Chapter 8.4, Problem 8.6AFP

(a)

Interpretation Introduction

Interpretation:

The condensed electronic configuration of ${\text{V}}^{3+}\left(\text{Z}=23\right)$ is to be determined. Also whether ${\text{V}}^{3+}$ is paramagnetic or not is to be determined.

Concept introduction:

The electronic configuration of an element tells about the distribution of electrons in the atomic orbitals. It is used to predict the physical, chemical, electrical and magnetic properties of the substance.

The condensed electronic configuration is a short way to write the configuration of elements in terms of the nearest noble gas configuration.

The electrons are filled up in accordance with three rules:

1. Aufbau principle which states that the electrons are filled up in the increasing order of their orbitals which follows as: $1s2s2p3s3p4s\text{}3d$.

2. Hund’s rule which states that the pairing of electrons will not start until each of the orbitals is singly occupied.

3. Pauli’s exclusion principle states that no two electrons can have the same value of all the four quantum numbers.

A species containing an unpaired number of electrons is said to be paramagnetic species and the species containing only paired electrons is said to be diamagnetic species.

(b)

Interpretation Introduction

Interpretation:

The condensed electronic configuration of ${\text{Ni}}^{2+}\left(\text{Z}=28\right)$ is to be determined. Also whether ${\text{Ni}}^{2+}$ is paramagnetic or not is to be determined.

Concept introduction:

The electronic configuration of an element tells about the distribution of electrons in the atomic orbitals. It is used to predict the physical, chemical, electrical and magnetic properties of the substance.

The condensed electronic configuration is a short way to write the configuration of elements in terms of the nearest noble gas configuration.

The electrons are filled up in accordance with three rules:

1. Aufbau principle which states that the electrons are filled up in the increasing order of their orbitals which follows as: $1s2s2p3s3p4s\text{}3d$.

2. Hund’s rule which states that the pairing of electrons will not start until each of the orbitals is singly occupied.

3. Pauli’s exclusion principle states that no two electrons can have the same value of all the four quantum numbers.

A species containing an unpaired number of electrons is said to be paramagnetic species and the species containing only paired electrons is said to be diamagnetic species.

(c)

Interpretation Introduction

Interpretation:

The condensed electronic configuration of ${\text{La}}^{3+}\left(\text{Z}=57\right)$ is to be determined. Also whether ${\text{La}}^{3+}$  is paramagnetic or not is to be determined.

Concept introduction:

The electronic configuration of an element tells about the distribution of electrons in the atomic orbitals. It is used to predict the physical, chemical, electrical and magnetic properties of the substance.

The condensed electronic configuration is a short way to write the configuration of elements in terms of the nearest noble gas configuration.

The electrons are filled up in accordance with three rules:

1. Aufbau principle which states that the electrons are filled up in the increasing order of their orbitals which follows as: $1s2s2p3s3p4s\text{}3d$.

2. Hund’s rule which states that the pairing of electrons will not start until each of the orbitals is singly occupied.

3. Pauli’s exclusion principle states that no two electrons can have the same value of all the four quantum numbers.

A species containing an unpaired number of electrons is said to be paramagnetic species and the species containing only paired electrons is said to be diamagnetic species.