The subshell that arises after \(f\) subshell is called \(g\) subshell. What is the total number of orbitals in the shell in which the \(g\) subshell first occur? (a) 9 (b) 16 (c) 25 (d) 36

The subshell and orbitals concept lies at the heart of understanding electron distribution in atoms. A subshell is a division within an electron shell that represents the distribution of electrons based on a set of quantum numbers. We label these subshells with letters: 's', 'p', 'd', 'f', 'g', and so forth, where 'g' is less commonly discussed as it involves elements not yet found or synthesized.

Each subshell comprises a specific number of orbitals, which are regions of space where there is a high probability of finding an electron. The 's' subshell has one orbital, the 'p' subshell has three, 'd' has five, and 'f' has seven. Following this pattern, the 'g' subshell contains nine orbitals. The significance of these subshells is profound, as they directly inform the electron configuration of an atom, which in turn affects the atom's chemical properties and reactivity.

The principal quantum number, symbolized as 'n', is critical in the organization of electrons within an atom. It primarily indicates the relative size and energy level of an orbital, where a higher 'n' value suggests a larger orbital with a higher energy state. The value of 'n' starts at 1 and increases with the energy levels of the electrons. This number not only determines the overall energy level of the orbital but also the maximum number of electrons that can inhabit a specific shell, given by the formula 2n².

When determining the position of the 'g' subshell, which arises after 'f', we consider the principal quantum number corresponding to the shell where 'g' appears for the first time—this happens to be when 'n' equals 5. Knowing the principal quantum number allows us to predict the electron configuration of elements, which is a foundation in studying chemical properties and reactions in physical chemistry, especially for exams like JEE.

Understanding electron configuration is essential for delving into the depths of atom interaction and chemistry. The electron configuration provides a detailed description of how electrons are distributed among the different orbitals and subshells of an atom. This information is crucial when predicting the chemical behavior of an element.

The configuration follows a set of principles like the Pauli Exclusion Principle, which states that each orbital can hold a maximum of two electrons with opposite spins, and Hund's rule, which prescribes the distribution of electrons across orbitals of the same subshell. Furthermore, the Aufbau principle suggests that lower-energy orbitals are filled before higher-energy ones. For example, the electron configuration of a 'g' subshell element, which would theoretically contain electrons in the fifth shell, could be predicted by applying these principles and recognizing the sequence in which electrons fill various subshells within the given energy level.

In the context of physical chemistry for JEE, understanding subshells and orbitals becomes critically important. JEE, or the Joint Entrance Examination, is a highly competitive exam for aspiring engineers in India. The physical chemistry portion assesses a student's understanding of atomic structure, amongst other topics.

For success in this exam, one must be adept at applying concepts such as electron configurations and quantum numbers to solve problems. For instance, questions may require determining the total number of orbitals within a given shell, or the specific type of subshell in which electrons would reside in a notional element. Mastery of these topics not only aids in solving direct questions but also equips students with the foundational knowledge required for understanding more complex chemical phenomena, which could be a deciding factor in their performance on the JEE.