Download Honors Chemistry Objectives

Honors Chemistry Objectives
Matter, Measurement, and Lab Equipment/Safety
Students will know and apply the components of the Metric (SI) system of measurement to
data analysis, know and articulate classification of matter, and know and model lab safety.
• Explain basic safety rules for working in the chemistry lab.
• Identify common lab equipment and demonstrate the use of equipment.
• Explain what causes uncertainty in measurements.
• Use significant digits and scientific notation.
• Calculate percent error.
• Describe dimensional analysis and solve problems using this method.
• Compare the physical and chemical properties of matter.
• Compare and contrast chemical and physical changes.
• Explain the difference between an element and a compound.
• Compare heterogeneous and homogeneous mixtures.
• Identify the base and derived units, and common prefixes of the metric system.
• Convert measurements within the metric system.
Atomic Theory
Students will comprehend and describe the major contributions to the development of the
atomic theory of matter and diagram the basic structure of the atom and nuclear theory.
• Define the term atom.
• List the postulates of Dalton's theory.
• Discuss how atoms are related to electricity.
• Discuss Rutherford's alpha-scattering experiment and its significance to atomic structure.
• Determine the number of protons, neutrons, and electrons in an atom or ion.
• Define isotopes, ions, atomic number, and atomic mass.
• Describe the changes that accompany nuclear reactions.
• Communicate the laws/theories developed by Democritus, Lavoisier, and Proust.
• Interpret the experiments and results of the work done by Thomson and Milliken.
Quantum Theory
Students will recognize and describe the components of the electromagnetic spectrum, be
able to analyze the interactions between energy and matter, and be able integrate these
concepts with modern atomic theory.
• Describe a wave.
• Identify the major regions of the electromagnetic spectrum.
• Explain what is meant by a quantum of energy.
• Relate the energy of radiation to its frequency.
• State the main idea in Bohr's model of the atom.
• Describe atomic orbitals in terms of their shape, size, and energy.
• Determine the electron configurations of several elements.
• Explain the seven colors of the rainbow.
• Compare and contrast the process of finding the location of a residence in an unfamiliar
area to the process used to identify the location of an electron within the atomic structure
of an atom.
Periodic Table
Students will recognize the arrangement of the elements on the periodic table and interpret
placement of elements due to trends of properties and characteristics.
• State the periodic law.
• Discuss the development of the periodic table.
• Explain why elements in a group have similar properties.
• Identify the four blocks of the periodic table.
• Identify periodic trends and explain how trends reflect the electron configurations of the
elements.
• Describe several periodic patterns in your everyday experiences.
Bonding + Chemical Equations
Students will compare and contrast properties of chemical bond types, identify molecule
shapes and characteristics, and will categorize and write chemical reactions
• Describe the characteristics of an ionic bond.
• State the octet rule.
• Describe the characteristics of a covalent bond.
• Describe the difference between polar and non-polar covalent bonds.
• Write names for ionic compounds, molecular compounds, and acids.
• Describe the VSEPR theory.
• Identify the common shapes of small molecules.
• Explain what determines the polarity of a molecule.
• Explain why water is a polar molecule.
• Describe the characteristics of a chemical reaction.
• Write balanced chemical equations.
• Classify chemical reactions.
Mole + Stoichiometry
Students will formulate a comprehension of the mole concept as it applies to chemistry by
illustrating mathematical applications of the mole concept using balanced chemical
equations.
• Define a mole.
• Identify and use Avogadro's number.
• Convert among the number of particles, moles, and mass of a substance.
• Use percentage composition to determine the formula of a substance.
• Find the empirical and molecular formulas.
• Define stoichiometry and describe its importance.
• Relate stoichiometry to balanced chemical equations.
• Identify and solve different types of stoichiometry problems.
• Determine the limiting reactant of a chemical reaction.
• Calculate the amount of product formed in a chemical reaction.
Thermodynamics
Students will explain the transfer of kinetic heat energy in reactions and calculate its effect
as a measure of enthalpy change.
• Distinguish between exothermic and endothermic reactions.
• Explain what is meant by enthalpy and enthalpy change.
• Apply Hess's law to determine H° for a reaction.
• Describe how a calorimeter determines heats of reactions.
• Compare heat and temperature.
Solutions
Students will identify solubility, solutes, and solvents, determine concentrations and
properties of solutions, and apply these concepts to colligative properties.
• Identify the different types of solutions.
• Measure the concentration of solutions.
• Differentiate among saturated, unsaturated, and supersaturated solutions.
• Define solubility and describe the factors that affect solubility.
• Define a colligative property of a solution.
• Describe four colligative properties of solutions.
Chemical Equilibrium
Students will evaluate factors that affect the equilibrium of a chemical system.
• To describe a reversible reaction.
• To define chemical equilibrium and explain how it is achieved.
• To determine the equilibrium constant for a given reaction.
• To analyze the extent of a reaction from its equilibrium constant.
• To use the reaction quotient of a reaction to determine if the reaction is at equilibrium.
• To explain Le Chatelier's principle.
• To describe how changes in concentration, pressure, and temperature affect equilibrium.
Acids and Bases
Students will identify common acids and bases, describe the nature of acidic and basic
solutions, calculate pH, and analyze the results of acid/base reactions.
• State the Brønsted -Lowry definition of acids and bases.
• Identify common physical and chemical properties of acids and bases.
• Explain what dissociation constants indicate.
• Explain what most acidic hydrogen atoms have in common.
• Explain what most bases have in common.
• Describe how acids and bases are named.
• Identify the ion concentrations in pure water.
• Describe the pH scale.
• Describe an acid-base titration.
Gas Laws + Kinetic Molecular Theory
Students will apply the kinetic molecular theory to concepts involving gases and the gas
laws.
• Describe the kinetic-molecular theory.
• Explain gas pressure and describe how it is measured.
• State the gas laws.
• Compare ideal and real gases.
• Relate gas density to temperature and molar mass.