The subshell that arises after \(f\) is called the \(g\) subshell. How many electrons may occupy the \(g\) subshell? (a) 9 (b) 7 (c) 5 (d) 18

In the context of atomic structure, quantum numbers play a vital role in determining the position and energy of electrons within an atom. The four quantum numbers are the principal (), azimuthal (), magnetic (), and spin () quantum numbers. The principal quantum number, , defines the energy level and size of the orbital. The azimuthal quantum number, , also known as the angular momentum quantum number, determines the shape of an orbital and is integral in identifying subshells such as s, p, d, f, and g. For instance, in our exercise, for the g subshell was determined to be 4. The magnetic quantum number, , specifies the orientation of an orbital in space, while the spin quantum number, , is related to the spin direction of the electron.To grasp the concept properly, think of the atom as a tiny city, where the quantum numbers are like addresses guiding you to find the exact location (orbital) of an electron within the city (atom). Just as a city's address system helps you find a particular house, the quantum numbers help you pinpoint the exact electron's location.

The electron configuration is a fundamental concept in chemistry, especially when preparing for exams like the JEE. It refers to the distribution of electrons in an atom's orbitals based on increasing energy levels. To understand electron configurations, one must be familiar with Aufbau's principle, Hund's rule, and Pauli's exclusion principle.Aufbau's principle suggests that electrons occupy orbitals starting from the lowest energy level, moving to higher levels subsequently. Hund's rule states that electrons will fill an orbital singly before pairing up, and Pauli's exclusion principle says that no two electrons in an atom can have the same set of four quantum numbers.When applying these rules, students can systematically determine the arrangement of electrons, such as knowing the electron capacity of the g subshell to be 18, as in our example. This systematic knowledge is crucial for students preparing for competitive exams like JEE where conceptual clarity can greatly enhance their problem-solving speed and accuracy.

Chemistry for JEE requires a deep understanding of concepts like atomic structure, bonding, and periodicity. Students must not only memorize facts but also comprehend the principles governing chemical behavior. The electron capacity of subshells, as highlighted in the exercise, is one such concept that forms the basis for more advanced topics in physical and inorganic chemistry.For JEE aspirants, questions often delve into the nuances of electron configurations and the rules that govern them. It's essential to integrate these concepts with problem-solving practices, ensuring a robust preparation. Indeed, a clear understanding of how many electrons a 'g' subshell can hold, appended by the capacity to apply this knowledge to predict chemical properties of elements, can distinguish top scorers on the JEE. When studying for JEE, always aim to build a strong conceptual foundation, something as foundational yet critical as knowing that a g subshell can hold 18 electrons, which can later help in predictions about atomic behavior in reactions and bonding.