General - Definitions (CAP 1)
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ATOMIC NUMBER
The number of protons in the nucleus of an atom.
MASS NUMBER
The total number of protons and neutrons in the nucleus of an atom.
ISOTOPES
Atoms of the same element (same number of protons and electrons) with different numbers of neutrons and different masses.
ATOMIC ORBITAL
A region around the nucleus that can hold up to two electrons, with opposite spins
p-BLOCK ELEMENT
Element which has the highest energy electron in a p sub-shell (or p orbital) (Applies to any element; s-, p-, d- or f-block)
MOLAR MASS
The mass, in g, per mole of a substance. (Units are gmol-1)
RELATIVE ISOTOPIC MASS
The mass of an atom of an isotope compared with 1/12 of the mass of an atom of Carbon-12.
RELATIVE ATOMIC MASS
The weighted mean mass of an atom of an element compared with 1/12 of the mass of an atom of Carbon-12.
ACID
A proton donor.
BASE
A proton acceptor.
ALKALI
A base that dissolves in water and releases OH- ions in aqueous solution.
SALT
A compound produced when a H+ ion from an acid is replaced by a metal ion or another positive ion, such as the ammonium ion.
STRONG ACID
A proton donor which completely dissociates into its ions in solution.
WEAK ACID
A proton donor which partially dissociates into its ions in solution.
MOLE
The amount of substance containing as many particles as there are carbon atoms in exactly 12g of Carbon-12.
AVOGADRO’S CONSTANT, NA
The number of particles per mole of a substance (6.02 x 1023 mol-1)
MOLAR GAS VOLUME
The gas volume per mole of a substance. This is 24.0 dm3mol-1 at room temperature and pressure (RTP).
IONIC BOND
The electrostatic attraction between positive and negative (oppositely charged) ions.
COVALENT BOND
The strong electrostatic attraction between a shared pair of electrons and the nuclei of the bonded atoms.
DATIVE COVALENT (CO-ORDINATE) BOND
The strong electrostatic attraction between a shared pair of electrons and the nuclei of the bonded atoms, where only one of the atoms supplies both the electrons shared.
ELECTRONEGATIVITY
The ability of an atom to attract the bonding electrons towards itself in a covalent bond.
ELECTRON PAIR REPULSION THEORY
• The shape of simple covalent molecules and ions are determined by the number & type of electron pairs around the central atom. • Electron pairs repel one another as far apart as possible • Lone pairs of electrons repel more strongly than bond pairs of electrons
METALLIC BONDING
The strong electrostatic attraction between metal cations (positive ions) and delocalised electrons (in a giant metallic lattice structure).