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.
Unit Conversions 2 - Scientific Notation and Significant Digits
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).
Chemical Equations
Covalent Bonds
Ionic Bonds
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.
Bohr Model of Hydrogen
Bohr Model: Introduction
Element Builder
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.
Bohr Model of Hydrogen
Bohr Model: Introduction
Electron Configuration
Element Builder
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.
Bohr Model of Hydrogen
Bohr Model: Introduction
Star 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.
Chemical Equations
Equilibrium and Concentration
Limiting Reactants
CHEM.B.2.1.2: Use stoichiometric relationships to calculate the amounts of reactants and products involved in a chemical reaction.
Chemical Equations
Limiting Reactants
Stoichiometry
CHEM.B.2.1.3: Classify reactions as synthesis, decomposition, single replacement, double replacement, or combustion.
Balancing Chemical Equations
Chemical Changes
Chemical Equations
Dehydration Synthesis
Equilibrium and Concentration
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.
Balancing Chemical Equations
Chemical Equations
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).
Boyle's Law and Charles's Law
Equilibrium and Pressure
Correlation last revised: 9/16/2020