Given the quantum numbers n = 2, l = 1, ml = 0, ms = +½ determine the neutral element.
The correct answer and explanation is:
The given quantum numbers n=2n = 2, l=1l = 1, ml=0m_l = 0, and ms=+12m_s = +\frac{1}{2} describe an electron in a specific energy state of an atom. Here’s a breakdown of each quantum number:
- Principal Quantum Number (n = 2): This represents the energy level or shell in which the electron resides. For n=2n = 2, the electron is in the second energy level.
- Azimuthal Quantum Number (l = 1): This number defines the orbital shape. For l=1l = 1, the electron is in a p orbital. P orbitals have a dumbbell shape and are found in the second and higher energy levels.
- Magnetic Quantum Number (m_l = 0): This specifies the orientation of the orbital within a given subshell. For ml=0m_l = 0, the electron is in a p orbital oriented along the axis (or the ml=0m_l = 0 orientation of the p orbital).
- Spin Quantum Number (m_s = +½): This indicates the direction of the electron’s spin. A value of +12+\frac{1}{2} means the electron is spinning in the “up” direction.
Neutral Element:
Given the quantum numbers, this corresponds to an electron in the second energy level (n = 2), specifically in a p orbital (l = 1), and with spin up (m_s = +½). This would be the first electron in the p orbital of the second energy level. Therefore, this electron belongs to the element boron (B), which has the electron configuration 1s22s22p11s^2 2s^2 2p^1. Boron is a neutral element in its ground state, as it has no charge, and the total number of protons equals the total number of electrons (5 protons and 5 electrons).
Thus, the correct neutral element corresponding to these quantum numbers is Boron (B).