The naturally occurring radioactive decay series that begins with \({ }_{92}^{235} \mathrm{U}\) stops with formation of the stable \({ }_{82}^{207} \mathrm{~Pb}\) nucleus. The decays proceed through a series of alpha-particle and beta-particle emissions. How many of each type of emission are involved in this series?
Text Transcription:
{92}^{235} U
{82}^{207} Pb
Step 1 of 5) The electron configuration of the nitrogen atom is 3He42s22p3. The element exhibits all formal oxidation states from +5 to -3 (Table 22.6). The +5, 0, and -3 oxidation states are the most common and generally the most stable of these. Because nitrogen is more electronegative than all other elements except fluorine, oxygen, and chlorine, it exhibits positive oxidation states only in combination with these three elements. Production and Uses of Nitrogen Elemental nitrogen is obtained in commercial quantities by fractional distillation of liquid air. Because of its low reactivity, large quantities of N2 are used as an inert gaseous blanket to exclude O2 in food processing, manufacture of chemicals, metal fabrication, and production of electronic devices. Liquid N2 is employed as a coolant to freeze foods rapidlyThe largest use of N2 is in the manufacture of nitrogen-containing fertilizers. These fertilizers provide a source of fixed nitrogen—nitrogen that has been incorporated into compounds. We have previously discussed nitrogen fixation in the “Chemistry and Life” box in Section 14.7 and in the “Chemistry Put to Work” box in Section 15.2. Our starting point in fixing nitrogen is the manufacture of ammonia via the Haber process. (Section 15.2) The ammonia can then be converted into a variety of useful, simple nitrogen-containing species (Figure 22.21). Hydrogen Compounds of Nitrogen Ammonia is one of the most important compounds of nitrogen. It is a colorless, toxic gas that has a characteristic irritating odor. As noted in previous discussions, the NH3 molecule
