Quantum Numbers and Atomic Orbitals

The video tutorial covers questions on atomic orbitals and quantum numbers, including electron accommodation in p orbitals, the relationship between the principal quantum number and orbital size, determining quantum numbers for rubidium's valence electron, and identifying impossible quantum number sets. The tutorial emphasizes the Pauli exclusion principle and the characteristics of different orbitals.

What is the main focus of the quiz questions discussed in the video?

• Chemical bonding and reactions

• Molecular geometry

• Periodic table trends

• Atomic orbitals and quantum numbers

How many electrons can a p orbital accommodate?

• 6

• 4

• 2

• 1

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

• Hund's Rule

• Pauli Exclusion Principle

• Aufbau Principle

• Heisenberg Uncertainty Principle

What does the principal quantum number (n) primarily relate to?

• Size of the orbital

• Spin of the electron

• Shape of the orbital

• Energy of the electron

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

• It remains the same

• It increases

• It becomes unpredictable

• It decreases

For rubidium's valence electron, what is the principal quantum number (n)?

• 5

• 6

• 4

• 3

What is the value of the azimuthal quantum number (l) for an s orbital?

• 0

• 1

• 2

• 3

Which of the following sets of quantum numbers is not possible?

• n=5, l=3, m_l=2, m_s=-1/2

• n=4, l=0, m_l=0, m_s=+1/2

• n=3, l=2, m_l=-3, m_s=+1/2

• n=3, l=2, m_l=-2, m_s=+1/2

What is the valid range of m_l for a d orbital?

• -3 to +3

• -2 to +2

• -1 to +1

• 0 to +4

Which quantum number determines the orientation of an orbital?

• Spin quantum number (m_s)

• Magnetic quantum number (m_l)

• Azimuthal quantum number (l)

• Principal quantum number (n)