Introductory Chemistry (CHM-117) Syllabus and Study Guide

Course Overview

Course Information

This syllabus outlines the structure and requirements for Introductory Chemistry (CHM-117) at County College of Morris. The course is designed for students in health-related and technical programs, providing foundational knowledge in chemistry with applications to biology, nutrition, horticulture, and related fields.

• Credits: 3 hours (lecture only)

• Prerequisites: Placement in College Level Math or completion of MAT-016/MAT-026 with a minimum grade of C

• Required Textbook: Chemistry: An Introduction to General, Organic and Biological Chemistry (14th Edition) by Karen Timberlake

• Calculator: Scientific calculator required (graphing calculators not permitted on quizzes/exams)

• Supplemental Materials: Mastering Chemistry online access

Course Description

Scope and Emphasis

This course introduces the basic concepts of inorganic, organic, and biochemistry. Emphasis is placed on the relationship of chemistry to allied health programs and technical fields. Students will learn about the structure and properties of matter, chemical reactions, and the role of chemistry in biological systems.

• Applications: Respiratory Therapy, Public Health, Biology, Nutrition, Landscape/Horticultural Technology, and related programs

Learning Outcomes

Skills and Competencies

Upon successful completion, students will be able to:

1. Apply the scientific method, analyze data, and draw conclusions from evidence

2. Use chemistry and mathematical concepts to solve problems

3. Identify key terms and concepts in chemistry

4. Classify molecules based on their functional groups

5. Relate properties of elements to their location in the periodic table

6. Describe the properties, structures, and functions of carbohydrates, lipids, nucleic acids, and proteins

Course Content Outline

Topics and Chapters

The following topics are covered, each corresponding to a chapter in the textbook:

• Scientific Method, Scientific Notation (Chapter 1)

• Measurements (Chapter 2)

• Matter and Energy (Chapter 3)

• Atoms and Elements (Chapter 4)

• Ionic and Molecular Compounds (Chapter 5)

• Chemical Reactions and Quantities (Chapter 6)

• Gases (Chapter 7)

• Solutions (Chapter 8)

• Equilibrium and Le Chatelier's Principle; Acids and Bases (Chapter 9, 10)

• Intro to Organic Chemistry: Hydrocarbons (Chapter 11)

• Alcohols, Thiols, Ethers, Aldehydes, and Ketones (Chapter 12)

• Carboxylic Acids, Esters, Amines, and Amides (Chapter 13)

• Lipids (Chapter 14)

• Amino Acids, Proteins, and Enzymes (Chapter 15, 16)

• Nucleic Acids and Protein Synthesis (Chapter 17)

• Metabolic Pathways and Energy Production (Chapter 18)

Grading and Assessment

Grading Policy

Grades are determined by the final course average, calculated as follows:

• Quiz Average: 10% of final course average

• Homework Average: 5% of final course average

• Discussion Post Average: 5% of final course average

• Lecture Exam Average: 60% of final course average

• Final Exam: 20% of final course average

Letter Grade Conversion Table

The following table shows the correspondence between letter grades, numerical averages, and GPA quality points:

Letter Grade	Numerical Average	GPA Quality Points
A	93.0 – 100.0	4.00
A-	90.0 – 92.9	3.67
B+	87.0 – 89.9	3.33
B	83.0 – 86.9	3.00
B-	80.0 – 82.9	2.67
C+	77.0 – 79.9	2.33
C	70.0 – 76.9	2.00
D	60.0 – 69.9	1.00
F	59.9 or below	0.00

Course Policies

Attendance

• Regular attendance is strongly correlated with higher grades.

• Absences may affect your ability to keep up with course material and assessments.

• Attendance during inclement weather is managed via the CCM Alert system.

Academic Integrity

• All students are expected to adhere to the highest standards of honesty and integrity.

• Cheating, plagiarism, unauthorized collaboration, and other forms of academic dishonesty are strictly prohibited.

• Violations may result in disciplinary action and impact your academic record.

Technology Requirements

• Access to Blackboard (Learning Management System) is required for course materials, quizzes, and communication.

• Students must have a computer with internet access, webcam, and microphone for online proctoring (SmarterProctoring).

• Homework is completed online using Mastering Chemistry.

Key Chemistry Concepts (from Course Outline)

Scientific Method and Measurement

The scientific method is a systematic approach to investigation, involving observation, hypothesis formation, experimentation, and analysis. Measurement in chemistry involves quantifying physical properties using units such as grams, liters, and meters.

• Scientific Notation: Used to express very large or small numbers, e.g., $6.02 \times 10^{23}$

• SI Units: Standard units for scientific measurement (meter, kilogram, second, mole, etc.)

Matter and Energy

Matter is anything that has mass and occupies space. Energy is the capacity to do work or produce heat.

• States of Matter: Solid, liquid, gas

• Law of Conservation of Mass: $\text{Mass}_{\text{reactants}} = \text{Mass}_{\text{products}}$

Atoms, Elements, and Compounds

Atoms are the basic units of matter, composed of protons, neutrons, and electrons. Elements are pure substances consisting of one type of atom. Compounds are substances formed from two or more elements chemically bonded.

• Atomic Number ($Z$): Number of protons in the nucleus

• Mass Number ($A$): $A = Z + \text{number of neutrons}$

• Chemical Formula: Represents the composition of compounds, e.g., $\text{H}_2\text{O}$

Chemical Reactions and Quantities

Chemical reactions involve the transformation of substances via breaking and forming chemical bonds. Quantitative relationships are described by stoichiometry.

• Balanced Equation: $\text{CH}_4 + 2\text{O}_2 \rightarrow \text{CO}_2 + 2\text{H}_2\text{O}$

• Mole Concept: $1 \text{mol} = 6.022 \times 10^{23}$ particles

Organic and Biological Chemistry

Organic chemistry focuses on carbon-containing compounds, while biological chemistry examines molecules essential for life, such as carbohydrates, lipids, proteins, and nucleic acids.

• Functional Groups: Specific groups of atoms within molecules that determine chemical properties (e.g., hydroxyl, carboxyl, amino)

• Biomolecules: Carbohydrates, lipids, proteins, nucleic acids

Example: Carbohydrate Structure

• Monosaccharide: Simple sugar, e.g., glucose ($\text{C}_6\text{H}_{12}\text{O}_6$)

• Disaccharide: Two monosaccharides joined, e.g., sucrose

Additional Info

• Students are expected to use online resources and participate in online assessments.

• Specialized equipment may be required for proctored online exams.

• Course policies regarding attendance, academic integrity, and technology use are strictly enforced.