1	Chapter 4 Nomenclature BEWARE!!! There is a lot memorization involved with this chapter.
2	"In the old days compounds..." In the old days compounds had common names like: water, milk of magnesia, gypsum, quicklime, etc. Today we know of over 4 million compounds. Common names won’t work Therefore we have a system! First we will learn about binary compounds, compounds made of two elements There are two classes: 1) metal/nonmetal 2) nonmetal/nonmetal
3	4.1 Naming Compounds that Contain a metal and a Nonmetal Metals tend to lose electrons e-, Nonmetals gain electrons e- Metals like to be positive + Nonmetals like to be negative - These get together to form binary ionic compounds
4	"When writing the" When writing the formula the cation is first, anion second When naming just say their names Some cations have only one charge ever (called Type I ion) Some have more than one (Type II ion) There are also Type I compounds and Type II compounds
5	Type I Binary ionic compounds Reviewing the rules:
6	Type II binary ionic compounds Some cations can form more than one charge!!! (Type II ion!) Let’s look at an example…. iron can form 2+ and 3+ ions so what is the iron in iron chloride? Fe²⁺ or Fe³⁺? must be a way to distinguish the two! use Roman numerals…
7	"So what is the name..." So what is the name of FeCl₂? Chloride always has a 1- charge, and there are two, so… The positive guy must have a total 2+ charge, and… There is only one cation so it get the whole 2+ charge all to itself, so… It must be iron(II), so… It is iron(II) chloride Know Table 4.2 (the systematic is emphasized in this class!!)
8	examples CuCl copper(I) chloride HgO mercury(II) oxide Fe₂O₃ iron(III) oxide Mn₂O₄ manganese(IV) oxide PbCl₄ lead(IV) chloride
9	"summary of Type I and..." summary of Type I and Type II
10	summary examples CoBr₂ cobalt(II) bromide CaCl₂ calcium chloride Al₂O₃ aluminum oxide CrCl₃ chromium(III) chloride
11	4.2 Naming Binary Compounds that Contain only Nonmetals (Type III) Type III contain only NM! think prefixes! (note: water and ammonia are Type III but always keep their common names)
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13	examples BF₃ boron trifluoride NO nitrogen monoxide N₂O₅ dinitrogen pentoxide PCl₅ phosphorus pentachloride SF₆ sulfur hexafluoride SO₂ sulfur dioxide
14	4.3 naming binary compounds: a review
15	4.4 Naming Compounds that contain Polyatomic Ions There is another(!) type of compound, one that involves… Polyatomic ions. Ions with more than one type of atom in it gotta know Table 4.4
16	"Notice many have O in..." Notice many have O in them Called oxyanions Most common is called root-ate (e.g. sulfate) One less O than most common? root-ite (nitrite) One less than that? hypo-root-ite (hypochlorite) One more than most common? per-root-ate (perchlorate) Must be able to recognize Polyatomic ions!!!
17	examples Na₂SO₄ sodium sulfate Fe(NO₃)₃ parentheses here mean there are 3 of what’s inside. “NO₃₃” is nonsense! iron(III) nitrate Mn(OH)₂ manganese(II) hydroxide
18	summary examples Na₂CO₃ sodium carbonate FeBr₃ iron(III) bromide PCl₃ phosphorus trichloride CsClO₄ cesium perchlorate CuSO₄ copper(II) sulfate
19	4.5 Naming Acids Some things when dissolved in water can lose an H⁺ right off them called acids taste sour know these! have their own name system…
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21	4.6 Writing Formulas from Names so far we’ve done formulas to names… now we do reverse! yippee! you HAVE TO KNOW all the names I warned you about!!!
22	examples potassium hydroxide KOH sodium carbonate Na₂CO₃ nitric acid HNO₃ calcium chloride CaCl₂ dinitrogen pentoxide N₂O₅ ammonium perchlorate NH₄ClO₄
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