3 Radiation & Atomic Theory+
3.4 Matter Interactions with EM Radiation
3.5 Atomic Theory for those in a Hurry
3.6 Quantum Numbers
3.9 Ionic Bonding
3.11 Covalent Bonding
3.42 Learning Outcomes
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Nomenclature is the naming of chemical elements and compounds
This is a good useable set of elements to memorize the symbol and name. Do not worry about the atomic number - remember, you will have a periodic table for all exams. The main thing is to know how to match element names to their symbols as in potassium = K. A perfect thing for homemade flash cards.
Now notice the dark blue line that starts just under boron (#5) - that is the transition line between the metals and the non-metals. Everything to the left of that line is a metal (except hydrogen, duh). Everything to the right is a non-metal. Elements bordering the line... for us that's boron, silicon, germanium, arsenic, and antimony (the ones you memorize) are metalloids (aka semiconductors). Why is this important? Because metals and non-metals tend to ionize in opposite ways. Metals lose electrons and become cations (positively charged ions - pronounced CAT·ion) and non-metals gain electrons and become anions (negatively charged ions - pronounced AN·ion). Each group is named in different ways.
Al3+, Zn2+, Ag+, Cd2+
The rest of the metals (all transition metals in the d-block) have to have their charge indicated in the name via a roman numeral suffix in parenthesis. This means that Fe2+ is called iron(II) and Fe3+ is called iron(III). Most cations don't go beyond a +4, so you don't have to count too far in roman numerals... although, do know that V4+ is named and written vanadium(IV).
The non-metals gain more electrons and reach noble gas electron configurations which means a full set of s and p orbital (s2p6). The naming is done by replacing the suffix with -ide. So Cl– is called chloride and S2– is called sulfide. See the table to learn all of them - but remember that it IS pretty systematic in the naming. Because all the non-metal monatomic anions match noble gas configuration, there are never more than one possible charge. ALL the halogens (group 17) make –1 anions. All the group 16 elements make –2 anions and so on... but only for the non-metals.
There are also a lot of ions that exist that are made up of 2 or more covalently bound elements. We call them the polyatomic ions. There is a fairly full listing of these in the appendix (section 10.6). To keep things a bit more manageable, I've honed this down to a "shortlist". This is where you just have to go ahead and memorize them. There is some method to the madness and you can learn it. This is a very helpful list and you need to know these polyatomic ions from here on.
Yes, you need to memorize this set of polyatomic ions: name, formula, and charge.
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