is the strong electrostatic force of attraction between oppositely charged ions formed by electron transfer.
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Metal
Metals consist of a giant lattices of metal ions in a sea of delocalised electrons
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Metallic bonding
A metallic bond is the electrostatic force of attraction between the positive metal ions and the delocalised electrons
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Covalent bond
A covalent bond strong and is caused by the electrostatic attraction between the bonding pair of electrons and nuclei.
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Dative covalent bond
forms when the shared pair of electrons in the covalent bond come from only one of the bonding atoms
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Enthalpy change of formation
is the energy transferred when 1 mole of the compound is formed from its elements under standard conditions (298K and 100kpa), all reactants and products being in their standard states
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Enthalpy of atomisation
The enthalpy of atomisation of an element is the enthalpy change when 1 mole of gaseous atoms is formed from the element in its standard state
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First Ionisation enthalpy
is the enthalpy change required to remove 1 mole of electrons from 1 mole of gaseous atoms to form 1 mole of gaseous ions with a +1 charge
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Second Ionisation enthalpy
is the enthalpy change to remove 1 mole of electrons from one mole of gaseous 1+ ions to produces one mole of gaseous 2+ ions
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First Electron Affinity
is the enthalpy change that occurs when 1 mole of gaseous atoms gain 1 mole of electrons to form 1 mole of gaseous ions with a –1 charge
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Second Electron Affinity
is the enthalpy change when one mole of gaseous 1- ions gains one electron per ion to produce gaseous 2- ions.
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Enthalpy of lattice formation
is the standard enthalpy change when 1 mole of an ionic crystal lattice is formed from its constituent ions in gaseous form.
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Card 2
Front
Metal
Back
Metals consist of a giant lattices of metal ions in a sea of delocalised electrons
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