Topic 1: Stoichiometric relationships (13.5 hours)
1.1 Introduction to the particulate nature of matter and chemical change
Nature of science:
Making quantitative measurements with replicates to ensure reliability—definite and multiple proportions. (3.1)
Understandings:
• Atoms of different elements combine in fixed ratios to form compounds, which
have different properties from their component elements.
• Mixtures contain more than one element and/or compound that are not
chemically bonded together and so retain their individual properties.
• Mixtures are either homogeneous or heterogeneous.
Applications and skills:
• Deduction of chemical equations when reactants and products are specified.
• Application of the state symbols (s), (l), (g) and (aq) in equations.
• Explanation of observable changes in physical properties and temperature
during changes of state.
Guidance:
• Balancing of equations should include a variety of types of reactions.
• Names of the changes of state—melting, freezing, vaporization (evaporation
and boiling), condensation, sublimation and deposition—should be covered
International-mindedness:
• Chemical symbols and equations are international, enabling effective
communication amongst scientists without need for translation.
• IUPAC (International Union of Pure and Applied Chemistry) is the world
authority in developing standardized nomenclature for both organic and
inorganic compounds.
Theory of knowledge:
• Chemical equations are the “language” of chemistry. How does the use of
universal languages help and hinder the pursuit of knowledge?
• Lavoisier’s discovery of oxygen, which overturned the phlogiston theory of
combustion, is an example of a paradigm shift. How does scientific
knowledge progress?
Utilization:
• Refrigeration and how it is related to the changes of state.
• Atom economy.
• Freeze-drying of foods.
1.1 Introduction to the particulate nature of matter and chemical change
Nature of science:
Making quantitative measurements with replicates to ensure reliability—definite and multiple proportions. (3.1)
Understandings:
• Atoms of different elements combine in fixed ratios to form compounds, which
have different properties from their component elements.
• Mixtures contain more than one element and/or compound that are not
chemically bonded together and so retain their individual properties.
• Mixtures are either homogeneous or heterogeneous.
Applications and skills:
• Deduction of chemical equations when reactants and products are specified.
• Application of the state symbols (s), (l), (g) and (aq) in equations.
• Explanation of observable changes in physical properties and temperature
during changes of state.
Guidance:
• Balancing of equations should include a variety of types of reactions.
• Names of the changes of state—melting, freezing, vaporization (evaporation
and boiling), condensation, sublimation and deposition—should be covered
International-mindedness:
• Chemical symbols and equations are international, enabling effective
communication amongst scientists without need for translation.
• IUPAC (International Union of Pure and Applied Chemistry) is the world
authority in developing standardized nomenclature for both organic and
inorganic compounds.
Theory of knowledge:
• Chemical equations are the “language” of chemistry. How does the use of
universal languages help and hinder the pursuit of knowledge?
• Lavoisier’s discovery of oxygen, which overturned the phlogiston theory of
combustion, is an example of a paradigm shift. How does scientific
knowledge progress?
Utilization:
• Refrigeration and how it is related to the changes of state.
• Atom economy.
• Freeze-drying of foods.