Semester 2 Final Exam 2015

The semester 2 exam will consist of 75-100 multiple choice questions and 10 short answer or extended response questions.

Gather together your notes, quizzes and tests for Units 4-8.

Use the learning targets for these units and your notes, quizzes and tests to prepare for the exam.

The Semester 2 Review WS includes examples of short answer and extended response questions.

Learning Targets

U4: Describing Substances

Student will be able to:

  • Distinguish between pure substances and mixtures
  • Describe how one could use differences in characteristic properties to separate the components of a mixture
  • Sketch particle diagrams that distinguish compounds, elements, and mixtures
  • Distinguish elements from compounds in terms of differences in their properties
  • Cite the evidence that supports the belief that some pure substances are "compounded" of simpler particles in a definite ratio
  • Cite evidence for Avogadro's Hypothesis. Use this with evidence from combining volumes to deduce the formulas of some compounds
  • State features of Dalton's model of the atom; use composition by mass data to account for the laws of definite and multiple proportions

Unit 5: Counting Particles Too Small To See

Student will be able to:

  • Use experimental data to determine the relative mass of two objects.
  • Use experimental data to determine the number of items in a sample without actually counting them.
  • Given the chemical formula of a substance, determine the molar mass.
  • Given the mass of a substance, determine the number of moles of the sample and the number of atoms or molecules of the sample.
  • Given the number of moles of a substance, find the mass of the sample and the number of atoms or molecules in the sample.
  • Given the formula of a compound, determine its percent composition.
  • Given data about the percent composition of a sample, determine the empirical formula of the compound.
  • Given the empirical formula and information about the molar mass of the compound, determine the molecular formula.

Unit 6: Particles With Internal Structure

Student will be able to:

  • Describe the evidence that supports the idea that the simple particles have a property we call charge
  • Describe the evidence that led Thomson to suggest that the mobile charge in atoms is negative.
  • Use the Thomson model of the atom to account for the fact that neutral atoms can become either positively or negatively charged by the loss or gain of electrons.
  • List properties that distinguish metals from non-metals.
  • Describe evidence that distinguishes ionic from molecular compounds.
  • Given the formula of an ionic or molecular substance, write its name.
  • Given the name of ionic or molecular substances, write the formula.
  • From the name or formula of a substance, determine whether that substance is ionic or molecular.

Unit 7: Chemical Reactions - Particles & Energy

Student will be able to:

  • Describe chemical changes in terms of rearranging atoms to form new substances.
  • Recognize that the total number of particles (sum of the coefficients) can change during a reaction because of differences in the bonding ratios of each substance.
  • Recognize that the total number of atoms does not change during a reaction because every reactant atom must be included in a product molecule.
  • Learn to describe reactions in terms of macroscopic observations.
  • Learn to describe reactions in terms of microscopic behavior of atoms.
  • Learn to write balanced equations to represent these changes symbolically.
  • Explain that the coefficients in a chemical equation describe the quantities of the individual atoms or molecules involved and the moles of the substances involved.
  • Observe basic patterns in the way substances react and learn to generalize them to other reactions students encounter - synthesis reactions,decomposition reactions, combustion reactions, single replacement reactions, & double replacement reactions.
  • Describe endo- and exothermic reactions in terms of storage or release of chemical potential energy and draw energy bar charts to show each.

Unit 8: Stoichiometry

Student will be able to:

  • Using a balanced equation, determine the change in the number of moles of any other reactant or product using the number of moles of reactant consumed or product formed.
  • Use molar mass to convert mass of a reactant or product to moles for use in stoichiometric calculations or to convert moles from stoichiometric calculations to mass.
  • Beginning with a balanced chemical equation, the mass of a reactant consumed and the mass of product actually produced, determine the percent yield for the reaction.
  • Beginning with a balanced chemical equation and the initial masses of the reactants, determine which reactant is limiting and what the theoretical yield is for each product.
  • Given a balanced chemical equation and the initial amounts of reactants,sketch particle diagrams to represent the mixture in the reaction vessel before and after the reaction.