Draw an orbital that has the following quantum numbers: n=3, ℓ=1, mℓ=-1, and ms=-(1)/(2).

Name: Problem 82, Chapter 4: Chemistry
Uploaded: 2021-06-10T15:58:25-08:00
Duration: 1 min 40 s
Channel: Jennifer Hudspeth
Description: Draw an orbital that has the following quantum numbers: n=3, ℓ=1, mℓ=-1, and ms=-(1)/(2).

step 1 Hi there, this is problem number 82. In problem number 82, they give us a set of four quantum nu

Draw an orbital that has the following quantum numbers: n=3,...

Key Concepts

Quantum Numbers

Quantum numbers are a set of numerical values that provide important information about the energy, shape, orientation, and spin of electrons within an atom. They are solutions derived from the Schrödinger equation and are subject to specific rules such as the Pauli exclusion principle and quantum mechanical restrictions.

Principal Quantum Number (n)

The principal quantum number, denoted as n, specifies the main energy level or shell in which an electron resides. It indicates the relative size and energy of the orbital, with higher values of n corresponding to orbitals that are larger and have higher energy.

Angular Momentum Quantum Number (l)

The angular momentum quantum number, represented by l, determines the shape of the electron's orbital. It can take on integer values from 0 up to n-1, with different values corresponding to different orbital types (such as s, p, d, f), each having characteristic shapes.

Magnetic Quantum Number (m_l)

The magnetic quantum number, m_l, defines the orientation of the orbital in space relative to an external magnetic field. Its range of values from -l to +l indicates the number of possible orientations for a given orbital type within a subshell.

Spin Quantum Number (m_s)

The spin quantum number, m_s, describes the intrinsic spin of the electron, which can take one of two values: +1/2 or -1/2. This quantum number accounts for the electron's magnetic properties and is essential for understanding electron pairing and the Pauli exclusion principle.

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