Concept explainers
Interpretation: The number of unpaired electrons in the given complex ion
Concept introduction:
Origin of color: The coordination compound exhibit color due to d-d transitions. Absorption of wavelength from visible region which excites electron from the lower energy level to the higher energy level transmits the complementary color. Thus, the coordination compound looks colored.
Spectrochemical series: The list of ligands arranged in an ascending order of
Crystal field splitting: The energy gap between the splitting of d-orbitals of the metal ion in presence of ligands is known as the crystal field splitting
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Chemistry: Atoms First
- For each of the following ions, draw diagrams (on a piece of paper), like the one to the right below, to show orbital occupancies for both weak and strong octahedral fields. Indicate (on the table below) the total number of unpaired electrons in each case. Ion # Unpaired Weak field # Unpaired Strong field (a) Pd4+ (b) Cr3+ (c) Cd 2(d) Ni2 + (e) Co2 +arrow_forward(a) What is the systematic name of Na3[AlF6]?(b) What is the systematic name of [Co(en)2Cl2]NO3? (c) What is the formula of tetraamminebromochloroplatinum(IV) chloride?(d) What is the formula of hexaamminecobalt(III) tetrachloroferrate(III)?arrow_forward(c) Give the ground-state electron configuration for each of following substances: (1) Phosphorus (ii) Cr(II) ion (iii) Sulfide ion (iv) Ti(IV) ionarrow_forward
- The complex ion [Co(H2O)6]3+ exhibits absorbance with max = 600 nm (orange region) , while [Co(NH3)6]3+ exhibits absorbance with max = 475 nm (blue region). (a) Determine the color of each complex ion. (b) Calculate the crystal-field splitting in each complex ion; expressed the splitting energy in kJ/mol. (No = 6.022 x 1023/mol; h = 6.626 x 10–34 J.s.; c = 3.00 x 108 m/s) Here are the answers for part (b), I am having a hard time trying to get these answers. Can you please show your work for part (b)? [Answers: (b) [Co(H2O)6]3+ : max = 600. nm; octahedral splitting energy, O = 200. kJ/mol; [Co(NH3)6]3+ : max = 475 nm; octahedral splitting energy, O = 252 kJ/mol]arrow_forwardWrite the ground state electronic configurations for: (a) Ca²+ (b) Cu (c) Crarrow_forwardHow many unpaired electrons are present in each of the following?(a) [CoF6]3− (high spin)(b) [Mn(CN)6]3− (low spin)(c) [Mn(CN)6]4− (low spin)(d) [MnCl6]4− (high spin)(e) [RhCl6]3− (low spin)arrow_forward
- (NH4)2[MnF6] What is the name of the compound?arrow_forwardAre compounds of these ground-state ions paramagnetic?(a) Ti²⁺(b) Zn²⁺(c) Ca²⁺(d) Sn²⁺arrow_forwardFor each of the following ions, draw diagrams (on a piece of paper), like the one to the right below, to show orbital occupancies for both weak and strong octahedral fields. Indicate (on the table below) the total number of unpaired electrons in each case. Ion # Unpaired Weak field # Unpaired Strong field (a) Pd4+ (b) Cr3+ (c) Cd2+ (d) Ni2+ (e) Co2+arrow_forward
- What is the abbreviated electron configuration of the metal ion in Cr2(SO4)3 ?arrow_forwardWhich of these compounds is/are expected to be optically active? (en = H2N–CH2–CH2–NH2) (A) cis–[Co(NH3)4Cl2]Cl (B) cis–[Co(en)2Cl2]Cl (C) trans–[Co(en)2Cl2]Cl (D) Compounds (A) and (B)arrow_forward(c) Give the ground-state electron configuration for each of following substances: (i) Phosphorus (ii) Cr(II) ion (iii) Sulfide ion (iv)Ti(IV) ionarrow_forward
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