General Chemistry I: Module Objectives Overview

Module 1: Introduction to Chemistry

Course Structure, Policies, and Chemistry Fundamentals

This module introduces students to the foundational aspects of chemistry, including course expectations, basic terminology, and the scope of the subject.

• Course Policies: Understanding course structure, policies, and instructor expectations is essential for success.

• Key Definitions: Chemistry is the study of matter, its properties, and the changes it undergoes.

• Classification of Matter: Matter can be classified as elements, compounds, and mixtures. Mixtures can be homogeneous or heterogeneous.

• Physical vs. Chemical Properties: Physical properties can be observed without changing the substance's identity (e.g., melting point), while chemical properties describe a substance's ability to undergo chemical changes (e.g., flammability).

• States of Matter: Matter exists as solids, liquids, and gases, each with distinct properties at macroscopic and submicroscopic levels.

• Chemical vs. Physical Changes: Chemical changes result in new substances, while physical changes do not alter the chemical identity.

Example: Melting ice is a physical change; burning wood is a chemical change.

Module 2: Atomic Structure and the Periodic Table

Atoms, Elements, and the Periodic Table

This module explores the structure of atoms, the arrangement of elements, and the use of the periodic table as a tool for understanding chemical behavior.

• Atomic Structure: Atoms are composed of protons, neutrons, and electrons. Protons and neutrons reside in the nucleus, while electrons occupy orbitals around the nucleus.

• Subatomic Particles: Protons (positive charge), neutrons (neutral), and electrons (negative charge) have distinct properties and locations within the atom.

• Atomic Number and Mass Number: The atomic number is the number of protons; the mass number is the sum of protons and neutrons.

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

• Periodic Table Organization: Elements are arranged by increasing atomic number. Groups (columns) and periods (rows) reflect recurring chemical properties.

• Elemental Symbols: Each element is represented by a unique one- or two-letter symbol.

• Predicting Properties: The periodic table can be used to predict trends in atomic radius, ionization energy, and other properties.

Example: Sodium (Na) is in Group 1 and is a highly reactive metal; chlorine (Cl) is in Group 17 and is a reactive nonmetal.

Module 3: Chemical Reactions and Stoichiometry

Types of Chemical Reactions and Quantitative Relationships

This module covers the identification, classification, and quantitative analysis of chemical reactions.

• Chemical Equations: Represent chemical reactions using symbols and formulas. Equations must be balanced to obey the law of conservation of mass.

• Types of Reactions: Synthesis, decomposition, single replacement, double replacement, and combustion reactions.

• Stoichiometry: The calculation of reactants and products in chemical reactions using balanced equations.

• Limiting Reactant: The reactant that is completely consumed first, limiting the amount of product formed.

• Theoretical Yield: The maximum amount of product that can be formed from given reactants.

• Percent Yield: $\text{Percent Yield} = \frac{\text{Actual Yield}}{\text{Theoretical Yield}} \times 100$

Example: In the reaction $2H_2 + O_2 \rightarrow 2H_2O$, two moles of hydrogen react with one mole of oxygen to produce two moles of water.

Module 4: Measurement, Data Analysis, and Applications

Measurement, Significant Figures, and Data Interpretation

This module emphasizes the importance of accurate measurement, data analysis, and the application of chemistry concepts to real-world problems.

• Measurement: Use of SI units and dimensional analysis to ensure accuracy and consistency in calculations.

• Significant Figures: The number of meaningful digits in a measurement. Rules for determining significant figures in calculations must be followed.

• Data Analysis: Interpretation of experimental data, including the use of graphs, tables, and statistical methods.

• Problem Solving: Application of chemical principles to solve quantitative and conceptual problems.

• Scientific Method: Systematic approach to experimentation and hypothesis testing.

Example: Calculating the density of a substance using $\text{Density} = \frac{\text{Mass}}{\text{Volume}}$.

Additional info: These module objectives provide a structured overview of the foundational topics in a General Chemistry I course, aligning with standard curriculum chapters such as atomic structure, chemical reactions, and measurement techniques.