A region of space that holds upto 2 electrons, with opposite spins.
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Definition of Isotopes
Isotopes are atoms of the same element with the same number of protons but a different number of neutrons which differing the mass.
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Definition of Relative Atomic Mass
The weighted average mass of an atom of an element compared to 1/12 the mass of an atom of carbon-12
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Definition of Relative Isotopic Mass
The average mass of an atom of an isotope compared to to 1/12 the mass of an atom of carbon-12
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Definition of Relative Formula Mass
The average mass of a formula of a substance compared to to 1/12 the mass of an atom of carbon-12
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Definition of Relative Molecular Mass
The average mass of a molecule of a substance compared to to 1/12 the mass of an atom of carbon-12
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Mole
Mole is the amount of substance that contains the same number of particles as there are atoms in 12 grams of carbon-12
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Empirical Formula
The simplest whole number ratio of all the atoms of each element in a compund
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Acid
A compound that releases H+ ions in aqueous solutions.
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Neutralisation
A Chemical reaction in which an acid and a base react together to produce a salt AND water.
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Salt
A compound formed when the H+ ion from an is replaced by a metal ion or an ammonium ion.
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Base
A proton acceptor
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Alkali
A water-soluble base which releases OH- ions in aqueous solutions.
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Spectator ions
ions that do not participate in reactions
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Molar gas Volume
Volume per mole of gas molecules at a stated temperature and pressure.
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First Ionisation energy
The first ionisation energy of an element is the energy needed to remove one electron from each atom in a mole of gaseous atoms of an element
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Second Ionisation energy
Second Ionistaion energy is the energy required to remove one electron from each ion in one mole of gaseous 1+ ions of an element to form one mole of gaseous 2+ ions.
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Ionic Bonding
Ionic bonding is the electrostatic attraction between positive and negative ions.
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Giant Ionic lattice
A regular array of alternating positive and negative ions.
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Covalent Bond
Electrostatic attraction between the shared pair of bonding electrons and the nuclei of the bonded atoms
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Dative Covalent bond
A covalent bond formed when the shared pair of electrons are provided by one of the atoms forming the bond.
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Lone Pair
Outer shell electrons not involved in bonding form pairs in the same orbital which are very important for shape of molecules.
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Electron Pair repulsion theory
States that the electron pairs in the outer shell of the central atoms in a molecule repel each other and therefore arrange themselves to be as far away from each other as possible.
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Electronegativity
relative ability of an atom to attract the bonding pair of electrons in a covalent bond.
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Metallic bonding
attraction between negative charged delocalised electrons, adjacent positive charged metal nuclei
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Volatility
Ease of vaporisation
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Other cards in this set
Card 2
Front
Definition of Isotopes
Back
Isotopes are atoms of the same element with the same number of protons but a different number of neutrons which differing the mass.
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