1: From Structures to Properties

1.1: Classification of Matter

1.1.4: use the periodic law as illustrated by the periodic table to identify and distinguish metals and non-metals, periods and groups, representative and transition elements, and families.

Electron Configuration
Ionic Bonds

1.2: The Underlying Structure of Matter

1.2.1: use standard atomic notation to represent atoms, define isotope and use isotopic notation.

Element Builder

1.2.4: provide definitions and examples of atoms, ions, and molecules, including subatomic particles, atomic mass, atomic number, mass number, valence electrons, isotopes.

Electron Configuration
Element Builder

1.2.5: identify the inadequacies in the Rutherford and Bohr models.

Bohr Model of Hydrogen

1.2.6: identify the new proposal in the Bohr model of the atom.

Bohr Model of Hydrogen
Bohr Model: Introduction
Element Builder

1.2.8: describe how the shapes of orbitals differ as it relates to different sublevels.

Electron Configuration

1.2.9: write electron configuration diagrams using Hund‟s rule, Pauli exclusion principle and Aufbau principle (diagonal rule).

Electron Configuration

1.2.10: demonstrate an introductory understanding of the Quantum Mechanical Model.

Bohr Model of Hydrogen

1.2.11: demonstrate an understanding of periodicity of Ionization Energy, electronegativity and atomic radii.

Electron Configuration

1.3: Elements and Compounds

1.3.1: define and differentiate between ionic and molecular compounds, including acids and bases, using conductivity and indicators.

Titration
pH Analysis
pH Analysis: Quad Color Indicator

1.3.2: identify, name and write formulas for ionic (binary, multivalent, polyatomic, and hydrates) and molecular compounds, and acids using IUPAC and classical systems.

Chemical Equations

1.4: Chemical Bonding

1.4.1: illustrate and explain the formation of ionic, covalent, and metallic bonds.

Covalent Bonds
Ionic Bonds

1.4.2: define valence electrons, electronegativity, ionic, metallic bond, nonpolar covalent and polar covalent bond.

Covalent Bonds
Electron Configuration
Ionic Bonds

1.4.3: identify lone pairs, bonding electrons, deduce bonding capacity, sketch Lewis Dot structures and structural diagrams.

Covalent Bonds
Ionic Bonds

1.4.8: identify coordinate covalent bonds in ozone, carbon monoxide and various polyatomic ions.

Covalent Bonds

1.5: Molecular Shape â?? VSEPR Theory

1.5.3: identify the type of intermolecular bonding.

Covalent Bonds

1.7: Properties

1.7.1: identify and describe the properties of ionic, molecular, metallic and covalent network substances.

Covalent Bonds
Ionic Bonds

1.7.2: classify ionic, molecular, metallic and covalent network substances according to their properties.

Covalent Bonds

1.7.3: describe how the different types of bonds account for the properties of ionic, molecular, metallic and covalent network substances.

Covalent Bonds
Ionic Bonds

2: Stoichiometry

2.1: The Mole and Balancing Equations

2.1.2: define the law of conservation of mass.

Balancing Chemical Equations
Chemical Equations
Limiting Reactants

2.1.3: demonstrate the proper use of SI units and significant digits in all computations.

Unit Conversions 2 - Scientific Notation and Significant Digits

2.1.4: Convert number of particles to mass and moles.

Chemical Equations

2.2: Molar Mass

2.2.1: define molar mass and determine the molar mass of an element and compound.

Chemical Equations
Stoichiometry

2.2.4: calculate the percent composition from a compound‟s formula.

Chemical Equations

2.2.5: calculate molecular formula from percent composition and molar mass.

Chemical Equations
Stoichiometry

2.3: Mole Ratio Calculations

2.3.1: identify mole ratios of reactants and products from balanced chemical equations.

Chemical Equations

2.3.2: perform calculations using mole-to-mole stoichiometric problems.

Chemical Equations
Limiting Reactants
Stoichiometry

2.3.3: perform stoichiometric calculations related to chemical equations.

Chemical Equations
Limiting Reactants
Stoichiometry

2.3.4: use instruments effectively and accurately for collecting data.

Triple Beam Balance

2.3.6: state a prediction and a hypothesis based on available evidence and background information.

Seed Germination
Temperature and Sex Determination - Metric

2.4: Chemical Changes

2.4.1: compare and contrast physical, chemical, and nuclear changes (in terms of the bonds broken and magnitude of energy changes involved).

Chemical Changes

2.4.2: investigate Kinetic Molecular Theory (KMT).

Diffusion
Temperature and Particle Motion

2.4.3: investigate Collision Reaction Theory.

Collision Theory

2.4.4: identify empirical evidence that may indicate that a chemical change has occurred.

Chemical Changes

2.4.5: differentiate between endothermic and exothermic changes.

Chemical Changes

2.4.6: predict products of chemical reactions.

Chemical Equations
Equilibrium and Concentration

2.4.7: identify the five types of chemical reactions: formation, decomposition, combustion, single, and double replacement including precipitation, neutralization.

Balancing Chemical Equations
Chemical Equations
Equilibrium and Concentration
Titration

2.4.8: write balanced chemical equations for the five different types of chemical reactions: formation, decomposition, combustion, single, and double replacement.

Balancing Chemical Equations
Chemical Equations

2.5: Solutions

2.5.3: identify different types of solutions (acids, bases, neutral, ionic and molecular) and their properties (conductivity, pH, solubility).

Titration
pH Analysis

2.6: Solubility Curves

2.6.1: perform a lab involving solubility curves.

2.6.1.a: plot the solubility and average temperature data.

Seasons Around the World
Solubility and Temperature

2.6.1.b: calculate solubility and perform calculations involving solubility.

Solubility and Temperature

2.7: Solution Concentration

2.7.4: demonstrate an understanding of colligative properties.

Freezing Point of Salt Water

2.9: Stoichiometric Calculations

2.9.2: perform stoichiometric calculations related to chemical equations â?? both gravimetric and volumetric.

Limiting Reactants
Stoichiometry

2.10: Limiting Reagents

2.10.1: explain the concept of limiting reagent.

Limiting Reactants

2.10.2: perform stoichiometric calculations related to chemical equations.

Chemical Equations
Limiting Reactants
Stoichiometry

2.11: Stoichiometric Experimentation

2.11.2: predict how the yield of a particular chemical process can be maximized.

Limiting Reactants

2.11.3: use instruments effectively and accurately for collecting data.

Triple Beam Balance

2.11.6: communicate questions, ideas, and intentions, and receive, interpret, understand, support, and respond to the ideas of others.

Sight vs. Sound Reactions

2.12: Applications of Stoichiometry

2.12.1: identify various stoichiometric applications.

Limiting Reactants
Stoichiometry

2.12.2: communicate questions, ideas, and intentions, and receive, interpret, understand, support, and respond to the ideas of others.

Sight vs. Sound Reactions

2.12.3: compare processes used in science with those used in technology.

Electromagnetic Induction

2.12.4: analyse society‟s influence on science and technology.

DNA Analysis

2.13: Gas Laws and Stoichiometry

2.13.1: describe the behavior of ideal and real gases in terms of the kinetic molecular theory.

Temperature and Particle Motion

2.13.3: perform calculations, using Boyle‟s, Gay-Lussac‟s and Charles‟ laws, and illustrating how they are related to the combined gas law.

Boyle's Law and Charles' Law

2.13.9: explain Graham‟s Law of Diffusion.

Diffusion

2.13.10: explain Dalton‟s Law of Partial Pressures.

Equilibrium and Pressure

Correlation last revised: 9/24/2019

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