Given the subshells 1s, 2s, 2p, 3s, 3p and 3d, identify those that meet the following descriptions. (a) Has l = 2

Verified step by step guidance

1. Step 1: Understand that in quantum mechanics, the quantum number 'l' represents the angular momentum of an electron in an atom. This quantum number also determines the shape of the orbital where the electron is likely to be found.
2. Step 2: The value of 'l' can range from 0 to (n-1), where 'n' is the principal quantum number. The values of 'l' are often represented by letters: l=0 is 's', l=1 is 'p', l=2 is 'd', and l=3 is 'f'.
3. Step 3: In this problem, we are asked to identify the subshells that have l=2. From the information in step 2, we know that l=2 corresponds to 'd' orbitals.
4. Step 4: Looking at the given subshells, we can see that the only subshell that meets the description of having l=2 is the 3d subshell.

Key Concepts

Quantum Numbers

Quantum numbers are a set of numerical values that describe the unique quantum state of an electron in an atom. The principal quantum number (n) indicates the energy level, while the azimuthal quantum number (l) defines the shape of the orbital. Each subshell corresponds to a specific value of l, which can range from 0 to n-1.

Subshells and Orbital Shapes

Subshells are divisions of electron shells that contain orbitals of the same energy level. Each subshell is characterized by a specific l value: s (l=0), p (l=1), d (l=2), and f (l=3). The shape of the orbitals varies with l, where d orbitals (l=2) have a more complex shape compared to s and p orbitals.

Identification of Subshells

To identify subshells based on their angular momentum quantum number (l), one must match the l value to the corresponding subshell type. For instance, a subshell with l=2 corresponds to the d subshell. In the given question, the only subshell that meets the criterion of l=2 is the 3d subshell.