To determine the number of lone pairs (unbonded pairs) and bonding pairs of electrons for O2 we first need to draw as valid Lewis Structure. Once we have a Lewis Structure for O2 then we can identify the lone and bonding pairs.
O2 Lewis Structure: [ Ссылка ]
O2 Molecular Geometry: [ Ссылка ]
Bonding pairs of electrons are the electrons between the atoms. These form the chemical bond and are shared between atoms. Often a pair of bonding electrons is represented by a line. Each line represents a pair of bonding electrons.
Lone pairs (unbonded pairs) of electrons are the remaining electrons around the atom. These are not between atoms and are not shared. The are important because they do occupy space and influence the shape of the molecule.
There is one lone pair of electrons on each O atom for O2 (Oxygen gas).
We often need to know the the number of lone pairs of electrons in a molecule like O2 (as well as electrons involved in bonds) to determine the molecular geometry, calculate formal charges, and understand polarity and chemical reactivity.
---Learning Resources---
- How to Draw Lewis Structures: [ Ссылка ]
- Lewis Structures Practice Video Worksheet: [ Ссылка ]
- Determining Formal Charge: [ Ссылка ]
- Finding Valence Electrons (molecule): [ Ссылка ]
- The Octet Rule: [ Ссылка ]
More help at [ Ссылка ]
