Curriculum Framework
AT.1.C.1: Summarize the discoveries of the subatomic particles
AT.1.C.1.a: Rutherford's gold foil
AT.1.C.2: Explain the historical events that led to the development of the current atomic theory
Bohr Model of Hydrogen
Bohr Model: Introduction
AT.2.C.1: Analyze an atom's particle position, arrangement, and charge using:
AT.2.C.1.a: proton
AT.2.C.1.b: neutron
AT.2.C.1.c: electron
AT.2.C.3: Draw and explain nuclear symbols and hyphen notations for isotopes:
AT.2.C.3.a: nuclear symbol: A/Z X
AT.2.C.5: Determine the arrangement of subatomic particles in the ion(s) of an atom
AT.3.C.2: Apply the following rules or principles to model electron arrangement in atoms:
AT.3.C.2.a: Aufbau Principle (diagonal filling order)
AT.3.C.2.b: Hund's Rule
AT.3.C.2.c: Pauli's Exclusion Principle
AT.3.C.3: Predict the placement of elements on the Periodic Table and their properties using electron configuration
AT.3.C.4: Demonstrate electron placement in atoms using the following notations:
AT.3.C.4.b: electron configuration notation
AT.3.C.4.c: Lewis electron dot structures
P.4.C.2: Describe the arrangement of the Periodic Table based on electron filling orders:
P.4.C.2.a: Groups
Electron Configuration
Ionic Bonds
P.4.C.2.b: Periods
P.4.C.3: Interpret periodic trends:
P.4.C.3.a: atomic radius
P.5.C.1: Write formulas for binary and ternary compounds:
P.5.C.1.a: IUPAC system
P.5.C.1.b: Greek prefixes
P.6.C.2: Distinguish between extensive and intensive physical properties of matter
Density Experiment: Slice and Dice
P.6.C.5: Predict the chemical properties of substances based on their electron configuration:
P.6.C.5.a: active
P.6.C.5.b: inactive
P.6.C.5.c: inert
B.8.C.3: Use the electronegativitiy chart to predict the bonding type of compounds:
B.8.C.3.a: ionic
B.9.C.1: Draw Lewis structures to show valence electrons for covalent bonding:
B.9.C.1.a: lone pairs
B.9.C.1.b: shared pairs
B.9.C.1.c: hybridization
B.9.C.2: Determine the properties of covalent compounds based upon double and triple bonding
B.11.C.1: Distinguish between amorphous and crystalline solids
B.11.C.2: Compare and contrast the properties of crystalline solids:
B.11.C.2.a: ionic
S.12.C.1: Balance chemical equations when all reactants and products are given
Balancing Chemical Equations
Chemical Equations
S.12.C.2: Use balanced reaction equations to obtain information about the amounts of reactants and products
Chemical Equations
Limiting Reactants
Stoichiometry
S.12.C.3: Distinguish between limiting reactants and excess reactants in balanced reaction equations
Balancing Chemical Equations
Chemical Equations
Limiting Reactants
Stoichiometry
S.12.C.4: Calculate stoichiometric quantities and use these to determine theoretical yields
Limiting Reactants
Stoichiometry
S.13.C.1: Apply the mole concept to calculate the number of particles and the amount of substance: Avogadro's constant = 6.02 x 10 to the 23rd power.
Chemical Equations
Limiting Reactants
Stoichiometry
S.13.C.2: Determine the empirical and molecular formulas using the molar concept:
S.13.C.2.a: molar mass
Chemical Equations
Stoichiometry
S.13.C.2.d: formula mass
Chemical Equations
Stoichiometry
GL.16.C.1: Demonstrate the relationship of the kinetic theory as it applies to gas particles:
GL.16.C.1.a: molecular motion
Temperature and Particle Motion
GL.16.C.1.b: elastic collisions
Collision Theory
Temperature and Particle Motion
GL.16.C.1.c: temperature
Temperature and Particle Motion
GL.16.C.1.d: pressure
Temperature and Particle Motion
GL.16.C.1.e: ideal gas
Temperature and Particle Motion
GL.17.C.1: Calculate the effects of pressure, temperature, and volume to gases
GL.17.C.1.b: Boyle's Law
GL.17.C.1.c: Charles' Law
GL.17.C.1.e: Dalton's Law of Partial Pressure
GL.17.C.1.f: Graham's Law of Effusion
GL.17.C.1.g: Guy-Lussac
GL.18.C.1: Calculate volume/mass relationships in balanced chemical reaction equations
AB.19.C.1: Compare and contrast the following acid/base theories:
AB.19.C.1.b: Bronsted-Lowry Theory
AB.21.C.1: Compare and contrast acid and base properties
pH Analysis
pH Analysis: Quad Color Indicator
AB.21.C.3: Explain the role of the pH scale as applied to acids and bases
pH Analysis
pH Analysis: Quad Color Indicator
AB.22.C.1: Perform a titration to solve for the concentration of an acid or base
AB.22.C.2: Use indicators in neutralization reactions
AB.22.C.3: Investigate the role of buffers
KE.23.C.4: Define specific heat capacity and its relationship to calorimetric measurements:
KE.23.C.4.a: q = m (deltaT)C sub p
E.24.C.1: List and explain the factors which affect the rate of a reaction and the relationship of these factors to chemical equilibrium:
E.24.C.1.b: reaction rate
E.24.C.1.c: nature of reactants
Collision Theory
Equilibrium and Concentration
Equilibrium and Pressure
E.24.C.1.d: concentration
Collision Theory
Diffusion
Equilibrium and Concentration
E.24.C.1.e: temperature
E.24.C.1.f: catalysis
E.24.C.2: Solve problems developing an equilibrium constant or the concentration of a reactant or product:
E.24.C.2.a: mA + nB --> sP + rQ
Equilibrium and Concentration
Equilibrium and Pressure
E.24.C.2.b: K (eq) = ([P]^5 [Q]^r)/([A]^m [B]^n)
Equilibrium and Concentration
Equilibrium and Pressure
E.24.C.3: Explain the relationship of LeChatelier's Principle to equilibrium systems:
E.24.C.3.b: pressure
E.24.C.3.c: concentration
E.24.C.4: Describe the application of equilibrium and kinetic concepts to the Haber Process:
E.24.C.4.c: precise temperature control
E.24.C.4.d: use of a contact catalyst
E.24.C.4.e: high pressure
OC.29.C.1: Differentiate among the biochemical functions of proteins, carbohydrates, lipids, and nucleic acids
OC.29.C.2: Describe the manufacture of polymers derived from organic compounds:
OC.29.C.2.a: polymerization
NC.30.C.1: Describe the following radiation emissions:
NC.30.C.1.a: alpha particles
NC.30.C.1.b: beta particles
NC.30.C.1.c: gamma rays
NC.30.C.1.d: positron particles
NC.30.C.2: Write and balance nuclear reactions
NC.30.C.4: Apply the concept of half life to nuclear decay
Correlation last revised: 5/8/2018