Bonding and structure Flashcards
Bonding pair
outer shell pair of electrons involved in bonding
Covalent bond
bond formed when atoms share a pair of electrons
Dative covalent bond
- shared pair of electrons
- provided by one atom ONLY
Electronegativity
ability of an atom to attract the pair of electrons in a covalent bond
Giant covalent lattice
3D structure
- atoms held together by strong covalent bonds
e.g. diamond, graphite, graphene, silicon, silicon
dioxide
Giant ionic lattice
3D structure
- oppositely charged ions
- held together by strong ionic bonds
i.e. ALL IONIC COMPOUNDS
Hydrogen bond
- strong dipole-dipole attraction
- between an electron deficient hydrogen atom
- (O-Hδ+,N-Hδ+, F-Hδ+) on one molecule and a lone pair on the O, N or F on a different molecule.
Intermolecular force
attractive force between molecules
Ionic bond
- electrostatic attraction
- between oppositely charged ions
Lone pair
outer shell pair of electrons that is not involved in bonding
Metallic bond
- electrostatic attraction
- between positive metal ions and delocalized electrons
Permanent dipole
- small charge difference across a bond
- as a result of a difference in electronegativity
Permanent dipole-dipole force
- weak attractive force
- between permanent dipoles in neighbouring molecules
Simple molecular lattice
- 3D structure of molecules
- held together by weak intermolecular forces
e.g. I2
Induced dipole-dipole (London) forces
- very weak attractive force
- between induced dipoles in neighbouring molecules
