IIT/JEE Chemistry Practice #13: Atomic Orbitals/Quantum Numbers

Dave explains atomic orbitals and quantum numbers through a series of questions. He covers the electron capacity of orbitals, the principal quantum number's relation to orbital size, and the correct quantum numbers for rubidium's valence electron. The video concludes with identifying impossible quantum number sets.

What is the maximum number of electrons that any orbital can accommodate?

• 1

• 3

• 2

• 4

Which principle states that no two electrons in an atom can have the same set of quantum numbers?

• Aufbau Principle

• Hund's Rule

• Pauli Exclusion Principle

• Heisenberg Uncertainty Principle

The principal quantum number is primarily related to which aspect of an orbital?

• Size

• Spin

• Orientation

• Shape

As the principal quantum number increases, what happens to the size of the orbital?

• It decreases

• It becomes unpredictable

• It remains the same

• It increases

For rubidium (Z = 37), what is the correct set of quantum numbers for its valence electron?

• n=5, l=2, m_l=0, m_s=+1/2

• n=5, l=1, m_l=0, m_s=+1/2

• n=5, l=0, m_l=0, m_s=+1/2

• n=6, l=0, m_l=0, m_s=+1/2

Which set of quantum numbers represents an impossible arrangement?

• n=3, l=2, m_l=-2, m_s=+1/2

• n=4, l=3, m_l=0, m_s=+1/2

• n=3, l=2, m_l=-3, m_s=+1/2

• n=5, l=3, m_l=2, m_s=+1/2

What is the correct value of the magnetic quantum number (m_l) for an s orbital?

• 0

• 2

• 1

• -1