If an electron has the quantum numbers n=3, l=1, what is the possible range of m
Practice Questions
Q1
If an electron has the quantum numbers n=3, l=1, what is the possible range of m_l?
-1, 0, +1
0, +1, +2
-2, -1, 0
-1, 0, +1, +2
Questions & Step-by-Step Solutions
If an electron has the quantum numbers n=3, l=1, what is the possible range of m_l?
Step 1: Understand what quantum numbers are. Quantum numbers describe the properties of electrons in an atom.
Step 2: Identify the given quantum numbers. Here, n=3 and l=1.
Step 3: Know what 'l' represents. The quantum number 'l' is called the azimuthal quantum number and it can take values from 0 to (n-1).
Step 4: Determine the possible values of 'm_l'. The magnetic quantum number 'm_l' can take values from -l to +l, including zero.
Step 5: Since l=1, the possible values for m_l are -1, 0, and +1.
Quantum Numbers – Quantum numbers describe the properties of atomic orbitals and the electrons in those orbitals. The principal quantum number (n) indicates the energy level, the azimuthal quantum number (l) indicates the subshell, and the magnetic quantum number (m_l) indicates the orientation of the orbital.
Magnetic Quantum Number (m_l) – The magnetic quantum number (m_l) can take integer values ranging from -l to +l, including zero. This means for a given l, m_l has a total of (2l + 1) possible values.
