Bonding and Structure Flashcards
Define the term ‘bonding pair’
An outer shell pair of electrons involved in bonding
Define the term ‘covalent bond’
The bond formed when atoms share a pair of electrons
Define the term ‘dative covalent bond (coordinate bond)’
A shared pair of electrons which has been provided by one atom only
Define the term ‘electronegativity’
A measure of the ability of an atom to attract the pair of electrons in a covalent bond
Define the term ‘giant covalent lattice’
A three dimensional structure of atoms held together by strong covalent bonds e.g. diamond, graphite, graphene, silicon, silicon dioxide
Define the term ‘giant ionic lattice’
A three dimensional structure of oppositely charged ions held together by strong ionic bonds
Define the term ‘hydrogen bond’
A strong dipole-dipole attraction between an electron deficient hydrogen atom (O-H, N-H, F-H) on one molecule and a lone pair on the O, N or F on a different molecule
Define the term ‘intermolecular force’
An attractive force between molecules
Define the term ‘ionic bond’
The electrostatic attraction between oppositely charged ions
Define the term ‘lone pair’
An outer shell pair of electrons that is not involved in bonding
Define the term ‘metallic bond’
The electrostatic attraction between positive metal ions and delocalised electrons
Define the term ‘permanent dipole’
A small charge difference across a bond as a result of a difference in electronegativity
Define the term ‘permanent dipole-dipole force’
A weak attractive force between permanent dipoles in neighbouring molecules
Define the term ‘simple molecular lattice’
A three dimensional structure of molecules held together by weak intermolecular forces e.g. I2
Define the term ‘induced dipole-dipole (London) forces’
A very weak attractive force between induced dipoles in neighbouring molecules
