Platinum ionization energy

Until about 40 years ago, these elements were referred to as "inert gases" they were believed to be entirely unreactive toward other substances. In 1962 Neil Bartlett, a 29-year-old chemist at the University of British Columbia, shook up the world of chemistry by preparing the first noble-gas compound. In the course of his research on platinum-fluorine compounds, he isolated a reddish solid that he showed to be 02+(PtFB-). Bartlett realized that the ionization energy of Xe (1170 kJ/mol) is virtually identical to that of the 02 molecule (1165 kJ/mol). This encouraged him to attempt to make the analogous compound XePtF6. His success opened up a new era in noble-gas chemistry. 

Identify the element with the higher first ionization energy in each of the following pairs (a) iron and nickel (b) nickel and copper (c) osmium and platinum (d) nickel and palladium ... 

Platinum metal is often used as a passive electrode because platinum is one of the least reactive elements. Platinum has a large ionization energy, so it can act as an electron shuttle without participating in redox chemistry. 

Since the redox potentials of dye aggregates adsorbed onto platinum electrode exhibit a broad distribution centred at the formal oxidation potential Eox, the direct information on the ionization energy of the aggregated cyanines can be obtained, even in case of irreversibly oxidizing dyes, from the potential dependence of the fractional degree of dye oxidation, 0, derived from the potential-step electrochemical measurements [52, 53]. The analogue of Nemst equation describing the oxidation process can be written as ... 

The increased ionization energies of the heavier transition metals should not be unexpected by anyone who has had a modicum of laboratory experience with any of these elements. Although none of the coinage metals is very reactive, gold has a well-deserved reputation for being less reactive than copper or silver iron, cobalt, and nickel rust and corrode, but osmium, indium, and platinum are noble and unreaclive and therefore are used in jewelry platinum wires are the material of choice fior flame tests without contamination and one generates hydrogen with zinc and simple adds, not with mercury. 

Which has the largest ionization energy, platinum, an element sometimes used in dental crowns, or cobalt, an element that provides a bright blue color to pottery ... 

The loss of free atoms in the atomizer is also a function of the chemistry of the sample. If the oxide of the analyte element is readily formed, the free atoms will form oxides in the flame and the population of free atoms will simultaneously decrease. This is the case with elements such as chromium, molybdenum, tungsten, and vanadium. On the other hand, some metal atoms are stable in the flame and the free atoms exist for a prolonged period. This is particularly so with the noble metals platinum, gold, and silver. Adjusting the fuel/oxidant ratio can change the flame chemistry and atom distribution in the flame as shown in Fig. 6.17(b). Atoms with small ionization energies will ionize readily at high temperatures (and even at moderate temperatures). In an air-acetylene flame, it can be shown that moderate concentrations of potassium are about 50% ionized, for example. Ions do not absorb atomic lines. 

Platinum (Pt) is often used as a passive electrode because it is very unreactive and will not form compounds with the elements in solution. Pt is unreactive due to having a very high ionization energy, yet is a rare element and quite expensive. Gold and graphite can also be used. 

It occurred to Bartlett that the ionization energies of the oxygen molecule (1180 kj/mol) and the xenon atom (1167 kj/mol) were remarkably similar. He decided to try the same reaction as above with xenon replacing the diatomic oxygen. He prepared known volumes of xenon (in slight excess) and platinum hexafluoride and carefully noted the pressure of each. When he allowed the two gases to mix. 

The first ionization energies of iron, cobalt, nickel, and the first three platinum metals are all about the same, but the first ionization energies of osmium, iridimn, and platinum are substantially greater. Suggest an explanation for this observation. 

It starts with a compilation of the properties of the isotopes, followed by the description of the formation and separation of the radioactive isotopes. The chapters on the atoms and atomic ions deal with the configuration of the outer-shell electrons, manifested by optical terms and spectra, ionization energy, and electron affinity, as well as with the energy levels of the inner-shell electrons, manifested by X-ray spectra and Auger electron spectra. The last section gives information on the formation and the physical properties of the platinum group molecules and clusters. 

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