Noble gases first ionization energy

For the element sodium, Na, the first ionization energy is 495.8 kJ/mol and the second ionization energy is about 5.5 times greater than the first ionization energy. Thus, the sodium, Na, atom gets a noble gas electron configuration after giving off one electron. 

The electron configuration for the noble gas with the highest first ionization energy... 

The noble gas with the most stable configuration and highest first ionization energy is helium. 

Does the first ionization energy increase or decrease from top to bottom in the periodic table for the noble gas family Explain. (Eigure 11.3)... 

The outermost electron in potassium is farther away from the nucleus than the outermost electrons in calcium, so the first ionization energy of potassium is lower than that of calcium. However, once potassium loses one electron, it achieves a noble gas electron configuration, and therefore taking a second electron away requires considerably more energy. For calcium, the second electron is still in the outermost shell and does not require as much energy to remove it. 

Figure 5-2 shows that each noble gas has the highest first ionization energy in its period. This should not be surprising because the noble gases are known to be very unre-active elements. It requires more energy to remove an electron from a helium atom (slightly less than 4.0 X 10 J/atom, or 2372 kJ/mol) than to remove one from a neutral... 

Periodicity of First Ionization Energy Figure 8.10 shows the variation in first ionization energy with atomic number. This up-and-down pattern—IE, rising across a period to the noble gas (purple) and then dropping down to the next alkali metal (brown)—is the inverse of the variation in atomic size (Figure 8.9) as size decreases, it takes more energy to remove an electron because the nucleus is closer, so lE increases. 

FIGURE 8.14 First Ionization Energy versus Atomic Number for the Elements through Xenon Ionization starts at a minimum with each alkali metal and rises to a peak with each noble gas. 

Use ideas presented in this chapter to indicate (a) three metals that you would expect to exhibit the photoelectric effect with visible light and three that you would not G ) the noble gas element that should have the highest density in the liquid state (c) the approximate first ionization energy j of fermium (Z = 100) (d) the approximate density of solid radium (Z = 88). 

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. 

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