![]() ![]() The isotope 85Kr can also be used in combination with phosphors to produce materials that shine in the dark due to the fact that this particular isotope of Krypton reflects off of phosphors. In neon lights, Krypton reacts with other gases to produce a bright yellow light as well. Due to Krypton's large number of spectral lines, it's ionized gas is white, which is why light bulbs that are krypton based are used in photography and studio lighting in the film industry. Krypton gas is used in various kinds of lights, from small bright flashlight bulbs to special strobe lights for airport runways. It simply took an element of high electronegativity, in this case Fluorine, to force Xe and Kr to react under high temperatures. ![]() Although both Kr and Xe have full valence shells, they are both the most easily ionized of the group. This proved that this group of gases is not necessarily inert. However, the inert quality of these gases was disproved when Xenon compounds were created in 1962 and a Krypton compound (KrF2) was synthesized successfully a year later. The name Krypton is derived from the Greek word "kryptos", meaning "hidden". One of these gases, Krypton, was discovered along with Neon and Xenon by Rayleigh and fellow chemist Morris Travers in 1898 in a residue left from evaporating almost all components of liquid air. A century later, British chemists John Rayleigh and William Ramsey began to isolate these inert gases (beginning with Argon) and seperated them in their own group on the periodic table since each of these elements had full electron valence shells. In 1785, Henry Cavendish suggested that air contained nonreactive gases after he was unsuccessful in getting a sample of air to react. Krypton is found in the Group 18 elements, otherwise known as the Noble Gases. Contrary to original thinking, however, Krypton has been made to react with the highly electronegative elements and is used in lighting and other commercial purposes. Krypton is one of the six Noble Gas elements ( Group 18), which are widely known for their relative "inertness" and difficulty in forming chemical compounds with any other elements, due to these elements having full valence shells. ![]()
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