CHEM 1210: General Chemistry I – Syllabus and Course Structure Study Guide

CHEM 1210: General Chemistry I – Course Overview

Course Description and Structure

This course is the first in a two-semester sequence introducing the fundamental concepts, models, and techniques of general chemistry. It covers essential topics such as stoichiometry, atomic structure, periodicity, reaction types, and molecular geometry, with a strong emphasis on laboratory skills and scientific methodology.

• Credits: 4 (3 hours lecture, 3 hours laboratory per week)

• Prerequisites: MATH 1600 or higher (grade C or above) or placement, and eligibility for ENG 1010

• Recommended Preparation: High school chemistry or CHEM 1010/1110

• Required Materials: Pearson eText (Chemistry: The Central Science, 15th ed.), lab manual, chemical safety goggles

Student Learning Outcomes

Core Competencies

• Mathematical Application: Apply mathematical concepts to chemical data analysis.

• Chemical Bonding: Predict and describe properties of chemical bonds and molecular geometry.

• Chemical Reactions: Use nomenclature and formulas to write balanced equations and analyze reactions, including thermochemistry.

• Laboratory Skills: Perform experiments, collect and interpret data, and communicate findings effectively and ethically.

• Safety: Demonstrate proper chemical hygiene and safety practices in the laboratory.

Course Topics Outline

1. Essential Ideas in Chemistry

• Scientific Method: Systematic approach to investigation and knowledge acquisition.

• Hypotheses, Theories, Facts, and Laws: Definitions and distinctions.

• Density: $\text{Density} = \frac{\text{Mass}}{\text{Volume}}$

• Measurements and Calculations: Use of SI units, accuracy, and precision.

• Scientific Notation, Dimensional Analysis, Significant Figures: Tools for expressing and manipulating chemical data.

• Physical vs. Chemical Changes/Properties: Classification and examples.

2. Atoms, Molecules, and Ions

• States of Matter: Solid, liquid, gas.

• Dalton’s Atomic Theory: Foundation of modern atomic theory.

• Subatomic Particles: Protons, neutrons, electrons; their masses and charges.

• Ions and Isotopes: Definitions and examples.

• Ionic vs. Covalent Compounds: Comparison of bonding types.

• Periodic Table Introduction: Organization and significance.

• Chemical Formulas and Nomenclature: Writing and naming compounds.

3. Chemical Reactions and Stoichiometry

• Atomic Mass: Weighted average of isotopes.

• Chemical Reactions: Types and balancing equations.

• Stoichiometric Calculations: Mass-mass, mole-mole, mole-mass conversions.

• Percent Composition and Empirical Formulas: Determination from experimental data.

• Limiting Reactant, Theoretical Yield, Percent Yield: Key concepts in reaction efficiency.

4. Reactions in Aqueous Solutions

• Solutes and Solvents: Definitions and examples.

• Electrolytes: Strong, weak, and nonelectrolytes.

• Types of Reactions:

  • Precipitation: Formation of insoluble products; ionic and net ionic equations.

  • Acid-Base Neutralization: Exchange of protons; predicting products.

  • Oxidation-Reduction (Redox): Electron transfer; identifying oxidizing and reducing agents.

• Solution Concentration: Molarity ($M = \frac{\text{moles solute}}{\text{liters solution}}$), dilution calculations.

• Solution Stoichiometry and Titration: Quantitative analysis of reactions in solution.

5. Gases

• Pressure and Units: atm, mmHg, Pa, etc.

• Gas Laws: Boyle’s, Charles’s, Avogadro’s, and the Ideal Gas Law ($PV = nRT$).

• Dalton’s Law of Partial Pressures: $P_{\text{total}} = \sum P_i$

• Kinetic-Molecular Theory: Model explaining gas behavior.

• Ideal vs. Real Gases: Deviations from ideality at high pressure/low temperature.

6. Thermochemistry

• Energy Principles: Conservation of energy, heat, and work.

• Enthalpy ($\Delta H$): Heat flow at constant pressure.

• Calorimetry: Measurement of heat changes.

• Hess’s Law: $\Delta H_{\text{rxn}} = \sum \Delta H_{\text{products}} - \sum \Delta H_{\text{reactants}}$

• Heats of Formation: Standard enthalpy changes for compound formation.

7. Electronic Structure and Periodic Properties

• Electromagnetic Radiation: Wavelength, frequency, and energy relationships ($E = h\nu$).

• Bohr Model and Energy Transitions: Quantized energy levels.

• Quantum Numbers and Atomic Orbitals: Describing electron positions.

• Electron Configuration: Aufbau principle, Hund’s rule, Pauli exclusion.

• Periodic Trends: Atomic radius, ionization energy, electronegativity.

8. Basic Concepts of Chemical Bonding

• Ionic and Covalent Bonding: Electron transfer vs. sharing.

• Electronegativity: Tendency to attract electrons.

• Lewis Structures and the Octet Rule: Visualizing valence electrons.

• Formal Charge: $\text{Formal charge} = \text{valence electrons} - (\text{lone pair electrons} + \frac{1}{2}\text{bonding electrons})$

• VSEPR Theory and Molecular Geometry: Predicting 3D shapes.

• Polarity of Molecules: Determined by shape and bond polarity.

9. Advanced Theories of Covalent Bonding

• Valence Bond Theory: Overlap of atomic orbitals.

• Hybridization: Mixing of atomic orbitals to form new hybrid orbitals.

• Molecular Orbital Theory: Delocalized electrons in molecules.

Laboratory Topics

• Lab Safety and Hygiene: Essential practices for safe experimentation.

• Measurements and Density: Use of balances and volumetric glassware.

• Separation Techniques: Gravity and vacuum filtration, paper chromatography.

• Chemical Formulas: Empirical formula determination, percent composition.

• Stoichiometry: Limiting reactants, percent yield, theoretical yield.

• Titration: Quantitative analysis of acid-base reactions.

• Gas Laws: Experimental verification and calculations.

• Thermochemistry: Measurement of heat changes in reactions.

• VSEPR Theory and Molecular Models: Building and analyzing molecular shapes.

Grading and Evaluation

Assessment Breakdown

• Lecture (75%):

  • Final Exam: 12%

  • 4 Unit Tests: 48% (12% each)

  • Homework: 15% (lowest two grades dropped)

• Lab (25%):

  • 2 Lab Tests: 13% (6.5% each)

  • Lab Reports: 12% (lowest grade dropped)

Grading Scale

Letter Grade	Grade Scale (%)	GPA	Description
A	93-100	4.0	Distinguished achievement
A-	90-92.99	3.7
B+	87-89.99	3.3
B	83-86.99	3.0	High level of achievement
B-	80-82.99	2.7
C+	77-79.99	2.3
C	73-76.99	2.0	Basic understanding
C-	70-72.99	1.7
D+	67-69.99	1.3
D	63-66.99	1.0	Minimal performance
D-	60-62.99	0.7
F	<60	0.0	Failure

Course Schedule (Selected Weeks)

Week	Lecture Topics	Lab Topics
1	Chapter 1: Essential Ideas	Lab Safety, Chapter 1
2	Chapter 2: Atoms, Molecules, Ions	Measurements and Density
3	Chapter 3: Chemical Reactions	Formula of a Hydrate
4	Unit Test 1 (Ch. 1-3.5)	Stoichiometry
5-6	Chapters 3-4: Reactions in Aqueous Solution	Acid-Base Titration
7	Unit Test 2 (Ch. 5, 10, 6, 7)	Single Displacement Reaction
8	Chapter 10: Gases	Lab Test 1 (Experiments 1-5)
9	Chapter 5: Thermochemistry	Gas Stoichiometry
10	Chapter 6: Electronic Structure	Calorimetry
11-12	Chapters 6-8: Bonding, Geometry	Copper Chemistry, Molar Mass by Vapor Density
13-14	Chapters 8-9: Molecular Geometry, Advanced Bonding	Molecular Models, Lewis Structures
15-16	Review, Final Exam	Lab Test 2 (Experiments 6-10)

Laboratory Policies and Safety

• Attendance of at least 75% of lab sessions is required to pass.

• Lab reports are due at the beginning of the next lab session; late reports may be penalized or not accepted.

• Lab safety rules must be followed at all times.

Academic Integrity

• Plagiarism and all forms of cheating are strictly prohibited.

• Examples of misconduct include unauthorized assistance, falsifying data, and submitting work not your own.

• Penalties include a grade of "F" for the assignment or course, and possible further disciplinary action.

Support and Resources

• Tutoring: Free tutoring is available at the campus tutoring center.

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

• Communication: All official communication is via college email and Blackboard.

Additional info:

• This syllabus provides a comprehensive overview of the CHEM 1210 course, including all major general chemistry topics as outlined in standard college-level curricula.

• For detailed content on each chapter, refer to the course textbook and lecture materials.