Quantum Numbers

What is the correct representation for an orbital which has an "n" value of 4 and an "L" value of 2?

• 4d

• 4s

• 4f

• 4p

Which orbital shows a violation of the Pauli Exclusion Principle?

• A

• B

• C

• D

Tags

NGSS.HS-PS1-1

This is a ____ orbital

• s

• d

• p

• d

Tags

NGSS.HS-PS1-1

Orbital sublevels, or L, represents:

• orbital color

• orbital shape

• electron spin

• energy level

Which quantum number determines the energy level of an electron in an atom?

• Principal quantum number (n)
  

• Azimuthal quantum number (l)
  

• Magnetic quantum number (mₗ)
  

• Spin quantum number (mₛ)

The spin quantum number (mₛ) can have which of the following values?

• -1 or +1
  

• 0 or 1
  

• +1/2​ or −1/2

• 1 or -1

Which quantum number cannot be 0?

• Principal quantum number (n)
  

• Azimuthal quantum number (l)
  

• Magnetic quantum number (mₗ)
  

• Spin quantum number (mₛ)

Which set of quantum numbers is incorrect for an electron?

• n= 3, l=1, m_l= −1,

  m_s= +1/2

• n= 2, l= 1, m_l =1,

  m_s= −1/2

• n=1, l=0, m_l=0, m_s=+1/2

• n=2, l=2, m_l=0, m_s=−1/2

How many possible values of mₗ are there for an electron in the p-orbital?

• 1
  

• 2

• 3

• 4

Which quantum number is associated with the shape of an electron's orbital?

• Principal quantum number (n)

• Azimuthal quantum number (l)

• Magnetic quantum number (mₗ)

• Spin quantum number (mₛ)