What determines the geometric shape of a molecule using hybridization?

The geometric shape of a molecule is determined by a combination of several factors, which is encapsulated well in the choice that includes all of them.

The number of lone pairs on the central atom is crucial because lone pairs occupy space and influence bond angles. They cause repulsion between electron pairs as per VSEPR (Valence Shell Electron Pair Repulsion) theory, affecting the overall molecular geometry.

The number of bonds formed between atoms also plays a significant role in defining the shape. Each bond (single, double, or triple) can contribute to the spatial arrangement of the atoms, determining how far apart they will be from each other in three-dimensional space.

The type of atomic orbitals involved in bonding (such as s, p, d, or f orbitals) influences the hybridization process, which combines atomic orbitals to form new hybrid orbitals that can accommodate the electron pairs in the best possible configuration. The resulting hybridization dictates the ideal bond angles and overall molecular shape.

Given all these interrelated factors—lone pairs, number of bonds, and the types of atomic orbitals involved—geometric shape emerges as a product of a comprehensive consideration of these elements together. Thus, the choice that indicates all aspects captures the complete picture