Question

On hybridisation of one \(s\) and three \(p\)-orbitals, we get (a) foar orbitals with tetrahedral orientation (b) three orbitals with trigonal orientation (c) two orbitals with linear arientation (d) two orbitals with perpendicular orientation.

Short answer

On hybridization of one s and three p-orbitals, we get four orbitals with tetrahedral orientation.

Step-by-step solution

Identify the Type of Hybridization

The combination of one s orbital with three p orbitals results in sp3 hybridization. These orbitals are formed by mixing one s orbital and three different p orbitals (px, py, pz) from the same atom.

Determine the Shape and Orientation

The sp3 hybridization leads to the formation of four equivalent orbitals that are oriented in tetrahedral geometry. This arrangement allows for the maximum separation between the orbitals, which is consistent with the principles of VSEPR theory, minimizing the electron pair repulsion.

Choose the Correct Option

Based on the identified hybridization type and the resulting geometry, the correct option can be selected.

Key concepts

What Are Hybrid Orbitals?

When it comes to understanding molecular shapes and bonding, the concept of hybrid orbitals is fundamental. Imagining the interaction of atomic orbitals can be a bit like picturing the blending of different colors of paint to create a new hue. In chemistry, atomic orbitals mix to form new orbitals known as hybrid orbitals, which have different energies, shapes, and orientations than the original orbitals.

Formation of sp3 Hybrid Orbitals

Consider a carbon atom, which has one s orbital and three p orbitals in its outer shell. Through the process of hybridization, these orbitals merge to form four equivalent sp3 hybrid orbitals. Each hybrid orbital is a blend of the one s and three p orbitals. The 'sp3' designation indicates the type and number of atomic orbitals involved: one s orbital and three p orbitals.

The formation of sp3 hybrid orbitals is like creating four new identical rooms from four different rooms in a house, each pointing to the corners of a tetrahedron. This allows atoms to form bonds that are evenly spaced apart, minimizing repulsion between electrons and ultimately leading to the stability of the molecule.

Understanding Tetrahedral Geometry

The shape that results from sp3 hybridization is called tetrahedral geometry, and it's like the tripod of molecular structures — stable and robust. Picture a pyramid with a triangular base; at the top is the atom, while the base corners represent the directions in which the four hybrid orbitals point.

Balancing Electrons in Tetrahedral Geometry

Each sp3 hybrid orbital can house a pair of electrons. With the tetrahedral shape, these electron pairs are spaced as far apart as possible, resulting in a 109.5-degree bond angle between them. This arrangement is not just aesthetically pleasing; it’s nature’s way of maintaining Electron Social Distancing, keeping repulsive interactions to a minimum and the molecule in a congenial state of equilibrium. Whether it's methane (CH4) or ammonia (NH3), the versatility of the tetrahedral shape underpins a vast array of molecular structures, proving that good geometry isn’t just for mathematicians.

The Essence of VSEPR Theory

Valence Shell Electron Pair Repulsion (VSEPR) theory is like the traffic laws for electrons: it explains how they move around in the space of a molecule. The VSEPR theory posits that because electron pairs repel each other, they will arrange themselves as far apart as possible. This 'personal space' requirement dictates the 3D geometry of molecules.

VSEPR's Role in Predicting Molecular Shapes

This theory is essential for predicting the shapes of molecules. Let's say you have a central atom with a certain number of electron pairs, both bonding (shared with other atoms) and lone (nonbonded). The VSEPR theory helps you figure out where these pairs will go in three-dimensional space to keep their repulsion to a minimum. When applied to a molecule undergoing sp3 hybridization, the VSEPR theory predicts that the molecule will adopt a tetrahedral geometry to keep those electronic