Gizmos for New Brunswick - Science: 11th Grade Chemistry (New Brunswick Curriculum adopted 2009)

This correlation lists the recommended Gizmos for this province's curriculum standards. Click any Gizmo title below for more information.

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.

1.2: : The Underlying Structure of Matter

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.

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.

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: : Elements and Compounds

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

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: : Chemical Bonding

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.

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: : Molecular Shape â?? VSEPR Theory

1.5.3: : identify the type of intermolecular bonding.

1.7: : Properties

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: : Stoichiometry

2.1: : The Mole and Balancing Equations

2.1.2: : define the law of conservation of mass.

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

2.1.4: : Convert number of particles to mass and moles.

2.2: : Molar Mass

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

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

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

2.3: : Mole Ratio Calculations

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.

2.3.3: : perform stoichiometric calculations related to chemical equations.

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.

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).

2.4.2: : investigate Kinetic Molecular Theory (KMT).

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.

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

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

2.5: : Solutions

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

2.6: : Solubility Curves

2.6.1: : perform a lab involving solubility curves.

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

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

2.7: : Solution Concentration

2.7.4: : demonstrate an understanding of colligative properties.

2.9: : Stoichiometric Calculations

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

2.10: : Limiting Reagents

2.10.1: : explain the concept of limiting reagent.

2.10.2: : perform stoichiometric calculations related to chemical equations.

2.11: : Stoichiometric Experimentation

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: : Applications of Stoichiometry

2.12.1: : identify various stoichiometric applications.

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: : Gas Laws and Stoichiometry

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

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

New Brunswick - Science: 11th Grade Chemistry

New Brunswick Curriculum | Adopted: 2009

1: : From Structures to Properties

2: : Stoichiometry