The structure of the superoxide ion, O 2 -, is too difficult to discuss at this level, needing a good knowledge of molecular orbital theory to make sense of it. Potassium, rubidium and caesium form superoxides, XO 2.Sodium (and to some extent potassium) form peroxides, X 2O 2, containing the more complicated O 2 2- ion (discussed below).Lithium (and to some extent sodium) form simple oxides, X 2O, which contain the common O 2- ion.In the video both look black! – I have no idea what is going on here! Why are Different Oxides Formed as You Go Down the Group? One major web source describes rubidium superoxide as being dark brown on one page and orange on another! Some Li, Cl, and B can be incorporated into secondary minerals (e.g. The rubidium doesn't show a clear flame colour in this video, although the caesium does show traces of blue-violet.īoth superoxides are described in most sources as being either orange or yellow. There is a bit of video from the Royal Society of Chemistry showing the two metals burning on exposure to air. The equations are the same as the equivalent potassium one. The element number is its atomic number, which is the number of protons in each of its atoms. Each element has a one- or two-letter symbol, which is an abbreviated form of its present or former name. The names and element symbols are provided. Both metals catch fire in air and produce superoxides, RbO 2 and CsO 2. Here's a list of the chemical elements ordered by increasing atomic number.
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