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26 Cards in this Set
- Front
- Back
relative atomic mass
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the weighted mean of the masses of the element's naturally occurring isotopes, relative to carbon-12 isotope (12 unites exactly)
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relative molecular mass
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sum of the relative atomic masses of the atoms in te molecular formula
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mass number
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sum of number of protons and number of neutrons in nucleus
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atomic number
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number of protons in nucleus
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isotopes
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atoms of the same element with same number of protons, but different number of neutrons
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first ionisation energy
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the energy required to remove one mole of electrons from one mole of atoms in the gaseous state
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electronegativity
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a relative measure of an atom's ability to attract a bonding part of electrons in a covalent bond
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average bond enthalpy
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amount of energy required to break one mole of bonds in gaseous state averaged across a range of compounds containing that bond under standard conditions
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rate of reaction
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rate of increase in concentration of products/ decrease in concentration of reactants
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activation energy
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min. value of kinetic energy which particles must have before they are able to react
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acids
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BL theory: proton donors
Lewis: electron pair acceptors |
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bases
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BL: proton acceptors
Lewis: electron pair donors |
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oxidizing agent
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a substance accepts electrons and causes another reactant to be oxidised
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reducing agent
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a substance supplies electrons to cause another reactant to be reduced
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ligand
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species that uses a lone pair of electrons to form a dative covalent bond with a metal ion
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standard state
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1 atm = 100kPa / 1.01x10^5 Pa
25oC = 298K 1kPa = 1000Pa |
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standard enthalpy of formation
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enthalpy change when 1 mole of a compound is made from its elements, in their standard states, at 298K and 1 atm
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standard enthalpy of combustion
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enthalpy change when 1 mole of a compound is burnt in an excess of oxygen under standard conditions
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lattice enthalpy
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enthalpy change that occurs when 1 mole of a solid ionic compound is separated into gaseous ions under standard conditions
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electron affinity
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enthalpy change when 1 mole of gaseous atoms attracts 1 mole of electrons
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standard electrode potential
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the voltage and potential generated when it is connected to the standard hydrogen electrode by an external circuit and a salt bridge, measured under standard conditions
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exothermic reaction
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a reaction results in a transfer of heat energy from the system to the surroundings
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endothermic reaction
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energy transfer from surroundings to the system
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standard enthalpy change of reaction
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the difference between the products and the enthalpy of the reactants under standard conditions
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oxidation
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adding oxygen, losing electrons
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reduction
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losing oxygen, gaining electrons
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