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.
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 (0C / 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.
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.
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.