New Brunswick Curriculum
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
1.2.1: use standard atomic notation to represent atoms, define isotope and use isotopic notation.
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.
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.
1.2.9: write electron configuration diagrams using Hund‟s rule, Pauli exclusion principle and Aufbau principle (diagonal rule).
1.2.10: demonstrate an introductory understanding of the Quantum Mechanical Model.
1.2.11: demonstrate an understanding of periodicity of Ionization Energy, electronegativity and atomic radii.
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.
1.4.1: illustrate and explain the formation of ionic, covalent, and metallic 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.
1.4.8: identify coordinate covalent bonds in ozone, carbon monoxide and various polyatomic ions.
1.5.3: identify the type of intermolecular bonding.
1.7.1: identify and describe the properties of ionic, molecular, metallic and covalent network substances.
1.7.2: classify ionic, molecular, metallic and covalent network substances according to their properties.
1.7.3: describe how the different types of bonds account for the properties of ionic, molecular, metallic and covalent network substances.
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.
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.
2.2.5: calculate molecular formula from percent composition and molar mass.
Chemical Equations
Stoichiometry
2.3.1: identify mole ratios of reactants and products from balanced 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.
2.3.6: state a prediction and a hypothesis based on available evidence and background information.
Seed Germination
Temperature and Sex Determination - Metric
2.4.1: compare and contrast physical, chemical, and nuclear changes (in terms of the bonds broken and magnitude of energy changes involved).
2.4.2: investigate Kinetic Molecular Theory (KMT).
Diffusion
Temperature and Particle Motion
2.4.3: investigate Collision Reaction Theory.
2.4.4: identify empirical evidence that may indicate that a chemical change has occurred.
2.4.5: differentiate between endothermic and exothermic 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
2.5.3: identify different types of solutions (acids, bases, neutral, ionic and molecular) and their properties (conductivity, pH, solubility).
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.
2.7.4: demonstrate an understanding of colligative properties.
2.9.2: perform stoichiometric calculations related to chemical equations â?? both gravimetric and volumetric.
Limiting Reactants
Stoichiometry
2.10.1: explain the concept of limiting reagent.
2.10.2: perform stoichiometric calculations related to chemical equations.
Chemical Equations
Limiting Reactants
Stoichiometry
2.11.2: predict how the yield of a particular chemical process can be maximized.
2.11.3: use instruments effectively and accurately for collecting data.
2.11.6: communicate questions, ideas, and intentions, and receive, interpret, understand, support, and respond to the ideas of others.
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.
2.12.3: compare processes used in science with those used in technology.
2.12.4: analyse society‟s influence on science and technology.
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.
2.13.9: explain Graham‟s Law of Diffusion.
2.13.10: explain Dalton‟s Law of Partial Pressures.
Correlation last revised: 9/16/2020