Atomic orbital: A volume within an atom that can only hold up to two electrons with opposite spin.
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First ionisation energy: The enthalpy change when one mole of individual gaseous atoms each lose one electron to form one mole of gaseous 1+ ions.
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Successive ionisation energy: The enthalpy change when one mole of individual gaseous ions each use one electron to form one mole of ions of a greater charge.
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Disproportionation- A specific redox reaction where a chemical species is simultaneously oxidised and reduced.
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Mole: The amount of a substance containing as many particles as there are carbon atoms in 12g of carbon 12.
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Empirical formula: the simplest whole number ratio of atoms of each element in a compound
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Molecular formula: The actual number of atoms of each element present in a molecule.
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Acid: A molecule which releases hydrogen ions when dissolved in water.
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Base: a substance which neutralises an acid.
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Salt: product formed when the hydrogen ion of an acid is replaced by a metal ion or ammonium.
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Ionic bond: the electrostatic attraction between oppositely charged ions.
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Covalent bond: shared pair of electrons
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Dative covalent: a bond where both electrons are donated by the same atom
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Oxidation number: the number of electron that an atom uses to bond with another atom in a molecule.
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Oxidation number: the number of electron that an atom uses to bond with another atom in a molecule.
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Redox: A reaction involving electron transfer where both oxidation and reduction occur.
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Relative atomic mass: the weighted mean mass of an atom of an element relative to 1/12 the mass of an atom of carbon 12; where carbon 12 is given as an arbitrary value.
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Relative isotopic mass: The mass of an atom of an element of an isotope, relative to the mass of an atom of carbon 12; where carbon 12 is given as an arbitrary value.
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Relative molecular mass: the mass of a molecule of the compound relative to the mass of an atom of carbon 12; where carbon 12 is given as an arbitrary value.
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Relative formula mass: the mass of the atoms in the empirical formula of the compound relative to the mass of carbon 12; where carbon 12 is given as an arbitrary value.
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Electronegativity: The ability of an atom to attract electrons into a covalent bond.
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Other cards in this set
Card 2
Front
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Back
First ionisation energy: The enthalpy change when one mole of individual gaseous atoms each lose one electron to form one mole of gaseous 1+ ions.
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