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Guest Speakers - Maria Pettyjohn and Juan Camilo Zapata Trujillo – UNSW This was from Juan who spoke at this I attended last night I will edit this reply and add some references soon. Supprisingly there are only around 50 for which we have absorption spectra that can be used for astrometry in studying exoplants and interstellar mediums. I found out about a special subset of molecules which would be interesting to explore. (And of course there’s a hybrid model, where some baseline editions have much of the shared functionality, but plugins are offered for the advanced stuff.) But to package them together and offer, say, the Organic Chemistry 101 molecules, the second model would be a more natural fit. In either of these models, adding additional compounds should be simple enough. With this, adding new features to a smaller wiki would usually be done just by importing additional plugins. Supporting multiple editions, each with its own collection of tools, and with some interdependencies managed on building these editions, containing no project-specific plugins at all.Īn organization into plugins, in which the equivalent of such multiple editions would involve embedding some subset of the available plugins (again with dependency tracking). I’m thinking of two different paths, and am not clear on which will be better for this project: That’s something I haven’t figured out yet. cycloalkanes need to be treated differently.Īnyway, this is getting tl dr and maybe should be split into a new thread (I don’t know how to do that and maybe only those with rights can) if we want to continue.īasing them on tiddlers we can then have a repository of formulae that when someone add a set they can package and submit them. Additionally, there isn’t a single algorithm for everthing – e.g. There are algorithms to calculate this sort of thing (see A000602 - OEIS and A000628 - OEIS for ignoring stereoisomers and including them, respectively and also List of straight-chain alkanes - Wikipedia). So for example, in the case of alkanes (CnH2n+2), for n=10 there are 75 isomers, n=15 it’s 4,347, n=20 it’s 366,319, n=30 it’s 4,111,846,763 and for n=187 I’ve read the number of isomers is greater than the number of ‘particles’ in the known universe… you get the picture! And that’s excluding stereoisomers.
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Maybe I don’t fully understand your intentions but the number of possible structures for a particular molecular formula increases very rapidly (although not exponentially) as the number of atoms increases. Sounds interesting… but I’m not sure this will be quite as easy. Thus, the formula mass of calcium hydrogen carbonate is 117.10 amu and the molar mass of calcium hydrogen carbonate is 117.10 grams per mole (g/mol).Next up: a list of molecules, and a reactor that lets you drag some elements into it and lets you know which of the molecules can be made from (some number of copies of) exactly those elements However when talking about a mole of an ionic compound we will still use the term molar mass. This is because there are no individual molecules in ionic compounds. For compounds that are not molecular (ionic compounds), it is improper to use the term “molecular mass” and “ formula mass” is generally substituted. The molar mass of the N 2 molecule is therefore 28.02 g/mol. This is referred to as the molecular mass and the molecular mass of any molecule is simply the sum of the atomic masses of all of the elements in that molecule. For nitrogen, the mass of the N 2 molecule is simply (14.01 + 14.01) = 28.02 amu. For a molecule (for example, nitrogen, N 2) the mass of molecule is the sum of the atomic masses of the two nitrogen atoms.
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The concept of molar mass can also be applied to compounds. Further, if you have 16.00 grams of oxygen atoms, you know from the definition of a mole that your sample contains 6.022 x 10 23 oxygen atoms.
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For example, the atomic mass of an oxygen atom is 16.00 amu that means the molar mass of an oxygen atom is 16.00 g/mol. Generalizing this definition, the molar mass of any substance in grams per mole is numerically equal to the mass of that substance expressed in atomic mass units. By definition, the molar mass of carbon-12 is numerically the same, and is therefore exactly 12 grams. We have defined a mole based on the isotopic atomic mass of carbon-12. The atomic mass of an element is the relative average of all of the naturally occurring isotopes of that element and atomic mass is the number that appears in the periodic table. ) a carbon atom with six proton and six neutrons in its’ nucleus, surrounded by six electrons.