Deck 1 Flashcards
Relative isotopic mass
Relative isotopic mass is the mass of an atom of an isotope compared with one twelfth of the mass of an atom of carbon-12
Relative atomic mass
Relative atomic mass is the weighted mean mass of an atom of an element compared with one-twelfth of the mass of an atom of carbon-12.
Relative molecular mass
Relative molecular mass,Mr, is the weighted mean mass of a molecule compared with one-twelfth of the mass of an atom of carbon-12.
Relative formula mass
Relative formula mass is the weighted mean mass of a formula unit compared with one-twelfth of the mass of an atom of carbon-12.
Amount of substance
Amount of substance is the quantity whose unit is the mole.
The Avogadro constant
The Avogadro constant is the number of atoms per mole of the carbon-12 isotope (6.02 x 10^23 mol^-1)
A mole
A mole is the amount of any substance containing as many particles as there are carbon atoms in exactly 12 g of the carbon-12 isotope.
Molar mass
Molar mass is the mass per mole of a substance. The units of molar mass are g mol^-1.
Empirical formula
The empirical formula is the simplest whole-number ratio of atoms of each element present in a compound.
A molecule
A molecule is a small group of atoms held together by covalent bonds.
Molecular formula
The molecular formula is the actual number of atoms of each element in a molecule.
Molar volume
Molar volume is the volume per mole of a gas. The units of molar volume are dm^3 mol^-1. At room temperature and pressure, the molar volume is approximately 24.0dm^3 mol^-1.
Concentration
The concentration of a solution is the amount of solute,in mol, dissolved per 1dm^3 of solution.
Standard solution
A standard solution is a solution of known concentration. Standard solutions are normally used in titration to determine unknown information about another substance.
