Gizmos for Newfoundland and Labrador - Science: 12th Grade Chemistry (Newfoundland and Labrador 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 Kinetics to Equilibrium

1.1: : Collision Theory, Reaction Mechanisms, and Catalysts

1.1.1: : describe collision theory and its connection to factors involved in altering reaction rates

1.1.1.a: : state the Kinetic Molecular Theory (KMT) of matter

1.1.1.b: : describe two pieces of evidence that support the KMT

1.1.1.b.i: : pressure

1.1.1.b.ii: : diffusion

1.1.1.c: : state the collision theory

1.1.1.d: : recognize that reaction rate can be measured by monitoring a variety of changing macroproperties including; mass, colour, volume and pH

1.1.1.e: : relate the rate of reaction to the number of successful collisions between reacting particles

1.1.2: : identify and discuss the properties and factors which affect reaction rate

1.1.2.a: : explain using collision theory how temperature, concentration/pressure, surface area and nature of reactants affect the rate of reaction

1.1.2.b: : describe the effect of a catalyst on the rate of reaction

1.1.5: : compile and display evidence and information in charts, tables and graphs

1.1.8: : describe a reaction mechanism and a catalystâ??s role in a chemical reaction

1.1.8.a: : define a reaction mechanism as a series of elementary reactions which determine the reaction rate and when added together result in an overall balanced equation

1.1.8.c: : define a reaction intermediate as a substance which is produced by an elementary process, only to be consumed by a later elementary process

1.1.8.d: : define rate determining step (RDS) as the slowest elementary process in the reaction mechanism, which is the step that determines the overall reaction rate

1.1.8.f: : given a reaction mechanism with the RDS identified, determine all catalysts, intermediates, the overall balanced equation and state the effect of changing a reactant concentration on the overall rate

1.1.8.g: : state that a catalyst speeds up a chemical reaction by means of providing an alternate mechanism (â??alternate pathwayâ??)

1.2: : Applications of Collision Theory

1.2.1: : analyze and describe examples where technologies were developed based upon scientific understanding.

1.3: : Dynamic Equilibrium

1.3.1: : define the concept of dynamic equilibrium as it pertains to reversible chemical reactions

1.3.1.a: : state the criteria that apply to a system at equilibrium: closed system with constant temperature, constancy of macroscopic properties, evidence of reversibility, and equal rates of forward and reverse processes

1.3.1.b: : describe the steps in which a chemical system attains dynamic equilibrium

1.3.1.c: : write and interpret chemical equations for chemical systems at equilibrium

1.3.2: : explain how different factors affect chemical equilibrium

1.3.2.a: : explain how the forward and reverse reaction rates in a chemical equilibrium are affected by changes in the temperature, pressure/ volume, and concentration (of one reactant or product), of a chemical equilibrium

1.3.2.b: : state Le ChÃ¢telierâ??s Principle

1.4: : Le ChÃ¢telierâ??s Principle

1.4.1: : explain how different factors affect chemical equilibrium

1.4.1.a: : use Le ChÃ¢telierâ??s Principle to predict, qualitatively, shifts in equilibrium caused by changes in temperature, pressure, volume or concentration

1.4.1.b: : use Le ChÃ¢telierâ??s Principle to determine how the concentration of a reactant and/or product changes after a change is imposed on an equilibrium (not relative to initial conditions)

1.4.2: : explain the roles of evidence and theories, in Le ChÃ¢telierâ??s Principle

1.4.4: : identify the theoretical basis of an investigation and develop a prediction

1.5: : Equlibrium Constant

1.5.1: : define the concept of equilibrium constant expression as it pertains to chemical systems

1.5.1.a: : write equilibrium constant expression, K, for chemical systems

1.5.1.b: : recognize that solids and liquids are not included in the equilibrium expression, K

1.5.1.d: : calculate equilibrium constants for simple chemical systems when concentrations at equilibrium are known

1.5.1.e: : calculate equilibrium concentrations for chemical systems when K and all other equilibrium concentrations are known

1.5.1.f: : predict whether or not reactants or products are favoured in a reversible reaction, on the basis of the magnitude of the equilibrium constant

1.5.2: : solve Keq problems involving the initial concentrations, the changes that occur in each substance, and the resulting equilibrium concentrations

1.5.2.a: : calculate equilibrium concentrations for simple chemical systems when

1.5.2.a.i: : initial concentrations of reactants and one equilibrium concentration are known

1.5.2.a.ii: : initial concentrations of reactants and the percent reaction is known

1.5.2.b: : calculate equilibrium constants, K, for simple chemical systems when:

1.5.2.b.i: : initial concentrations, and one equilibrium concentration are known

1.5.2.b.ii: : initial concentrations, and the percent reaction of one of the reactants are known

2: : Acids and Bases

2.1: : Properties and Definitions of Acids and Bases

2.1.2: : describe and apply classification systems and nomenclature used in acids and bases

2.1.2.a: : define acids and bases operationally in terms of their effect on pH, taste, reactions with metals, reactions with each other, solution conductivity, and effect on indicators

2.1.3: : explain the roles of evidence, theories, and paradigms in acid-base theories

2.1.3.a: : trace the development of acid-base theories from the original operational definition to Arrhenius theory, to the modern revised Arrhenius concept up to the BrÃ¸nsted-Lowry theory

2.1.4: : describe various acid-base definitions up to the BrÃ¸nsted-Lowry definition, including the limitations of these definitions

2.1.4.a: : define and identify Arrhenius, modern Arrhenius and BrÃ¸nsted- Lowry acids and bases.

2.2: : Acids/Base Calculations

2.2.3: : define pH and calculate it for an acid (or base) given the initial concentration and vice-versa

2.2.3.h: : differentiate between strength and concentration operationally, using pH, indicator colour, and rate of reaction with metals (acids), for acid and base solutions of equal concentration

2.4: : Acid/Base Titrations

2.4.1: : calculate the concentration of an acid or base solution using stoichiometry

2.4.1.b: : describe the process of a titration

2.4.1.c: : define primary standard and recognize its importance in a titration procedure

2.4.1.d: : differentiate between indicator end point and equivalence (stoichiometric) point

2.4.1.e: : perform stoichiometric titration calculations where one of molarity of acid, molarity of base, volume of acid or volume of base is to be determined from the others

2.4.2: : use instruments effectively and accurately for collecting titration data

2.4.2.a: : perform a titration experiment and related calculations to determine the concentration of an acid or base solution

2.4.3: : select appropriate instruments and use them safely, for collecting evidence and appropriate processes for titrations

2.4.4: : select and use appropriate symbolic, graphical modes of representation to communicate titrations and results

2.4.5: : interpret patterns and trends in data and infer or calculate relationships among variables from titration labs

2.4.8: : explain how acid-base indicators function

2.4.8.a: : define acid/base indicators operationally

2.4.8.b: : define acid/base indicators theoretically

2.4.8.c: : determine an appropriate indicator for an acid-base titration

2.4.8.d: : determine the appropriate pH of a solution using indicator colours, and vice versa

2.4.10: : identify a line of best fit on a scatter plot and interpolate and extrapolate based on the line of best fit

2.4.10.a: : draw titration curve graphs, using data from titration experiments involving acids and bases in various combinations

2.4.11: : interpret patterns and trends in data and infer or calculate relationships among variables from titration labs

2.4.11.a: : interpret titration curve graphs

2.4.11.c: : sketch and interpret titration curves qualitatively

2.4.11.d: : determine qualitatively the nature of the equilibrium at the stoichiometric equivalence point when a strong acid is mixed with a weak base and vice versa

2.5: : Determining Ka

2.5.1: : perform an experiment identifying and controlling major variables

2.5.2: : evaluate and select appropriate instruments for collecting evidence and appropriate processes for problem solving, inquiring, and decision making

2.5.3: : compile and display data in charts, tables and graphs

2.5.4: : use instruments effectively, accurately and safely for collecting data

3: : Thermochemistry

3.1: : Temperature and Kinetic Energy

3.1.1: : explain temperature and heat using the concept of kinetic energy and the particle model of matter

3.1.1.b: : identify and describe the changes to particle movement in systems in which the energy change is accompanied by a change in temperature of the system

3.1.2: : calculate and compare the energy involved in changes of temperature

3.1.2.a: : define the terms: joule, heat capacity and specific heat capacity

3.2: : Calculating Heat

3.2.1: : calculate and compare the energy involved in changes of temperature

3.2.1.a: : identify that the amount of heat lost or gained by an object is dependent upon; type of material, change in temperature of material, and mass of material

3.2.1.b: : perform calculations involving heat capacity, C, and specific heat capacity, c

3.2.1.f: : state the First Law of Thermodynamics and apply it to determine the amount of heat an object contains

3.2.1.g: : define the calorimeter and identify it as the basic instrument for measuring heat transfer

3.2.1.h: : calculate the heat gained or lost from a system using the formulas q = mc delta T or q = C delta T where c is the specific heat capacity, C is the heat capacity and delta T is the change in temperature

3.3: : Enthalpy Change

3.3.1: : define enthalpy, endothermic process, exothermic process, and molar enthalpy

3.3.2: : calculate and compare the energy involved in changes of state and that in chemical reactions

3.3.2.f: : identify and explain that energy changes are observed during phase changes and chemical changes where forces of attractions between particles are formed or broken yet no change in the temperature of the system occurs

3.4: : Thermochemistry and Potential Energy

3.4.3: : write and balance thermochemical equations including the combustion reaction of alkanes

3.4.3.b: : calculate the heat gained or lost from a system using the formula q = n delta H when delta H is the molar heat of a phase change or chemical reaction

3.4.3.d: : perform calculations which apply the First Law of Thermodynamics in determining the heat of a reaction (or phase change) given experimental data for changes to the surroundings

3.4.4: : perform an experiment identifying and controlling major variables

3.4.5: : evaluate instruments for collecting data

3.5: : Heating and Cooling Curves

3.5.1: : compile, display and interpret evidence and information in a graphical format

3.5.1.c: : calculate the total heat for a multi-step process that includes a temperature and phase change

3.6: : Science Decisions Involving Thermochemistry

3.6.1: : analyze the knowledge and skills acquired in their study of thermochemistry to identify areas of further study

3.6.1.b: : compare physical, chemical, and nuclear changes in terms of the species and the magnitude of energy involved

3.8: : Determining Enthalpy Change

3.8.1: : determine experimentally the changes in energy of various chemical reactions

3.8.5: : evaluate and select appropriate instruments for collecting evidence and appropriate processes for problem solving, inquiring, and decision making