Chemistry 211 Syllabus and Study Guide

Chemistry 211: General Chemistry I

Course Overview

This course provides an introduction to the fundamental principles of chemistry, including atomic structure, chemical bonding, molecular structure, chemical reactions, and thermodynamics. It is designed for students expecting to major in a natural science and serves as a prerequisite for upper-division chemistry courses.

• Credits: 5 hours

• Prerequisites: Algebra and a Chemistry class

• Textbook: "Chemistry: Atoms First" by Julia Burdge and Jason Overby (McGraw Hill)

Course Structure and Grading

Assignments and Evaluations

• Exams: Four exams (100 points each)

• Labs: 10 completed labs required (100 points total)

• Quizzes: Best 10 out of 13 quizzes (150 points total)

• Homework: Online via ALEKS (150 points total)

• Final Exam: Cumulative ACS national exam (200 points)

Total Points Possible: 1000

Grading Scale

Grades are assigned using a +/- system. The following table summarizes the grading scale:

Points	Letter Grade	Grade Point	Interpretation
92-100	A	4.00	The A range denotes excellent
90-91.99	A-	3.70
88-89.99	B+	3.30
82-87.99	B	3.00	The B range denotes good
80-81.99	B-	2.70
78-79.99	C+	2.30
72-77.99	C	2.00	The C range denotes satisfactory
70-71.99	C-	1.70
68-69.99	D+	1.30	The D range denotes unsatisfactory
62-67.99	D	1.00
60-61.99	D-	0.70
Below 60	F	0.00	F denotes failing performance

Note: A grade higher than C in Chem 211 is required to enroll in Chem 212.

Weekly Topics and Readings

Week	Topics, Readings, Assignments
1	Introduction, Read chapter 1 & start chapter 2
2	Atomic Structure, Read chapters 2 & 3
3	Electronic structure of atoms, Read chapter 3
4	Read chapter 4 and Exam 1
5	Nomenclature introduction, Read chapter 5
6	Molecular structure introduction, Read chapter 6
7	More shapes and hybridization of molecules, Read chapter 7
8	Chapter 7 continued and Exam 2
10	Chemical Reactions, Read chapter 8
11	Solution Chemistry, Read chapters 8 & 9
12	Acid-base reactions
13	Redox reactions and Exam 3
14	Thermodynamics, Read chapter 10
15	Gas laws, Read chapter 11
16	Exam 4
Final	Final Exam

Measurable Student Learning Outcomes

• Identify key components of the scientific method.

• Differentiate between states of matter.

• Determine whether a mixture is heterogeneous or homogeneous.

• Categorize properties of matter as quantitative or qualitative; physical or chemical; extensive or intensive.

• Recall the common base SI units of measurement and their associated symbols.

• Utilize SI unit prefixes.

• Perform conversions between different temperature scales.

• Apply derived units, such as volume and density, to perform calculations.

• Apply significant figure rules in calculations.

• Distinguish between accuracy and precision.

• Apply dimensional analysis toward solving problems with multiple steps or conversions.

• Understand the concept of the atom and the nature of an element.

• Recognize the importance of experiments conducted by Thomson, Millikan, Röntgen, and Rutherford in understanding atomic structure.

• Understand the different types of radiation that radioactive substances can produce.

• Identify the location and physical properties of electrons, protons, and neutrons in atoms.

• Understand the nature and importance of isotopes.

• Utilize the mass number of an isotope to determine the number of electrons, protons, and neutrons given other relevant information.

• Calculate the average atomic mass of an element given the atomic mass and relative abundance of each of its naturally occurring isotopes.

• Use the relationship between Avogadro’s number, moles, molar mass, and grams to conduct calculations.

• Identify the concept of moles and number of atoms.

• Identify energy as being kinetic or potential and as being chemical or electrostatic.

• Understand the law of conservation of energy.

Key Concepts and Definitions

States of Matter

• Solid: Definite shape and volume.

• Liquid: Definite volume, indefinite shape.

• Gas: Indefinite shape and volume.

Mixtures and Pure Substances

• Homogeneous mixture: Uniform composition throughout (e.g., salt water).

• Heterogeneous mixture: Non-uniform composition (e.g., salad).

• Pure substance: Consists of only one type of element or compound.

Physical vs. Chemical Properties

• Physical property: Can be observed without changing the substance’s identity (e.g., melting point).

• Chemical property: Describes a substance’s ability to undergo chemical change (e.g., flammability).

SI Units and Prefixes

• Base units: meter (m), kilogram (kg), second (s), mole (mol), kelvin (K), ampere (A), candela (cd)

• Common prefixes: kilo- (103), centi- (10-2), milli- (10-3), micro- (10-6)

Significant Figures

• Rules for determining the number of significant digits in a measurement.

• Important for reporting the precision of calculated results.

Dimensional Analysis

• Method for converting between units using conversion factors.

• Example: To convert 10 inches to centimeters: $10 \text{ in} \times \frac{2.54 \text{ cm}}{1 \text{ in}} = 25.4 \text{ cm}$

Atomic Structure

• Atom: The smallest unit of an element, consisting of protons, neutrons, and electrons.

• Isotope: Atoms of the same element with different numbers of neutrons.

• Atomic number (Z): Number of protons in the nucleus.

• Mass number (A): Total number of protons and neutrons.

• Average atomic mass: Weighted average of all naturally occurring isotopes.

• Avogadro’s number: $6.022 \times 10^{23}$ particles/mol

Energy and Conservation

• Kinetic energy: Energy of motion.

• Potential energy: Stored energy due to position or composition.

• Law of Conservation of Energy: Energy cannot be created or destroyed, only transformed.

Laboratory Component

• 10 labs are required; none are dropped. Lab 10 can be doubled to replace a missed lab (with approval).

• Lab topics include safety, emission spectra, Avogadro’s number, chemical formula determination, titration, and reactions of copper.

• Lab points: Labs (100 pts), Final (50 pts), Quizzes (50 pts) = 200 pts total.

Academic Honesty

• All work must be the student’s own. No unauthorized materials or devices are allowed during exams or quizzes.

• Violations may result in a grade of "F" for the assignment or course and further disciplinary action.

• Refer to the university’s Academic Integrity Policy for details.

Additional Policies

• Attendance: Regular attendance and participation are expected.

• Incompletes: Only granted under specific conditions (see syllabus for details).

• Makeup Work: Only allowed for documented illness or emergencies.

Example Formulas and Equations

• Density: $\text{Density} = \frac{\text{mass}}{\text{volume}}$

• Average Atomic Mass: $\text{Average atomic mass} = \sum (\text{isotope mass} \times \text{fractional abundance})$

• Energy of a photon: $E = h\nu$

• Relationship between wavelength and frequency: $c = \lambda \nu$

Summary

This syllabus outlines the structure, expectations, and key learning outcomes for Chemistry 211. Students are responsible for keeping up with readings, assignments, and laboratory work, and for adhering to academic honesty policies. Mastery of the foundational concepts in this course is essential for success in further chemistry studies.