According to VSPER theory multiple bonds is treated as a single electron pair and 2 or 3 electron pairs of a multiple bonds are treated as a single pair.

Multiple Bonds and Electron Pair Repulsion Theory

Introduction
When atoms form chemical bonds, they can share one or more pairs of electrons. In some cases, atoms can form multiple bonds, such as double or triple bonds. The electron pair repulsion theory (VSEPR theory) is a model used to predict the shapes of molecules based on the repulsion between electron pairs. According to this theory, electron pairs in a molecule arrange themselves in a way that minimizes repulsion.

Multiple Bond as a Single Electron Pair
In the context of the VSEPR theory, a multiple bond is treated as if it is a single electron pair. This is because multiple bonds involve the sharing of more than one pair of electrons between atoms. However, from a molecular geometry perspective, the multiple bond is considered as a single "super pair" due to the way the electron pairs repel each other.

Electron Pair Repulsion in Multiple Bonds
When a multiple bond is formed, the electron pairs involved in the bond are treated as a single entity. The repulsion between electron pairs determines the shape of the molecule. The repulsion between a multiple bond and other electron pairs is similar to the repulsion between two separate electron pairs.

Effect on Molecular Geometry
The VSEPR theory predicts the molecular geometry based on the repulsion between electron pairs. The repulsion between a multiple bond and other electron pairs affects the overall shape of the molecule. The presence of a multiple bond can influence the bond angles and distort the molecular shape.

Example: Carbon Dioxide (CO2)
Let's consider the example of carbon dioxide (CO2). Carbon dioxide consists of two double bonds between carbon and oxygen atoms. According to the VSEPR theory, the electron pairs in the double bonds are treated as a single super pair. This super pair repels the electron pairs of the two oxygen atoms.

As a result, the molecule adopts a linear geometry, with a bond angle of 180 degrees between the carbon and oxygen atoms. The repulsion between the double bond and the electron pairs of the oxygen atoms pushes the oxygen atoms closer together, resulting in a linear arrangement.

Conclusion
In summary, the VSEPR theory considers a multiple bond as a single electron pair. The repulsion between the electron pairs in the multiple bond and other electron pairs in the molecule influences the molecular geometry. By treating the multiple bond as a single entity, the VSEPR theory provides a framework for predicting the shapes of molecules with multiple bonds.