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Bond enthalpy
Energy needed to break one mole of a specified bond in gas phase
Born-Haber cycle
Method to calculate lattice enthalpy using Hess's law and formation enthalpies
Covalent character
Partial electron sharing in atoms with an ionic bond
Enthalpy of atomisation
Energy change forming one mole of gaseous atoms from elements
Enthalpy of formation
Energy change forming one mole of a compound from elements
Enthalpy of hydration
Energy change when one mole of gaseous ion dissolves in water
Enthalpy of lattice dissociation
Energy change converting one mole of solid ionic compound into gaseous ions
Enthalpy of lattice formation
Energy change forming one mole of solid ionic compound from gaseous ions
Enthalpy of solution
Energy change when one mole of ionic solid dissolves in water
Entropy
Measure of system disorder, higher for gases than liquids or solids
Feasible reaction
Reaction occurring spontaneously at a given temperature
First electron affinity
Energy change adding one electron to each atom in one mole of gaseous atoms
First ionisation energy
Energy change when one mole of gaseous atoms gains one mole of electrons
Gibbs free-energy change
Measure of reaction feasibility, ΔG = ΔH - TΔSsystem
Ionic character
Degree of electron sharing between atoms, higher sharing indicates more ionic character
Concentration-time graph
Graph used to determine reaction rate by drawing tangents
Order of reaction
Indicates how reactant concentration affects reaction rate
Overall order of a reaction
Sum of individual orders of all reactants in a chemical reaction
Rate-concentration data
Used to deduce the order with respect to a reactant
Rate constant
Relates reaction rate to concentrations of reactants at a given temperature
Rate determining step
Slowest step in a multi-step reaction determining overall rate
Rate equation
Describes relationship between reaction rate and reactant concentrations
Equilibrium
State where forward and backward reaction rates are equal
Equilibrium constant (KP)
Expresses relationship between gaseous products and reactants at equilibrium
Catalyst
Increases reaction rate without affecting equilibrium constant
Homogeneous system
System where all reactants and products are in the same phase
Partial pressures
Pressure exerted by a specific gas in a mixture
Reversible reaction
Reaction where products can reform original reactants
Anode
Positive electrode where oxidation occurs
Cathode
Negative electrode where reduction occurs
Electrochemical cell
Combination of two half cells used to measure electrode potentials
Electrode potential
Potential difference of a cell with a specific electrode
EMF
Difference in potential differences of cathode and anode in a cell
Fuel cell
Converts chemical energy into electricity through redox reactions
Redox reaction
Simultaneous occurrence of reduction and oxidation
Salt bridge
Porous substance with inert electrolyte to balance charges in cells
Acidic buffer
Buffer with weak acid and its conjugate base
Basic buffer
Buffer with weak base and its conjugate acid
Brønsted-Lowry acid
Donates protons, forms hydroxonium ions in water
Brønsted-Lowry base
Accepts protons from water molecules
Buffer solution
Resists pH change with added strong acid/base
Diprotic acid
Acid releasing two H+ ions, e.g. H2SO4
End point
Titration point of indicator colour change
Equivalence point
Neutralisation point, [H+] = [OH-]
Indicators
Solutions changing colour with pH change
Ka
Acid dissociation constant, measures acid strength
Kw
Ionic product of water, Kw = 1.0 x 10^-14 mol^2 dm^-6
Monoprotic acid
Acid releasing one H+ ion, e.g. HCl
Neutralisation
Acid-base reaction forming water and salt
pH
Value indicating solution acidity or alkalinity
pH curve
Graph plotting pH vs. volume of acid/base added
pH meter
Instrument measuring solution pH
pH scale
0-14 scale indicating acidity or alkalinity
Strong acid
Acid fully dissociating in water, e.g. HCl
Strong base
Base fully ionising in water, e.g. NaOH
Titration
Technique to determine unknown solution concentration
Weak acid
Acid with minimal dissociation, e.g. Ethanoic acid
Weak base
Base with slight ionisation in water, e.g. NH3