Mikes Videos - General Chemistry Lesson Outline - Chapter 0 - General and Lab Concepts Review

Sep 17, 2026

Uploaded by Sage

General Chemistry lesson outline covering core concepts from Chapter 0 through lab basics and early atomic theory. Topics include atoms, ions, molecules, and naming ionic, molecular, binary acid, and oxyacid compounds; metric units, dimensional analysis, significant figures, percent error, and lab safety. It also introduces pH-related weights and measures plus Beer-Lambert Law variables and examples. Subsequent chapters begin stoichiometry with moles, reaction balancing, formulas, percent composition, limiting reactants, and yields, then atomic structure, Bohr model, orbitals, quantum numbers, and electron configuration.

LanguageEnglish

CategoryExam

FormatPDF

Pages61

Reading Time2 h 34 min

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Chapter 0: General and Lab Concepts Review

Lesson 0.1 – Atoms, Ions, and Molecules

Lesson 0.2 – Naming Ionic Compounds

Lesson 0.3 – Naming Molecular Compounds and Acids

Lesson 0.4 – Metric Units and Dimensional Analysis

Lesson 0.5 – Significant Figures and Percent Error

Lesson 0.6 – Lab Safety

Lesson 0.7 – Weights, Measures, and pH

Lesson 0.8 – Beer-Lambert Law

Chapter 1: Stoichiometry

Lesson 1.1 – The Mole and Molecular Weights

Lesson 1.2 – Balancing Reactions

Lesson 1.3 – Molecular Formulas and Percent Composition

Lesson 1.4 – Product and Reactant Amounts

Lesson 1.5 – Limiting Reactants

Lesson 1.6 – Theoretical and Percent Yields

Chapter 2: Atomic and Electronic Structure

Lesson 2.1 – Atomic Structure and the Bohr Model

Lesson 2.2 – Atomic Orbitals

Lesson 2.3 – Quantum Numbers

Lesson 2.4 – Electron Configuration

Lesson 2.5 – Condensed Electron Configuration, Valence, and Energy Diagrams

Chapter 0: General and Lab Concepts Review Lesson 0.1 – Atoms, Ions, and Molecules • Atom – smallest unit of an element • Molecule – atom bonded to at least one other atom • Ion – atom that has lost of gained an electron Lesson 0.2 – Naming Ionic Compounds • Diatomic elements o H2, N2, O2, F2, Cl2, Br2, and I2 • Allotropes – Elemental molecules with different formulas. i.e. O2 and O3 • Ionic compounds – metal and nonmetal (can be polyatomic too) • Molecular compounds – two or more nonmetals • Naming ionic compounds o 1. Name the metal. o 2. Write the metal’s oxidation state as a Roman numeral in parenthesis. o 3. Name the nonmetal using an “ide” ending 􀁨 Ex. Iron (II) Chloride, FeCl2 Lesson 0.3 – Naming Molecular Compounds and Acids • Naming molecular compounds o 1. Give the appropriate numerical prefix to the first element o 2. Name the first element using its regular name on the periodic table o 3. Give the appropriate numerical prefix to the second element o 4. Name the nonmetal using an “ide” ending 􀁨 Ex. dinitrogen monoxide, N2O • Naming binary acids o 1. Hydro o 2. Insert the name of element 2, replacing “-ine” with “-ic acid” 􀁨 Ex. hydrochloric acid, HCl • Naming oxyacids o HClO – hypochlorous acid o HClO2 – chlorous acid o HClO3 – chloric acid o HClO4 – perchloric acid Lesson 0.4 – Metric Units and Dimensional Analysis Lesson 0.5 – Significant Figures and Percent Error Significant Figures 1. Zeroes between nonzero digits are always significant: a. 1005 kg (four sig-figs); 7.03 cm (three sig-figs) . 2. Zeroes at the start of a number are never significant: a. 0.02 g (one sig-fig); 0.0026 cm (two sig-figs) . 3. Zeroes at the end of a number are significant only if the zeroes are AFTER a decimal point: a. 0.0200 g (three sig-figs); 3.0 cm (two sig-figs) Precision vs. Accuracy Percent Error Calculations Lesson 0.6 – Lab Safety [https://datbootcamp.com/general-chemistry-strategy/general-chemistry-lab-techniques/](https://datbootcamp.com/general-chemistry-strategy/general-chemistry-lab-techniques/) [Lesson 0.7](Lesson 0.7) – Weights, Measures, and pH [https://datbootcamp.com/general-chemistry-strategy/general-chemistry-lab-techniques/](https://datbootcamp.com/general-chemistry-strategy/general-chemistry-lab-techniques/) [Lesson 0.8](Lesson 0.8) – Beer-Lambert Law Absorbance = εcl • ε = molar extinction coefficient (molar absorptivity) • Note: Things that are brightly-colored have higher ε values • c = sample’s concentration • l = path length (distance between the light source and the detector in a spectrophotometer) • DAT Tip: If you know the absorbance of a solution, you can calculate its concentration Chapter 1: Stoichiometry Lesson 1.1 – The Mole and Molecular Weights 1 mol = 6.022 x 1023 If you have a 150-gram sample of CrO3 : • How many moles of CrO3 do you have? • How many oxygen atoms do you have? • How many grams of oxygen do you have? Lesson 1.2 – Balancing Reactions CO + O2 → CO2 CH4 + Cl2 → CCl4 + HCl Lesson 1.3 – Molecular Formulas and Percent Composition Empirical vs. Molecular Formulas What is the empirical formula for glucose, C6 H12O6 ? Percent Composition What is the percentage of carbon in C6 H12O6 ? What is the percent composition of nitrogen in morphine, whose molecular formula is C17 H19 NO3? What is the empirical formula of a compound that is 17.3% H and 82.7% C? If your compound’s actual molecular weight is 58.123 amu, then what is its molecular formula? Lesson 1.4 – Product and Reactant Amounts How many moles of C2 H6 are needed to react with excess O2 to form 22 moles of CO2 in the following reaction? C2 H6 + O2 → CO2 + H2 O How many grams of C2 H6 does this represent? Lesson 1.5 – Limiting Reactants If you react 6 grams of C2 H6 (M.W. = 30 g/mol) with 9.6 grams of O2 (M.W. = 32 g/mol), which reactant will run out first? Unde

FAQs

What does the outline cover in Chapter 0?

Chapter 0 reviews atoms, ions, and molecules, compound-naming rules for ionic and molecular substances, binary acids and oxyacids, plus measurement and lab calculation skills like significant figures and percent error.

How are naming rules for ionic compounds structured in Lesson 0.2?

The outline specifies naming the metal, writing the metal oxidation state as a Roman numeral in parentheses, then naming the nonmetal with an “ide” ending.

Which stoichiometry skills are emphasized in Chapter 1?

Chapter 1 focuses on moles and molecular weights, balancing reactions, empirical vs. molecular formulas and percent composition, reactant/product amount problems, limiting reactants, and theoretical vs. percent yields.

Sep 17, 2026

Uploaded by Sage