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does the outline cover in Chapter 0?","Question",{"text":63,"@type":64},"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.","Answer",{"name":66,"@type":61,"acceptedAnswer":67},"How are naming rules for ionic compounds structured in Lesson 0.2?",{"text":68,"@type":64},"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.",{"name":70,"@type":61,"acceptedAnswer":71},"Which stoichiometry skills are emphasized in Chapter 1?",{"text":72,"@type":64},"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 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Molecule – atom bonded to at least one other atom  \n• Ion – atom that has lost of gained an electron  \nLesson 0.2 – Naming Ionic Compounds  \n• Diatomic elements  \no H2, N2, O2, F2, Cl2, Br2, and I2  \n• Allotropes – Elemental molecules with different formulas. i.e. O2 and O3  \n• Ionic compounds – metal and nonmetal (can be polyatomic too)  \n• Molecular compounds – two or more nonmetals  \n• Naming ionic compounds  \no 1. Name the metal.  \no 2. Write the metal’s oxidation state as a Roman numeral in parenthesis.  \no 3. Name the nonmetal using an “ide” ending  \n􀁨 Ex. Iron (II) Chloride, FeCl2  \nLesson 0.3 – Naming Molecular Compounds and Acids  \n• Naming molecular compounds  \no 1. Give the appropriate numerical prefix to the first element  \no 2. Name the first element using its regular name on the periodic table  \no 3. Give the appropriate numerical prefix to the second element  \no 4. Name the nonmetal using an “ide” ending  \n􀁨 Ex. dinitrogen monoxide, N2O  \n• Naming binary acids  \no 1. Hydro  \no 2. Insert the name of element 2, replacing “-ine” with “-ic acid”  \n􀁨 Ex. hydrochloric acid, HCl  \n• Naming oxyacids  \no HClO – hypochlorous acid  \no HClO2 – chlorous acid  \no HClO3 – chloric acid  \no HClO4 – perchloric acid  \nLesson 0.4 – Metric Units and Dimensional Analysis  \nLesson 0.5 – Significant Figures and Percent Error  \nSignificant Figures  \n1. Zeroes between nonzero digits are always significant:  \na. 1005 kg (four sig-figs); 7.03 cm (three sig-figs) .  \n2. Zeroes at the start of a number are never significant:  \na. 0.02 g (one sig-fig); 0.0026 cm (two sig-figs) .  \n3. Zeroes at the end of a number are significant only if the zeroes are AFTER a decimal point:  \na. 0.0200 g (three sig-figs); 3.0 cm (two sig-figs)  \nPrecision vs. Accuracy  \nPercent Error Calculations  \nLesson 0.6 – Lab Safety  \n[https://datbootcamp.com/general-chemistry-strategy/general-chemistry-lab-techniques/](https://datbootcamp.com/general-chemistry-strategy/general-chemistry-lab-techniques/)  \n[Lesson 0.7](Lesson 0.7) – Weights, Measures, and pH  \n[https://datbootcamp.com/general-chemistry-strategy/general-chemistry-lab-techniques/](https://datbootcamp.com/general-chemistry-strategy/general-chemistry-lab-techniques/)  \n[Lesson 0.8](Lesson 0.8) – Beer-Lambert Law  \nAbsorbance = εcl  \n• ε = molar extinction coefficient (molar absorptivity)  \n• Note: Things that are brightly-colored have higher ε values  \n• c = sample’s concentration  \n• l = path length (distance between the light source and the detector in a spectrophotometer)  \n• DAT Tip: If you know the absorbance of a solution, you can calculate its concentration  \nChapter 1: Stoichiometry  \nLesson 1.1 – The Mole and Molecular Weights  \n1 mol = 6.022 x 1023  \nIf you have a 150-gram sample of CrO3 :  \n• How many moles of CrO3 do you have?  \n• How many oxygen atoms do you have?  \n• How many grams of oxygen do you have?  \nLesson 1.2 – Balancing Reactions  \n  CO +   O2 →   CO2  \n  CH4 +   Cl2 →   CCl4 +   HCl  \nLesson 1.3 – Molecular Formulas and Percent Composition  \nEmpirical vs. Molecular Formulas  \nWhat is the empirical formula for glucose, C6 H12O6 ?  \nPercent Composition  \nWhat is the percentage of carbon in C6 H12O6 ?  \nWhat is the percent composition of nitrogen in morphine, whose molecular formula is C17 H19 NO3?  \nWhat is the empirical formula of a compound that is 17.3% H and 82.7% C?  \nIf your compound’s actual molecular weight is 58.123 amu, then what is its molecular formula?  \nLesson 1.4 – Product and Reactant Amounts  \nHow many moles of C2 H6 are needed to react with excess O2 to form 22 moles of CO2 in the following reaction?  \n  C2 H6 +   O2 →   CO2 +   H2 O  \nHow many grams of C2 H6 does this represent?  \nLesson 1.5 – Limiting Reactants  \nIf 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?  \nUnde","cbCaihewJ7xpCnMm","https://ap.wps.com/l/cbCaihewJ7xpCnMm","pdf",1969894,61,"English","# Chapter 0: General and Lab Concepts Review\n## Lesson 0.1 – Atoms, Ions, and Molecules\n## Lesson 0.2 – Naming Ionic Compounds\n## Lesson 0.3 – Naming Molecular Compounds and Acids\n## Lesson 0.4 – Metric Units and Dimensional Analysis\n## Lesson 0.5 – Significant Figures and Percent Error\n## Lesson 0.6 – Lab Safety\n## Lesson 0.7 – Weights, Measures, and pH\n## Lesson 0.8 – Beer-Lambert Law\n# Chapter 1: Stoichiometry\n## Lesson 1.1 – The Mole and Molecular Weights\n## Lesson 1.2 – Balancing Reactions\n## Lesson 1.3 – Molecular Formulas and Percent Composition\n## Lesson 1.4 – Product and Reactant Amounts\n## Lesson 1.5 – Limiting Reactants\n## Lesson 1.6 – Theoretical and Percent Yields\n# Chapter 2: Atomic and Electronic Structure\n## Lesson 2.1 – Atomic Structure and the Bohr Model\n## Lesson 2.2 – Atomic Orbitals\n## Lesson 2.3 – Quantum Numbers\n## Lesson 2.4 – Electron Configuration\n## Lesson 2.5 – Condensed Electron Configuration, Valence, and Energy Diagrams","[{\"question\":\"What does the outline cover in Chapter 0?\",\"answer\":\"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.\"},{\"question\":\"How are naming rules for ionic compounds structured in Lesson 0.2?\",\"answer\":\"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.\"},{\"question\":\"Which stoichiometry skills are emphasized in Chapter 1?\",\"answer\":\"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.\"}]","Mikes Videos - General Chemistry Lesson Outline - Chapter 0 - General and Lab Concepts Review | PDF",154]