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Atomic Structure and Chemical Reactions

Discover the atomic structure, understand fundamental particles, calculate atomic mass, name compounds, solve stoichiometry problems, and analyze chemical reactions.

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Atomic Structure and Chemical Reactions

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  1. Chemistry II Objectives Unit II - Chapter 2-4 • Summarize the discovery of atomic structure (Who found what, and how?). • Identify the fundamental particles of atomic structure and describe them in terms of mass, charge, and location. • III.   Distinguish between atomic number (Z#) and mass number (A#) and know what they mean. • IV. Define Atomic Mass Unit (amu) and explain why the masses in the periodic table are relative. • Be able to calculate average atomic mass for an element given • the masses and relative abundance of isotopes. • VI. Compare and contrast neutral atoms, ions, and isotopes. Be able to write their complete chemical symbols. • VII.   Be able to draw structural formulas and write empirical • and/or molecular formulas for compounds • VIII.   Be able to write chemical formulas for a variety of binary • molecular and ionic compounds (and acids) given their names.

  2. Chemistry II Objectives Unit II - Chapter 2-4 • IX. Use the stock and traditional systems to name binary ionic • and molecular compounds (and acids) given their formulas. • X.  Recognize and use polyatomic ions to write formulas and name • ternary compounds and acids using the stock and traditional • systems. • Memorize and use Avogadro’s number to calculate the number • of particles from moles or the number of moles from particles.  • XII.  Define and be able to calculate molar mass of an element and • formula mass of a compound (gram atomic/formula mass). • Use this to calculate moles from mass or mass from moles. • XIII. Use molar volume (22.4 dm3) to calculate the number of • moles in a gas sample at standard conditions of temperature • (0C / 273 K) and pressure (1 atm / 760 Torr / 101.3 kpa). • Use the mole diagram to convert from and to mass, volume, particles or moles of an element or compound given any one of those properties.  • XV.  Calculate % composition of a given formula. Use percent • composition to determine the empirical formula of an unknown.

  3. Chemistry II Objectives Unit II - Chapter 2-4 • XVI.  Be able to use the empirical formula and molar mass to • calculate the molecular formula of a given compound. • Relate stoichiometry to the coefficients in balanced • chemical equations and conservation of mass. • XVIII.  Be able to solve the following types of stoichiometry • problems: Mass – Mass, Volume – Volume, Particle – • Particle, Any combination of mass, volume & particles. • Determine the limiting reactant in a chemical reaction and • the reactant in excess. Explain how the limiting reactant • controls the amount of product(s). • XX.   Use the limiting reactant concept to determine the amount(s) • of product(s) (theoretical yield) if reactants are not present in • stoichiometric proportions. • XXI. Calculate theoretical yield and use the actual yield to find the • percent (%) yield. XXII. Calculate Solution concentrations in Molarity (M) and be able to solve dilution problems. XXIII. Compare and contrast electrolytes and non-electrolytes and give examples of each.

  4. Chemistry II Objectives Unit II - Chapter 2-4 XXIV. Compare and contrast precipitation reactions, acid base reactions, and oxidation-reduction reactions. Be able to balance give examples of each. • Use titration calculations to determine the concentrations of • unknown solutions. • Be able to assign oxidation numbers to atoms in pure • elements and compounds and use the half reaction method to • balance oxidation-reduction (REDOX) reactions.

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