transition metals KEYdoc

By Yolanda Sims,2014-11-16 16:59
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transition metals KEYdocmetal,Metal

     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

    K: +1

    Cu: +1

    Cl: - 1

    b. (NH)[Ni(CN)] 424

    NH: +1 4

    Ni: +2

    CN: -1

    c. [Ti(HO)](SO) 26243

    Ti: +3

    HO: 0 2

    SO: -2 4

    d. Al[V(CN)] 463

    Al: +3

    V: +2

    CN: -1

    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