AT: Atomic Theory

AT.1: Students shall understand the historical development of the model of the atom.

AT.1.C.1: Summarize the discoveries of the subatomic particles

AT.1.C.1.a: Rutherford's gold foil

 Element Builder

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: Student shall understand the structure of the atom.

AT.2.C.1: Analyze an atom's particle position, arrangement, and charge using:

AT.2.C.1.a: proton

 Element Builder

AT.2.C.1.b: neutron

 Element Builder

AT.2.C.1.c: electron

 Element Builder

AT.2.C.3: Draw and explain nuclear symbols and hyphen notations for isotopes:

AT.2.C.3.a: nuclear symbol: A/Z X

 Element Builder

AT.2.C.5: Determine the arrangement of subatomic particles in the ion(s) of an atom

 Element Builder

AT.3: Students shall understand how the arrangement of electrons in atoms relates to the quantum model.

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)

 Electron Configuration

AT.3.C.2.b: Hund's Rule

 Electron Configuration

AT.3.C.2.c: Pauli's Exclusion Principle

 Electron Configuration

AT.3.C.3: Predict the placement of elements on the Periodic Table and their properties using electron configuration

 Electron Configuration

AT.3.C.4: Demonstrate electron placement in atoms using the following notations:

AT.3.C.4.b: electron configuration notation

 Electron Configuration

AT.3.C.4.c: Lewis electron dot structures

 Covalent Bonds
 Ionic Bonds

P: Periodicity

P.4: Students shall understand the significance of the Periodic Table and its historical development.

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

 Electron Configuration

P.4.C.3: Interpret periodic trends:

P.4.C.3.a: atomic radius

 Electron Configuration

P.5: Students shall name and write formulas for binary and ternary compounds.

P.5.C.1: Write formulas for binary and ternary compounds:

P.5.C.1.a: IUPAC system

 Chemical Equations

P.5.C.1.b: Greek prefixes

 Chemical Equations

P.6: Students shall explain the changes of matter using its physical and chemical properties.

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

 Electron Configuration

P.6.C.5.b: inactive

 Electron Configuration

P.6.C.5.c: inert

 Electron Configuration

B: Bonding

B.8: Students shall understand the process of ionic bonding.

B.8.C.3: Use the electronegativitiy chart to predict the bonding type of compounds:

B.8.C.3.a: ionic

 Ionic Bonds

B.9: Students shall understand the process of covalent bonding.

B.9.C.1: Draw Lewis structures to show valence electrons for covalent bonding:

B.9.C.1.a: lone pairs

 Covalent Bonds
 Ionic Bonds

B.9.C.1.b: shared pairs

 Covalent Bonds
 Ionic Bonds

B.9.C.1.c: hybridization

 Covalent Bonds
 Ionic Bonds

B.9.C.2: Determine the properties of covalent compounds based upon double and triple bonding

 Covalent Bonds

B.11: Students shall relate the physical properties of solids to different types of bonding.

B.11.C.1: Distinguish between amorphous and crystalline solids

 Ionic Bonds

B.11.C.2: Compare and contrast the properties of crystalline solids:

B.11.C.2.a: ionic

 Ionic Bonds

S: Stoichiometry

S.12: Students shall understand the relationship between balanced chemical equations and mole relationships.

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: Students shall understand the mole concept and Avogadro's number.

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: Gas Laws

GL.16: Students shall understand the behavior of gas particles as it relates to the kinetic theory.

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: Students shall understand the relationship among temperature, pressure, volume and moles of gas.

GL.17.C.1: Calculate the effects of pressure, temperature, and volume to gases

GL.17.C.1.b: Boyle's Law

 Boyle's Law and Charles' Law

GL.17.C.1.c: Charles' Law

 Boyle's Law and Charles' Law

GL.17.C.1.e: Dalton's Law of Partial Pressure

 Equilibrium and Pressure

GL.17.C.1.f: Graham's Law of Effusion

 Diffusion

GL.17.C.1.g: Guy-Lussac

 Boyle's Law and Charles' Law

GL.18: Students shall apply the stoichiometric mass and volume relationships of gases in chemical reactions.

GL.18.C.1: Calculate volume/mass relationships in balanced chemical reaction equations

 Stoichiometry

AB: Acids and Bases

AB.19: Students shall understand the historical development of the acid/base theories.

AB.19.C.1: Compare and contrast the following acid/base theories:

AB.19.C.1.b: Bronsted-Lowry Theory

 Titration

AB.21: Students shall apply rules of nomenclature to acids, bases, and salts.

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: Students shall demonstrate an understanding of titration as a laboratory tool.

AB.22.C.1: Perform a titration to solve for the concentration of an acid or base

 Titration

AB.22.C.2: Use indicators in neutralization reactions

 Titration

AB.22.C.3: Investigate the role of buffers

 Titration

KE: Kinetics and Energistics

KE.23: Students shall understand enthalpy, entropy, and free energy and their relationship to chemical reactions.

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

 Energy Conversion in a System

E: Equilibrium

E.24: Students shall understand the factors that affect reaction rate and their relationship to quantitative chemical equilibrium.

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

 Collision Theory

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

 Collision Theory
 Diffusion

E.24.C.1.f: catalysis

 Collision Theory

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

 Equilibrium and Pressure

E.24.C.3.c: concentration

 Equilibrium and 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

 Collision Theory

E.24.C.4.d: use of a contact catalyst

 Collision Theory

E.24.C.4.e: high pressure

 Equilibrium and Pressure

OC: Organic Chemistry

OC.29: Students shall demonstrate an understanding of the role of organic compounds in living and non-living systems.

OC.29.C.1: Differentiate among the biochemical functions of proteins, carbohydrates, lipids, and nucleic acids

 RNA and Protein Synthesis

OC.29.C.2: Describe the manufacture of polymers derived from organic compounds:

OC.29.C.2.a: polymerization

 Dehydration Synthesis

NC: Nuclear Chemistry

NC.30: Students shall understand the process transformations of nuclear radiation.

NC.30.C.1: Describe the following radiation emissions:

NC.30.C.1.a: alpha particles

 Nuclear Decay

NC.30.C.1.b: beta particles

 Nuclear Decay

NC.30.C.1.c: gamma rays

 Nuclear Decay

NC.30.C.1.d: positron particles

 Nuclear Decay

NC.30.C.2: Write and balance nuclear reactions

 Nuclear Decay

NC.30.C.4: Apply the concept of half life to nuclear decay

 Half-life

Correlation last revised: 5/8/2018

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