24-11 Applications of Coordination Chemistry

24-11 Applications of Coordination Chemistry

• There are many applications of coordination chemistry.
• They range from analytical chemistry to biochemistry.
• The examples in this section give an idea of the diversity.

• Some types of cancer can be treated with Cisplatin.

• NH3 uses drugs to destroy cancer cells.

• The discovery of the anticancer activity of cisplatin was made by a professor at Michigan State University.

• Let's first consider the synthesis of cisplatin.

• In two stages, -3PtI21NH3224 is a key step.

• The conversion of K23PtI 44 to K23PtI 44 is a 2O.

• The following steps are needed to prepare cisplatin.

• The essential features of the activity of cis platin are discussed.
• One of the cisplatins is replaced by a water molecule inside the cell.

• The binding of 3Pt1Cl21H2O21NH3224+ to a cellular DNA molecule is associated with the activity of cisplatin.
• When 3Pt1Cl21H2O21NH3224+ is binding to a DNA mol ecule, there are structural defects in the molecule that lead to cell death.

• Transplatin is less effective in killing cancer cells because of its increased reactivity.

• The discovery of the activity of cisplatin was monumental.
• Thousands of compounds containing platinum have been investigated as potential drugs.
• Platinum-based drugs are the top selling drugs in the world.

• When a compound is crystallised from an ion solution, the crystals are often hydrated.
• A Hydrate is a substance that has a fixed number of water molecule associated with each formula unit.
• The water molecule can beBonded directly to a metal ion.

• There is a chance that the water molecule may be incorporated into definite positions in the solid crystal but not associated with any particular cations or anions.

• This large positive value shows that Co3 is strong enough to oxidize water to O21g2.

• 3Co1NH32643+ is one of the complex ion featured in this chapter.

• The ion is stable in the water solution even though it has cobalt in it.
• If the concentration of Co3+ is too high and 3Co3+4 is too low, the reaction won't happen.

• 3Co1NH32643+ + 0.10 V is also a consequence.

• The ability of strong electron-pair donors to stabilizing high oxidation states in the way that does in Co(III) complexes and O2 NH3 in Mn(VII) complexes gives a means of attaining certain oxidation states that might otherwise not be possible.

• A black-and-white photographic film is an emulsion of a finely divided silver halide coated on a strip of polymer.
• The reduction of Ag+ to Ag is promoted by the photons.
• The intensity of the light absorbed affects the number of Ag atoms in the lattice.
• The silver is invisible to the eye because the number of Ag atoms produced in the exposure is not large.
• The film is developed to get a visible image.

• An oxidation-reduction reaction occurs in which hydroquinone and Ag are reduced.
• Reduction of Ag+ to Ag occurs only in the AgBr(s) that contain Ag atoms, because of the developer's action.
• The number of Ag atoms in the film is increased and the image becomes visible.
• Bright regions of the object appear to be dark in the photo.
• Reduction of Ag+ to Ag could still occur in the previously unexposed granules of AgBr(s), which is why this negative cannot be exposed to light.

• A common fix is a solution of sodium thiosulfate.
• The complex ion 3Ag1S2O32243 has a large formation constant, so the following reaction is driven to completion.

• Light is projected onto a piece of photographic paper.
• When the photographic paper is developed and fixed, the dark regions of the negative will no longer transmit light to the paper.
• Light areas of the negative will appear dark in the final print.
• The areas of light and dark in the final print are the same as in the photo.

• In discussing qualitative cation analysis in Section 18-9, we showed how the group 1 is separated by taking advantage of the stable complex ion formed by Ag.

• If a trace amount is present in the solution, there is a problem.

• The complex ion 3CoF442- is less stable than the one in 3Co1SCN2432.
• The blue-green solution color can be used to detect the 3Co1SCN2442-1aq2.

• Metal ion can act as catalysts in promoting undesirable chemical reactions in a manufacturing process, or they can alter the properties of the material being manufactured.
• It is important to remove mineral impurities from water.
• If Ksp is small, precipitation of metal ion can be done, but only in trace amounts.
• The water can be treated with a chelating agent.
• The cations can no longer enter into objectionable reactions if the free cation concentrations are reduced.

• The high stability of such complexes can be attributed to the presence of five, five-member chelate rings.
• The stability of the complexes can be attributed to this effect.

• Thepale green can be Ca2+, Fe2+, Fe3+, and so on.

• Hard water can't form boiler scale or be used as insoluble soaps because of the presence of Fe3+.

• Some cases of metal poison ing can be treated with quenching with EDTA.
• The following exchange occurs if a person with lead poisoning is fed 3Ca1EDTA242-.

• The body excretes the lead complex and the Ca2+ remains as a food.
• In the treatment of plutonium poisoning, a similar method can be used to rid the body of radioactive isotopes.

• Some plant fertilization contain a form of the metal ion that is called a sol Tom Pantages uble form of the metal ion.

• Some products have something in them.

• The concentration of metal is reduced by the use of EDTA.

• The main structural materials of plants areCarbohydrates.

• The porphyrin structure green pigment absorbs sunlight and directs the storage of this energy into the chemical bonds of the carbohydrates.
• There is a central metal ion.

• We should expect green to absorb light in the red region of the spectrum because it's the same color as magenta.
• Experiments show that green plants grow better in red light than they do in other colors.
• The maximum rate of formation of O21g2 occurs with red light.

• In Chapter 28, we will look at another porphyrin structure that is essential to life.

• Transition metal ion is responsible for the brilliant colors in gemstones.
• For a discussion of the ion responsible for the colors of rubies and emeralds, and the mechanisms that allow these gemstones to maintain their colors indefinitely, go to the Focus On feature for Chapter 24, Colors in Gemstones.

• There are bonds between metal centers.

• A polydentate ligand is stance when placed in a magnetic field.

• The name of a complex conveys colors displayed by coordination complexes, the arise from the absorption of certain wavelength oxidation state of the metal center.

• The positions at which the ligands are in the absorbed wavelength and hence of a different attached to the metal center are not always equivalent in color.

• There are two molecule from aqua complex ion in coordination complexes.
• When a metal ion is binding to a side of a square in a structure, an increased stability is observed.
• The ture is a greater stability achieved.

• The qualitative analysis scheme and AgBr can be used to sequester the ion in Complex-ion formation.
• Other applications include tion.

• Large proportions of the light entering a solution being absorbed correspond to high absorbances.
• Large proportions of the light are transmitted with low absorbances.

• The central ion in the complex ion is 3Ar43d1.

• The observed color of the solution is a blend of red and blue.

• The amount of energy we seek is the amount of energy that comes from the peak of the absorption spectrum.

• The energy is per photon.

• The wavelength components of white light that the complex cation absorbs were determined using ideas of subtractive color mixing.
• The metal to oxygen bonds cause the absorption band to be broad.
• The most probable energy of the absorbed photons was calculated using the maximum absorption curve.

• A number of isomeric forms have been prepared for the compound.
• One form has no reaction with either AgNO3 or en.
• A second form reacts with AgNO3 to form a white precipitate, but does not react with en.
• A third form reacts with both AgNO and en.

• Pick out each of the three isomeric forms by name, and sketch each of the structures.

• A compound has 46.2% Pt, 33.6% Cl, 16.6% N, and 3.6% H.

• A 0.1 M solution of the compound has a freezing point of -0.74 degC.

• The structures of four ionized water are given.

• To represent the observations, write equations.

• The mixture is back to pale blue.

• To represent the observations, write equations.

• A pale trated HCl(aq) is added to CuSO41aq2 and produces a yellow solution.
• If NH31aq2 is added, the pre solution is increased to twice its volume with water and cipitate redissolves, producing a solution with an assumes green color.
• Its deep blue color was ten times more intense on dilution.
• The solution becomes pale blue if it is original volume.

• There is a 2.24 when chromium metal is dissolved.
• The formation constant blue solution quickly turns green.

• NH31aq2 contains ZnCO31s2 but not ZnS(s).

• To show the complex-ion formation, write a series of equations.

• For log10 K1 of ylenediamine to be unstable, it must be reduced to log10 K2 and freed from O21g2.

• 3Co1NH32643+ should occur spontaneously in a solution with H2O2 as an oxidizer.

• They should sketch their structures.

• It is a compound.

• Make sketches of the two complexes.

• That is, Ka W Ka W.

• This mul 34 has a value of 0.1 M.

• The concentration cell is being built.

• When electric conductiv AgfAg+10.10 M3Ag1CN224-, 0.10 M CN-2 ity is plotted as a function of the number of chlorido f, make a rough sketch of the expected graph.

• One of the ways to calculate the pH of the solution is by using the compound CoCl # 2 2 H2O # 4 NH3.

• The solution's pH can be maintained.

• A solution of 0.010 M in Pb2+ is equal.

• A visible yellow color can be produced by 4.

• The anion acac- can act as a bidentate with the enol.

• We have seen that complex formation can be stable.
• An illustration of this fact is the oxidation of water in acidic solutions by Co3 and not by 3 Co1en.
• The following data can be used.

• Show that Co3 is not stable in water.

• The graph has the amino acid glycine in it.

• The graph shows the Molar conducti 100 tivity of Pt(IV) complexes.

• Draw the structure of Explain.

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• The compound that was prepared was described in Are You Wondering 24-3.

• There are 2468 electrons in the dz2 and dx2 orbitals.

• The number of the metals shown is Fe.

• A line of negative slope is obtained.

• The value of C/o for the Fe(II) ion in a hydration is more negative than the lines drawn on the water molecule.

• The one that exhibits ble is a complex ion.

• You have a reason for doing that.

• The theory explains the colors and magnetic properties of metal complexes.