F325 Key Definitions

This is a set of key definition flashcards for the OCR A chemistry unit F325: Equilibria, Energetics & Elements 

RATES AND ENTROPY DEFINITIONS TO BE ADDED SOON  

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  • Created by: abbiemca
  • Created on: 21-04-16 00:13
Redox
A reaction where both oxidation and reduction take place
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Oxidation Number
A measure of the number of electrons that an atom uses to bona with atoms of a different element
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Oxidising Agent
A reagent that oxidises (takes electrons from) another species
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Reducing Agent
A reagent that oxidises (takes electrons from) another species
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Standard Electrode Potential
Is the e.m.f of a half cell compared to the standard hydrogen half cell, measured at 298K with all solutions' concentrations at 1mol/dm^3 and a gas pressure of 100kPa (1 atm).
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Fuel Cell
Uses the energy from the reaction of a fuel with oxygen to create a voltage
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d-block Elements
The highest energy sub-shell is a d sub-shell
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Ligand
A molecule or ion that can donate a pair of electrons to a transition metal ion to form a coordinate bond
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Complex Ion
A transition metal ion bonded to one or more ligands by coordinate bonds (dative covalent bonds).
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Coordinate Bond
A shared pair of electrons in which one of the bonded atoms provides both electrons for the shared pair
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Coordination Number
The total number of coordinate bonds formed between a central metal ion and is ligands
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Bidentate Ligand
A ligand which can donate two lone pairs of electrons to a metal ion to form two coordinate bonds
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Ligand Substitution
A reaction in which one ligand in a complex ion is replaced by another ligand
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Stereoisomers
Species with the same structural formula but a different arrangement of atoms in space
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Optical Isomers
Stereoisomers that are a pair of non-superimposable mirror images of each other
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Stability Constant, Kstab
The equilibrium constant for an equilibrium existing between a transition metal ion surrounded y water ligands and the complex formed when the same ion has undergone ligand substitution
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le Chatlier's Principle
When a system in dynamic equilibrium is subjected to a change, the equilibrium position will shift to minimise the change
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Acid
Proton Donor
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Base
Proton Acceptor
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Conjugate Acid-Base Pairs
A pair of two species that transform into each other by gain or loss of a proton
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Strong Acid
A proton donor that completely dissociates in solution
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Weak Acid
A proton donor that partially dissociates in solution
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Buffer Solution
A system that minimise pH changes on addition of small amounts of an acid or a base
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Enthalpy Change of Neutralisation
The energy change that accompanies the neutralisation of an aqueous acid by an aqueous base to form one mole of H20 (l) under standard conditions
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Lattice Enthalpy
The enthalpy change that accompanies the formation of one mole of an ionic compound from its gaseous ions under standard conditions
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Enthalpy Change of Solution
The enthalpy change that takes place when one mole of a compound is completely dissolved in water under standard conditions
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Enthalpy Change of Hydration
The enthalpy change that takes place when one mole of isolated gaseous ions is dissolved in water forming one mole of aqueous ions under standard conditions
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Enthalpy Change of Formation
The enthalpy change that takes place when one mole of a compound is formed from its constituent elements in their standard states under standard conditions
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First Ionisation Energy
The enthalpy change accompanying the removal of one electron from each atom in one mole of gaseous atoms to form one mole of gaseous 1+ ions
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Second Ionisation Energy
The enthalpy change accompanying the removal one one electron from each ion in one mole of gaseous 1+ ions to form one mole of gaseous 2+ ions
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Enthalpy Change of Atomisation
The enthalpy change that takes place when one mole of gaseous atoms forms from the element in its standard state
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First Electron Affinity
The enthalpy change accompanying the addition of one electron to each atom in one mole of gaseous atoms to from one mole of gaseous 1- ions
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Second Electron Affinity
The enthalpy change accompanying the addition of one electron to each ion in one mole of gaseous 1- ions to form one mole of gaseous 2- ions
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Other cards in this set

Card 2

Front

A measure of the number of electrons that an atom uses to bona with atoms of a different element

Back

Oxidation Number

Card 3

Front

A reagent that oxidises (takes electrons from) another species

Back

Preview of the back of card 3

Card 4

Front

A reagent that oxidises (takes electrons from) another species

Back

Preview of the back of card 4

Card 5

Front

Is the e.m.f of a half cell compared to the standard hydrogen half cell, measured at 298K with all solutions' concentrations at 1mol/dm^3 and a gas pressure of 100kPa (1 atm).

Back

Preview of the back of card 5
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