sigma bond

The result is formation of one sigma bond and two pi bonds.

It forms for an instant a single sigma bond to both of the carbon atoms involved.

The molecule can be described as having two pi bonds but without a sigma bond.

The shift in the sigma bond may be antarafacial or suprafacial.

These may have their own names, such as sigma bond and pi bond.

Electron density is donated directly to the metal like a sigma bond would be formed.

The reaction center can be a p-orbital, a conjugated system or even a sigma bond.

In a sigma bond, the atomic orbitals from two atoms which are nearby go one on top of each other.

Pi-bonds are more spread out bonds than the sigma bonds.

The sigma bond in this compound is destroyed in reaction with ethanol.

The X represents the number of sigma bonds between the central atoms and outside atoms.

The pi bond is a weaker attraction than the sigma bond.

Usually, a single bond is a sigma bond.

This is why a sigma bond is stronger.

This triple bond consists of a sigma bond and two pi bonds.

Both MO's form the oxygen to hydrogen sigma bonds.

When the carbon atoms approach each other, two of the sp orbitals overlap to form a sigma bond.

The extra strength of a multiple bond versus a single (sigma bond) is shown in many ways.

Sigma bonds occur when the orbitals of two shared electrons overlap head-to-head.

In the second step, the nucleophilic reagent attacks the carbocation and forms a sigma bond.

In some cases of multiple bonds between two atoms, there is no sigma bond at all, only pi bonds.

The inductive effect drops across every sigma bond involved limiting its effect to only a few bonds.

Overlap of an sp orbital from each atom forms one sp-sp sigma bond.

From a molecular perspective, traditional polymers yield to mechanical stress though cleavage of sigma bonds.

This also means that only single bonds (sigma bonds) will be present between adjacent carbon atoms of the tail.