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Concept explainers
a)
Interpretation:
The crystal field energy level diagrams for
Concept Introduction:
Coordination compounds: The compounds having coordination covalent bonds which form when metal ions react with polar molecules or anions.
Ligands: The ions or molecules that forms coordination covalent bond with metal ions in a coordination compound. Ligands should have minimum one lone pair of electron, where it donates two electrons to the metal. Metal atom accepts the electron pair from a ligand forming a coordination bond.
The strong-field ligands results in pairing of electrons present in the complex and leads to diamagnetic species , while the low-field ligand do not have tendency to pair up the electrons therefore forms paramagnetic species.
Ligand field theory: It is used to explain the bonding between metal and ligand in a coordination complex. Ligand field theory is explained in terms of electrostatic interaction of between metal ion and ligands.
The five d orbitals get divided into two sets that are
b)
Interpretation:
The crystal field energy level diagrams for
Concept Introduction:
Coordination compounds: The compounds having coordination covalent bonds which form when metal ions react with polar molecules or anions.
Ligands: The ions or molecules that forms coordination covalent bond with metal ions in a coordination compound. Ligands should have minimum one lone pair of electron, where it donates two electrons to the metal. Metal atom accepts the electron pair from a ligand forming a coordination bond.
The strong-field ligands results in pairing of electrons present in the complex and leads to diamagnetic species , while the low-field ligand do not have tendency to pair up the electrons therefore forms paramagnetic species.
Ligand field theory: It is used to explain the bonding between metal and ligand in a coordination complex. Ligand field theory is explained in terms of electrostatic interaction of between metal ion and ligands.
The five d orbitals get divided into two sets that are
c)
Interpretation:
The crystal field energy level diagrams for
Concept Introduction:
Coordination compounds: The compounds having coordination covalent bonds which form when metal ions react with polar molecules or anions.
Ligands: The ions or molecules that forms coordination covalent bond with metal ions in a coordination compound. Ligands should have minimum one lone pair of electron, where it donates two electrons to the metal. Metal atom accepts the electron pair from a ligand forming a coordination bond.
The strong-field ligands results in pairing of electrons present in the complex and leads to diamagnetic species , while the low-field ligand do not have tendency to pair up the electrons therefore forms paramagnetic species.
Ligand field theory: It is used to explain the bonding between metal and ligand in a coordination complex. Ligand field theory is explained in terms of electrostatic interaction of between metal ion and ligands.
The strong field ligands lead to splitting to a higher extent than the weak field ligands and the wavelength of light absorbed depends on the energy gap that is produced by a particular ligand.
The five d orbitals get divided into two sets that are
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Chapter 20 Solutions
General Chemistry: Atoms First
- Four different octahedral chromium coordination compounds exist that all have the same oxidation state for chromium and have H2O and Cl as the ligands and counterions. When 1 mole of each of the four compounds is dissolved in water, how many moles of silver chloride will precipitate upon addition of excess AgNO3?arrow_forwardPlatinum(II) forms many complexes, among them those with the following ligands. Give the formula and charge of each complex. (a) two ammonia molecules and one oxalate ion (C2O42-) (b) two ammonia molecules, one thiocyanate ion (SCN-), and one bromide ion (c) one ethylenediamine molecule and two nitrite ionsarrow_forwardDraw the energy diagram for d-orbital electron configuration in the octahedral field for each of the following complex ions. Indicate whether the ion is paramagnetic or diamagnetic: (a) [Cr(H2O)6]3+ (H2O is a weak-field ligand) (b) [Cr(NH3)6]3+ (NH3 is a strong-field ligand) (c) [CoF6]3– (F– is a weak-field ligand) (d) [Co(CN)6]3– (CN– is a strong-field ligand) (e) [Ni(H2O)6]2+ (H2O is a weak-field ligand) (f) [Ni(en)3]2+ (en is a strong-field ligand)arrow_forward
- For complexes of the same metal ion with no change in oxidation number, the stability increases as the number of electrons in the t2g orbitals increases. Which complex in each of the following pairs of complexes is more stable?(a) [Fe(H2O)6]2+ or [Fe(CN)6]4−(b) [Co(NH3)6]3+ or [CoF6]3−(c) [Mn(CN)6]4− or [MnCl6]4−arrow_forwardWhat type of isomerism is shown by [CO(NH3)5ONO]Cl2? (ii) On the basis of crystal field theory, write the electronic configuration for d4 ion if A0 < P. (iii) Write the hybridization and shape of [Fe(CN)6]3-. (Atomic number of Fe — 26)arrow_forwardDraw 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
- For any of the following that can exist as isomers, state the type of isomerism and draw the structures:(a) [Co(NH3)5Cl]Br2 (b) [Pt(CH3NH2)3Cl]Br(c) [Fe(H2O)4(NH3)2]2+arrow_forward3. Give the draw the d orbital diagram and give electron count, state whether the metal is high spin, low spin or no choice. (a) [Mn(CN)6]4- (d) [PdCl₂(en)] (b) [CoCl6]³- (f) [TI(OH₂)6]³+ (c) [Fe(NH3)6]³+ (g) [Cr(CN)6]4-arrow_forwarda) Draw the d-orbital splitting diagram for [Fe(CN)6]3- and [CoCl4]2- (tetrahedral). b) Classify the complexes as paramagnetic or diamagnetic.arrow_forward
- Uses crystal field theory (CCT) to predict the number of unpaired electrons in the following compounds. Indicate if the compound is diamagnetic or paramagnetic: a) [Fe(H2O)s]Cl, b) [Os(en)3]Cl2 c) Ka[Fe(CN)s] d) [Mn(acac)2(H20)2]SO4arrow_forwardDraw orbital-energy splitting diagrams and use the spectro-chemical series to show the orbital occupancy for each of the fol-lowing (assuming that H₂O is a weak-field ligand):(a) [Fe(C₂O₄)₃]³⁻(C₂O₄²⁻creates a weaker field than H₂O does.)(b) [Co(CN)₆]⁴⁻(c) [MnCl₆]⁴⁻arrow_forwardFor the low-spin coordination compound [Fe(en)2Cl2]Cl, identify the following.(a) the oxidation number of iron(b) the coordination number for iron(c) the coordination geometry for iron(d) the number of unpaired electrons per metal atom(e) whether the complex is diamagnetic or paramagnetic(f) the number of geometric isomersarrow_forward
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