If an electron has quantum numbers n=2, l=0, and m_l=0, which orbital does it oc
Practice Questions
Q1
If an electron has quantum numbers n=2, l=0, and m_l=0, which orbital does it occupy?
2s
2p
1s
3s
Questions & Step-by-Step Solutions
If an electron has quantum numbers n=2, l=0, and m_l=0, which orbital does it occupy?
Correct Answer: 2s orbital
Step 1: Identify the quantum numbers given: n=2, l=0, m_l=0.
Step 2: Understand what each quantum number represents: n is the principal quantum number, l is the azimuthal quantum number, and m_l is the magnetic quantum number.
Step 3: Determine the type of orbital based on the value of l: l=0 corresponds to an s orbital.
Step 4: Determine the principal energy level based on n: n=2 indicates the second energy level.
Step 5: Combine the information: Since l=0 (s orbital) and n=2, the electron occupies the 2s orbital.
Quantum Numbers – Quantum numbers (n, l, m_l) define the energy level, shape, and orientation of an electron's orbital.
Orbital Types – The value of l determines the type of orbital: l=0 corresponds to s orbitals, l=1 to p orbitals, etc.
