Trigonal bi pyramidal: the shape of a molecule in which the central atom has 5 bonding pairs.
Trigonal Planar: the shape of a molecule in which the central atom has 3 bonding pairs.
Hydroxide: an ion with the formula OH -
Ionic Compound: a compound which is made up of oppositely charged ions that are held together by electrostatic forces
Nitrate: an ion with the formula NO 3 -
Silver ion: has the formula Ag +
State symbols: symbols within a chemical equation which indicate the state of each compound under the reaction conditions
Atomic Orbital: a region of space aroundthenucleus that can hold up to 2electrons with opposite spins
There is 1 orbital in the s subshell, 3 orbitals in the p subshell and 5 orbitals in the d subshell
Orbitals are filled in order of increasing energy, with orbitals of the same energy occupied singly before pairing
ElectronicConfiguration: the arrangement of electrons into orbitals and energylevels around the nucleus of an atom / ion
Energy Level: the shell that an electron is in
Shell: the orbit that an orbital is in around the nucleus of an atom.
The shell closest to the nucleus is the firstshell
The outermostshell that is occupied by electrons is the valence shell
Sub-shell: a subdivision of the electronic shells into different orbitals.
The types of subshell are s, p, d and f.
Permanent Dipole: a permanent unevendistribution of charge.
Types of intermolecular forces including permanent dipole - dipole interactions and induced dipole - dipole interactions (both of these are also known as van der Waals’ forces) as well as hydrogen bonding.
Molecular substances don’t conduct electricity.
Ionic Bond: electrostatic attraction between positive and negative ions.
Hydrogen Bonding: a type of intermolecular bonding that occurs between molecules containing N, O or F and a H atom of - NH, - OH or HF.
Tetrahedral: the shape of a molecule in which the central atom has 4 bonding pairs.
Lone pairs offer more repulsion than bonding pairs as they are closer to the nucleus of the central atom.
Polar Bond: a covalent bond that has a permanent dipole due to the different electronegativities of the atoms that make up the bond.
Ionic Lattice: a giant structure in which oppositely charged ions are strongly attracted in all directions.
Electron Pair Repulsion Theory: pairs of electrons around a nucleus repel each other so the shape that a molecule adopts has these pairs of electrons positioned asfarapart as possible.
Ionic compounds are soluble and can conduct electricity when liquid or aqueous (but not when solid).
Macroscopic Properties: properties of a bulk material rather than the individual atoms/ molecules that make up the material.
Intermolecular Forces: interactions between different molecules.
Non-linear: the shape of a molecule in which the central atom has 2 bonding pairs and 2 lone pairs.
Pyramidal: the shape of a molecule in which the central atom has 3 bonding pairs and 1 lone pair.
Lone Pair: a pair of outer-shell electrons not involved in bonding.
Polar Molecule: a molecule that contains polar bonds with dipoles that don’t cancel out due to their direction (must be unsymmetrical).
Linear: the shape of a molecule in which the central atom has 2bonding pairs.
Simple Molecular Lattice: a solid structure made up of covalently bonded molecules attracted by intermolecular force (e.g. I2 and ice).
London (Dispersion) Forces: induced dipole - dipole interactions caused when the random movement of electrons creates a temporary dipole in one molecule which then induces a dipole in a neighbouring molecule.
Octahedral: the shape of a molecule in which the central atom has 6 bonding pairs.