electron pair

Such a group is referred to as an electron pair.

Such an arrangement makes electron pairs closer together than they need to be.

It places electron pairs 90 degrees from their nearest neighbors.

This is usually dictated by lone electron pairs on the metal centre.

This electron pair forms the bond with a proton (H+).

In the meanwhile oxygen takes complete control of the electron pair and becomes negatively charged.

The number of electron pairs, therefore, determine the overall geometry that they will adopt.

A fundamental factor in these molecular structures is the existence of electron pairs.

An especially odd quality of the electron pairs is that their members, though coordinated, remain relatively far apart in space.

The electron pair then expels the leaving group and the double bond is formed.

In that state, they are all Lewis acids (electron pair acceptors).

Before the above reaction, the sulfur atom has two lone electron pairs.

Likewise, for 4 electron pairs, the optimal arrangement is tetrahedral.

This gives a total of eight electrons, or four electron pairs that are arranged tetrahedrally.

These rules are addition and extensions to polyhedral skeletal electron pair theory.

The electron count for each of these complexes is 26 electron pairs.

As a result the electron pairs are attracted by the nuclei less and less strongly.

All electron pairs repel each other, bonding or lone.

When the electron pair moves towards the attacking reagent, it is termed as the +E effect.

The two dots on the P represent the lone electron pair of the phosphorus atom.

An alternative form of representation, not shown here, has bond-forming electron pairs represented as solid lines.

Extra electron pairs are added for open polyhedra that have p number of vertices missing.

For Cooper electron pairs, "a" and "c" represent different spin directions.

It depends on the number of electron pairs and the chemical nature of the atoms to which they belong.

The four electron pairs are spread so as to point roughly towards the apices of a tetrahedron.