BEWARE!!! There is a lot memorization involved with this chapter. Chapter 4 Nomenclature BEWARE!!! There is a lot memorization involved with this chapter.

SHORT CHAPTER VERY IMPORTANT CHAPTER THE REST OF THE YEAR YOU WILL BE EXPECTED TO KNOW THE CHEMICAL NAMES! If you have a photographic memory this chapter will be a breeze BUY FLASHCARDS!!

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

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

Type I Compounds Type I & Type II is referring to the cation Type I cations only have 1 charge! First 2 rows of the periodic table NOTE – ALUMINUM(+3) AND SILVER(+1)

Questions Aluminum is a group 3A metal. Which ion does Al typically form? a. Al3- c. Al5- b. Al3+ d. Al5+

Type I Examples CsF Cesium Fluoride AlCl3 Aluminum Chloride MgI2 Magnesium Iodide CaS Calcium Sulfide KI Potassium Iodide Sodium Iodide NaI Calcium Fluoride CaF2 Lithium Oxide Li2O Aluminum Sulfide Al2S3 Strontium Oxide SrO

Type I Binary ionic compounds Reviewing the rules:

Question What type of ions have names ending in -ide? a. only cations c. only metal ions b. only anions d. only gaseous ions

Questions What is the correct name for the N3- ion? a. nitrate ion c. nitride ion b. nitrogen ion d. nitrite ion

Questions Which of the following formulas represents an ionic compound? a. CS c. NO b. BaI d. PCl

Questions Which element, when combined with fluorine, would most likely form an ionic compound? lithium c. phosphorus b. carbon d. chlorine

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…

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!!)

examples CuCl copper(I) chloride HgO mercury(II) oxide Fe2O3 iron(III) oxide Mn2O4 manganese(IV) oxide PbCl4 lead(IV) chloride

examples FeI3 iron(III) iodide MnCl2 manganese(II) chloride HgO mercury(II) oxide Cu2O copper(I) oxide CuO copper(II) oxide

summary of Type I and Type II

Questions What is the correct name for the compound CoCl? a. cobalt(I) chlorate c. cobalt(II) chlorate b. cobalt(I) chloride d. cobalt(II) chloride

Questions  In which of the following is the name and formula given correctly? a. sodium oxide, NaO c. cobalt (I) chloride, CoCl b. barium nitride, BaN d. tin (IV) fluoride, SnF4

Questions Which of the following compounds contains the Mn3+ ion? a. MnS c. Mn2O3 b. MnBr2 d. MnO

summary examples CoBr2 cobalt(II) bromide CaCl2 calcium chloride Al2O3 aluminum oxide CrCl3 chromium(III) chloride summary examples

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)

examples BF3 boron trifluoride NO nitrogen monoxide N2O5 dinitrogen pentoxide PCl5 phosphorus pentachloride SF6 sulfur hexafluoride SO2 sulfur dioxide examples

examples sulfur trioxide SO3 dinitrogen trioxide N2O3 silicon dioxide SiO2 dioxygen diflouride O2F2 tetraphosphorus hexoxide P4O6 xenon hexaflouride XeF6 examples

Questions Which of the following formulas represents a molecular compound (molecular means between two non-metals)? a. ZnO c. SO b. Xe d. BeF

Questions Select the correct formula for sulfur hexafluoride. a. S2F6 c. F6S2 b. FSO d. SF6

4.3 naming binary compounds: a review

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

-ate ClO3- SO42- PO43- NO3- CO32- THE ROOT, MOST IMPORTANT! chlorate SO42- sulfate PO43- phosphate NO3- nitrate CO32- carbonate THE ROOT, MOST IMPORTANT! NOTICE TRENDS ON THE PT Subtle but helpful Charge 1-2-3-1-2 Oxygens 3-4-4-3-3

-ite ClO3-  ClO2- chlorite Minus 1 Oxygen SO42-  SO32- Same Charge sulfite NO3-  NO2- nitrite Minus 1 Oxygen Same Charge

Hypo- ClO3-  ClO2-  ClO- hypochlorite Minus one more oxygen from the –ite Charge still the same Think hypo is the opposite of hyper Hyper = more Hypo = less

per- ClO4-  ClO3-  ClO2-  ClO- perchlorate MnO4- permanganate O22- peroxide Per means we add an oxygen Bottom two just need to memorize

hydrogen ___ HPO42- hydrogen phosphate H2PO4- dihydrogen phosphate HCO3- hydrogen carbonate HSO4- hydrogen sulfate Just add the name hydrogen to the beginning of the name Adding hydrogen decreases the overall charge by 1

Some more -ates CrO42- chromate Cr2O72- dichromate C2H3O2- Acetate aka CH3COO- There is no rhyme or reason to these. You just have to know them.

Few More Outliers OH- hydroxide (VERY IMPORTANT!!!) CN- cyanide NH4+ ammonium

examples Na2SO4 sodium sulfate Fe(NO3)3 iron(III) nitrate Mn(OH)2 parentheses here mean there are 3 of what’s inside. “NO33” is nonsense! iron(III) nitrate Mn(OH)2 manganese(II) hydroxide examples

summary examples Na2CO3 sodium carbonate FeBr3 iron(III) bromide PCl3 phosphorus trichloride CsClO4 cesium perchlorate CuSO4 copper(II) sulfate

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… All acids are named based on their anion ending.

When dissolved in water, acids produce ____. a. negative ions c. hydrogen ions b. polyatomic ions d. oxide ions

-ide ending(no oxygen) Hydro – root – ic HF hydrofluoric acid HCl hydrochloric acid HBr hydrobromic acid HI hydroiodic acid HCN hydrocyanic acid H2S hydrosulfuric acid

-ate ending root-ic (with oxygen) ClO3-  HClO3 chlorate  chloric acid SO42-  H2SO4 sulfate  sulfuric acid PO43-  H3PO4 phosphate  phosphoric acid NO3-  HNO3 nitrate  nitric acid CO32-  H2CO3 carbonate  carbonic acid Notice, the number of hydrogens added is the same as the number of the charge.

-ite ending root-ous ClO2-  HClO2 chlorite  chlorous acid SO32-  H2SO3 sulfite  sulfurous acid NO2-  HNO2 nitrite  nitrous acid Once again, notice the charges balance out with the Hydrogens

Questions Compared with acids that have the suffix -ic, acids that have the suffix -ous contain a. more hydrogen. c. less oxygen. b. more oxygen. d. the same amount of oxygen.

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!!!

examples potassium hydroxide KOH sodium carbonate Na2CO3 nitric acid HNO3 calcium chloride CaCl2 dinitrogen pentoxide N2O5 ammonium perchlorate NH4ClO4 examples

if this helps, use it. if it doesn’t, don’t!