yes
Such pairs of electrons are called as lone pairs.
4io3orho3ihr33
These pairs of electrons are referred to as lone pairs.
IF6+ cation has no lone pairs, the IF6- anion has one lone pair. SF6 has no lone pairs.
Two lone pair
3 bond pairs and no lone pairs
Chlorine (nucleus) has 1 lone pair and 3 polar-covalent bonding pairs (the shared pairs with O). Each oxygen (nucleus) has 3 lone pairs and 1 polar-covalent bonding pair (the shared pair with Cl)
Such pairs of electrons are called as lone pairs.
4io3orho3ihr33
Lone-pair electrons, Bonded pairs of electrons
These pairs of electrons are referred to as lone pairs.
IF6+ cation has no lone pairs, the IF6- anion has one lone pair. SF6 has no lone pairs.
Nitrogen normally makes three covalent bond pairs and has one lone pair remaining.
The repulsion between lone pairs are stronger than the repulsion between bonding pairs between one bonding pair and lone pair due to electrostatic interactions.
A lone pair of electrons takes up space despite being very small. Lone pairs have a greater repulsive effect than bonding pairs. This is because there are already other forces needing to be taken into consideration with bond pairs. So to summarize: Lone pair-lone pair repulsion > lone pair-bond pair repulsion > bond pair-bond pair repulsion. This makes the molecular geometry different.
Two lone pair
There are 2 lone pairs in each Oxygen atom. So there are 4 lone pairs in total, which means 8 lone pair electrons.