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:

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.