General, Organic, and Biological Chemistry for Nursing (CHE1210) – Syllabus and Study Guide

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General, Organic, and Biological Chemistry for Nursing (CHE1210)

Course Overview

This course introduces the foundational principles of inorganic, organic, and biological chemistry with a focus on their relevance to nursing and health sciences. Students will learn about the structure and function of biological molecules, chemical reactions, and the chemical basis of physiological processes.

Textbook: General, Organic, and Biological Chemistry, 4th edition, Laura D. Frost & S. Todd Deal
Schedule: MWF, 8:30am–9:20am, Brock 109
Professor: Dr. Adam Brunet
Office Hours: Monday and Tuesday 10:30am–12:30pm and by appointment

Course Objectives

To learn the basic and advanced concepts of chemistry, including cellular biology, biochemistry, and physiology.
To develop study habits for success in health science education.
To understand homeostasis, the relationship between structure and function, and chemical physiology in body systems.

Major Topics and Subtopics

1. Chemistry Basics – Matter and Measurement

This section covers the fundamental concepts of chemistry, including the nature of matter, measurement techniques, and the scientific method.

Matter: Anything that has mass and occupies space. Classified as elements, compounds, and mixtures.
Measurement: Use of SI units (meter, kilogram, second, mole, etc.) and understanding significant figures.
Scientific Method: Systematic approach to research and experimentation.
Example: Measuring the mass of a sample using a balance and reporting the value with correct significant figures.

2. Atoms and Radioactivity

This topic explores atomic structure, isotopes, and the basics of radioactivity.

Atom: The smallest unit of an element, consisting of protons, neutrons, and electrons.
Isotopes: Atoms of the same element with different numbers of neutrons.
Radioactivity: Spontaneous emission of particles or energy from unstable atomic nuclei.
Equation: (Beta decay of carbon-14)

3. Compounds – How Elements Combine

This section discusses chemical bonding and the formation of compounds.

Ionic Bonds: Formed by the transfer of electrons from one atom to another (e.g., NaCl).
Covalent Bonds: Formed by the sharing of electrons between atoms (e.g., H2O).
Example: Water (H2O) is a covalent compound formed by sharing electrons between hydrogen and oxygen.

4. Chemical Reactions

Chemical reactions involve the transformation of substances through the breaking and forming of bonds.

Reactants and Products: Substances present before and after the reaction.
Types of Reactions: Synthesis, decomposition, single replacement, double replacement, and combustion.
Equation:

5. States of Matter and Their Attractive Forces

This topic covers the physical states of matter and the forces that hold particles together.

States: Solid, liquid, gas.
Intermolecular Forces: Hydrogen bonding, dipole-dipole, London dispersion forces.
Gas Laws: Relationships between pressure, volume, temperature, and amount (e.g., Boyle's Law: ).

6. Carbohydrates

Carbohydrates are essential biomolecules that provide energy and structural support.

Monosaccharides: Simple sugars (e.g., glucose, fructose).
Disaccharides: Two monosaccharides linked together (e.g., sucrose).
Polysaccharides: Long chains of monosaccharides (e.g., starch, glycogen).

7. Food as Fuel – Overview of Metabolism

Metabolism refers to the chemical processes that occur within living organisms to maintain life.

Catabolism: Breakdown of molecules to release energy.
Anabolism: Synthesis of complex molecules from simpler ones.
ATP: Adenosine triphosphate, the primary energy carrier in cells.

8. Solution Chemistry – Sugar and Water Do Mix

This section explains the properties of solutions, solubility, and concentration calculations.

Solution: Homogeneous mixture of solute and solvent.
Concentration: Amount of solute per unit volume of solution (e.g., molarity ).
Solubility: The ability of a substance to dissolve in a solvent.

9. Acids, Bases, and Buffers in the Body

Acids and bases are crucial for maintaining physiological pH, and buffers help resist changes in pH.

Acid: Substance that donates protons (H+).
Base: Substance that accepts protons.
pH Scale: Measures acidity or basicity; .
Buffer: Solution that resists changes in pH when acids or bases are added.
Example: Bicarbonate buffer system in blood:

10. Proteins – Workers of the Cell

Proteins are large biomolecules essential for structure, function, and regulation of the body's tissues and organs.

Amino Acids: Building blocks of proteins.
Peptide Bonds: Covalent bonds linking amino acids.
Enzymes: Proteins that catalyze biochemical reactions.

11. Nucleic Acids – Big Molecules with a Big Role

Nucleic acids store and transmit genetic information.

DNA (Deoxyribonucleic Acid): Stores genetic information.
RNA (Ribonucleic Acid): Involved in protein synthesis.
Nucleotides: Monomers of nucleic acids, composed of a sugar, phosphate, and nitrogenous base.

Assessment and Grading

Grades are based on homework, quizzes, exams, and participation. The following table summarizes the letter grade assignments:

Letter Grade	Percentage
A	93–100%
A-	90–92.99%
B+	87–89.99%
B	83–86.99%
B-	80–82.99%
C+	77–79.99%
C	73–76.99%
C-	70–72.99%
D+	67–69.99%
D	63–66.99%
D-	60–62.99%
F	0–59.99%

Additional Information

Attendance: Required for all classes; participation is part of the grade.
Homework: 10% of grade, completed online.
Exams: Four exams and a final exam; no make-ups for missed exams.
Accessibility: Accommodations available for students with disabilities.

Additional info: The above study guide is based on the course syllabus and schedule, providing a structured overview of the main chemistry topics relevant to nursing students. For detailed content, refer to the assigned textbook chapters and lecture materials.