ELECTRONIC CONFIGURATION (CHEMISTRY DK014)

Which quantum number defines the orientation of orbital?

• s

• l

• m

• n

Which principle states that electrons fill the orbitals of lower energy level first?

• aufbau

• Hund

• Pauli

• Paschen

Which set of quantum numbers uniquely defines one of the electrons in an atomic orbital with n = 2 and l = 0.

• (2,0,+1,+1)

• (2,0,+1,+1/2)

• (2,0,0,+1)

• (2,0,0,+1/2)

Which of the following sub-shells contains only one orbital?

• 4d

• 6p

• 7s

• 5d

Pauli’s exclusion principle describe that

• An atomic orbital can only hold a maximum of 2 electrons, each with opposite spins

• An atomic orbital can only hold a maximum of 6 electrons, each of the same spin

• An atomic orbital can hold a minimum of 6 electrons, each with opposite spins

• An atomic orbital can hold a minimum 2 electrons, each with opposite spins.

What is the maximum number of electrons in the third shell of an atom?

• 2

• 18

• 8

• 32

Which of the following orbitals are spherically symmetrical?

• s

• p

• d

• f

What is the value of azimuthal quantum number, l for d orbital?

• 0

• 1

• 2

• 3

Which of the rule is being ignored in the orbital diagram shown above.

• aufbau principle

• The Pauli's exclusion principle

• Hund's rule

• The Heisenberg uncertainty principle

The magnetic quantum number (m) refers to

• Orientation of orbital

• Direction of electron spin

• Shape of orbital

• Energy level of the electron