CHEM 1123 Survey of General, Organic, and Biochemistry: Syllabus and Unit Study Guide

Course Overview

This course, CHEM 1123 – Survey of General, Organic, and Biochemistry, is designed for students in nursing and allied health programs, as well as those seeking a general overview of chemistry. It covers foundational concepts in general chemistry, organic chemistry, and biochemistry, with an emphasis on their relevance to human health.

Course Structure and Grading

• Required Materials: Chemistry: An Introduction to General, Organic and Biological Chemistry (14th edition) by Karen C. Timberlake, scientific calculator, scanning app for PDF uploads.

• Assessment: PDF upload practice (3 pts), five unit exams (100 pts each), five online Mastering Chemistry assignments (20 pts each), comprehensive final exam (100 pts).

• Grading Scale:

  • A: 90.0–100%

  • B: 80.0–89.9%

  • C: 70.0–79.9%

  • D: 60.0–69.9%

  • F: <60.0%

Unit 1: Introduction to Chemistry – Classifying Matter and Doing Calculations

Key Concepts

• Scientific Method: Observation, hypothesis, experiment, conclusion.

• Elements and Symbols: Know names and symbols for common elements (e.g., Ca, Mn, C, Cl, Cr, Co, Cu, F, H, I, Fe, Mg, Mo, N, O, P, K, Se, Na, S, Zn).

• Scientific Notation: Express numbers in scientific notation with correct significant figures.

• Measured vs. Exact Numbers: Distinguish between measured values (with uncertainty) and exact values.

• Significant Figures: Identify, count, and round to the correct number of significant figures.

• Units and Conversions: Recognize metric and English units for length, volume, mass, time, and temperature. Use metric prefixes (kilo, deci, centi, milli, micro).

• Dimensional Analysis: Convert between units using conversion factors and significant figures.

• Density Calculations: $\text{Density} = \frac{\text{Mass}}{\text{Volume}}$

• Classification of Matter: Element, compound, pure substance, mixture, homogeneous mixture, heterogeneous mixture.

• Periodic Table Classification: Metal, nonmetal, metalloid, main group, transition metal, lanthanide, actinide, alkali metal, alkaline earth metal, halogen, noble gas.

• Subatomic Particles: Electron (negative, outside nucleus), proton (positive, in nucleus), neutron (neutral, in nucleus).

• Isotopes: Atomic number, mass number, protons, neutrons, electrons.

• Nuclear Symbols: Alpha ($\alpha$), beta ($\beta$), gamma ($\gamma$) particles.

• Radiation Safety: Preventative methods and biological effects.

Unit 2: Physical and Chemical Changes, Energy Changes, Ionic and Molecular Compounds

Key Concepts

• Physical vs. Chemical Properties/Changes: Classify and describe changes; use endothermic and exothermic terminology.

• States of Matter: Solids, liquids, gases – shape, volume, particle motion.

• Temperature Conversions:

  • $\text{K} = \text{°C} + 273$

  • $\text{°F} = \frac{9}{5} \times \text{°C} + 32$

  • $\text{°C} = \frac{5}{9} \times (\text{°F} - 32)$

• Phase Changes: Melting, freezing, evaporation, condensation, sublimation, deposition; heat gained/lost, endothermic/exothermic.

• Heat Calculations: Use heat of fusion/vaporization to calculate energy required for phase changes.

• Common Ions: Know names and symbols for monoatomic ions (e.g., H+, Na+, Cl-, Mg2+, Fe2+, Fe3+, etc.).

• Valence Electrons: Determine number for main group elements; draw Lewis symbols.

• Chemical Formulas: Count atoms in formulas.

• Ionic Compounds: Name and write formulas using periodic table and polyatomic ions.

• Covalent Compounds: Name and write formulas for binary covalent compounds; draw Lewis structures.

• Polarity: Identify polar covalent bonds using electronegativity; indicate partial charges.

Unit 3: Chemical Reactions, Chemical Quantities, and Gases

Key Concepts

• Chemical Equations: Balance equations; identify reactants and products.

• Energy Diagrams: Activation energy, heat of reaction ($\Delta H$), endothermic/exothermic.

• Types of Reactions: Combination, decomposition, single/double replacement, combustion.

• Oxidation-Reduction: Identify oxidized/reduced substances in reactions.

• Mole Calculations: Molar mass, mass-to-mole and mole-to-mass conversions.

• Stoichiometry: Use balanced equations to determine mole-mole relationships and calculate reactant/product quantities.

• Kinetic Molecular Theory: Properties of gases: low density, compressibility, diffusion, pressure, no definite shape/volume.

• Pressure Units: 1 atm = 760 mmHg = 760 torr.

• Gas Laws:

  • Boyle's Law: $P_1 V_1 = P_2 V_2$ (constant T, n)

  • Charles' Law: $\frac{V_1}{T_1} = \frac{V_2}{T_2}$ (constant P, n)

  • Avogadro's Law: $\frac{V_1}{n_1} = \frac{V_2}{n_2}$ (constant P, T)

  • Gay-Lussac's Law: $\frac{P_1}{T_1} = \frac{P_2}{T_2}$ (constant V, n)

• STP Conditions: 0°C (273 K), 1 atm; molar volume = 22.4 L/mol.

• Dalton's Law: $P_{\text{total}} = P_1 + P_2 + \ldots$

• Breathing Mechanisms: Boyle's Law explains inhalation/exhalation; O2 and CO2 movement via partial pressures.

Unit 4: Solutions, Acids, and Bases

Key Concepts

• Solutions: Identify solute and solvent; properties of solutions.

• Water Structure: Draw Lewis structure; show geometry and partial charges; illustrate hydrogen bonding.

• Solubility: Predict solubility based on polarity; effect of temperature on solubility.

• Dissolution of Ionic Compounds: Write balanced equations for strong electrolytes.

• Electrolytes: Strong, weak, and nonelectrolytes; ion formation in water.

• Saturation: Determine if solution is saturated or unsaturated.

• Concentration Calculations:

  • Mass/Volume Percent: $\text{Percent} = \frac{\text{Mass of solute}}{\text{Volume of solution}} \times 100$

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

• Dilution: $M_1 V_1 = M_2 V_2$

• Eq/mEq Calculations: Convert between moles and equivalents/milliequivalents.

• Osmosis: Predict water movement; classify solutions as isotonic, hypotonic, hypertonic; effects on red blood cells.

• Acids and Bases: Recognize by formula; properties; write formulas/names for common acids and bases.

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

• Acidic, Basic, Neutral: Identify based on pH, [H+], [OH-].

• Normal pH Values:

  Name	pH	Classification
  Blood	7.35–7.45	Basic
  Urine	6.0	Acidic
  Gastric juice	1.6	Acidic
  Bile	8.1	Basic
  Pure water	7.0	Neutral

• Buffers: Role in maintaining pH; bicarbonate and phosphate buffers in blood.

• Acidosis/Alkalosis: Metabolic and respiratory causes.

Unit 5: Introduction to Organic and Biochemistry

Organic Chemistry Concepts

• Organic vs. Inorganic Compounds: Compare properties.

• Carbon Geometry: Tetrahedral for four single bonds.

• Alkanes: Name and write structures for first ten straight-chain alkanes; combustion equation.

• Functional Groups: Identify alkenes, alkynes, aromatics, haloalkanes, alcohols, ethers, thiols, aldehydes, ketones, carboxylic acids, esters, amines, amides.

• Examples and Uses: Name and use for each functional group class.

• Cis/Trans Isomers: Recognize in alkenes.

• Hydroxyl Group Effects: Water solubility and boiling points of alcohols.

• Chirality: Recognize chiral molecules.

Biochemistry Concepts

• Monosaccharides: Classify by functional group and carbon number; recognize D and L forms.

• Haworth Structures: Recognize cyclic forms of fructose and glucose (alpha and beta).

• Disaccharides/Polysaccharides: Hydrolysis equations; identify glycosidic bonds; characteristics of amylose, amylopectin, glycogen, cellulose.

• Lipids: Classes and features; identify fatty acids as saturated, monounsaturated, polyunsaturated; steroid nucleus; functional groups in steroids.

• Cell Membranes: Fluid mosaic model; lipids, proteins, cholesterol, carbohydrates.

• Amino Acids and Proteins: General structure; classes (polar, nonpolar, acidic, basic); peptide linkage formation.

• Protein Structure: Primary, secondary, tertiary, quaternary levels.

• Protein Classes: Structural, contractile, transport, storage, hormone, enzyme, protection; examples for each.

• Denaturation: Effects and agents causing denaturation.

• Enzyme Action: Lock-and-key and induced fit models; factors influencing activity.

Comprehensive Final Exam Objectives

• Apply all calculation, classification, and conceptual skills from Units 1–5.

• Integrate knowledge across general, organic, and biochemistry topics.

• Demonstrate proficiency in unit conversions, chemical equations, solution chemistry, acid-base calculations, organic functional groups, and biomolecule structure/function.

Course Schedule (Spring 2026)

Date	Topic/Assignment
Jan 21–Feb 9	Unit 1, Upload Practice, MC #1, Unit 1 Exam
Feb 11–Mar 4	Unit 2, MC #2, Unit 2 Exam
Mar 9–Apr 1	Unit 3, MC #3, Unit 3 Exam
Apr 6–Apr 20	Unit 4, MC #4, Unit 4 Exam
Apr 22–May 11	Unit 5, MC #5, Unit 5 Exam
May 13	Comprehensive Final Exam

Note: All assignments and exams must be completed by May 15th. Schedule may change due to extenuating circumstances; check Moodle and campus email for updates.

Grade Record Table

Assignment	Points Possible
PDF Upload Practice	3
MC #1–#5	20 each
Unit 1–5 Exams	100 each
Comprehensive Final	100
Total	703

Additional info: This syllabus provides a comprehensive outline of the course content, learning objectives, and assessment structure for a one-semester general, organic, and biochemistry course. It is suitable for exam preparation and as a reference for the scope of topics covered in CHEM 1123.