Module 5 Definitions Flashcards
bronsted-lowry base
H+ acceptor
bronsted-lowry acid
H+ donator
alkali
soluble base that releases OH- ions
salt
when the H+ in an acid is replaced by a metal or ammonium ion
conjugate acid
a species formed when a proton is added to a base
conjugate base
a species formed when a proton is removed from an acid
conjugate acid-base pair
two species that differ by H+
first ionisation energy
-The change in energy when one mole of electrons is removed from one mole of gaseous atoms to form one mole of gaseous 1+ ions
-positive enthalpy change as breaking the attraction between electron and proton
First electron affinity
-The change in energy when one mole of gaseous atoms gain one mole of electrons to form one mole of gaseous 1- ions
-negative enthalpy change as forming a bond between electron and protons
Second electron affinity
-The change in energy when one mole of gaseous 1- ions gain one mole of electrons to form one mole of gaseous 2- ions
-positive enthalpy change as overcome repulsion between negative ion and electron
Standard enthalpy change of combustion
-The enthalpy change when one mole of a substance is completely burned in excess oxygen, under standard conditions
-negative enthalpy change as energy is released
Standard enthalpy change of formation
-The enthalpy change when one mole of a compound is formed from it’s elements in the standard states, under standard conditions
-usually negative
Standard enthalpy change of neutralisation
-The enthalpy change when an acid and an alkali are neutralised forming one mole of water, under standard conditions
-negative enthalpy change as making H2O
Enthalpy change of atomisation
-The enthalpy change when one mole of gaseous atoms are formed from an element in it’s standard state
-positive enthalpy change as breaking a bond
Lattice enthalpy
-The enthalpy change for the formation of one mole of an ionic compound from it’s gaseous ions under standard conditions
-negative enthalpy change as forming a bond
Enthalpy change of hydration
-The enthalpy change when one mole of gaseous ions dissolve in water to form one mole of aqueous ions
-negative enthalpy change as bond formation with H2O
Enthalpy change of solution
-The enthalpy change when one mole of a compound is completely dissolved in water
-positive or negative enthalpy change
Standard enthalpy change of reaction
-The enthalpy change when a reaction occurs in the molar quantities shown in the chemical equation with all reactants and products in their standard states, under standard conditions
-positive or negative enthalpy change
average bond enthalpy
the enthalpy change for breaking one mole of bonds in gaseous molecules
transition element
a d-block element that forms an ion with a partially filled d sub-shell
ligand
a species that donates an electron pair to a metal ion and forms a dative covalent bond with the metal ion
monodentate ligand
donates one lone pair of electrons to the central metal ion forming one dative bond
bidentate ligand
donates two lone pairs of electrons to the central metal ion forming two dative bonds
complex ion
an ion which is bonded to ligands
