Chem 170: Introductory Chemistry

Course Overview

This course provides a foundational introduction to general chemistry, covering essential vocabulary, principles, concepts, laboratory techniques, and problem-solving skills. It prepares students for more advanced chemistry courses and includes both lecture and laboratory components.

• Units: 4 (3 hours lecture, 3 hours lab per week)

• Prerequisites: Intermediate algebra proficiency

• Textbook: Introductory Chemistry by Nivaldo J. Tro (7th Edition, Pearson) or OpenStax Chemistry

• Required Supplies: Laboratory notebook, scientific calculator, USB flash drive, safety goggles, soap, towel, nitrile gloves, lab coat

Grading Structure

• Lecture Exams (3): 40%

• Final Exam (Cumulative): 25%

• Homework: 10%

• Laboratory & Assignments: 25%

• Passing Grade: 60% or better in both lecture and lab

• Grade Scale: 90% = A, 80-89% = B, 70-79% = C, 60-69% = D

Course Topics

Chemical Foundations

Establishes the basic concepts and vocabulary of chemistry, including measurement, significant digits, dimensional analysis, and density.

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

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

• Density: Mass per unit volume. Formula:

• Matter: Anything that has mass and occupies space.

Heat and Energy

Explores energy concepts, calorimetry, and energy changes in chemical processes.

• Energy: Capacity to do work or produce heat.

• Calorimetry: Measurement of heat flow.

• Energy Changes: Associated with chemical reactions and phase changes.

Atomic Structure

Describes the structure of atoms, including subatomic particles and isotopes.

• Subatomic Particles: Protons, neutrons, electrons

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

• Atomic Number: Number of protons in the nucleus.

• Mass Number: Sum of protons and neutrons.

Naming Compounds

Covers nomenclature for binary compounds, polyatomic ions, and acids.

• Binary Compounds: Composed of two elements.

• Polyatomic Ions: Ions composed of multiple atoms.

• Acids: Compounds that release H+ ions in solution.

Stoichiometry

Focuses on quantitative relationships in chemical reactions, including molar mass, mole concept, Avogadro's number, percent composition, empirical and molecular formulas, balancing equations, and limiting reactants.

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

• Mole: SI unit for amount of substance. particles.

• Avogadro's Number:

• Percent Composition:

• Empirical Formula: Simplest whole-number ratio of atoms in a compound.

• Molecular Formula: Actual number of atoms in a molecule.

• Balancing Equations: Ensures conservation of mass.

• Limiting Reactant: Reactant that determines the amount of product formed.

Atomic Theory and Periodic Table

Explains atomic models, electron structure, and periodic trends.

• Bohr Atom: Model with electrons in quantized energy levels.

• Electron Structure: Arrangement of electrons in orbitals.

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

• Periodic Trends: Includes atomic radius, ionization energy, electronegativity.

Chemical Bonding

Describes types of chemical bonds, polarity, ion size, electron configuration, Lewis structures, and VSEPR theory.

• Polarity: Distribution of electrical charge in a molecule.

• Ion Size: Size of ions compared to their parent atoms.

• Electron Configuration: Distribution of electrons among orbitals.

• Lewis Structures: Diagrams showing valence electrons.

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

Gases

Examines gas laws and kinetic molecular theory.

• Boyle's Law: (Pressure and volume inversely related)

• Charles' Law: (Volume and temperature directly related)

• Avogadro's Law: (Volume and moles directly related)

• Dalton's Law: (Total pressure is sum of partial pressures)

• Ideal Gas Law:

• Gas Stoichiometry: Quantitative relationships involving gases.

Liquids, Solids, and Intermolecular Forces

Discusses properties of liquids and solids, evaporation, changes of state, and hydrogen bonding.

• Evaporation: Process by which molecules escape from liquid to gas phase.

• Changes of State: Transitions between solid, liquid, and gas.

• Hydrogen Bond: Strong intermolecular force involving H and N, O, or F.

Solution Chemistry

Explores solubility, precipitation, and concentration calculations.

• Solubility: Amount of solute that dissolves in a solvent.

• Precipitation: Formation of a solid from a solution.

• Concentration:

Acids and Bases

Defines acids, bases, salts, electrolytes, pH, and net ionic equations.

• Acids: Donate H+ ions (Arrhenius and Bronsted-Lowry definitions).

• Bases: Donate OH- ions or accept H+ ions.

• Strong/Weak Electrolytes: Degree of ionization in solution.

• pH:

• Net Ionic Equations: Show only species that change during reaction.

Chemical Equilibrium

Describes rates of reaction, equilibrium expressions, and Le Chatelier’s Principle.

• Equilibrium Expression: (for balanced equation)

• Le Chatelier’s Principle: System at equilibrium responds to disturbances to restore equilibrium.

Oxidation and Reduction

Explains oxidation numbers and redox reactions.

• Oxidation Number: Assigned value indicating electron transfer.

• Redox Reaction: Involves transfer of electrons between species.

Learning Objectives

• Perform metric and English unit conversions.

• Apply concepts of atomic number, mass number, isotopes, and electron configuration.

• Understand periodic table principles and trends.

• Draw Lewis structures for molecules and ions.

• Apply nomenclature for ionic and molecular compounds.

• Solve problems involving mass, mole, density, and volume.

• Balance chemical equations and perform stoichiometric calculations.

• Describe gases using kinetic molecular theory and solve gas law problems.

• Differentiate acids and bases (Arrhenius and Bronsted-Lowry theories).

• Calculate pH, pOH, [H3O+], and [OH-].

• Identify reaction types and predict products.

• Write equilibrium constant expressions and perform related calculations.

• Perform laboratory experiments, interpret results, and apply safety procedures.

Laboratory Requirements

• Strict adherence to safety regulations (goggles, lab coat, closed-toed shoes).

• Lab notebook: Record data directly, sign and date pages, cross out unused areas.

• Formal lab reports: Typed, include title, abstract, introduction, materials, protocols, results, calculations, discussion, conclusion, bibliography.

• Lab reports due at the beginning of class; one late report allowed with penalty.

Academic Integrity and Conduct

• Honesty, trustworthiness, fairness, and respect are expected.

• Violations (cheating, plagiarism, misconduct) may result in disciplinary action.

• Disruptive behavior or misuse of electronic devices is not tolerated.

Recommended Homework Problems

Success in the course is linked to completion and understanding of assigned problems. Problems are listed by chapter and are collected and graded. Similar problems may appear on exams.

• Chapter 1: 7, 16, 17, 20, 25

• Chapter 2: 31, 35, 39, 42, 44, 49, 55, 57, 59, 69, 71, 73, 77, 83, 86, 89, 91, 95, 97, 99, 101, 103, 106, 110, 111, 117, 123, 125, 138

• Chapter 3: 31, 34, 35, 38, 39, 41, 44, 45, 47, 49, 52, 53, 57, 61, 67, 69, 73, 78, 79, 82, 86, 89, 95, 108, 109, 117, 119, 120, 128

• Chapter 4: 27, 29, 31, 32, 34, 35, 38, 41, 43, 45, 47, 49, 51, 55, 57, 59, 61, 64, 65, 67, 69, 73, 75, 77, 80, 82, 83, 85, 87, 89, 91, 93, 95, 97, 100, 103, 105, 111, 113, 129

• Chapter 5: 25, 27, 29, 32, 33, 36, 39, 41, 44, 52, 53, 56, 58, 60, 62, 66, 69, 71, 73, 75, 78, 81, 83, 86, 87, 97, 102, 104, 109, 116

• Chapter 6: 19, 20, 21, 29, 31, 37, 38, 43, 49, 52, 55, 56, 65, 68, 69, 71, 73, 75, 77, 80, 81, 83, 86, 87, 91, 93, 95, 97, 103, 104, 109, 111, 125

• Chapter 7: 35, 37, 40, 44, 45, 47, 49, 51, 56, 58, 59, 65, 67, 69, 71, 73, 75, 77, 83, 88, 89, 91, 93, 97, 99, 101, 105, 109, 114, 118

• Chapter 8: 17, 19, 21, 23, 25, 28, 30, 31, 33, 35, 37, 39, 41, 43, 47, 53, 55, 57, 60, 61, 65, 68, 69, 73, 75, 77, 79, 81, 83, 91, 93, 95, 97

• Chapter 9: 29, 31, 33, 35, 37, 40, 43, 45, 47, 50, 51, 53, 55, 57, 59, 61, 75, 81, 83, 85, 87, 90, 91, 97, 98, 103

• Chapter 10: 23, 31, 33, 37, 39, 41, 47, 50, 52, 53, 55, 57, 59, 61, 63, 65, 67, 69, 71, 73, 75, 77, 81, 83, 85, 87, 89, 91, 98, 100, 107, 109, 113

• Chapter 11: 23, 25, 27, 33, 35, 37, 39, 41, 43, 45, 47, 49, 51, 53, 55, 57, 59, 61, 63, 65, 67, 69, 71, 74, 76, 77, 80, 81, 85, 87, 89, 91, 93, 95, 99, 101, 103, 107, 110, 121, 125

• Chapter 12: 36, 37, 45, 53, 55, 57, 59, 61, 63, 65, 67, 69, 71, 73, 76, 79, 80, 82, 95, 97, 101, 103, 106

• Chapter 13: 26, 29, 43, 45, 47, 51, 53, 57, 61, 63, 65, 67, 69, 71, 73, 75, 77, 79, 81, 83, 85, 87, 89, 91, 93, 95, 111, 113, 115, 117, 119

• Chapter 14: 29, 31, 33, 35, 37, 39, 47, 49, 51, 55, 57, 59, 61, 63, 65, 67, 69, 71, 73, 75, 77, 79, 81, 83, 85, 93, 105, 107

Tentative Schedule

The course schedule follows the sequence of textbook chapters, with lectures and labs aligned to reinforce concepts. Exams are scheduled after major topic blocks, and the final exam is cumulative.

Academic Support

• Academic Success Center, Writing Center, Math Center, MESA Center, and online resources available for tutoring and learning assistance.

• Students with disabilities should contact Disability Support Services for accommodations.

Summary Table: Major Chemistry Topics

Additional info: The syllabus covers all major topics listed in the introductory chemistry curriculum, including measurement, matter, atomic structure, chemical reactions, bonding, gases, solutions, acids and bases, equilibrium, and redox. Laboratory safety and academic integrity are emphasized throughout. Students are expected to complete homework, attend labs, and participate in academic support services for success.