Chapter 2, Problem 2.47P

(a)

Interpretation Introduction

Interpretation: The number of orbital present in one set g-orbital should be determined.

Concept introduction: The electrons that are present in an outermost orbital are known as valence electrons whereas those present in the orbitals with lower quantum numbers are termed as core electrons. Electrons are filled within orbitals by following three rules: Aufbau principle, Hund’s rule, and Pauli’s exclusion principle. Aufbau principle states, electrons are filled in the orbitals from lower to higher energy level as follows:

  $1s<2s<2p<3s<3p<4s<3d<4p<5s<4d<5p<6s<4f<5d<6p<7s$

Hund’s rule states, initially each orbital is singly occupied and then pairing occurs and Pauli’s exclusion principle states, spin of two different electrons in one orbital is always different.

(b)

Interpretation Introduction

Interpretation: The angular nodes of g-orbital should be explained.

Concept introduction: The electrons that are present in an outermost orbital are known as valence electrons whereas those present in the orbitals with lower quantum numbers are termed as core electrons. Electrons are filled within orbitals by following three rules: Aufbau principle, Hund’s rule, and Pauli’s exclusion principle. Aufbau principle states, electrons are filled in the orbitals from lower to higher energy level as follows:

  $1s<2s<2p<3s<3p<4s<3d<4p<5s<4d<5p<6s<4f<5d<6p<7s$

Hund’s rule states, initially each orbital is singly occupied and then pairing occurs and Pauli’s exclusion principle states, spin of two different electrons in one orbital is always different.

(c)

Interpretation Introduction

Interpretation: The relation between principal quantum number and radial nodes should be explained.

Concept introduction: The electrons that are present in an outermost orbital are known as valence electrons whereas those present in the orbitals with lower quantum numbers are termed as core electrons. Electrons are filled within orbitals by following three rules: Aufbau principle, Hund’s rule, and Pauli’s exclusion principle. Aufbau principle states, electrons are filled in the orbitals from lower to higher energy level as follows:

  $1s<2s<2p<3s<3p<4s<3d<4p<5s<4d<5p<6s<4f<5d<6p<7s$

Hund’s rule states, initially each orbital is singly occupied and then pairing occurs and Pauli’s exclusion principle states, spin of two different electrons in one orbital is always different.