Question

"The orbitals of two different shells of an atom combine and form one hybrid orbital." State whether the statement is true or false and justify your answer.

Short answer

Justify your answer. Answer: The statement is false. Hybridization involves the mixing of orbitals within the same shell, not between different shells, because orbitals in different shells have significantly different energies.

Step-by-step solution

Understanding hybrid orbitals

Hybrid orbitals are formed when atomic orbitals of an atom mix together to create new, equivalent orbitals that are used for bonding. This occurs in order to minimize the energy of the system and maximize stability, particularly when atoms bond together to form molecules. Hybrid orbitals typically involve mixing orbitals that belong to the same shell, such as s and p orbitals, which have similar energies.

Evaluate the given statement

The statement claims that orbitals of two different shells combine to form one hybrid orbital. In a hybridization process, the mixing of orbitals typically occurs within the same energy level (shell) to create new, equivalent orbitals. Orbitals from different energy levels (shells) have vastly different energies, making it energetically unfavorable for them to combine.

Conclude and justify

Based on our understanding of hybrid orbitals, the statement "The orbitals of two different shells of an atom combine and form one hybrid orbital" is false. Hybridization involves the mixing of orbitals within the same shell, not between different shells because orbitals in different shells have significantly different energies.

Key concepts

Chemical Bonding

Chemical bonding is the process by which atoms join together to form compounds. Atoms bond with each other by either sharing or transferring electrons, which leads to the stability of the resultant molecule. There are three primary types of chemical bonds: ionic, covalent, and metallic. Ionic bonds occur when electrons are transferred from one atom to another, resulting in a positive ion (cation) and a negative ion (anion). Covalent bonds form when atoms share electrons to achieve a full outer electron shell, which can occur either equally in non-polar covalent bonds or unequally in polar covalent bonds. In metallic bonds, electrons are shared among a lattice of metal ions, with electrons free to move, which explains the conductivity of metals.

Understanding the concept of bonding is essential, as it underpins the structure and properties of every material we encounter. The strength, flexibility, and even the electric conductivity of materials are determined by the type of chemical bonds that hold atoms together in the material's structure.

Atomic Orbitals

Atomic orbitals are regions around an atom's nucleus where the probability of finding an electron is highest. Historically, these orbitals are described by quantum numbers that define their shape (spherical, dumbbell, etc.) and energy levels. The most commonly discussed orbitals are designated as s, p, d, and f. Each orbital can hold a specific maximum number of electrons: s can hold 2, p can hold 6, d can hold 10, and f can hold 14.

It is important to realize that atomic orbitals are not static; instead, they describe the behavior of electrons in terms of probability, with different shapes representing areas where an electron is likely to be found. Understanding orbitals helps us understand why atoms bond the way they do and the resulting molecular geometry. Hybridization, in the context of chemistry, is a direct extension of the concept of atomic orbitals and is critical in explaining the shapes of molecules.

Hybridization Process

The hybridization process is a refinement that explains how atoms bond in molecules with specific geometries. It involves the mathematical combination or 'mixing' of standard atomic orbitals (such as s, p, d, and f orbitals) to form new orbitals called hybrid orbitals. These hybrid orbitals have different shapes and energies than the original atomic orbitals and are better suited for forming bonds. For example, sp3 hybridization involves mixing one s orbital and three p orbitals to form four equivalent sp3 hybrid orbitals, each of which is capable of forming a sigma bond.

Hybridization is essential in predicting the three-dimensional structure of molecules, which is critical for understanding their chemical reactivity and physical properties. However, it is important to note that hybridization occurs within the same energy level or shell, and orbitals from different shells with significant energy differences do not hybridize. Hybrid orbitals are merely an explanatory tool and not a physical process; yet, this concept helps accommodate the observed bond angles and molecular shapes that differ from those predicted by non-hybridized orbitals.