Chemical species which can donate a proton (H+). Strong acids dissociate fully into ions. Weak acids only partly dissociate.
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Alkali
A soluble base that releases OH- ions into aqueous solution.
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Anhydrous
Without water of crystallisation.
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Atomic radius
Half the distance between the nuclei of two covalently bonded atoms.
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Base
A substance that readily accepts a proton (H+) from an acid.
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Dative covalent bond
A covalent bond where both electrons come from one atom.
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Disproportionation
A type of redox reaction in which the same species is both reduced and oxidised.
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Electronegativity
Describes the ability of an atom to attract the bonding electrons in a covalent bond.
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Empirical formula
The simplest whole number ratio of the elements present in a compound.
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Hydrogen bond
A weak intermolecular bond formed between molecules containing a hydrogen atom bonded to one of the most electronegative elements.( F, N, O)
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Ion
A positively or negatively charged atom or covalently bonded group of atoms.
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Ionic bonding
The electrostatic attraction between oppositely charged ions.
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Ionisation energy
The first ionisation energy is the energy needed to remove one electron from each atom in one mole of gaseous atoms to form one mole of gaseous +1 atoms.
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Isotopes
Atoms of an element with the same number of protons but different numbers of neutrons.
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Mole
One mole of a substance is the mass that has the same number of particles as there are atoms in exactly 12g of carbon-12.
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Molecular formula
Shows the total number of atoms present in a molecule of the compound.
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Oxidation
The loss of electrons.
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Polar covalent bond
A covalent bond in which the two bonding electrons are not shared equally by the two bonded atoms. The atom that gets the bigger share of the two electrons becomes delta -.
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Precipitate
An insoluble solid formed when two solids react.
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Redox
Reactions which involve reduction and oxidation processes.
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Reduction
The gain of electrons.
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Relative atomic mass
The mean weighted mass of an element taking into account the relative abundance of its naturally occurring isotopes, measured on a scale on which carbon-12 has a mass of exactly 12.
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Salt
A compound produced when the H+ ion of an acid is replaced by a metal ion or an ammonium ion.
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Stoichiometry
The stoichiometry for a reaction shows the mole ratio of reactants and products in the balanced equation for he reaction.
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Thermal decomposition
The breakdown of a compound by heat.
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Titration
Measurement of the exact amount of one solution needed to react with a fixed amount of another solution.
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Van der Waal's forces
the weak forces of attraction between molecules based on instantaneous and induced dipoles.
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Water of crystallisation
Water molecules incorporated into the crystal structure of a salt.
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Other cards in this set
Card 2
Front
A soluble base that releases OH- ions into aqueous solution.
Back
Alkali
Card 3
Front
Without water of crystallisation.
Back
Card 4
Front
Half the distance between the nuclei of two covalently bonded atoms.
Back
Card 5
Front
A substance that readily accepts a proton (H+) from an acid.
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