CHEM 1010: Introduction to Chemistry I – Syllabus and Study Guide

Course Overview

This course, CHEM 1010: Introduction to Chemistry I, provides a foundational understanding of chemistry, focusing on classical chemical concepts and their applications to the world around us. The course is designed for non-science majors and covers a broad range of topics, including atomic and molecular structure, chemical bonding, chemical reactions, solutions, acids and bases, and redox reactions.

Course Information

• Instructor: Derek Vander Molen

• Contact: [e-mail] | Phone: [phone]

• Office: SSC D309 | Office Hours: MWF 10 am – 11 am, 8–9 am (by appointment)

• Class Time: MWF 11:15 am – 12:10 pm in SSC E310

Course Description

This course introduces the nature of matter and energy, the development of chemical technology, and the interaction of this technology with humans and their environment. Topics include atomic structure, energy in matter, chemical bonding and molecular structure, solutions, acid-base reactions, and redox reactions.

• Credit Hours: 3

• Prerequisite: Developmental reading, writing, and math

• Corequisite: CHEM 1011

Course Objectives

Upon completion, students will be able to:

• Apply chemical concepts and the scientific method to everyday observations

• Understand matter (atoms, molecules, and compounds)

• Use chemical nomenclature

• Describe chemical and nuclear reactions

• Understand models of chemical bonding

• Characterize mathematical calculations of matter

• Recognize hazards associated with chemicals

• Explain acids and bases

• Describe oxidation-reduction reactions

Student Learning Outcomes

• Develop skills in inquiry, abstract and logical thinking, and critical analysis

• Apply understanding of scientific methods and statistics

• Understand the scientific method

Required Learning Resources

• Calculator: Scientific calculator (capable of scientific notation, logarithms, exponents, etc.)

• Technology: Computer with internet access for online homework and course materials

• Textbooks: Chemistry for Changing Times, 15th Edition by Hill, Terry W. McCreary, Marilyn D. Duerst, Bill W. Reuter (ISBN: 9780135720153 or 9780134877566)

• Online Homework: Mastering Chemistry website

Major Topics and Weekly Schedule

Week	Main Topics
1	Course Introduction, Chapter 1: Chemistry
2–3	Chapter 1: Chemistry (continued)
4–5	Chapter 2: Atoms
6–7	Chapter 3: Atomic Structure
8–9	Chapter 4: Chemical Bonds
10–11	Chapter 5: Chemical Accounting
12–13	Chapter 6: Gases, Liquids, Solids, and Intermolecular Forces
14	Chapter 7: Acids and Bases
15	Chapter 8: Oxidation and Reduction
16	Review and Final Exam

Key Chemistry Concepts

Atoms, Molecules, and Compounds

Atoms are the basic units of matter, consisting of protons, neutrons, and electrons. Molecules are groups of atoms bonded together, and compounds are substances formed from two or more different elements chemically bonded in fixed proportions.

• Atomic Structure: Atoms have a nucleus (protons and neutrons) and electrons in orbitals.

• Example: Water (H2O) is a compound made of two hydrogen atoms and one oxygen atom.

Chemical Bonding

Chemical bonds are forces that hold atoms together in compounds. The main types are ionic, covalent, and metallic bonds.

• Ionic Bonds: Formed by the transfer of electrons from one atom to another (e.g., NaCl).

• Covalent Bonds: Formed by the sharing of electrons between atoms (e.g., O2).

• Metallic Bonds: Involve a 'sea' of delocalized electrons around metal ions.

Chemical Reactions

Chemical reactions involve the transformation of substances into new products. They are represented by chemical equations.

• General Equation:

$\text{Reactants} \rightarrow \text{Products}$

• Example: $2H_2 + O_2 \rightarrow 2H_2O$

Solutions, Acids, and Bases

Solutions are homogeneous mixtures of solutes dissolved in solvents. Acids release hydrogen ions ($H^+$) in solution, while bases release hydroxide ions ($OH^-$).

• pH Scale: Measures acidity or basicity; $pH = -\log[H^+]$

• Example: Hydrochloric acid ($HCl$) is a strong acid; sodium hydroxide ($NaOH$) is a strong base.

Redox (Oxidation-Reduction) Reactions

Redox reactions involve the transfer of electrons between substances. Oxidation is the loss of electrons, and reduction is the gain of electrons.

• Example: $Zn + Cu^{2+} \rightarrow Zn^{2+} + Cu$

Assessment and Grading

• Homework: Assignments on Mastering Chemistry (total of 280 points)

• Quizzes: 6 quizzes (20 points each, total 120 points)

• Examinations: 3 in-class exams (100 points each, total 300 points)

• Final Exam: Comprehensive (200 points)

• Essay Assignment: 100 points

• Other Assignments: 50 points (podcast, etc.)

Grading Scale

Letter Grade	Percentage
A	90–100%
B	80–89%
C	70–79%
D	60–69%
F	<60%

Policies and Support

• Attendance: Regular attendance is expected; students are responsible for missed material.

• Disability Services: Accommodations available through the Office of Student Disability Resource Center.

• Academic Integrity: Cheating and plagiarism are not tolerated; use of unauthorized AI is prohibited.

• Tutoring: Free tutoring is available through the university.

• Technology: Students must have access to a computer and internet for course materials and assignments.

Summary Table: Major Chemistry Topics

Topic	Description
Atoms & Atomic Structure	Basic units of matter, structure of atoms, subatomic particles
Chemical Bonding	Types of bonds (ionic, covalent, metallic), bond properties
Chemical Reactions	Types of reactions, balancing equations, energy changes
Solutions	Solubility, concentration, properties of solutions
Acids & Bases	Definitions, pH, neutralization reactions
Redox Reactions	Electron transfer, oxidation numbers, applications
States of Matter	Gases, liquids, solids, intermolecular forces

Additional Info

• Students are encouraged to develop critical thinking and scientific reasoning skills.

• Make-up exams and accommodations are available under specific circumstances.

• Regular use of the course website and email is required for updates and assignments.