Introduction to Chemistry: Course Overview and Foundational Concepts

Course Format and Description

Course Format

This course is delivered in-person, focusing on face-to-face instruction. Students are required to attend all class meetings and participate in scheduled exams and assignments.

• Attendance: Regular attendance is mandatory for success and is tracked for grading.

• Communication: Course announcements and assignments are managed via Brightspace and email.

Course Description

This course covers qualitative and quantitative aspects of non-organic general chemistry for science majors and pre-health professions. Topics include atomic and molecular structure, the periodic table, acids and bases, chemical reactions, and solutions.

• Emphasis: Foundational principles, problem-solving, and laboratory skills.

• Applications: Preparation for advanced chemistry and health science courses.

Prerequisites and Recommended Preparation

Prerequisites

• Reading & Writing Skills 2 and Math Skills 2 are required.

• Recommended: CHEM 120L (laboratory course).

Students not meeting prerequisites may be dropped from the course.

Required Materials

• Textbook: Introductory Chemistry, Seventh Edition by Nivaldo J. Tro (with Mastering Chemistry access).

• Calculator: Scientific calculator capable of basic and exponential/logarithmic calculations. No sharing allowed during exams.

• Technical Skills: Ability to use email, download/upload documents, and create word processing/presentation files.

Course Learning Outcomes

Upon successful completion, students will be able to:

1. Read and interpret directions.

2. Complete basic algebraic calculations and use a scientific calculator.

3. Download/upload files and documents.

4. Create and submit files in common word processing/presentation formats.

5. Describe the basic structure of an atom using subatomic particles and apply these concepts to nuclear reactions.

6. Formulate and name chemical compounds, including ionic and covalent compounds.

7. Write and balance chemical reactions, using balanced equations in stoichiometric calculations.

8. Describe the difference between solids, liquids, and gases, and apply the gas laws in calculations.

9. Apply density concepts to everyday situations.

10. Describe characteristics and behaviors of acids and bases and the nature of buffer solutions.

11. Identify organic compounds, naming simple hydrocarbons and functional groups.

12. Predict mass, molarity, dilution, and solution stoichiometry.

Major Topics and Weekly Schedule

Week	Main Topic	Subtopics	Assignments
1	Math Review	Basic algebra, scientific notation, unit conversions	Mastering Chapter 2
2	Atoms, Quantum Models & Electrons	Atomic structure, electron configuration	Mastering Chapter 4 & 5
3	Chemical Compounds	Bonding, nomenclature	Mastering Chapter 6
4	Chemical Reactions	Types of reactions, balancing equations	Mastering Chapter 7
5	Stoichiometry	Mole concept, mass-mole conversions	Mastering Chapter 7
6	Intermolecular Forces & Organic Chemistry	Forces, organic nomenclature	Mastering Chapter 10 & 18
7	Solutions	Concentration, molarity, dilution	Mastering Chapter 13
8	Acids and Bases	pH, buffer solutions	Mastering Chapter 14
9	Gases	Gas laws, properties	Mastering Chapter 11
10	Nuclear Chemistry	Radioactivity, nuclear reactions	Mastering Chapter 17

Key Concepts and Definitions

Atomic Structure

Atoms are the basic units of matter, composed of protons, neutrons, and electrons. The arrangement of these subatomic particles determines the element's identity and properties.

• Proton: Positively charged particle in the nucleus.

• Neutron: Neutral particle in the nucleus.

• Electron: Negatively charged particle orbiting the nucleus.

Example: The atomic number (Z) equals the number of protons in an atom.

Formula: $Z = \text{number of protons}$

Chemical Reactions and Stoichiometry

Chemical reactions involve the rearrangement of atoms to form new substances. Stoichiometry is the calculation of reactants and products in chemical reactions.

• Balanced Equation: Shows equal numbers of each atom on both sides.

• Mole Concept: Relates mass to number of particles.

Formula: $\text{Moles} = \frac{\text{Mass (g)}}{\text{Molar Mass (g/mol)}}$

Solutions and Concentration

Solutions are homogeneous mixtures of solute and solvent. Concentration measures the amount of solute in a given volume of solution.

• Molarity (M): Moles of solute per liter of solution.

Formula: $M = \frac{\text{moles of solute}}{\text{liters of solution}}$

Acids and Bases

Acids release hydrogen ions (H+) in solution, while bases release hydroxide ions (OH-). The pH scale measures acidity or basicity.

• Acid: Substance that donates H+ ions.

• Base: Substance that donates OH- ions.

Formula: $\text{pH} = -\log[\text{H}^+]$

Gas Laws

Gas laws describe the 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)

• Ideal Gas Law: $PV = nRT$

Grading and Assessment

Assessment	Weight
Homework	30%
Exams (3, one dropped)	40%
Final Exam	30%

Grading Scale:

• 100-90% = A

• 89.9-80% = B

• 79.9-70% = C

• 69.9-60% = D

• <60% = F

Student Support and Policies

• Accessibility Services: Accommodations for students with disabilities are available.

• Tutoring: Free tutoring is available on campus and online.

• Academic Integrity: Students are expected to adhere to CNM's policies regarding honesty and conduct.

• Veteran Services: Support for military and veteran students is available.

Additional info: The syllabus includes details on campus resources, grading policies, and alternate access plans for online materials.