Alberta Program of Studies

20?A.1.2k: explain why formulas for ionic compounds refer to the simplest whole-number ratio of ions that result in a net charge of zero

20?A.1.3k: define valence electron, electronegativity, ionic bond and intramolecular force

Electron Configuration

Ionic Bonds

20?A.1.4k: use the periodic table and electron dot diagrams to support and explain ionic bonding theory

20?A.1.5k: explain how an ionic bond results from the simultaneous attraction of oppositely charged ions

20?A.1.6k: explain that ionic compounds form lattices and that these structures relate to the compounds? properties; e.g., melting point, solubility, reactivity.

20-A.1.2s.1: draw electron dot diagrams

20-A.1.4s.1: use appropriate International System of Units (SI) notation, fundamental and derived units and significant digits

Unit Conversions 2 - Scientific Notation and Significant Digits

20?A.2.3k: relate electron pairing to multiple and covalent bonds

20?A.2.4k: draw electron dot diagrams of atoms and molecules, writing structural formulas for molecular substances and using Lewis structures to predict bonding in simple molecules

20-A.2.2s.1: build models depicting the structure of simple covalent molecules, including selected organic compounds

20-A.2.4s.1: analyze and evaluate, objectively, models and graphs constructed by others

Determining a Spring Constant

Seasons Around the World

20?B.1.1k: describe and compare the behaviour of real and ideal gases in terms of kinetic molecular theory

Temperature and Particle Motion

20-B.1.4k.2: perform calculations, based on the gas laws, under STP, SATP and other defined conditions.

20-B.1.2s.1: perform an experiment, in which variables are identified and controlled, to illustrate gas laws

Boyle's Law and Charles' Law

Diffusion

20?C.1.9k: define solubility and identify related factors; i.e., temperature, pressure and miscibility

20?C.1.1sts: explain how science and technology are developed to meet societal needs and expand human capability

20?C.1.2sts: explain that science and technology have influenced, and been influenced by, historical development and societal needs

20-C.1.2s.3: use a balance and volumetric glassware to prepare solutions of specified concentrations

20-C.1.2s.4: perform an investigation to determine the solubility of a solute in a saturated solution

20?C.2.2k: recall the empirical definitions of acidic, basic and neutral solutions determined by using indicators, pH and electrical conductivity

20?C.2.4k: use appropriate SI units to communicate the concentration of solutions and express pH and concentration answers to the correct number of significant digits; i.e., use the number of decimal places in the pH to determine the number of significant digits of the concentration

20?C.2.5k: compare magnitude changes in pH and pOH with changes in concentration for acids and bases

20?C.2.6k: explain how the use of indicators, pH paper or pH meters can be used to measure H3O+(aq)

20?C.2.10k: differentiate, qualitatively, between strong and weak acids and between strong and weak bases on the basis of ionization and dissociation; i.e., pH, reaction rate and electrical conductivity

20?C.2.11k: identify monoprotic and polyprotic acids and bases and compare their ionization/dissociation.

20-C.2.1s.1: design an experiment to differentiate among acidic, basic and neutral solutions

20-C.2.2s.1: construct a table or graph to compare pH and hydronium ion concentration, illustrating that as the hydronium ion concentration increases, the pH decreases

20-C.2.3s.1: use indicators to determine the pH for a variety of solutions

20?C.2.4s: work collaboratively in addressing problems and apply the skills and conventions of science in communicating information and ideas and in assessing results

20?D.1.1k: predict the product(s) of a chemical reaction based upon the reaction type

Balancing Chemical Equations

Chemical Equations

Equilibrium and Concentration

20?D.1.2k: recall the balancing of chemical equations in terms of atoms, molecules and moles

Balancing Chemical Equations

Chemical Equations

20?D.1.5k: calculate the quantities of reactants and/or products involved in chemical reactions, using gravimetric, solution or gas stoichiometry.

Chemical Equations

Limiting Reactants

Stoichiometry

20-D.1.1s.1: plan and predict states, products and theoretical yields for chemical reactions

Chemical Equations

Equilibrium and Concentration

Limiting Reactants

20-D.1.2s.2: balance chemical equations for chemical reactions, using lowest whole-number coefficients

Balancing Chemical Equations

Chemical Equations

20-D.1.3s.1: interpret stoichiometric ratios from chemical reaction equations

Chemical Equations

Limiting Reactants

Stoichiometry

20-D.1.3s.2: perform calculations to determine theoretical yields

Limiting Reactants

Stoichiometry

20-D.1.3s.3: use appropriate SI notation, fundamental and derived units and significant digits when performing stoichiometric calculations

Limiting Reactants

Stoichiometry

20?D.1.4s: work collaboratively in addressing problems and apply the skills and conventions of science in communicating information and ideas and in assessing results

20?D.2.1k: explain chemical principles (i.e., conservation of mass in a chemical change), using quantitative analysis

Chemical Changes

Chemical Equations

20?D.2.2k: identify limiting and excess reagents in chemical reactions

20?D.2.3k: define theoretical yields and actual yields

Limiting Reactants

Stoichiometry

20?D.2.5k: draw and interpret titration curves, using data from titration experiments involving strong monoprotic acids and strong monoprotic bases

20?D.2.6k: describe the function and choice of indicators in titrations

20?D.2.7k: identify equivalence points on strong monoprotic acid?strong monoprotic base titration curves and differentiate between the indicator end point and the equivalence point.

20-D.2.1s.1: design a procedure, using crystallization, filtration or titration, to determine the concentration of a solution

20-D.2.1s.3: predict the approximate equivalence point for a strong monoprotic acid?strong monoprotic base titration and select an appropriate indicator

20-D.2.2s.1: perform a titration to determine the concentration of an acid or a base restricted to strong monoprotic acid?strong monoprotic base combinations

20-D.2.3s.1: calculate theoretical and actual yield and percent yield and error, and account for discrepancies between the theoretical and actual yields

Limiting Reactants

Stoichiometry

20-D.2.3s.3: graph and analyze titration curves for acid-base experiments restricted to strong monoprotic acid?strong monoprotic base combinations

20-D.2.3s.4: use appropriate SI notation, fundamental and derived units and significant digits when performing stoichiometric calculations

Limiting Reactants

Stoichiometry

20-D.2.4s.1: standardize an acidic or a basic solution and compare group results

Correlation last revised: 9/24/2019

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