level 5
Topic #1: Stoichiometric Relationships - 13.5 Hours for SL and HL
1.1 Introduction to the particulate nature of matter and chemical change
- "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."
1.2 The mole concept
- "The mole is a fixed number of particles and refers to the amount, n, of substance."
- "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)."
- "Molar mass (M) has the units g mol-1."
- "The empirical formula and molecular formula of a compound give the simplest ratio and the actual number of atoms present in a molecule respectively."
1.3 Reacting masses and volumes
- "Reactants can be either limiting or excess."
- "The experimental yield can be different from the theoretical yield."
- "Avogadro’s law enables the mole ratio of reacting gases to be determined from volumes of the gases."
- "The molar volume of an ideal gas is a constant at specified temperature and pressure."
- "The molar concentration of a solution is determined by the amount of solute and the volume of solution."
- "A standard solution is one of known concentration."
2017年09月16日 08点09分
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1.1 Introduction to the particulate nature of matter and chemical change
- "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."
1.2 The mole concept
- "The mole is a fixed number of particles and refers to the amount, n, of substance."
- "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)."
- "Molar mass (M) has the units g mol-1."
- "The empirical formula and molecular formula of a compound give the simplest ratio and the actual number of atoms present in a molecule respectively."
1.3 Reacting masses and volumes
- "Reactants can be either limiting or excess."
- "The experimental yield can be different from the theoretical yield."
- "Avogadro’s law enables the mole ratio of reacting gases to be determined from volumes of the gases."
- "The molar volume of an ideal gas is a constant at specified temperature and pressure."
- "The molar concentration of a solution is determined by the amount of solute and the volume of solution."
- "A standard solution is one of known concentration."
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