AS key words Flashcards
Lattice energy
The energy change when 1 mol of the solid is formed from its consistency gaseous ions that start infinitely far apart.
Enthalpy change of atomisation
The enthalpy change when 1 mol of gaseous atoms is made from an element in its standard state.
Atomic number
The number of protons in the nucleus of the atom of that element
The relative atomic mass
The weighted average mass of an atom of that divided by 1/12 the mass of carbon-12
The mass number of an isotope
The sum of the number of protons and neutrons in the nucleus of an atom of that isotope
Periodicity
There is a pattern of regular repeating physical and chemical properties.
Elecrtonegativity
The extent to which it attracts a pair of electrons in a covalent bond towards itself
First ionisation energy
The energy required to remove one electron from the ground state of each atom of a mole of gaseous atoms of that element
The second ionisation energy
The energy required to remove one electron from each ion of a mole of gaseous singly charged positive ions of that element.
The first electron affinity
The energy change one one mole of electron is added to each atom in a mole of neutral gaseous atoms.
The second electron affinity
The energy change when one electron is added to each ion in a mole of singly charged gaseous negatively charged ions.
Electrophile
Is a species that bonds to an electron rich site in a molecule. It accepts a pair of electrons from that site and forms a new covalent bonds.
Enthalpy of formation.
The standard enthalpies of formation is the enthalpy change when 1 mol of a substance is formed from its elements in their standard conditions
Enthalpy change of the reaction
The enthalpy change when the number of moles of the substance in the equation as written react under standard condition
Enthalpy change of combustion
The standard enthalpy change when 1 mol os a substance is burt in excess oxygen under standard conditions
