5.3 : Covalent Bonding Flashcards
Define covalent bonding
The strong electrostatic attraction between a shared pair of electrons and the nuclei of the bonded atoms.
Where does covalent bonding occur?
Between :
Non-metallic elements (H2, O2)
Compounds of non metallic elements ( H2o, CO2)
Polyatomic ions ( NH4+ )
Explain covalent bonding in terms of orbitals
It is the overlap of atomic orbitals, each containing one electron.
Doesn’t necessarily have noble gas structure.
Are covalent bonds localised or delocalised?
Localised : acts solely between the shared pair of electrons and the nuclei of the two bonded atoms.
What are lone pairs?
Electron pairs that are not bonded
What is a double covalent bond?
The electrostatic attraction is between two shared pairs of electrons and the nuclei of the bonding atoms.
Has noble gas structure.
What is a triple covalent bond?
The electrostatic attraction is between three shared pairs of electrons and the nuclei of the bonded atoms.
Has noble gas structure.
What is a dative covalent bond?
Also called a coordinate bond.
The shared pair of electrons has been supplied by one of the bonded atoms only.
How does average bond enthalpy relate to covalent bonds?
The larger the average bond enthalpy, the stronger the covalent bond.