Hi, guys. As you can see, the site has undergone a bit of an overhaul recently, as I have simplified the design and made the text a bit easier on the eyes. The site may continue to be updated and changed over the next few weeks or so, as I finalize a plan for what I would like the site to look like. Originally, when I considered making this site, I was more concerned about the content that I would be placing on it, than the aesthetics associated with it. In the future, I may even potentially create a store from which fans and readers can shop. On another note, you may or may not have noticed that my posts are not showing subscripts and superscripts. At this point, it is not something I can fix, and has to do with the website host’s text editor. Please bear with me on this, and for now, understand that when I write formulas, directly following the element’s abbreviation is the subscript or superscript associated with it.
Moving on, in this post I will begin a discussed on how to name simple compounds. This post may be broken down into a few separate posts, because there is a lot to cover. We will utilize the appropriate rules of chemical nomenclature as defined by IUPAC, or the systematic naming of chemical compounds. As you can imagine, with the millions of compounds that have come to be known in our current day and age, without a system that defines a set of rules for naming compounds, coping with the multitude of substances that exist would be extremely difficult, on top of being disorganized. Back in the day, compounds might have been named after people, places, or the characteristics they had, such as Glauber’s salt for its discoverer, J. R. Glauber, which is actually sodium sulfate. This is no longer the case (Ebbing and Gammon 2009).
We learned what organic compounds were, but a small note on inorganic compounds is that they are composed of elements other than carbon. Remember, however, that there are exceptions to the rule, and many carbon-containing compounds are indeed inorganic compounds, such as carbon monoxide, carbon dioxide, and cyanides, for whatever reason. Because naming can get complex, this post will focus on the naming of inorganic compounds, specifically beginning with simple, ionic compounds that are monatomic (Ebbing and Gammon 2009).
Ionic compounds, as we learned before, are compounds containing ions. Metal and nonmetal atoms are usually a part of ionic compounds, such as in the case of NaCl. Moreover, exceptions to this also excise, as in the case of ammonium salts such as NH4Cl. The way in which you name an ionic compound is by first giving the name of the cation, followed by the name of the anion. For example, if you’re given the name of a substance that is potassium sulfate, you know that potassium is the cation, and sulfate is the anion (Ebbing and Gammon 2009).
When naming a monatomic ion, which is an ion that is composed of a single atom, you must know the charge of the ion. There are some rules to know for predicting the charges of ions, and then rules for naming the monatomic ions. I would like you to have a periodic table of elements with you as you go over these rules and regularities. It will help you to visualize the information properly.
Predicting Charges on Monoatomic Ions: Rules as Per Ebbing and Gammon
Naming Monoatomic Ions: Rules as Per Ebbing and Gammon
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