Definitions Flashcards
Molecular ion
Two or more atoms covalently bonded with an overall charge
Avogadro’s constant
Number of atoms in 12.000g of carbon-12
Mole
The amount of substance which contains the Avogadro constant of atoms, molecules or groups of ions
Molar mass
The mass of one mole of a substance
Anhydrous
A salt which contains no water of crytallisation
Hydrated
A salt which contains water of crystallisation
Water of crystallisation
Water chemically bonded within a crystal structure
Atomic number
The number of protons in an atom
Mass number
The total number of protons and neutrons in an atom
Relative atomic mass
The average mass of an atom of an element relative to one-twelfth the mass of an atom of carbon-12
Relative isotopic mass
The mass of an atom of an isotope of an element relative to one-twelfth the mass of an atom of carbon-12
Isotopes
Atoms that have the same atomic number but a different mass number
Relative Formula Mass
The average mass of a formula unit relative to one-twelfth the mass of an atom of carbon-12
Relative molecular mass
The average mass of a molecule relative to one-twelfth the mass of an atom of carbon-12
First ionisation energy
The energy required to convert one mole of gaseous atoms into gaseous ions with a single positive charge
Second ionisation energy
The energy required to convert one mole of gaseous ions with a single positive charge into gaseous ions with a double positive charge
Third ionisation energy
The energy required to convert one mole of gaseous ions with a double positive charge into one mole of gaseous ions with a triple positive charge
Covalent bond
The electrostatic attraction between a shared pair electrons and the nuclei of bonded atoms
Co-ordinate bond
A shared pair of electrons between two atoms. One atom provides both electrons
Octet rule
When reacting, an atom tends to gain, lose or share electrons to achieve eight in its outer shell
Electronegativity
The extent to which an atom attracts the bonding electrons in a covalent bond
Polar bond
A covalent bond in which there is unequal sharing of the bonding electrons
Delocalised electrons
Outer electrons do not have fixed positions but move freely
Intermolecular
Between neighbouring molecules