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Essential ideas:
- Physical and chemical properties depend on the ways in which different atoms combine.
- The mole makes it possible to correlate the number of particles with the mass that can be measured.
- Mole ratios in chemical equations can be used to calculate reacting ratios by mass and gas volume.
1.1 States of matter, changes of state and state symbols
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This video covers states of matter, changes of state and state symbols.
Applications and skills: Application of the state symbols (s), (l), (g) and (aq) in equations. |
1.1 Elements, compounds, mixtures
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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: Explanation of observable changes in physical properties and temperature during changes of state. |
1.1 Physical and chemical changes
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This video covers the differences between physical and chemical changes.
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1.1 Balancing chemical equations
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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. Guidance: Balancing of equations should include a variety of types of reactions. |
1.2 Relative atomic mass and molecular mass
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Understandings:
Masses of atoms are compared on a scale relative to 12C and are expressed as relative atomic mass (Ar) and relative formula/molecular mass (Mr). |
1.1 Atom economy
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Utilization:
Atom economy - the atom economy of chemical reaction is a measure of the amount of starting materials that become useful products. |
1.2 The mole concept
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Understandings:
The mole is a fixed number of particles and refers to the amount, n, of substance. Applications and skills: Calculation of the molar masses of atoms, ions, molecules and formula units. |
1.2 Molar ratio
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This video explains how to use the coefficients in a balanced equation to calculate amounts of products.
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1.2 Molar mass
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Understandings:
Molar mass (M) has the units g mol-1. Applications and skills: Calculation of the molar masses of atoms, ions, molecules and formula units. |
1.2 Mole calculations
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Applications and skills:
Solution of problems involving the relationships between the number of particles, the amount of substance in moles and the mass in grams. |
1.2 Empirical and molecular fomula
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Understandings:
The empirical formula and molecular formula of a compound give the simplest ratio and the actual number of atoms present in a molecule respectively. Applications and skills: Determination of the molecular formula of a compound from its empirical formula and molar mass. |
1.2 Calculating percentage composition by mass
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This video covers how to calculate the percentage composition by mass of an element in a compound.
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1.2 Calculating empirical formula from % composition by mass
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Applications and skills:
Interconversion of the percentage composition by mass and the empirical formula. |
1.2 Calculating empirical formula from combustion analysis
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This video covers how to calculate the empirical formula organic compound from combustion data.
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1.2 Water of crystallisation
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This video covers how to calculate the water of crystallisation from experimental data.
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1.2 Calculate empirical formula from experimental data
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Applications and skills:
Obtaining and using experimental data for deriving empirical formulas from reactions involving mass changes. |
1.3 Limiting and excess reactants
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Understandings:
Reactants can be either limiting or excess. Applications and skills: Solve problems relating to reacting quantities and limiting and excess reactants. |
1.3 Percentage yield
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Understandings:
Reactants can be either limiting or excess. The experimental yield can be different from the theoretical yield. Applications and skills: Solve problems relating to reacting quantities, limiting and excess reactants, theoretical, experimental and percentage yields. |
1.3 Percentage purity
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This video covers how to calculate percentage purity.
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1.3 Molar volume of a gas
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Understandings:
The molar volume of an ideal gas is a constant at specified temperature and pressure. |
1.3 Avogadro's law
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Understandings:
Avogadro’s law enables the mole ratio of reacting gases to be determined from volumes of the gases. Applications and skills: Calculation of reacting volumes of gases using Avogadro’s law. |
1.3 Solve problems involving temperature and volume for an ideal gas.
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Applications and skills:
Solution of problems and analysis of graphs involving the relationship between temperature, pressure and volume for a fixed mass of an ideal gas. |
1.3 Ideal gas equation
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Applications and skills:
Solution of problems relating to the ideal gas equation. |
1.3 Calculating molar mass of a gas using PV=nRT
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Applications and skills:
Solve problems relating to the ideal gas equation. Obtaining and using experimental values to calculate the molar mass of a gas from the ideal gas equation. |
1.3 Determine molar mass of a gas experimentally
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Applications and skills:
Obtaining and using experimental values to calculate the molar mass of a gas from the ideal gas equation. |
1.3 Ideal gases
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Applications and skills:
Explanation of the deviation of real gases from ideal behaviour at low temperature and high pressure. |
1.3 Concentration of solutions
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Understandings:
The molar concentration of a solution is determined by the amount of solute and the volume of solution. Applications and skills: Solve problems involving molar concentration, amount of solute and volume of solution. Units of concentration to include: g dm-3, mol dm-3 and parts per million (ppm). |
1.3 Thermometric titration
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This video covers how to calculate the concentration of a solution using a thermometric titration.
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1.3 Back titration
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This video covers how to determine the percentage calcium carbonate in an egg shell using a back titration.
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Review of past exam questions (old syllabus) but still relevant for new syllabus.
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A review of some past quantitative chemistry exam questions for the old syllabus.
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