up allowed for any quiz, test, lab and the final.
Grading Policy:
Lab Assignments
Quizzes
Tests
Final Exam:
20% of your final grade (the lowest lab score is dropped)
15% of your final grade (the lowest two quizzes scores are dropped)
40% of your final grade (the lowest of the three test scores is dropped)
25% of your final grade (this is a system-wide comprehensive final)
Total:
100%
Grading scale:
90-----100 A; 80-----89 B; 70-----79 C; 60-----69 D; Below 60 F
Homework Assignments
It is very important to do the homework. Homework assignments will be given but
not collected or included in formal calculation of grade due to availability of
solutions. (Solutions will be posted in my learning web). Extra exercises and practice
exam problems and their solutions for chapters will also be posted on my learning
web for your practice and preparation for the quizzes and tests
(http://learning.hccs.edu/faculty/zhen.fu)
Homework from the 11th edition of the Chemistry textbook by Raymond Chang,
Chapter
1
2
3
4
5
6
7
8
9
10
Problems
1.6, 1.9, 1.12, 1.16, 1.22, 1.24, 1.29, 1.34, 1.35, 1.38, 1.84, 1.104
2.12, 2.16, 2.18, 2.21, 2.22, 2.26, 2.36, 2.50, 2.58, 2.60, 2.70, 2.90, 2.110
3.5, 3.14, 3.16, 3.20, 3.24, 3.44, 3.48, 3.52, 3.60(a,c,e,g,i), 3.66, 3.83, 3.94
4.9, 4.18, 4.20, 4.22(a+c), 4.32, 4.44(c+d), 4.50, 4.54, 4.56, 4.59, 4.62, 4.72
5.1, 5.14, 5.18, 5.19, 5.22, 5.23, 5.32, 5.34, 5.40, 5.52, 5.63, 5.88,
6.16, 6.18, 6.20, 6.26, 6.34, 6.35, 6.54, 6.57, 6.62, 6.64, 6.71, 6.84
7.1, 7.8, 7.16, 7.20, 7.52, 7.56, 7.58, 7.66, 7.76, 7.78, 7.90
8.5, 8.12, 8.20, 8.28, 8.30, 8.35, 8.38, 8.44, 8.52, 8.56, 8.62, 8.76, 8.88
9.5, 9.16, 9.36(use Fig 9.5), 9.40, 9.44, 9.46, 9.48, 9.54, 9.64, 9.72, 9.76
10.2, 10.10, 10.14, 10.24, 10.38, 10.46, 10.52, 10.53, 10.80, 10.82, 10.93
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CHEM 1411 – page 5
11
11.6, 11.10, 11.12, 11.16(explain why!), 11.27, 11.38, 11.42, 11.44, 11.48,
11.49, 11.54, 11.59, 11.94, 11.122
General Suggestions: Chemistry is a vast field, ranging from the study of simple
inorganic salts to enormously complex molecules such as enzymes and nucleic acids in
living organisms. In this course, the major topics we will be covering are chemical
formulas, reactions, and stoichiometry calculations, chemical thermodynamics,
electron configuration and chemical bonding, gas laws, and solutions. As you might
suspect, it can be easy to fall behind and, as a result, to not be ready for the exams.
Following are some general tips that may be helpful:

Learning chemistry takes time. A reasonable guide is to allow yourself two
hours of study for each hour of lecture. Heavy work and/or class loads are
not compatible with learning chemistry!

Attend class regularly (!) and take generous notes during class. Ask
questions.

When beginning a new chapter, I recommend that you read through it
quickly the first time, just to give yourself a good feel for what it is about.
You will understand what's going on in class much better if you do this.

Next, focus on the homework and practice exam problems! Often, working
problems facilitates understanding much better than just reading and
rereading the chapter itself. Chemistry is a "hands on" course - working
problems is essential.

Study groups can be very helpful. Keep the group small though, no more
than three or four people.

Finally, keep a positive attitude! Chemistry can be hard, but with the right
attitude and approach, you will succeed in mastering it!
I hope you find chemistry to be an interesting and rewarding subject which will not
only be useful in your academic major, but will give you a better insight into the
many scientific challenges we are facing today. I look forward to working with you
this semester!
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CHEM 1411 – page 6
5-WEEK Tentative Daily Schedule
Mon,Wed 12:45PM - 5:30 PM, in classroom 416
Tue,Thu 12:45PM - 5:30 PM, in Labroom 414
Date
1
Mon, 6/2/2014
Lecture
Lab Safety Video,
EXP 1. Measuring Techniques
and Calculation
EXP 2. Separation of a Mixture
Ch 3. Mass Relationship in Chemical
Reactions.
EXP 6. Formula of a Hydrate and
Percentage
Water of Hydration.
Thu, 6/5/2014
2
Mon, 6/9/2014
EXP 7. The Iron-Copper Molar
Ration—Single
Replacement Reaction and
Limiting Reagent.
Mon,
6/16/2014
Ch 6. Thermochemistry.
Thu, 6/19/2014
4
Mon,
6/23/2014
Tue, 6/24/2014
Exp 7
TEST-2 (chapters 4-6)
Ch 7. Quantum Theory and the
Electronic Structure of Atoms.
Exp. 8: Reactions in Aqueous
Solution (#4,5,6,10,11,14)
Exp. 9: Reactivity of MetalsActivity Series (Part I)
Tue, 6/17/2014
Wed,
6/18/2014
Exp 6
Ch 5. Gases.
Thu, 6/12/2014
3
Exp 1 and 2
TEST-1 (chapters 1-3)
Ch 4. Reactions in Aqueous Solutions.
Tue, 6/10/2014
Wed,
6/11/2014
Lab report to
turn in:
Introduction, Syllabus review,
Ch 1. Chemistry: The Study of
Change.
Ch 2. Atoms, Molecules, and Ions.
Unit Analysis and Math Review
Tue, 6/3/2014
Wed, 6/4/2014
Lab to do
Ch 8. Periodic Relationships Among
the Elements.
Ch 9. Chemical Bonding I : Basic
Concepts.
Exp 8 and 9
TEST-3 (chapters 7-9)
EXP 10. Conductivity of Solutions
Measured
by Vernier Computer Interface.
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CHEM 1411 – page 7
EXP 12. Heat of Neutralization
Measured
by Vernier Computer Interface
Wed,
6/25/2014
Ch 10. Chemical Bonding II:
Molecular
Geometry
and
Hybridization of Atomic Orbitals,
Molecular Models and Molecular
Shapes.
Thu, 6/26/2014
5
Mon,
6/30/2014
Thu, 7/3/2014
Exp 10 &12
Comprehensive Review
(Chapters 1-11)
Exp 13
Ch 11. Intermolecular Forces and
Liquids and Solids.
Tue, 7/1/2014
Wed, 7/2/2014
Exp. 13: Ideal Gas Law:
Determination of the Molar
No class
Cummulative Final Exam (Chapters
1-11).
Disclaimer: Although much thought and effort has gone into the construction of this
syllabus, changes may be necessary. If changes are made to anything in
the syllabus they will be announced in class and/or lab or via email.
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CHEM 1411 – page 8
Appendix I
EGLS3 – Evaluation for Greater Learning Student Survey System
At Houston Community College, professors believe that thoughtful student feedback
is necessary to improve teaching and learning. During a designated time, you will be
asked to answer a short online survey of research-based questions related to
instruction. The anonymous results of the survey will be made available to your
professors and division chairs for continual improvement of instruction. Look for the
survey as part of the Houston Community College Student System online near the
end of the term.
Repeat Course Fee
The State of Texas encourages students to complete college without having to repeat
failed classes. To increase student success, students who repeat the same course
more than twice are required to pay extra tuition. The purpose of this extra tuition fee
is to encourage students to pass their courses and to graduate. Effective fall 2006,
HCC will charge a higher tuition rate to students registering the third or subsequent
time for a course. If you are considering course withdrawal because you are not
earning passing grades, confer with your instructor/counselor as early as possible
about your study habits, reading and writing homework, test taking skills, attendance,
course participation, and opportunities for tutoring or other assistance that might be
available.
Classroom Behavior
You have a shared responsibility with your instructor and your classmates to develop
and maintain a positive learning environment for everyone. Your instructor takes this
responsibility very seriously and will take action to address the behavior of any
student who is hurting the learning environment. As a fellow learner, you are asked
to respect the learning needs of your classmates and to assist your instructor in this
critical goal.
Electronic Devices in the Classroom
In order to maximize learning and minimize distractions in the classroom and lab:
• Please bring your calculator to every class and lab session.
• Cell phones must be silent or off during all lectures and labs.
• During tests, cell phones must be turned off and stored out of sight.
8 CHEM 1411, Summer 2014, June 2 – July 6, 2014
CHEM 1411 – page 9
•
•
•
•
•
No text messaging on cell phones is to be done during class or lab.
During the class break, you may take care of any phone or text communications.
Laptop computers are not to be used during class for any reason.
No headphones or ear buds are to be worn during class or lab.
Cameras and recording devices are not allowed.
Instructor Responsibilities
As your instructor, it is my responsibility to:
 Supply and explain the course syllabus describing the topics to be covered, the
grading scale and detailed grading formula explaining how student grades are
to be calculated, the required course materials, and the class policies.
 Provide laboratory safety training.
 Cover the topics in textbook chapters 1 - 11 and answer questions on the
material.
 Facilitate an effective learning environment through lectures, class activities,
and laboratory work.
 Assess student performance on laboratory work, quizzes, tests, and the final
exam.
 Arrange to meet with individual students before and after class as needed.
• Assign final course grades according to the grading formula given.
Student Responsibilities
To be successful in this class, it is the student’s responsibility to:
 Attend class and lab regularly, missing no more than 3 sessions for the
semester.
 Be on time for lecture and lab; if you are late to a lab session and miss the
discussion of lab procedures and safety precautions, you may receive a 0 (zero)
for that lab session. If you are late to lecture and miss a quiz, you will receive
a 0 (zero) on that quiz.
 Obtain the required textbook, lab manual, safety goggles, and calculator.
 Follow all lab directions and work safely in the laboratory.
 Listen carefully and actively participate in class and lab exercises.
 Read and comprehend the textbook.
 Make time in your busy schedule outside the classroom to study chemistry and
keep up with the coursework.
 Complete the required reading, homework, lab assignments, quizzes, tests, and
final exam.
9 CHEM 1411, Summer 2014, June 2 – July 6, 2014
CHEM 1411 – page 10





Ask for help when there is a question or problem.
Utilize the free tutoring services if you need additional help.
Determine and make up if possible what was missed during an absence.
Analyze and learn from mistakes on assignments, quizzes, and tests.
Keep copies of all paperwork, including this syllabus, every handout, and all
assignments.
10 CHEM 1411, Summer 2014, June 2 – July 6, 2014
CHEM 1411 – page 11
Appendix II
Student Learning Outcomes
A student will:
1. Develop an understanding of basic concepts of chemical measurements and calculations, structures of
atoms, molecules, and ions, the periodic table, chemical compound nomenclature, chemical reactions,
reactions in aqueous solution, the structure and properties of gases, liquids, and solids, thermochemistry,
quantum theory, chemical bonding, and molecular geometry.
2. Build a chemistry vocabulary so that he/she can communicate easily with chemistry professionals.
3. Learn and use a variety of tools, techniques, and strategies to solve problems in chemistry.
4. Practice laboratory skills in working safely, using common lab equipment, making measurements,
handling chemicals, running reactions, recording/analyzing/ communicating data, assessing experimental
error, and operating scientific instruments.
Learning Objectives
By the end of this course, a student should be able to do each of the actions listed below. This list of learning
objectives is useful to review before each test and the final exam!
Chapter 1: Chemistry
1. Define homogeneous mixture, heterogeneous mixture, element, and compound.
2. Differentiate between a physical change and a chemical change.
3. Know the SI base units and the prefixes used with SI units.
4. Calculate the density of a substance.
5. Convert temperatures between the Fahrenheit, Celsius, and Kelvin scales.
6. Use scientific notation for numbers.
7. Determine the correct number of significant figures in a calculation.
8. Distinguish between accuracy and precision.
9. Use dimensional analysis to solve problems and determine the correct units.
Chapter 2: Atoms, Molecules, and Ions
1. Describe the structure of an atom in terms of protons, neutrons, and electrons.
2. Define atomic number and mass number for an element and determine them from a periodic table.
3. Understand the definition and the notation for isotopes.
4. Distinguish between metals, metalloids, and nonmetals.
5. Define a period and a group on a periodic table of elements.
6. Identify alkali metals, alkaline earth metals, halogens, and noble gases.
7. Define molecules, ions, cations, and anions.
8. Determine chemical formulas for molecules and ions.
9. Determine the names of simple inorganic ionic and molecular compounds.
10. Define acid, base, and hydrate.
11. Know the names of the first ten straight-chain alkanes.
Chapter 3: Mass Relationships in Chemical Reactions
1. Determine the average atomic mass of an element.
2. Define a mole and know Avogadro’s number.
3. Calculate the molecular mass and the molar mass of an element or compound.
4. Convert between moles and mass of an element or compound.
5. Calculate the percent composition of a compound.
6. Determine the empirical and molecular formulas of a compound.
7. Write a chemical equation describing a chemical reaction.
8. Balance a chemical equation.
9. Determine the amounts of reactants and products in a given chemical reaction.
11 CHEM 1411, Summer 2014, June 2 – July 6, 2014
CHEM 1411 – page 12
10. Identify the limiting reagent in a chemical reaction.
11. Calculate the theoretical yield and percent yield of a chemical reaction.
Chapter 4: Reactions in Aqueous Solution
1. Define solution, solute, solvent, and aqueous solution.
2. Define strong electrolyte, weak electrolyte, and nonelectrolytes and give examples.
3. Describe hydration.
4. Define solubility and use the solubility rules to determine if a compound is soluble.
5. Determine if a precipitate will form in a chemical reaction.
6. Write molecular, ionic, and net ionic equations for precipitation reactions.
7. Identify Brønsted acids and bases.
8. Describe a neutralization reaction in terms of the reactants and products.
9. Describe an oxidation-reduction reaction and write the half-reactions.
10. Assign oxidation numbers using the basic set of rules provided in this chapter.
11. Classify redox reactions into combination, decomposition, combustion, displacement, and
disproportionation reactions.
12. Calculate the concentration of a solution in terms of molarity (M=mol/L).
13. Calculate how much water is needed to dilute a solution to a specified concentration.
14. Describe the process of titration and define the equivalence point.
Chapter 5: Gases
1. Describe the characteristics of a gas.
2. Define the pressure of a gas and know the units used to measure pressure.
3. Understand the relationships between the pressure and volume of a gas (Boyle’s Law), the temperature
and the volume of a gas (Charles’s and Gay-Lussac’s Law), and the relationship between the volume and
moles of a gas (Avogadro’s Law).
4. Know the ideal gas equation and how to use it.
5. Calculate partial pressures in a mixture of ideal gases.
6. Describe the kinetic molecular theory of gases.
7. Describe the distribution of molecular speeds as a function of temperature.
8. Understand the application of van der Waals equation for nonideal gas behavior.
Chapter 6: Thermochemistry
1. Understand the law of conservation of energy and list different forms of energy.
2. Define heat, exothermic process, and endothermic process.
3. Define system, surroundings, open system, closed system, and isolated system.
4. Define a state function.
5. State the first law of thermodynamics.
6. Calculate the work of gas expansion or contraction.
7. Calculate the change in internal energy, ∆E, of a specified system.
8. Calculate the change in enthalpy, ∆H, of a specified system.
9. Calculate the heat change of a substance based on its specific heat, s, or heat capacity, C.
10. Describe a constant-volume calorimeter and a constant-pressure calorimeter.
11. Calculate the standard enthalpy of reaction based on the enthalpies of formation for products and
reactants using the direct method and the indirect method (Hess’s Law).
12. Understand the concepts of the heat of solution and the heat of dilution.
Chapter 7: Quantum Theory and the Electronic Structure of Atoms
1. Describe a wave in terms of wavelength, frequency, and amplitude.
2. Define an electromagnetic wave and be familiar with the electromagnetic radiation spectrum.
3. Describe Planck’s quantum theory: E = hn
4. Use Bohr’s Theory of the Hydrogen Atom to calculate the energies that an electron can possess in a
hydrogen atom.
5. Explain the emission spectra of various elements.
12 CHEM 1411, Summer 2014, June 2 – July 6, 2014
CHEM 1411 – page 13
6. Describe the dual particle and wave nature of the electron.
7. State the Heisenberg uncertainty principle.
8. Describe the four quantum numbers: n, l, ml, and ms.
9. Determine the relationship between the quantum numbers and the atomic orbitals.
10. Know the shapes of the s, p, and d atomic orbitals.
11. Determine the electron configuration of an atom of any element.
12. State the Pauli exclusion principle and Hund’s rule.
13. Predict whether an element will be paramagnetic or diamagnetic.
14. Explain how the periodic table is arranged relative to electron configuration.
Chapter 8: Periodic Relationships Among the Elements
1. Explain why the periodic table is arranged according to atomic number rather than atomic mass.
2. Define a representative element.
3. Explain what valence electrons are.
4. Determine the electron configuration of cations and anions.
5. Identify isoelectronic ions.
6. Predict how effective nuclear charge, atomic radius, and ionic radius vary through the periodic table.
7. Predict how ionization energies vary for the electrons in an element.
8. Define electron affinity and know which elements have high electron affinities.
9. Be familiar with diagonal relationships on the periodic table.
10. Predict whether oxides will be acidic, basic, or amphoteric.
Chapter 9: Chemical Bonding I
1. Draw Lewis dot symbols for any representative element.
2. Explain the difference between an ionic bond and a covalent bond.
3. Define single bond, double bond, and triple bond, and predict how bond length varies with type of
covalent bond.
4. Explain the octet rule.
5. Compare the properties of ionic and covalent compounds.
6. Define electronegativity and classify bonds as ionic, polar covalent, or covalent based on electronegativity
differences.
7. Draw Lewis structures for molecules.
8. Determine the formal charge on an atom in a molecule.
9. Explain the concept of resonance and show how resonance is represented.
10. Know the exceptions to the octet rule: incomplete octets, odd-electron molecules, and expanded octets.
11. Define bond enthalpy and calculate the enthalpy of reaction based on bond enthalpies.
Chapter 10: Chemical Bonding II
1. Predict the geometry of a molecule from the Valence-Shell Electron-Pair Repulsion (VSEPR) model.
2. Define dipole moment and predict whether a molecule will be polar or nonpolar.
3. Describe the Valence Bond Theory and determine the type of hybridized orbital used to describe the
bonding of a central atom in a molecule.
4. Describe the difference between sigma bonds and pi bonds.
5. Describe Molecular Orbital Theory and draw molecular orbital configurations for simple molecules.
6. Calculate the bond order of a bond in a molecule.
7. Describe delocalized molecular orbitals such as those found in benzene.
Chapter 11: Intermolecular Forces and Liquids and Solids
1. Compare the properties of gases, liquids, and solids.
2. Describe the types of intermolecular forces between molecules.
3. Describe hydrogen bonding and its effects on the properties of compounds.
4. Define the surface tension and viscosity of a liquid.
5. Differentiate between cohesion and adhesion.
13 CHEM 1411, Summer 2014, June 2 – July 6, 2014
CHEM 1411 – page 14
6. Describe the unusual properties of water.
7. Explain the difference between amorphous and crystalline solids.
8. Draw simple cubic, body-centered cubic, and face-centered cubic structures and calculate the density,
unit cell edge length, or number of atoms in a unit cell for a given substance.
9. Use Bragg’s law to calculate an atomic spacing in a crystalline compound.
10. Classify crystals into ionic, covalent, molecular, or metallic types.
11. Describe phase changes of a substance and be able to define evaporation, vaporization, boiling,
condensation, melting, freezing, sublimation, and deposition.
12. Define critical temperature, critical pressure, and triple point.
13. Draw and use a phase diagram to determine the phase of a compound at a given temperature and
pressure or to illustrate phase changes.
14 CHEM 1411, Summer 2014, June 2 – July 6, 2014