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(ii) Explain the Jahn-Teller distortion in [Cu(H2O)2 (ii) If a solution with a dissolved octahedral complex...
a. Predict the structure of [Cr(OH2)6]2+ - I wrote that the complex will undergo Jahn-Teller distortion,...
a. Predict the structure of [Cr(OH2)6]2+ - I wrote that the complex will undergo Jahn-Teller distortion, making the octahedral complex become tetragonal (don't know if that's correct) b. Account for the variation in the lattice enthalpy of Mn (2780 kJ/mol), Fe (2926 kJ/mol), Co (2976 kJ/mol), Ni (3060 kJ/mol), and Zn (2985 kJ/mol) flouride given that the metal center in all of the flourides is surrounded by an octahedral array of F-ions. c. Explain the effect on the d-orbital energies...
Would a 5-coordinate trigonal bipyramidal Copper(II) complex exhibit Jahn-Teller distortion?
Would a 5-coordinate trigonal bipyramidal Copper(II) complex exhibit Jahn-Teller distortion?
5. The complex [Cu(CN).]* undergoes tetragonal elongation due to Jahn-Teller distortion Draw the Crystal field splitting...
5. The complex [Cu(CN).]* undergoes tetragonal elongation due to Jahn-Teller distortion Draw the Crystal field splitting diagram for the complex and fill orbitals with electrons.
An octahedral metal complex absorbs light with wavelength 580 nm. a. What is the crystal field...
An octahedral metal complex absorbs light with wavelength 580 nm. a. What is the crystal field splitting A, in kJ/mol for the complex? (Hint: Energy is based on wavelength of light absorbed. See data sheet.) (3 marks) b. What color does the complex appear to the eye? (2 marks) 750 nm, 400 nm Red Violet 630 nm 430 nm Blue Orange 590 nm 480 nm Yellow Green 560 nm
The Fe(ox)33- ion forms an emerald green solution when it is dissolved. As stated in the...
The Fe(ox)33- ion forms an emerald green solution when it is dissolved. As stated in the Introduction section above, the crystal field splitting affects the color of the compound. In fact, compounds with different magnitudes of Δo will appear different colors, corresponding to the wavelength of light that enters our eyes. If the ion in solution appears emerald green to our eyes, what color of visible light is it mostly absorbing? What does that tell you about the magnitude of...
Electronic absorption spectrum of copper ammine complexes (i) Draw the electron distribution in the d orbitals of an octahedral Cu(II) complex and show the electronic transition responsible for the...
Electronic absorption spectrum of copper ammine complexes
(i) Draw the electron distribution in the d orbitals of an
octahedral Cu(II) complex and show the electronic transition
responsible for the absorptions observed.
(ii) Assign the transition you observe for each complex and give
the value of Δ (in cm-1).
Visible absorption spectra of Cu(ll) complexes 1.2 Cu (H20)2(NH3)4 Cu (H2O)6 Cu (H20)3(NH3)3 0.8 0.6 Cu (H20)s(NH3) Cu (H20)4(NH3)2 0.4 0.2 850 500 550 600 650 700 750 800 900 450 nm...
Question 5 6 pts A student has three test tubes containing a metal (M) nitrate solution...
Question 5 6 pts A student has three test tubes containing a metal (M) nitrate solution M(NO3)2 (aq) (where "M" represents a generic transition metal). The student adds aqueous ammonia (NH3) to one test tube, aqueous hydrochloric acid (HCI) to the second tube, and nothing more to the third tube, but forgets to label the tubes. After this, one test tube contains a red solution, one an orange solution, and one a yellow solution. Note: This metal, M, would follow...
Q1. The following species a)-c) all contain complex ions of transition metals, which you can assume...
Q1. The following species a)-c) all contain complex ions of transition metals, which you can assume take up an octahedral geometry. a) [RuCl3(H2O)3] b) [Ir(bpy)3]Cl3 ; bipy = 2,2'-bipyridine c) K2[Mo(NCS)6] For each species: i) draw all the possible isomers of the complex ions; ii) calculate the charge of the metal, and the dn configuration; iii) draw a diagram showing d orbital occupancy and, where high and low spin cases are possible, predict which will be favoured considering the spectrochemical...
In the complex ion [ML6]n+, Mn+ has five d electrons and L is a strong field...
In the complex ion [ML6]n+, Mn+ has five d electrons and L is a strong field ligand. According to crystal field theory, the magnetic properties of the complex ion correspond to how many unpaired electrons? A. 0 B. 1 C. 2 D. 3 E. 5 Which one of these complex ions would absorb light with the shortest wavelength? A. [Co(H2O)6]2+ B. [Co(NH3)6]2+ C. [CoF6]4– D. [Co(CN)6]4– E. [Co(en)6]2+ The ion [Co(NH3)6]2+ is octahedral and high spin. This complex is (4pts)...
A 300.0-mL saturated solution of copper(II) periodate, Cu(IO4)2, contains 0.38 grams of dissolved salt. Determine the...
A 300.0-mL saturated solution of copper(II) periodate, Cu(IO4)2, contains 0.38 grams of dissolved salt. Determine the Ksp. a. 1.6 x 10-5 b. 3.2 x 10-5 c. 2.8 x 10-3 d. 9.2 x 10-8 e. 2.5 x 10-9
5. The complex [Cu(CN).]* undergoes tetragonal elongation due to Jahn-Teller distortion Draw the Crystal field splitting diagram for the complex and fill orbitals with electrons.
An octahedral metal complex absorbs light with wavelength 580 nm. a. What is the crystal field splitting A, in kJ/mol for the complex? (Hint: Energy is based on wavelength of light absorbed. See data sheet.) (3 marks) b. What color does the complex appear to the eye? (2 marks) 750 nm, 400 nm Red Violet 630 nm 430 nm Blue Orange 590 nm 480 nm Yellow Green 560 nm
Electronic absorption spectrum of copper ammine complexes
(i) Draw the electron distribution in the d orbitals of an
octahedral Cu(II) complex and show the electronic transition
responsible for the absorptions observed.
(ii) Assign the transition you observe for each complex and give
the value of Δ (in cm-1).
Visible absorption spectra of Cu(ll) complexes 1.2 Cu (H20)2(NH3)4 Cu (H2O)6 Cu (H20)3(NH3)3 0.8 0.6 Cu (H20)s(NH3) Cu (H20)4(NH3)2 0.4 0.2 850 500 550 600 650 700 750 800 900 450 nm...
Question 5 6 pts A student has three test tubes containing a metal (M) nitrate solution M(NO3)2 (aq) (where "M" represents a generic transition metal). The student adds aqueous ammonia (NH3) to one test tube, aqueous hydrochloric acid (HCI) to the second tube, and nothing more to the third tube, but forgets to label the tubes. After this, one test tube contains a red solution, one an orange solution, and one a yellow solution. Note: This metal, M, would follow...
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