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A2 Chemistry OCR Definitions:
Rates, acids and enthalpy
- Enthalpy change
- Enthalpy change of atomisation
- The enthalpy change when 1 mole of gaseous atoms forms the element at 298K, 101kPa
- The enthalpy change when 1 mole of gaseous atoms forms the element at 298K, 101kPa
- 1st Ionisation energy
- The energy needed to remove 1 electron from every atom in 1 mole of gaseous atoms, to form 1+ ions
- 2nd Ionisation energy
- Energy needed to remove the second electron from every atom in 1 mole of gaseous 1+ ions
- Energy needed to remove the second electron from every atom in 1 mole of gaseous 1+ ions
- The energy needed to remove 1 electron from every atom in 1 mole of gaseous atoms, to form 1+ ions
- Lattice enthalpy
- The enthalpy change when 1 mole of an ionic compound is formed from its gaseous ions, at 298K, 101kPa
- The enthalpy change when 1 mole of an ionic compound is formed from its gaseous ions, at 298K, 101kPa
- Enthalpy change of formation
- The enthalpy change when 1 mole of a compound is formed from its elements, at 298K, 101 kPa
- The enthalpy change when 1 mole of a compound is formed from its elements, at 298K, 101 kPa
- Standard enthalpy of electron affinity
- Enthalpy change when 1 electron is gained by every atom in 1 mole of gaseous atoms, to form 1- ions
- NB: 1st EA always exothermic, 2nd & 3rd always endothermic
- Enthalpy change when 1 electron is gained by every atom in 1 mole of gaseous atoms, to form 1- ions
- Enthalpy change of solution
- Enthalpy change when 1 mole of an ionic compound dissolves in
sufficient water to make a very dilute solution, at 298K, 101kPa
- NB: Exothermic = Soluble
- Enthalpy change when 1 mole of an ionic compound dissolves in
sufficient water to make a very dilute solution, at 298K, 101kPa
- Enthalpy change of hydration
- The enthalpy change when 1 mole of gaseous ions dissolves in
sufficient water to form a very dilute solution
- The enthalpy change when 1 mole of gaseous ions dissolves in
sufficient water to form a very dilute solution
- Enthalpy of neutralisation
- Enthalpy change when enough acid/alkali is neutralised to make 1 mole H2O
- Enthalpy change when enough acid/alkali is neutralised to make 1 mole H2O
- Enthalpy change of atomisation
- Hess' Law
- The enthalpy change going from reactant to product is independent of the route taken
- The enthalpy change going from reactant to product is independent of the route taken
- Acids/bases
- Acid
- Proton donor
- Proton donor
- Base
- Proton acceptor
- Proton acceptor
- Strong acid
- One that ionises fully
- One that ionises fully
- Weak acid
- One that only partially ionises
- One that only partially ionises
- Conjugate acid/base pairs
- A conjugate acid becomes its own conjugate base when it gives a H+ to another base. Vice versa for base
- NB: If conj. acid is v/ strong, conj. base is v/ weak
- A conjugate acid becomes its own conjugate base when it gives a H+ to another base. Vice versa for base
- Acid
- Kw
- Ionic product of water
- NB: 1x10-4
- Ionic product of water
- pH
- -log(Concentration of H+)
- -log(Concentration of H+)
- Ka
- Acid dissociation constant
- Acid dissociation constant
- Indicators
- Weak acids which have 2 colours (one for acid, one for its conj. base)
- Weak acids which have 2 colours (one for acid, one for its conj. base)
- Buffer
- A system that minimises pH changes on addition of moderate amounts of acid/alkali
- A system that minimises pH changes on addition of moderate amounts of acid/alkali
- Rates
- Rate of Reaction
- How the concentration of a reactant decreases over time
- How the concentration of a reactant decreases over time
- Order
- The power to which we raise the conc. of a particular reactant in a rate equation
- The power to which we raise the conc. of a particular reactant in a rate equation
- Rate constant (k)
- The proportionality constant in a rate equation
- The proportionality constant in a rate equation
- Rate Determining Step (RDS)
- The slowest step in a reaction mechanism (series of reactions not shown in overall reaction)
- Determines overall rate
- The slowest step in a reaction mechanism (series of reactions not shown in overall reaction)
- Half-life
- The time taken for the concentration of a reactant to halve
- The time taken for the concentration of a reactant to halve
- Rate of Reaction
- Free energy (ΔG)
- The balance between enthalpy, entropy and temperature for a process
- NB: Reaction is spontaneous is ΔG<0
- The balance between enthalpy, entropy and temperature for a process
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