Distribution of d-electrons in the complex ion [ N i ( H 2 O ) 6 ] 2 + has to be determined. Concept Introduction: The term Crystal field splitting refers to segregation of d-orbitals in to higher energy orbitals and lower energy orbitals when ligands approaches metal ion to co-ordinate. Crystal field splitting is said to be larger when the energy gap between higher energy d-orbitals and lower energy d-orbitals is larger. Crystal field splitting is said to be smaller when the energy gap between higher energy d-orbitals and lower energy d-orbitals is smaller. Spectrochemical series refers to the arrangement of ligands with respect to crystal field splitting they cause in the d-orbitals of a metal ion. The ligand that causes larger splitting pattern is referred to as stronger ligand. The ligands are arranged in increasing order of crystal field splitting they produce. I − < B r − < S 2 − < S C N − < C l − < N O 3 − < N 3 − < F − < O H − < C 2 O 4 2 − < H 2 O < N C S − < C H 3 C N < p y < N H 3 < e n < b i p y < p h e n < N O 2 − < P P h 3 < C N − < C O The ligand that causes larger crystal field splitting is strong ligand and the ligand that causes smaller splitting is termed as weak ligand. Pairing energy refers to the energy required to pair the electrons - that is energy required to make two electrons to be paired in same orbital with opposite spins. If the pairing energy of a complex is high it means the electrons are difficult to be paired and so the complex will be high spin complex with unpaired electrons. If the pairing energy of a complex is low it means the electrons are readily paired and so the complex will be low spin complex with paired electrons. A complex with high splitting energy will have low pairing energy because high splitting energy indicates larger energy gap between lower and higher energy levels that the electrons need lesser energy to be paired and they tend to remain paired in lower energy orbitals. A complex with low splitting energy will have high pairing energy because low splitting energy indicates smaller energy gap between lower and higher energy levels that the electrons disperse among orbitals more randomly and they need higher energy to be paired.

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Chapter 22.7, Problem 22.5E

Interpretation Introduction

Interpretation:

Distribution of d-electrons in the complex ion [Ni(H2O)6]2+ has to be determined.

Concept Introduction:

The term Crystal field splitting refers to segregation of d-orbitals in to higher energy orbitals and lower energy orbitals when ligands approaches metal ion to co-ordinate. Crystal field splitting is said to be larger when the energy gap between higher energy d-orbitals and lower energy d-orbitals is larger. Crystal field splitting is said to be smaller when the energy gap between higher energy d-orbitals and lower energy d-orbitals is smaller.

Spectrochemical series refers to the arrangement of ligands with respect to crystal field splitting they cause in the d-orbitals of a metal ion. The ligand that causes larger splitting pattern is referred to as stronger ligand.

The ligands are arranged in increasing order of crystal field splitting they produce.

I−<Br−<S2−<SCN−<Cl−<NO3−<N3−<F−<OH−<C2O42−<H2O<NCS−<CH3CN<py<NH3<en<bipy<phen<NO2−<PPh3<CN−<CO

The ligand that causes larger crystal field splitting is strong ligand and the ligand that causes smaller splitting is termed as weak ligand.

Pairing energy refers to the energy required to pair the electrons - that is energy required to make two electrons to be paired in same orbital with opposite spins.

If the pairing energy of a complex is high it means the electrons are difficult to be paired and so the complex will be high spin complex with unpaired electrons. If the pairing energy of a complex is low it means the electrons are readily paired and so the complex will be low spin complex with paired electrons.

A complex with high splitting energy will have low pairing energy because high splitting energy indicates larger energy gap between lower and higher energy levels that the electrons need lesser energy to be paired and they tend to remain paired in lower energy orbitals. A complex with low splitting energy will have high pairing energy because low splitting energy indicates smaller energy gap between lower and higher energy levels that the electrons disperse among orbitals more randomly and they need higher energy to be paired.

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