Chemistry 10: General, Organic, and Biological Chemistry – Course Overview and Study Guide

Chemistry 10: Course Overview

Course Description

This course introduces students to the fundamental principles of inorganic chemistry and provides an introduction to organic and biological chemistry. It is designed for health science majors and non-science majors requiring a one-semester chemistry course with laboratory. The course prepares students for higher-level chemistry courses and emphasizes problem-solving using the scientific method.

Prerequisites

• Passing grade (C or better) in MATH 130

Course Measurable Objectives (CMOs)

• Express measurements using correct significant figures; perform calculations and solve problems using conversion factors.

• Analyze atomic structure; write electron configurations for elements in the Periodic Table.

• Differentiate types of radioactivity; write nuclear equations; solve problems relating to half-lives.

• Identify types of chemical bonds; predict bond polarity; write names and formulas for inorganic compounds.

• Compare and contrast the three states of matter and forms of energy; evaluate energy profiles of reactions; calculate energy for changes of state.

• Complete and balance chemical equations, including oxidation-reduction reactions; apply the mole concept to solve for quantities in reactions.

• Explain chemical equilibrium using reversible reactions.

• Apply gas laws to describe and solve problems involving gases.

• Solve solution problems including solubility, concentration, and dilution; compare properties such as osmosis, dialysis, electrolytes, and non-electrolytes.

• Identify characteristics of acids and bases; calculate pH; evaluate buffer systems.

• Compare and contrast organic compound structures and properties; apply IUPAC naming; identify functional groups; draw structural formulas.

• Demonstrate proper and safe laboratory techniques; record and analyze data; form conclusions from experiments.

Student Learning Outcomes (SLOs)

• Molecular Bonding: Demonstrate understanding of chemical bonding concepts, including Lewis structures, molecular geometry, and bond types (ionic, nonpolar covalent, polar covalent).

• Acids, Bases, and pH: Predict products of neutralization reactions; compare acidity based on pH; calculate concentrations of hydronium and hydroxide ions, and pH of solutions.

Course Topics and Schedule

Lecture and Laboratory Topics

• Chapter 1: Introduction to Chemistry

• Chapter 2: Measurements (Significant Figures, Units, Conversion Factors)

• Chapter 3: Matter & Energy (States of Matter, Energy Changes)

• Chapter 4: Atoms & Elements (Atomic Structure, Electron Configuration)

• Chapter 5: Electronic Structure & Periodic Trends

• Chapter 6: Ionic & Molecular Compounds (Bonding, Polarity)

• Chapter 7: Chemical Reactions & Quantities (Balancing Equations, Mole Concept)

• Chapter 8: Gases (Gas Laws, Properties)

• Chapter 9: Solutions (Solubility, Concentration, Electrolytes)

• Chapter 10: Acids, Bases & Equilibrium (pH, Buffers, Ionization)

• Chapter 11: Organic Chemistry (Functional Groups, IUPAC Naming)

• Chapter 5 (Nuclear Chemistry): Types of Radioactivity, Nuclear Equations, Medical Applications

Laboratory Techniques and Procedures

• Safe laboratory procedures and proper attire (lab coat, goggles, gloves, closed-toe shoes, long pants)

• Use and care of laboratory equipment (balances, pipets, burets, glassware)

• Measurement techniques (mass, volume, temperature, pH)

• Preparation and dilution of solutions

• Calorimetry and energy measurements

• Volumetric analysis and titrations

• Recording and analyzing experimental data

• Waste disposal and laboratory safety regulations

Sample Laboratory Safety Rules

• Always wear chemical splash goggles and lab coat.

• Wear closed-toe, non-absorbent shoes and long pants.

• No food or drink in the lab.

• Dispose of chemical waste in labeled containers; never return unused chemicals to original bottles.

• Report injuries and accidents immediately; fill out incident reports.

• Know the location of emergency equipment (safety shower, eyewash, fire extinguisher).

• Clean work areas before and after experiments.

Key Chemistry Concepts

Measurements and Significant Figures

Measurements in chemistry must be expressed with the correct number of significant figures to reflect the precision of the instrument used. Conversion factors are used to change units and solve quantitative problems.

• Example: Converting 25.0 cm to meters using the conversion factor $1 \text{ m} = 100 \text{ cm}$.

• Formula: $\text{Value in meters} = \text{Value in cm} \times \frac{1 \text{ m}}{100 \text{ cm}}$

Atomic Structure and Electron Configuration

Atoms consist of protons, neutrons, and electrons. Electron configuration describes the arrangement of electrons in an atom.

• Example: Electron configuration for sodium: $1s^2 2s^2 2p^6 3s^1$

Nuclear Chemistry

Nuclear chemistry involves the study of radioactivity, nuclear reactions, and their applications.

• Types of Radioactivity: Alpha ($\alpha$), Beta ($\beta$), Gamma ($\gamma$) emissions

• Half-life Formula: $N = N_0 \left( \frac{1}{2} \right)^{\frac{t}{t_{1/2}}}$

Chemical Bonding

Chemical bonds include ionic, covalent, and polar covalent bonds. Bond polarity is determined by the difference in electronegativity between atoms.

• Lewis Structures: Electron-dot diagrams representing valence electrons

• Molecular Geometry: VSEPR theory predicts shapes (linear, bent, trigonal planar, tetrahedral)

States of Matter and Energy

Matter exists as solids, liquids, and gases. Energy changes accompany phase transitions and chemical reactions.

• Energy Calculation: $q = m \cdot c \cdot \Delta T$ (where $q$ is heat, $m$ is mass, $c$ is specific heat, $\Delta T$ is temperature change)

Chemical Reactions and Quantities

Chemical reactions are represented by balanced equations. The mole concept is used to relate quantities of reactants and products.

• Balancing Equations: Ensure equal numbers of atoms on both sides.

• Mole Calculation: $\text{Moles} = \frac{\text{Mass}}{\text{Molar Mass}}$

Gas Laws

Gas behavior is described by laws such as Boyle's, Charles', and the Ideal Gas Law.

• Ideal Gas Law: $PV = nRT$

• Variables: $P$ = pressure, $V$ = volume, $n$ = moles, $R$ = gas constant, $T$ = temperature

Solutions

Solutions are homogeneous mixtures. Key properties include solubility, concentration, and electrolyte behavior.

• Concentration Formula: $\text{Molarity} = \frac{\text{Moles of solute}}{\text{Liters of solution}}$

• Electrolytes: Substances that conduct electricity in solution

Acids, Bases, and Equilibrium

Acids and bases are characterized by their ionization in water, strength, and reactions. The pH scale measures acidity.

• pH Formula: $\text{pH} = -\log_{10}[\text{H}^+]$

• Buffer Systems: Resist changes in pH upon addition of acid or base

Organic Chemistry

Organic chemistry focuses on compounds containing carbon. Functional groups and IUPAC naming are essential for classification.

• Functional Groups: Alcohols, ethers, aldehydes, ketones, carboxylic acids, amines

• IUPAC Naming: Systematic method for naming organic compounds

Laboratory Objectives

• Implement safe laboratory procedures

• Maintain a chemistry lab notebook

• Use laboratory equipment correctly

• Perform experiments using standard techniques

• Record and analyze data

• Calculate percent error: $\text{Percent Error} = \frac{|\text{Experimental Value} - \text{True Value}|}{\text{True Value}} \times 100\%$

• Understand precision and accuracy

Grading Policy

Component	Points	Percentage
Lab Reports (14)	240	24%
Lab Equipment Quiz	10	1%
Lecture Exams (3)	200	25%
Quizzes (4)	80	15%
Homework (5)	50	10%
Final Exam	220	25%
Total	1000	100%

Letter Grade Scale

Grade	Percentage
A	90–100%
B	80–89%
C	70–79%
D	55–69%
F	Below 55%

Tips for Success

• Study regularly; plan for 8 hours per week outside of class.

• Actively participate and solve problems independently.

• Read lecture notes and assigned chapters before and after class.

• Practice with assigned and additional problems.

• Attend all lectures, labs, and office hours for support.

Academic Honesty

• Cheating and plagiarism are strictly prohibited and result in severe penalties.

• Lab reports must be written individually unless group work is specified.

• Turnitin will be used to check for similarity in assignments.

Laboratory Safety and Cleanliness

• Follow all safety regulations and wear appropriate attire.

• Clean work areas before and after experiments.

• Know emergency procedures and equipment locations.

Course Schedule (Sample Weeks)

Week	Tuesday Lecture	Thursday Lecture	Lab
1	Course Intro; Syllabus; Chapter 1	Chapter 1 (cont.)	Lab Safety & Equipment
2	Chapter 2 – Measurements	Chapter 2 (cont.)	Common Lab Measurements
3	Chapter 3 – Matter & Energy	Chapter 3 (cont.)	Density
4	Dimensional Analysis Review	Chapter 4 – Atoms & Elements	Conversion Factors
5	Catch-up / Review	Exam #1 (Ch 1–4)	Calorimetry
6	Chapter 5 – Electronic Structure	Chapter 5 (cont.)	Electron Energies
7	Chapter 6 – Ionic & Molecular Compounds	Chapter 6 (cont.)	Covalent Bonding
8	Chapter 7 – Chemical Reactions	Chapter 7 (cont.)	Writing Equations
9	Chapter 8 – Gases	Chapter 8 (cont.)	Stoichiometry
10	Catch-up / Exam Review	Exam #2 (Ch 6–8)	Properties of Gases
11	Chapter 9 – Solutions	Chapter 9 (cont.)	Electrolytes & Dilution
12	Chapter 10 – Acids, Bases & Equilibrium	Chapter 10 (cont.)	Solubility & Separations
13	Chapter 11 – Organic Chemistry	Exam #3 (Ch 9–11)	pH & Buffers
14	No Class Monday	Chapter 5 – Nuclear Chemistry	Analysis of Ions
15	Catch-up Review	Organic Compounds / Check-out
16	Final Exam Week	No class	No class

Additional Info

• Internet access, scientific calculator, and proper lab attire are required.

• Canvas is used for assignment submission and course materials.

• Student resources are available for health, academic, and accessibility support.