Physical Chemistry II Definitions- AQA Chemistry A-level

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58 Terms

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Bond enthalpy

Energy needed to break one mole of a specified bond in gas phase

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Born-Haber cycle

Method to calculate lattice enthalpy using Hess's law and formation enthalpies

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Covalent character

Partial electron sharing in atoms with an ionic bond

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Enthalpy of atomisation

Energy change forming one mole of gaseous atoms from elements

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Enthalpy of formation

Energy change forming one mole of a compound from elements

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Enthalpy of hydration

Energy change when one mole of gaseous ion dissolves in water

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Enthalpy of lattice dissociation

Energy change converting one mole of solid ionic compound into gaseous ions

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Enthalpy of lattice formation

Energy change forming one mole of solid ionic compound from gaseous ions

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Enthalpy of solution

Energy change when one mole of ionic solid dissolves in water

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Entropy

Measure of system disorder, higher for gases than liquids or solids

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Feasible reaction

Reaction occurring spontaneously at a given temperature

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First electron affinity

Energy change adding one electron to each atom in one mole of gaseous atoms

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First ionisation energy

Energy change when one mole of gaseous atoms gains one mole of electrons

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Gibbs free-energy change

Measure of reaction feasibility, ΔG = ΔH - TΔSsystem

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Ionic character

Degree of electron sharing between atoms, higher sharing indicates more ionic character

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Concentration-time graph

Graph used to determine reaction rate by drawing tangents

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Order of reaction

Indicates how reactant concentration affects reaction rate

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Overall order of a reaction

Sum of individual orders of all reactants in a chemical reaction

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Rate-concentration data

Used to deduce the order with respect to a reactant

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Rate constant

Relates reaction rate to concentrations of reactants at a given temperature

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Rate determining step

Slowest step in a multi-step reaction determining overall rate

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Rate equation

Describes relationship between reaction rate and reactant concentrations

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Equilibrium

State where forward and backward reaction rates are equal

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Equilibrium constant (KP)

Expresses relationship between gaseous products and reactants at equilibrium

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Catalyst

Increases reaction rate without affecting equilibrium constant

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Homogeneous system

System where all reactants and products are in the same phase

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Partial pressures

Pressure exerted by a specific gas in a mixture

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Reversible reaction

Reaction where products can reform original reactants

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Anode

Positive electrode where oxidation occurs

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Cathode

Negative electrode where reduction occurs

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Electrochemical cell

Combination of two half cells used to measure electrode potentials

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Electrode potential

Potential difference of a cell with a specific electrode

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EMF

Difference in potential differences of cathode and anode in a cell

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Fuel cell

Converts chemical energy into electricity through redox reactions

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Redox reaction

Simultaneous occurrence of reduction and oxidation

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Salt bridge

Porous substance with inert electrolyte to balance charges in cells

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Acidic buffer

Buffer with weak acid and its conjugate base

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Basic buffer

Buffer with weak base and its conjugate acid

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Brønsted-Lowry acid

Donates protons, forms hydroxonium ions in water

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Brønsted-Lowry base

Accepts protons from water molecules

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Buffer solution

Resists pH change with added strong acid/base

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Diprotic acid

Acid releasing two H+ ions, e.g. H2SO4

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End point

Titration point of indicator colour change

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Equivalence point

Neutralisation point, [H+] = [OH-]

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Indicators

Solutions changing colour with pH change

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Ka

Acid dissociation constant, measures acid strength

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Kw

Ionic product of water, Kw = 1.0 x 10^-14 mol^2 dm^-6

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Monoprotic acid

Acid releasing one H+ ion, e.g. HCl

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Neutralisation

Acid-base reaction forming water and salt

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pH

Value indicating solution acidity or alkalinity

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pH curve

Graph plotting pH vs. volume of acid/base added

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pH meter

Instrument measuring solution pH

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pH scale

0-14 scale indicating acidity or alkalinity

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Strong acid

Acid fully dissociating in water, e.g. HCl

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Strong base

Base fully ionising in water, e.g. NaOH

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Titration

Technique to determine unknown solution concentration

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Weak acid

Acid with minimal dissociation, e.g. Ethanoic acid

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Weak base

Base with slight ionisation in water, e.g. NH3