CHEM-101: College Chemistry I – Structured Study Notes for GOB Chemistry Students

Course Overview

Introduction to College Chemistry I

This course provides a foundational understanding of the principles and theories of general, organic, and biological (GOB) chemistry. It is designed for students pursuing health sciences and related fields, emphasizing both qualitative and quantitative problem-solving, laboratory skills, and scientific reasoning.

• Required Textbook: Chemistry: Structures of Life, 6th edition by K. Timberlake, Pearson.

• Course Duration: September 2nd – December 21st

• Prerequisites: Completion of introductory math courses (MTH 092, ENG 096, RDG 096, or equivalent).

Course Objectives

Measurable Performance Objectives

Upon successful completion, students will be able to:

• Demonstrate knowledge of fundamental chemistry concepts and theories.

• Apply problem-solving skills to chemical phenomena using formulas, units, and scientific methods.

• Utilize laboratory equipment such as triple beam balances, pH meters, and glassware.

• Analyze and interpret data from chemical experiments.

Main Topics & Subtopics

Unit One: Introduction to Chemistry

This unit introduces the role of chemistry in everyday life and the scientific method as applied to chemical investigations.

• Chemistry in Our Lives: The study of matter, its properties, and changes.

• Scientific Method: Systematic approach to research and experimentation.

• Measurements & Conversion Factors: Understanding units, significant figures, and dimensional analysis.

Unit Two: Atomic Structure & Nuclear Chemistry

This unit explores the structure of atoms, the periodic table, and the basics of nuclear chemistry.

• Atoms: Basic building blocks of matter, composed of protons, neutrons, and electrons.

• Nuclear Chemistry: Study of radioactive decay, nuclear reactions, and their applications.

• Ionic & Molecular Compounds: Formation, nomenclature, and properties.

Unit Three: Chemical Reactions & Quantities

This unit covers chemical reactions, stoichiometry, and the behavior of gases.

• Chemical Reactions: Processes in which substances are transformed into new substances.

• Stoichiometry: Quantitative relationships in chemical reactions.

• Gases: Properties, laws (Boyle's, Charles's, Ideal Gas Law), and calculations.

Unit Four: Solutions, Equilibrium, Acids & Bases

This unit examines the properties of solutions, chemical equilibrium, and acid-base chemistry.

• Solutions: Homogeneous mixtures, concentration units (molarity, percent), and solubility.

• Chemical Equilibrium: Dynamic balance in reversible reactions.

• Acids & Bases: Definitions (Arrhenius, Brønsted-Lowry), pH, and buffer systems.

Key Concepts & Definitions

Measurements & Significant Figures

• Significant Figures: Digits in a measurement that are known with certainty plus one estimated digit.

• Dimensional Analysis: Technique for converting between units using conversion factors.

• Example: Converting 25.0 cm to inches using $1~\text{in} = 2.54~\text{cm}$.

Atomic Structure

• Atom: Smallest unit of an element, consisting of a nucleus (protons and neutrons) and electrons.

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

• Example: Carbon-12 and Carbon-14 are isotopes of carbon.

Nuclear Chemistry

• Radioactive Decay: Spontaneous emission of particles or energy from an unstable nucleus.

• Types: Alpha ($\alpha$), Beta ($\beta$), Gamma ($\gamma$) decay.

• Equation Example: $^{14}_{6}\text{C} \rightarrow ^{14}_{7}\text{N} + \beta^{-}$

Chemical Bonding & Nomenclature

• Ionic Bonds: Electrostatic attraction between cations and anions.

• Covalent Bonds: Sharing of electron pairs between atoms.

• Nomenclature: Systematic naming of compounds based on their composition.

• Example: NaCl is named sodium chloride.

Stoichiometry

• Mole Concept: $1~\text{mol} = 6.022 \times 10^{23}$ particles.

• Molar Mass: Mass of one mole of a substance (g/mol).

• Balanced Equation Example: $2\text{H}_2 + \text{O}_2 \rightarrow 2\text{H}_2\text{O}$

Gas Laws

• Boyle's Law: $P_1V_1 = P_2V_2$ (at constant temperature)

• Charles's Law: $\frac{V_1}{T_1} = \frac{V_2}{T_2}$ (at constant pressure)

• Ideal Gas Law: $PV = nRT$

Solutions & Concentration

• Molarity (M): $M = \frac{\text{moles of solute}}{\text{liters of solution}}$

• Percent Concentration: $\% = \frac{\text{part}}{\text{whole}} \times 100$

Chemical Equilibrium

• Equilibrium Constant ($K$): $K = \frac{[\text{products}]}{[\text{reactants}]}$

• Le Châtelier's Principle: System at equilibrium responds to disturbances to restore balance.

Acids, Bases, and Buffers

• Acid: Substance that donates protons ($\text{H}^+$).

• Base: Substance that accepts protons or donates hydroxide ions ($\text{OH}^-$).

• pH Scale: $\text{pH} = -\log[\text{H}^+]$

• Buffer: Solution that resists changes in pH upon addition of acid or base.

Course Assessment Structure

Grading Breakdown

The following table summarizes the grading components and their respective weights:

Assignment	Individual Assignment %	Number of Assignments	Total Percent
Four Exams	10	4	40
Quizzes (via Moodle/Mastering)	2	10	20
Homework (via Moodle/Mastering)	1	10	10
Lab Reports (1-10)	2.5	10	25
Attendance	15 (weeks)	1	3
Final Exam	1	1	2
Total			100

Laboratory Component

Lab Skills & Safety

Students will perform experiments to reinforce theoretical concepts, develop laboratory techniques, and practice safety protocols.

• Lab Safety: Proper handling of chemicals and equipment.

• Data Collection: Recording observations and measurements accurately.

• Lab Reports: Analysis and interpretation of experimental results.

Academic Integrity & Conduct

Expectations

• Plagiarism: Presenting another's work as your own is strictly prohibited.

• Cheating: Unauthorized assistance during exams or assignments is not allowed.

• Attendance: Minimum 90% attendance required for successful completion.

Course Schedule Overview

Weekly Topics & Labs

Week	Lecture Topic	Laboratory Session
1	Introduction, Chemistry in Our Lives, Measurements & Conversion Factors	Lab Safety Guidelines & Video
2	Chapter 2: Chemistry & Matter	Experiment 1: Measurements & Lab Safety Quiz
3	Chapter 3: Energy & Matter	Experiment 2: Conversion Factors
4	Chapter 4: Atomic Structure, Review & Exam I	Lab 3: Energy & Specific Heat Capacity
5	Chapter 5: Nuclear Chemistry, Exam I	Lab 4: Experiment 4: Energy & Specific Heat Capacity
6	Chapter 6: Ionic & Molecular Compounds	Lab 5: Compounds & Their Formulas
7	Chapter 7: Chemical Reactions & Quantities, Gases	Lab 6: Chemical Reactions & Quantities
8	Chapter 8: Gases, Exam II	Lab 7: Solutions, Electrolytes, & Concentration
9	Chapter 9: Solutions	Lab 8: Experiment 8: Solutions
10	Chapter 10: Reaction Rates & Chemical Equilibrium	Lab 9: Experiment 9: Reaction Rates & Chemical Equilibrium
11	Chapter 11: Acids & Bases	Lab 10: Experiment 10: Acids & Bases
12	Review & Exam VI: Chapters 1-11	Final Lab Quiz

Additional Info

• Support Services: Accommodations available for students with disabilities.

• Artificial Intelligence Tools: Use only as permitted by the syllabus; unauthorized use is considered academic dishonesty.

Additional info: These notes are structured to provide a comprehensive overview of the CHEM-101 College Chemistry I syllabus, suitable for GOB Chemistry students preparing for exams and laboratory work.