Course Overview

Introduction to General Chemistry I

CHY 121 is the first course in the general chemistry sequence at the University of Maine, designed to introduce students to the fundamental principles of chemistry. The course emphasizes reasoning, analysis, and evidence-based understanding of the physical world at the atomic and molecular level. It covers chapters 1–9 of Chemistry: The Central Science (Brown, LeMay, Bursten).

• Atomic and molecular scale: Understanding why substances behave as they do.

• Molecular structure: Structure determines properties such as reactivity, solubility, acidity, and phase.

• Scientific thinking: Develop skills in problem-solving, critical analysis, and quantitative reasoning.

• Active learning: Engage in interpreting chemical formulas, reactions, and real-world observations.

Course Topics and Schedule

Weekly Topics and Chapter Coverage

The course is structured around weekly topics, each corresponding to chapters in the textbook. Below is a summary of the main topics covered:

• Chapter 1: Classifications of matter, properties of matter, energy, units of measurement, significant figures, dimensional analysis.

• Chapter 2: Atomic theory and structure, atomic weights, periodic table, molecules and molecular compounds, ions and ionic compounds, nomenclature.

• Chapter 3: Chemical equations, patterns of reactivity, formula weights, mole concept, empirical formulas, quantitative information from chemical equations, limiting reactants.

• Chapter 4: Aqueous solutions, precipitation reactions, neutralization reactions, redox reactions, concentrations of solutions, solution stoichiometry.

• Chapter 5: Chemical energy, thermodynamics, enthalpy, enthalpies of reaction, calorimetry, Hess’s law, bond enthalpies, foods and fuels.

• Chapter 6: Wave nature of light, quantized energy, Bohr model, wave behavior of matter, quantum mechanics, atomic orbitals, electron configurations, periodic table.

• Chapter 7: Periodic table, effective nuclear charge, atomic and ionic sizes, ionization energy, electron affinity, metals and nonmetals.

• Chapter 8: Lewis symbols, octet rule, ionic and covalent bonding, bond polarity, electronegativity, Lewis structures, resonance, exceptions to the octet rule, bond strengths and lengths, bond enthalpies.

• Chapter 9: Molecular geometry, VSEPR theory, molecular shape, molecular polarity.

Course Schedule Table

The following table summarizes the weekly schedule, topics, assessments, and homework assignments:

Additional info: University holidays are noted in the schedule; class will not meet on those dates.

Course Goals and Learning Outcomes

Fundamental Objectives

• Apply chemical principles: Use atomic structure, periodic trends, and bonding to explain and predict properties.

• Perform quantitative calculations: Master units, significant figures, stoichiometry, and solution concentrations.

• Interpret chemical information: Connect symbolic, macroscopic, and particulate-level models.

• Evaluate claims and solutions: Analyze assumptions, select models/equations, and justify solutions.

• Communicate reasoning: Use terminology, equations, graphs, and written explanations.

• Monitor learning: Reflect on performance, identify misunderstandings, and use feedback to improve.

Assessment and Grading

Grading Breakdown

• Participation: 10%

• Homework: 10%

• Quizzes: 15%

• Exam 1: 15%

• Exam 2: 15%

• Exam 3: 15%

• Final Exam: 20%

Letter Grade Scale:

Progression Policy: Minimum grade of C– required to proceed to CHY 122.

Course Policies and Resources

Participation and Attendance

• Active engagement in lectures and recitations is required.

• Attendance is tracked; participation credit can be earned through quizzes, iClicker questions, activities, and office hours.

Homework and Quizzes

• Weekly homework via Mastering Chemistry; lowest score dropped.

• Six quizzes in recitation; two lowest scores dropped.

• No makeup quizzes; late homework loses 10% credit per 24 hours.

Exams

• Three midterm exams and one cumulative final exam.

• Final exam score may replace one lower midterm score if all exams are taken in-person.

• Makeup exams only for university-sanctioned conflicts, religious holidays, or emergencies.

Recitations

• Mandatory attendance; focus on problem-solving and conceptual understanding.

• Opportunity to ask questions and reflect on learning.

Extra Credit

• Adaptive Follow-Ups in Mastering Chemistry (0.5% per follow-up).

• Participation in astronomy program (1% extra credit).

Student Support Resources

• Accessibility Services, Tutoring, Writing Center, Library, Health and Wellness, Counseling, Multicultural Center, Chemistry Learning Center.

• Digital tutoring platform: Knack.

Academic Integrity and Conduct

Honesty and AI Use Policy

• Cheating, plagiarism, and falsification of results are prohibited.

• AI tools may be used for learning assistance, but not for submitting work as one's own.

Sexual Discrimination Reporting

• Faculty are required to report incidents; confidential resources are available on and off campus.

Religious Observance

• Students may make up course requirements missed due to religious holidays with adequate notice.

Suggestions for Success

Effective Study Strategies

• Attend all lectures and recitations; keep up with material.

• Engage actively: take notes, ask questions, attempt problems.

• Seek help early; use office hours and tutoring resources.

• Test your knowledge by teaching others and practicing problems.

• Avoid cramming; study consistently and get adequate rest before exams.

Summary of Key Chemistry Concepts (Chapters 1–9)

Selected Definitions and Examples

• Matter: Anything that has mass and occupies space.

• Energy: The capacity to do work; includes kinetic and potential energy.

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

• Dimensional Analysis: Method for converting units using conversion factors. Example:

• Atomic Theory: Atoms are the fundamental units of matter; elements are composed of atoms.

• Stoichiometry: Quantitative relationships in chemical reactions. Example:

• Mole Concept:

• Periodic Table: Organizes elements by atomic number and properties.

• Bonding: Atoms form ionic or covalent bonds to achieve stable electron configurations.

• Lewis Structures: Visual representations of valence electrons in molecules.

• VSEPR Theory: Predicts molecular geometry based on electron pair repulsion.

Additional info: For detailed explanations, refer to the textbook chapters and recitation materials.