(71 pts) Bonding in Transition Metal Complexes This problem for [Cr(NH3)sCI]Ch w
ID: 590135 • Letter: #
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(71 pts) Bonding in Transition Metal Complexes This problem for [Cr(NH3)sCI]Ch will highlight two very important points: (1) the valence orbitals on the central cobalt metal ion that are involved in covalent bonding to the lone pairs on the cyanide ligands, and (2) the non-valence d-orbital electrons on central metal are not involved in bonding, but are responsible for the color and magnetic properties of the coordination compound that is formed from the ligands and the central metal. (a) What is the oxidation state of the central metal ion for [CrONHs)sCI]C12? (b) What is the complete electron configuration for this central metal ion? (c) Clearly identify (type and periodic row) which orbitals (empty or filled) in part (b) are yalence orbitals for this compound: (d) Given that [Cr(NH3)sCI]Clh is a six-coordinated complex, how many empty orbitals must be available on the central chromium metal (Lewis acid) to accept the lone pairs from the ammine and chloro Lewis base ligands? (e) What is the hybridization of the orbitals listed in part (d)?Explanation / Answer
a) Oxidation state of Cr is +3
[Cr(NH3)5Cl]Cl2 = x+(5x0)+(-1) = +2
x = +3
b) Cr(III) = 1s2,2s2,2p6,3s2,3d3,4s0, 4p0
c) For Cr, 3d, 4s and 4p orbitals are considered as valence orbitals
d) In octahedral complexes, 6 ligands will be attached to central metal ion hence 6 empty orbital are needed to form the complex. They are 3d, 4s and 4p(2+1+3)
e) Hybridization of Cr in [Cr(NH3)5Cl]Cl2 is d2sp3
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