Along with the Periodic table, the chemical bond is one of core mainstays of chemistry. A key moment in the development of this concept was the paper by Gilbert N. Lewis in 1916 introducing the shared two-electron bond, along with the associated "octet" rule for main group elements. Shortly after quantum mechanics was formulated in the 1930s, speculation started in earnest about whether the octet "rule" could be exceeded for compounds of main group elements. By the 1950s, most text books in organic and inorganic chemistry were depicting molecules such as sulfuric acid or sulfur hexafluoride with six "bonds" or "valencies" associated with the sulfur and carrying the implication of twelve, not eight valence electrons. Such depiction of "hypervalence" became firmly embedded not only in text books but in lectures and tutorials. But is this the best we can do nowadays? The lecture will try to get rid of some of the confusion, including in the terminology itself, by exploring some famous recent examples of claimed hypervalence, including SF6 itself, CLi6, 6-coordinate carbon cations and very recently claimed examples of hypervalent molecules such as diazomethane and the radical anion of HF. Two brand new (as yet unpublished) suggestions where the octet rule is "violated" will be revealed. Along with these conclusions, the underpinning data for anyone wishing to explore further the features of the molecules presented are made available as "managed research data" or RDM as it is now called by funding councils. A few minutes of the lecture will be spent showing how this very new evolution of the standard journal article has the potential to change how science will be done in the future. Finally a call will be made for nominations for the Bradley-Mason annual award to an undergraduate and a postgraduate for their contribution to Open Chemistry.