Fenstermacher

2015 Intensified Chemistry Final Exam Multiple Choice Study GuidePage 1 of 2

  • Given a chemical formula, you will need to be able to count the number of atoms of a given element in a given number or formula units/molecules.
  • Given mass data of two elements in a compound, be able to determine the percent composition of one of the elements.
  • Given an empirical formula and a molar mass, be able to determine the molecular formula of a compound.
  • Know the relationship between empirical and molecular formulas.
  • Know the rules for balancing chemical reaction equations.
  • Given a series of reactant pairs for a single replacement reaction, be able to use the activity series (will be provided) to determine which reaction(s) will or won’t occur.
  • Know the types of information that can be obtained directly from the coefficients of a balanced chemical reaction equation.
  • Given a balanced chemical reaction equation, be able to determine the basic type of reaction described by it (synthesis, decomposition, single replacement/displacement, double replacement/displacement, combustion).
  • Given a balanced chemical reaction equation, be able to determine how many moles of a reactant are required to produce a given quantity of moles of a product in that reaction.
  • Know the definitions of limiting and excess reactants.
  • Know the definitions of theoretical (expected) yield, actual yield, and percent yield and be able to calculate one of them when provided with the other two.
  • Given a balanced reaction equation, be able to determine the ratio of moles of a reactant used to moles of product produced.
  • Know the law of conservation of matter (mass) and how it relates to masses of reactants and products.
  • Given a balanced chemical reaction equation, be able to determine how many moles of a reactant are required to react completely with a given mole quantity of another reactant.
  • Be able to determine the coefficients of an unbalanced formula equation.
  • Know how the addition of a certain mole quantity of gas to another known mole quantity of gas will affect the pressure (Dalton’s Law of Partial Pressures).
  • Know what happens to the temperature of a system that is changing its phase when heat is added to it.
  • Know what happens to the average kinetic energy of the particles in a system when the temperature is increased.
  • Know which states of matter can flow/diffuse and how and why the rates of diffusion differ for these different states.
  • Be able to convert pressure values between atmospheres (atm), kilopascals (kPa), and millimeters of mercury (mm Hg).
  • Be able to describe the states of matter and their properties in terms of particle motion, particle spacing, particle organization, density, and compressibility.
  • Know how to define endothermic and exothermic processes.
  • Know the values of standard temperature and pressure.
  • Understand and be able to identify the effect of intermolecular forces (hydrogen bonding, weaker dipole-dipole forces, and van der Waals forces) on the physical properties of matter, such as surface tension, boiling point, melting point, and equilibrium vapor pressure.
  • Be able to use Boyle’s Law to predict the effect of a volume change on the pressure of a gas system at constant temperature.
  • Be able to use your knowledge of Graham’s Law of diffusion/effusion to determine which of a series of gases will diffuse most rapidly.
  • Be able to use your knowledge of the molar volume of a gas at STP to determine the volume of a certain number of moles contained in a gas sample held at STP.
  • Given a series of physical changes, be able to distinguish between those that are phase changes, and those that are not.
  • Be able to use your knowledge of Gay-Lussac’s Law to determine the effect of a temperature change on the pressure of a gas in a constant-volume container.
  • Know what explains the high surface tension in water droplets.
  • Given a series of chemical reaction equations, be able to determine which constitutes an increase (or a decrease) in entropy.
  • Be able to correctly identify a description of a system in physical or chemical equilibrium.
  • Know what substance will be soluble together (HINT: “Like dissolves like.”)
  • Given a list of compounds, be able to use knowledge of relative solubility (you will be provided a chart on your exam) and solute nature to determine which will be a strong electrolyte.
  • Know the factors that affect the rate of solubility (how fast dissolving occurs).
  • Given a complete (total) ionic equation, be able to determine the spectator ion(s).
  • Given a list of physical properties, be able to identify those that are colligative, and those that are not.
  • Given a solution volume and its molarity, be able to calculate the number of moles of solute in the solution sample.
  • Know the relationship between the solubility of a gas solute and its partial pressure in the gas phase above the solution (Henry’s Law).
  • Given the names of reactants in a precipitation (double replacement) reaction, be able to determine the correct net ionic equation for that reaction.
  • Given identical quantities of a series of solutes dissolved in water, determine which will raise the boiling point or lower the freezing point the most.
  • Given four substances be able to determine which will NOT be water-soluble.
  • Know the relationship between temperature and vapor pressure.
  • Know the definition of a colligative property.
  • Know the effect of molal concentration of solute on colligative properties.
  • Know how to define electrolytes and nonelectrolytes.
  • Given a reaction equation with heat as either a reactant or product, be able to use your knowledge of Le Châtelier’s Principle to determine if the reaction will be pushed to the right or the left when the temperature is increased.
  • Know how to define boiling point, critical temperature, freezing point, and critical pressure for any substance.
  • Given a solute solubility in 100 g of water, be able to determine how many grams of that same solute will dissolve in a different quantity of water at the same conditions.
  • Be able to distinguish between the different types of homogenous and heterogeneous mixtures that we discussed in the solutions unit (solutions, suspensions, colloids, etc.).
  • Given an equilibrium equation, be able to determine which species in the equation are acting as Brønsted-Lowry acids or bases.
  • Know both the Arrhenius and Brønsted-Lowry definitions of acids and bases.
  • Given an equilibrium equation, be able to identify which pair of species in the equation constitutes a conjugate acid-base pair.
  • Given a value for [H3O+], be able to calculate the pH.
  • Using the definitions of acidic, basic, and neutral solutions to determine the relative concentrations of [H3O+] and [OH] in those solutions.
  • Given an acid name, be able to correctly identify its formula.
  • Given starting reactant concentrations and initial reaction rate data, be able to determine the rate expression.