Keystone Exams Assessment Anchors and Eligible Content
CHEM.A.1: Properties and Classification of Matter
CHEM.A.1.1: Identify and describe how observable and measurable properties can be used to classify and describe matter and energy.
CHEM.A.1.1.2: Classify observations as qualitative and/or quantitative.
CHEM.A.1.1.3: Utilize significant figures to communicate the uncertainty in a quantitative observation.
CHEM.A.1.1.5: Apply a systematic set of rules (IUPAC) for naming compounds and writing chemical formulas (e.g., binary covalent, binary ionic, ionic compounds containing polyatomic ions).
CHEM.A.1.2: Compare the properties of mixtures.
CHEM.A.1.2.1: Compare properties of solutions containing ionic or molecular solutes (e.g., dissolving, dissociating).
CHEM.A.1.2.3: Describe how factors (e.g., temperature, concentration, surface area) can affect solubility.
CHEM.A.2: Atomic Structure and the Periodic Table
CHEM.A.2.1: Explain how atomic theory serves as the basis for the study of matter.
CHEM.A.2.1.1: Describe the evolution of atomic theory leading to the current model of the atom based on the works of Dalton, Thomson, Rutherford, and Bohr.
CHEM.A.2.1.2: Differentiate between the mass number of an isotope and the average atomic mass of an element.
CHEM.A.2.2: Describe the behavior of electrons in atoms.
CHEM.A.2.2.1: Predict the ground state electronic configuration and/or orbital diagram for a given atom or ion.
CHEM.A.2.2.2: Predict characteristics of an atom or an ion based on its location on the periodic table (e.g., number of valence electrons, potential types of bonds, reactivity).
CHEM.A.2.2.4: Relate the existence of quantized energy levels to atomic emission spectra.
CHEM.A.2.3: Explain how periodic trends in the properties of atoms allow for the prediction of physical and chemical properties.
CHEM.A.2.3.1: Explain how the periodicity of chemical properties led to the arrangement of elements on the periodic table.
CHEM.A.2.3.2: Compare and/or predict the properties (e.g., electron affinity, ionization energy, chemical reactivity, electronegativity, atomic radius) of selected elements by using their locations on the periodic table and known trends.
CHEM.B.1: The Mole and Chemical Bonding
CHEM.B.1.1: Explain how the mole is a fundamental unit of chemistry.
CHEM.B.1.1.1: Apply the mole concept to representative particles (e.g., counting, determining mass of atoms, ions, molecules, and/or formula units).
CHEM.B.1.3: Explain how atoms form chemical bonds.
CHEM.B.1.3.1: Explain how atoms combine to form compounds through ionic and covalent bonding.
CHEM.B.1.3.2: Classify a bond as being polar covalent, non-polar covalent, or ionic.
CHEM.B.1.4: Explain how models can be used to represent bonding.
CHEM.B.1.4.1: Recognize and describe different types of models that can be used to illustrate the bonds that hold atoms together in a compound (e.g., computer models, ball-and-stick models, graphical models, solid-sphere models, structural formulas, skeletal formulas, Lewis dot structures).
CHEM.B.1.4.2: Utilize Lewis dot structures to predict the structure and bonding in simple compounds.
CHEM.B.2: Chemical Relationships and Reactions
CHEM.B.2.1: Predict what happens during a chemical reaction.
CHEM.B.2.1.1: Describe the roles of limiting and excess reactants in chemical reactions.
CHEM.B.2.1.2: Use stoichiometric relationships to calculate the amounts of reactants and products involved in a chemical reaction.
CHEM.B.2.1.3: Classify reactions as synthesis, decomposition, single replacement, double replacement, or combustion.
CHEM.B.2.1.4: Predict products of simple chemical reactions (e.g., synthesis, decomposition, single replacement, double replacement, combustion).
CHEM.B.2.1.5: Balance chemical equations by applying the Law of Conservation of Matter.
CHEM.B.2.2: Explain how the kinetic molecular theory relates to the behavior of gases.
CHEM.B.2.2.1: Utilize mathematical relationships to predict changes in the number of particles, the temperature, the pressure, and the volume in a gaseous system (i.e., BoyleÂ?s law, CharlesÂ?s law, DaltonÂ?s law of partial pressures, the combined gas law, and the ideal gas law).
Correlation last revised: 1/20/2017