Module 1 - F321 Flashcards
Isotopes
Isotopes are atoms of the same element with different numbers of neutrons.
Atomic (proton) number
Atomic (proton) number is the number of protons in the nucleus of an atom.
Mass (nucleon) number
Mass (nucleon) number is the number of particles (protons and neutrons) in the nucleus.
Ion
An ion is a positively or negatively charged atom or group of atoms.
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, 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. Chemists use ‘amount of substance’ as a means of counting atoms.
Avogadro constant
Avogadro constant, is the number of atoms per mole of the carbon-12 isotope.
Mole
A mole is the amount of any substance containing as many particles as there are carbon atoms in exactly 12g 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.
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