Introductory Chemistry I (CHEM-1405) Syllabus & Study Guide

Introductory Chemistry I (CHEM-1405)

Course Overview

This course is designed for non-science majors and covers the fundamental concepts of chemistry. Topics include the periodic table, atomic structure, chemical bonding, chemical reactions, stoichiometry, states of matter, properties of metals, nomenclature of compounds, chemical nomenclature, acid-base theory, oxidation-reduction, and solutions. Emphasis is placed on descriptive chemistry and practical applications.

Instructor Contact Information

• Professor: Dr Prem Adhikari

• Email: [e-mail]

• Office: B2074

• Phone: [phone]

• Office Hours: Monday, Tuesday & Thursday: 12:00-1:00; Friday: 7:00-9:00 AM

• Response Time: Instructors typically respond to emails within 24 hours (may be delayed on weekends/holidays).

Course Description

This course introduces basic chemical principles through lecture and laboratory. Students will learn to apply chemical concepts to everyday life and develop problem-solving skills relevant to chemistry.

State-Defined Learning Outcomes

• Apply chemical concepts to interpret and solve problems.

• Demonstrate understanding of chemical nomenclature, reactions, and properties.

• Utilize scientific notation and measurement in chemical calculations.

Instructor-Defined Learning Outcomes

The following weekly topics outline the major learning objectives and skills students are expected to master.

Week 1: Measurement & Significant Figures

• Place Values, Positive and Negative Numbers: Understanding the decimal system and how to interpret numbers in scientific calculations.

• Scientific Notation: Expressing very large or small numbers in the form $a \times 10^n$.

• Significant Figures: Identifying which digits in a measurement are meaningful for precision.

• Example: $0.00450$ has three significant figures.

Week 2: Atoms & Elements, Metric & SI Units

• Metric & SI Units: Standard units of measurement in science (meter, kilogram, second, mole, etc.).

• Temperature: Celsius, Kelvin, and Fahrenheit scales.

• Atomic Structure: Protons, neutrons, electrons, atomic number, and mass number.

• Example: Carbon-12 has 6 protons, 6 neutrons, and 6 electrons.

Week 3: Elements, Periodic Table, Atoms, Isotopes, Periodic Properties

• Periodic Table: Arrangement of elements by increasing atomic number; groups and periods.

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

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

• Example: Sodium (Na) and Potassium (K) are both alkali metals in Group 1.

Week 4: Lewis Structure, Electronegativity & Polarity, VSEPR

• Lewis Structures: Diagrams showing the bonding between atoms and lone pairs of electrons.

• Electronegativity: The tendency of an atom to attract electrons in a bond.

• Polarity: Distribution of electrical charge over the atoms in a molecule.

• VSEPR Theory: Predicts the three-dimensional shape of molecules based on electron pair repulsion.

• Example: Water ($H_2O$) has a bent shape due to two lone pairs on oxygen.

Week 5/6: Chemical Formulas, Moles, Stoichiometry, Chemical Reactions

• Mole Concept: The mole is a counting unit for atoms, molecules, and ions. $1 \text{ mole} = 6.022 \times 10^{23}$ particles.

• Molar Mass: The mass of one mole of a substance, expressed in grams per mole.

• Stoichiometry: Calculations involving the quantities of reactants and products in chemical reactions.

• Types of Chemical Reactions: Combination, decomposition, single replacement, double replacement, combustion.

• Example: $2H_2 + O_2 \rightarrow 2H_2O$

Week 5/6: Gas Laws, Pressure, Volume, Temperature, Partial Pressure

• Gas Laws: Relationships between pressure, volume, temperature, and amount of gas.

• 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)

• Avogadro's Law: $\frac{V_1}{n_1} = \frac{V_2}{n_2}$ (at constant temperature and pressure)

• Ideal Gas Law: $PV = nRT$

• Partial Pressure: The pressure exerted by each gas in a mixture.

Week 7: Solutions, Acids & Bases, pH, Buffers

• Solutions: Homogeneous mixtures of solute and solvent.

• Electrolytes vs. Nonelectrolytes: Electrolytes conduct electricity; nonelectrolytes do not.

• Acids & Bases: Brønsted-Lowry theory: acids donate protons ($H^+$), bases accept protons.

• pH Scale: Measures acidity or basicity; $pH = -\log[H^+]$

• Buffers: Solutions that resist changes in pH.

• Example: Vinegar (acetic acid) is a weak acid; sodium hydroxide is a strong base.

Week 8: Radiation

• Types of Radiation: Alpha ($\alpha$), beta ($\beta$), positron, gamma ($\gamma$).

• Radioactive Decay: The process by which unstable nuclei lose energy by emitting radiation.

• Half-life: The time required for half of the radioactive atoms to decay.

• Applications: Use of radioisotopes in medicine (diagnosis and treatment).

• Example: $^{14}C$ decay is used in radiocarbon dating.

Texas Core Objectives

• Critical Thinking Skills: Innovation, inquiry, analysis, evaluation, and synthesis of information.

• Communication Skills: Effective development, interpretation, and expression of ideas.

• Empirical & Quantitative Skills: Manipulation and analysis of numerical data.

• Teamwork: Ability to work effectively with others.

• Social Responsibility: Knowledge of civic responsibility and engagement.

Required Course Materials

• Lecture Materials (provided via online links)

• Laboratory Materials (provided via online links)

Graded Work

Evaluation Item	Points
Quiz 1	45
Quiz 2	45
Quiz 3	45
Exam 1	100
Exam 2	100
Exam 3	100
Homework Assignments	200 (10 submissions @ 20 pts each)
Lab Reports	200 (10 labs @ 20 pts each)
Discussion Topics	15
Syllabus Quiz	10

Grade Breakdown

Grade	Range
A	90-100
B	80-89
C	70-79
D	60-69
F	59 or less

Course Schedule

The course schedule provides a summary of topics and due dates. The instructor will notify students of any changes during the term.

Additional info: This syllabus is structured to support GOB Chemistry students in mastering foundational chemical concepts, preparing for exams, and understanding the relevance of chemistry in everyday life and health sciences.