A Sulphur atom in its ground state has the electronic configuration How many orbitals are occupied by at least one electron?

Let's break down the problem and explain the solution in a simple and detailed way. The question asks us to determine how many orbitals are occupied by at least one electron in the ground-state electronic configuration of a sulfur atom.

Step-by-Step Solution:

1. Electronic Configuration of Sulfur:The electronic configuration is: 1s2 2s2 2p6 3s2 3p4.This means electrons are arranged in orbitals starting from the lowest energy to the highest, filling according to the Aufbau principle.
2. Orbital Types and Electron Occupancy:
   • 1s orbital: Holds 2 electrons (fully occupied).
   • 2s orbital: Holds 2 electrons (fully occupied).
   • 2p orbitals: There are 3 2p orbitals (px, py, pz), and they are fully filled with 6 electrons (each orbital has 2 electrons).
   • 3s orbital: Holds 2 electrons (fully occupied).
   • 3p orbitals: There are 3 3p orbitals (px, py, pz). With 4 electrons, two orbitals are fully filled (2 electrons each), and the third orbital has 1 electron.

3. Counting the Orbitals with at Least One Electron:

   • 1s: 1 orbital (occupied).
   • 2s: 1 orbital (occupied).
   • 2p: 3 orbitals (all occupied).
   • 3s: 1 orbital (occupied).
   • 3p: 3 orbitals (all occupied with at least one electron).

   Total number of orbitals occupied by at least one electron = 1 + 1 + 3 + 1 + 3 = 9.

   Answer: The correct answer is 9 orbitals.