Chapter 20, Problem 20.34SP

(a)

Interpretation Introduction

Interpretation:

The number of unpaired electrons in ${\text{Cu}}^{\text{2+}}$ has to be given.

Concept introduction:

Coordination compounds: The compounds having coordination covalent bonds which form when metal ions react with polar molecules or anions.

Electronic configuration shows the electrons distribution of atoms or molecule in its molecular or atomic orbitals. The electrons are distributed in orbitals by following three important rules, Aufbau's Principle, Pauli-exclusion principle, and Hund's Rule.

If the complex has minimum one unpaired electron, then they are paramagnetic and are attracted towards the magnetic field. If all the electrons are paired in a complex, then they are diamagnetic and are repelled from the magnetic field.

The order of orbitals in their increasing energy is given by

$\begin{array}{l}1s\text{<}2s\text{<}2p\text{<}3s\text{<}3p\text{<}4s\text{<}3d\text{<}4p\text{<}5s\text{<}4d\text{<}5p\text{<}6s\text{<}4f\text{<}5d\text{<}6p\\ \text{<}7s\text{<}5f\text{<}6d\text{<}7p\end{array}$

(b)

Interpretation Introduction

Interpretation:

The number of unpaired electrons in ${\text{Ti}}^{\text{+2}}$ has to be given.

Concept introduction:

Coordination compounds: The compounds having coordination covalent bonds which form when metal ions react with polar molecules or anions.

Electronic configuration shows the electrons distribution of atoms or molecule in its molecular or atomic orbitals. The electrons are distributed in orbitals by following three important rules, Aufbau's Principle, Pauli-exclusion principle, and Hund's Rule.

If the complex has minimum one unpaired electron, then they are paramagnetic and are attracted towards the magnetic field. If all the electrons are paired in a complex, then they are diamagnetic and are repelled from the magnetic field.

The order of orbitals in their increasing energy is given by

$\begin{array}{l}1s\text{<}2s\text{<}2p\text{<}3s\text{<}3p\text{<}4s\text{<}3d\text{<}4p\text{<}5s\text{<}4d\text{<}5p\text{<}6s\text{<}4f\text{<}5d\text{<}6p\\ \text{<}7s\text{<}5f\text{<}6d\text{<}7p\end{array}$

(c)

Interpretation Introduction

Interpretation:

The number of unpaired electrons in ${\text{Zn}}^{\text{2+}}$ has to be given.

Concept introduction:

Coordination compounds: The compounds having coordination covalent bonds which form when metal ions react with polar molecules or anions.

Electronic configuration shows the electrons distribution of atoms or molecule in its molecular or atomic orbitals. The electrons are distributed in orbitals by following three important rules, Aufbau's Principle, Pauli-exclusion principle, and Hund's Rule.

If the complex has minimum one unpaired electron, then they are paramagnetic and are attracted towards the magnetic field. If all the electrons are paired in a complex, then they are diamagnetic and are repelled from the magnetic field.

The order of orbitals in their increasing energy is given by

$\begin{array}{l}1s\text{<}2s\text{<}2p\text{<}3s\text{<}3p\text{<}4s\text{<}3d\text{<}4p\text{<}5s\text{<}4d\text{<}5p\text{<}6s\text{<}4f\text{<}5d\text{<}6p\\ \text{<}7s\text{<}5f\text{<}6d\text{<}7p\end{array}$

(d)

Interpretation Introduction

Interpretation:

The number of unpaired electrons in ${\text{Cr}}^{\text{3+}}$ has to be given.

Concept introduction:

Coordination compounds: The compounds having coordination covalent bonds which form when metal ions react with polar molecules or anions.

Electronic configuration shows the electrons distribution of atoms or molecule in its molecular or atomic orbitals. The electrons are distributed in orbitals by following three important rules, Aufbau's Principle, Pauli-exclusion principle, and Hund's Rule.

If the complex has minimum one unpaired electron, then they are paramagnetic and are attracted towards the magnetic field. If all the electrons are paired in a complex, then they are diamagnetic and are repelled from the magnetic field.

The order of orbitals in their increasing energy is given by

$\begin{array}{l}1s\text{<}2s\text{<}2p\text{<}3s\text{<}3p\text{<}4s\text{<}3d\text{<}4p\text{<}5s\text{<}4d\text{<}5p\text{<}6s\text{<}4f\text{<}5d\text{<}6p\\ \text{<}7s\text{<}5f\text{<}6d\text{<}7p\end{array}$