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18 Dec 2019

Solid CrF3 contains a Cr(III) ion surrounded by six F- ions in an octahedral geometry, all at distances of 190 pm. However, MnF3 is in a distorted geometry with Mn-F distances of 179, 191, and 209 pm (two of each). Suggest an explanation.

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Related questions

Constants | Periodic Table

A complex ion is a species in which a central metal ion is attached to a group of surrounding ions or molecules by coordinate covalent bonds. The surrounding species are called ligands. Within a ligand, the atoms that are directly attached to the metal ion (or atom) are called donor atoms. Most ligands contain a single donor atom (monodentate), but some contain two donor atoms (bidentate), six donor atoms (hexadentate), or another combination of donor atoms. A complex ion that is associated with one or more counter ions is called a coordination compound. For example [PdCl4]2−is a complex ion, and Na[PdCl4] is a coordination compound. The following table lists some common ligands.
Ligand Number of
donor atoms
Cl− 1
F− 1
Br− 1
CO32− 2
CN− 1
gly− 2
EDTA4− 6
NH3 1
H2O 1
CO 1
The coordination number for a complex is the total number of donor atoms surrounding the central atom. The overall charge on a complex is the sum of the charges of the metal and all the ligands.

Part A

What is the coordination number for each of the following complexes or compounds?

[Co(NH3)4Cl2]+

[Cr(EDTA)]−

[Zn(H2O)4]2+

Na[Ag(CN)2]

Enter the coordination numbers, in the order that the complexes are listed, as four integers separated by commas (e.g., 1,2,3,4).

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Part B

What is the charge on each of the following complex ions?

hexaaquamanganese(II), [Mn(H2O)6]?

tris(carbonato)aluminate(III), [Al(CO3)3]?

amminepentachloroplatinate(IV), [Pt(NH3)Cl5]?

Express the charges numerically, in the order that the complexes are listed, separated by commas. For a nonzero charge, be sure to include the sign (e.g., +1,-2,+3).

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Part C

What is the oxidation number of the central metal ion in each of the following complexes or compounds?

[NiCl2Br2]2−

[Cr(H2O)2(NH3)4]3+

Na[Au(CN)2]

Express the oxidation numbers numerically, in the order that the complexes are listed, separated by commas. For a nonzero oxidation number, be sure to include the sign (e.g., +1,-2,+3).

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Submit

A complex ion is a species in which a central metal ion is attached to a group of surrounding ions or molecules by coordinate covalent bonds. The surrounding species are called ligands. Within a ligand, the atoms that are directly attached to the metal ion (or atom) are called donor atoms. Most ligands contain a single donor atom (monodentate), but some contain two donor atoms (bidentate), six donor atoms (hexadentate), or another combination of donor atoms. A complex ion that is associated with one or more counter ions is called a coordination compound. For example [PdCl4]2− is a complex ion, and Na[PdCl4] is a coordination compound. The following table lists some common ligands.

Ligand Number of
donor atoms
Cl− 1
F− 1
Br− 1
CO32− 2
CN− 1
gly− 2
EDTA4− 6
NH3 1
H2O 1
CO 1

The coordination number for a complex is the total number of donor atoms surrounding the central atom. The overall charge on a complex is the sum of the charges of the metal and all the ligands.

Part A

What is the coordination number for each of the following complexes or compounds?

a) [Co(NH3)4Cl2]+

b) [Pb(EDTA)]2−

c) [Pt(NH3)4]2+

d) [Ag(NH3)2]NO3

Part B

What is the charge on each of the following complex ions?

a) hexaaquachromium(II), [Cr(H2O)6]?

b) tris(carbonato)aluminate(III), [Al(CO3)3]?

c) amminepentachloroplatinate(IV), [Pt(NH3)Cl5]?

Part C

What is the oxidation number of the central metal ion in each of the following complexes or compounds?

a) [NiCl2Br2]2−

b) [Cr(H2O)2(NH3)4]3+

c) Na[Ag(CN)2]

(Spontaneity of Redox Reactions – 13 points) For this entire question, assume T is constant at 300. K, H2(g) is maintained at standard state conditions, R = 8.314 J mol-1 K-1, F = 96485C mol-1, and all activity coefficients are equal to 1.0. a. (8 points) You have four beakers, each one containing 1.0 L of an aqueous solution buffered to a pH = 1.0 (i.e [H3O+] = [H+] = 0.1M) and with 1 M of dissolved metal ions in each. You place a bar of silver (Ag) in beaker #1 which contains 1M Ag+, a bar of copper in beaker #2 which contains 1M Cu2+, a bar of lead in beaker #3 which contains 1M Pb2+, and a bar of zinc in beaker #4 which contains 1M Zn2+. Using the table of standard reduction potentials provided to the right, identify and report which beaker(s) a spontaneous dissolution (M(s) ? Mn+(aq); where “M” represents the solid metal and “Mn+” represents the metal cations) of some portion of the metal bar would or would not occur – provide an answer for each of the four beakers and show some justification for your answer to receive any credit

b. (5 points) You now prepare a fifth beaker also containing 1.0 L of an aqueous solution buffered to a pH = 1.0 (i.e [H3O+] = [H+] = 0.1M). To this beaker you then add a bar of pure copper (Cu(s)). Will there be a spontaneous dissolution of some portion of the copper bar in order to the system to establishes equilibrium? If yes, utilize the provided table of standard reduction potentials and the Nernst equation to calculate and report the concentration of Cu2+ ions in solution once the system attains equilibrium. Note : this system is different than Part A above in which beaker #2 initially had 1M of Cu2+ ions present; in this beaker #5 there is initially zero Cu2+ ions. Report your final answer with 1 significant digit.

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