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Concept explainers
Interpretation:
Distribution of d-electrons in the complex ion
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.
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 Solutions
OWLv2 with Student Solutions Manual eBook for Ebbing/Gammon's General Chemistry, 11th Edition, [Instant Access], 4 terms (24 months)
- Draw the octahedral crystal field d orbital splitting diagrams for [Fe(OH2)6] 2+ and [Fe(CN)6] 3. Indicate if the diagrams are high spin and low spin. give the names of the d-orbitals (dxz, dxy, dzy, dz2, dx2 - y2) label the appropriate orbital sets eg* and t2g and show how the electrons populate the diagram. (Hint: Pairing energy for 3d orbitals Fe 2+ = 29875 cm-1, Fe 3+ = 19150 cm-1; delta OH for Fe(OH2)6]2+ = 14300 cm-1 and delta OH for [Fe(CN)6]3 - is 35000 cm-1arrow_forward[Co(H2O)6]3+ has how many unpaired electrons? the answer was 4 but I don't know how I get to the answer.arrow_forwardThe self exchange electron-transfer reaction between [Co(en)3]3+ and [Co(en)3]2+ is rather slow. Explain this observation on the basis of d-orbital occupations.arrow_forward
- How many d electrons are present in [Ti(H2O)6]³+?arrow_forwardProvide the name and identify the oxidation state, coordination number, and the molecular geometry of [Fe(H20)6]3+.arrow_forwardPlease predict the number of unpaired electrons in [Ni(CN)4]² and [Fe(CN)6]*, explain your results using crystal field theory.arrow_forward
- Draw the structures of the four geometrical isomers of [Co(NH3)2(en)BrCl]+. Two of these are optically active. Identify these, and draw the structures of their optical isomers.arrow_forwardIn [Cr(NH₃)₆]Cl₃, the [Cr(NH₃)₆]³⁺ ion absorbs visiblelight in the blue-violet range, and the compound is yellow-orange. In [Cr(H₂O)₆]Br₃, the [Cr(H₂O)₆]³⁺ ion absorbs visiblelight in the red range, and the compound is blue-gray. Explain these differences in light absorbed and color of the compoundarrow_forwardExplain the origin of the color of K3[Fe(C2O4)3] ∙3H2O.arrow_forward
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
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