CHEM 120: General Chemistry I – Syllabus and Course Overview

CHEM 120: General Chemistry I – Syllabus and Course Overview

Course Information

• Course Title: General Chemistry I (CHEM 120)

• Institution: Southern Connecticut State University

• Semester: Fall 2023

• Lecturer: Dr. Belinda Hurdle

• Lecture Times: Section 01-04, multiple times and locations

• Contact: Email and office hours provided

Required Materials

• Textbook: Chemistry, OpenStax, Rice University (2019) – free online access

• Lab Manual: SCSU General Chemistry I Laboratory Manual (2023-2024)

• Calculator: Scientific calculator required for exams and laboratory work

• Other: Access to Blackboard Learn for course materials and announcements

Course Description

This course is the first semester of a two-semester introduction to the fundamental principles of chemistry. Topics include atomic and molecular structure, chemical bonding, chemical reactions, stoichiometry, thermochemistry, and introductory quantum mechanics. Laboratory exercises reinforce lecture material and develop basic laboratory skills.

Course Objectives

• Classify matter into categories such as solid, liquid, gas, homogeneous, heterogeneous, mixture, element, compound, molecule, and ionic solid.

• Understand the differences between chemical and physical properties, chemical and physical changes.

• Understand basic atomic structure.

• Understand the electronic structure of atoms and molecules.

• Know how to use the periodic table and understand periodic trends.

• Learn the names of common simple molecules and ions and understand inorganic nomenclature.

• Write and balance chemical equations.

• Use the mole concept for quantitative chemical analysis.

• Understand the relationship between empirical and molecular formulas.

• Understand the concept of limiting reagent and percent yield for chemical reactions.

• Learn how to calculate solution concentrations and perform calculations using solubility rules.

• Learn principles of stoichiometry with single and multiple reactions using suitability rules for predicting reactions.

• Be able to solve gas law equations using stoichiometric and gas law relationships.

• Understand energy changes and heat flow in chemical processes.

• Write and interpret chemical equations to describe heat exchange with enthalpy changes in the system.

Course Outline

Week	Lecture Dates	Lecture Topic	Lab	Recitation
1	Aug 29, 31	Ch. 1: Essential Ideas	none	Will meet
2	Sep 5, 7	Ch. 1 continued	Exp#1	Quiz 1
3	Sep 12, 14	Ch. 2: Atoms, Molecules and Ions	Exp#2	Quiz 2
4	Sep 19, 21	Ch. 2 continued	Exp#3	Quiz 3
5	Sep 26, 28	Ch. 3: Composition of Substances and Solutions	Exp#4	Quiz 4
6	Oct 3, 5	Ch. 4: Stoichiometry of Chemical Reactions	Exp#5	Quiz 5
7	Oct 10, 12	Ch. 4 continued	Exp#6	Quiz 6
8	Oct 17, 19	Ch. 5: Thermochemistry	Exp#7	Quiz 7
9	Oct 24, 26	Ch. 6: Electronic Structure and Periodic Properties of Elements	Exp#8	Quiz 8
10	Oct 31, Nov 2	Ch. 7: Chemical Bonding and Molecular Geometry	Exp#9	Quiz 9
11	Nov 7, 9	Ch. 8: Advanced Theories of Chemical Bonding	Exp#10	Quiz 10
12	Nov 14, 16	Ch. 9: Gases	Exp#11	Quiz 11
13	Nov 21	Ch. 9 continued (review, if needed)	none	none
14	Nov 28, 30	Comprehensive Final Exam	none	none

Major Topics Covered

• Matter and Measurement: Classification of matter, units of measurement, significant figures, and dimensional analysis.

• Atoms, Molecules, and Ions: Atomic theory, structure of the atom, isotopes, ions, and introduction to the periodic table.

• Composition of Substances and Solutions: Chemical formulas, percent composition, empirical and molecular formulas, and solution concentration calculations.

• Chemical Reactions and Stoichiometry: Types of chemical reactions, balancing equations, mole relationships, limiting reactants, and percent yield.

• Thermochemistry: Energy changes in chemical reactions, heat, work, enthalpy, calorimetry, and Hess's Law.

• Electronic Structure and Periodic Properties: Quantum mechanical model, electron configurations, periodic trends, and atomic properties.

• Chemical Bonding and Molecular Geometry: Ionic and covalent bonding, Lewis structures, VSEPR theory, and molecular shapes.

• Theories of Chemical Bonding: Valence bond theory, hybridization, and molecular orbital theory.

• Gases: Gas laws, kinetic molecular theory, and real gases.

Evaluation and Assessment

• One-Hour Examinations: 30%

• Weekly Recitation Quizzes: 25%

• Laboratory Grade: 20%

• Final Examination (2 hours, cumulative): 25%

Grading Scale:

Grade	Points
A	93 – 100
A-	90 – 92
B+	87 – 89
B	83 – 86
B-	80 – 82
C+	77 – 79
C	73 – 76
C-	70 – 72
D+	67 – 69
D	63 – 66
D-	60 – 62
F	0 – 59

Course Policies (Summary)

• Laboratory: Attendance and completion of all laboratory sessions are mandatory. The first lab session includes a safety video and quiz.

• Attendance: Regular and prompt attendance is required for both lectures and labs.

• Academic Honesty: Cheating and plagiarism are strictly prohibited and will result in disciplinary action.

• Electronic Devices: Must be silenced and put away during class and exams.

• Make-up Exams: Only allowed for documented, substantial illness or emergency.

• Disability Services: Accommodations are available for students with documented needs.

Study and Success Tips

• Read textbook sections and review lecture slides before class.

• Practice problems regularly to reinforce concepts.

• Attend recitations and utilize office hours for additional help.

• Form study groups for collaborative learning.

Additional info:

• This syllabus provides a comprehensive overview of the CHEM 120 course, including all major topics relevant to a first-semester General Chemistry curriculum.

• Students are expected to engage with both lecture and laboratory components to develop a foundational understanding of chemical principles and laboratory techniques.