Name: _________________________________________ Date:____________________________
Optional Homework 8 – do not turn in!!
1.) Write the electron configurations for the following species:
11022626210629a. Ag 1s2s2p3s3p4s3d4p5s4d ， 5s4d
010226262106+1b. Ag 1s2s2p3s3p4s3d4p5s4d
010226262106+2 c. Cd1s2s2p3s3p4s3d4p5s4d
014622626210621062147+3d. Ir 1s2s2p3s3p4s3d4p5s4d5p6s4f5d ， 6s4f5d
2.) Find the charge of all species in each of the following coordination compounds, if it is a polyatomic
ion, I just want the overall charge of that ion, not individual oxidation numbers of every element!:
HINT: you may need to go back and review your polyatomic ion charges!!
a. K[CuCl] 2
Cl: - 1
b. (NH)[Ni(CN)] 424
NH: +1 4
c. [Ti(HO)](SO) 26243
HO: 0 2
SO: -2 4
d. Al[V(CN)] 463
3.) Identify the complex ion and the ligands in the compound K[Fe(CN)CO]. Find the oxidation 35
number of the metal ion in complex ion: be sure to label the inner sphere (ligands bonded
covalently to the metal) and outer sphere ligands (counter ions) in the complex!
K[Fe(CN)CO]: K is an outer sphere ligand 35
CN is an inner sphere ligand (-1)
CO is an inner sphere ligand (0)
Iron is the transition metal oxidation state = +2
4.) Find the charge on the nitrosyl ligand (NO) in the Co(III) compound: Na[Co(CN)NO] 25
Na[Co(CN)NO] Na = +1 x 2 = +2 25
CN = -1 x 5 = -5
Co = +3
So the NO ligand must be neutral!
5.) If the coordination complex [Cr(NH)Cl]Cl dissociated into its ions, what ions would be formed? 352
Write a balanced equation showing this dissociation!
[Cr(NH)Cl]Cl ? ??? 352
+2-1[Cr(NH)Cl]Cl ? [Cr(NH)Cl] + 2Cl35235 (aq) (aq)
6.) Using the ideas of Lewis and resonance structures, determine which of the following ligands can
participate in linkage isomerism (meaning can they cause a compound to be a linkage isomer).
DRAW the resonance structures in order to explain! Remember that a linkage isomer can bond to
the metal ion from two distinctly different places on the molecule. And in order to have a bond –
you need electrons!!!
-1a. NO 2
There are lone pairs present on
both the N and the O so the species can bond through either the N or O which means this species can be a linkage isomer
b. SO 2
There are lone pair electrons
on the S and the O in the molecule, therefore this species can participate in linkage isomerism
-1c. NO 3