Chapter 4 Nomenclature BEWARE There is a lot

Chapter 4 Nomenclature BEWARE!!! There is a lot memorization involved with this chapter. 1

• 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!! 2

• 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 3 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 4

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) 5

Questions • Aluminum is a group 3 A metal. Which ion does Al typically form? a. Al 3 c. Al 5 b. Al 3+ d. Al 5+ 6

Type I Examples • • • Cs. F Cesium Fluoride Al. Cl 3 Aluminum Chloride Mg. I 2 Magnesium Iodide Ca. S Calcium Sulfide KI Potassium Iodide • • • Sodium Iodide Na. I Calcium Fluoride Ca. F 2 Lithium Oxide Li 2 O Aluminum Sulfide Al 2 S 3 Strontium Oxide Sr. O 7

Type I Binary ionic compounds • Reviewing the rules: 8

Question • What type of ions have names ending in ide? a. only cations c. only metal ions b. only anions d. only gaseous ions 9

Questions • What is the correct name for the N 3 - ion? a. nitrate ion c. nitride ion b. nitrogen ion d. nitrite ion 10

Questions • Which of the following formulas represents an ionic compound? a. CS c. NO b. Ba. I d. PCl 11

Questions • Which element, when combined with fluorine, would most likely form an ionic compound? a. lithium c. phosphorus b. carbon d. chlorine 12

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? Fe 2+ or Fe 3+? • must be a way to distinguish the two! • use Roman numerals… 13

• So what is the name of Fe. Cl 2? • 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!!) 14

• • • Cu. Cl copper(I) chloride Hg. O mercury(II) oxide Fe 2 O 3 iron(III) oxide Mn 2 O 4 manganese(IV) oxide Pb. Cl 4 lead(IV) chloride examples 15

• • • Fe. I 3 iron(III) iodide Mn. Cl 2 manganese(II) chloride Hg. O mercury(II) oxide Cu 2 O copper(I) oxide Cu. O copper(II) oxide examples 16

• summary of Type I and Type II 17

Questions • What is the correct name for the compound Co. Cl? a. cobalt(I) chlorate c. cobalt(II) chlorate b. cobalt(I) chloride d. cobalt(II) chloride 18

Questions • In which of the following is the name and formula given correctly? a. sodium oxide, Na. O c. cobalt (I) chloride, Co. Cl b. barium nitride, Ba. N d. tin (IV) fluoride, Sn. F 4 19

Questions • Which of the following compounds contains the Mn 3+ ion? a. Mn. S c. Mn 2 O 3 b. Mn. Br 2 d. Mn. O 20

summary examples • • Co. Br 2 cobalt(II) bromide Ca. Cl 2 calcium chloride Al 2 O 3 aluminum oxide Cr. Cl 3 chromium(III) chloride 21

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) 22

23

• • • BF 3 boron trifluoride NO nitrogen monoxide N 2 O 5 dinitrogen pentoxide PCl 5 phosphorus pentachloride SF 6 sulfur hexafluoride SO 2 sulfur dioxide examples 24

• • • sulfur trioxide SO 3 dinitrogen trioxide N 2 O 3 silicon dioxide Si. O 2 dioxygen diflouride O 2 F 2 tetraphosphorus hexoxide P 4 O 6 xenon hexaflouride Xe. F 6 examples 25

Questions • Which of the following formulas represents a molecular compound (molecular means between two non-metals)? a. Zn. O c. SO b. Xe d. Be. F 26

Questions • Select the correct formula for sulfur hexafluoride. a. S 2 F 6 c. F 6 S 2 b. FSO d. SF 6 27

4. 3 naming binary compounds: a review 28

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 29

• Cl. O 3– chlorate -ate • THE ROOT, MOST IMPORTANT! • SO 42– sulfate • PO 43– phosphate • NO 3– nitrate • CO 32– carbonate • NOTICE TRENDS ON THE PT • Subtle but helpful • Charge – 1 -2 -3 -1 -2 • Oxygens – 3 -4 -4 -3 -3 30

-ite • • • Cl. O 3 - Cl. O 2 chlorite SO 42 - SO 32 sulfite NO 3 - NO 2 nitrite • Minus 1 Oxygen • Same Charge 31

Hypo • Cl. O 3 - Cl. O 2 - Cl. O • hypochlorite • Minus one more oxygen from the –ite • Charge still the same • Think hypo is the opposite of hyper – Hyper = more – Hypo = less 32

per • • • Cl. O 4 - Cl. O 3 - Cl. O 2 - Cl. O- • Per means we add an oxygen perchlorate Mn. O 4 • Bottom two just permanganate need to 2 O 2 memorize peroxide 33

hydrogen ___ • • HPO 42 hydrogen phosphate H 2 PO 4 dihydrogen phosphate HCO 3 hydrogen carbonate HSO 4 hydrogen sulfate • Just add the name hydrogen to the beginning of the name • Adding hydrogen decreases the overall charge by 1 34

Some more -ates • • • Cr. O 42 chromate Cr 2 O 72 dichromate C 2 H 3 O 2 Acetate • There is no rhyme or reason to these. You just have to know them. – aka CH 3 COO 35

Few More Outliers • • • OHhydroxide (VERY IMPORTANT!!!) CNcyanide NH 4+ ammonium 36

• Na 2 SO 4 • sodium sulfate • Fe(NO 3)3 examples – parentheses here mean there are 3 of what’s inside. “NO 33” is nonsense! • iron(III) nitrate • Mn(OH)2 • manganese(II) hydroxide 37

summary examples • Na 2 CO 3 • sodium carbonate • Fe. Br 3 • iron(III) bromide • PCl 3 • phosphorus trichloride • Cs. Cl. O 4 • cesium perchlorate • Cu. SO 4 • copper(II) sulfate 38

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. 39

When dissolved in water, acids produce ____. a. negative ions c. hydrogen ions b. polyatomic ions d. oxide ions 40

• • -ide ending(no oxygen) Hydro – root – ic HF hydrofluoric acid HCl hydrochloric acid HBr hydrobromic acid HI hydroiodic acid • • HCN hydrocyanic acid H 2 S hydrosulfuric acid 41

• • • -ate ending root-ic (with oxygen) Cl. O 3 - HCl. O 3 chlorate chloric acid • Notice, the number of SO 42 - H 2 SO 4 hydrogens sulfate sulfuric acid added is the 3 - H PO PO 4 3 4 same as the phosphate phosphoric acid number of the NO 3 - HNO 3 charge. nitrate nitric acid CO 32 - H 2 CO 3 42 carbonate carbonic acid

-ite ending root-ous • • • Cl. O 2 - HCl. O 2 • Once again, notice the charges balance out chlorite chlorous acid with the Hydrogens 2 - H SO SO 3 2 3 sulfite sulfurous acid NO 2 - HNO 2 nitrite nitrous acid 43

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. 44

45

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!!! 46

examples • • • potassium hydroxide KOH sodium carbonate Na 2 CO 3 nitric acid HNO 3 calcium chloride Ca. Cl 2 dinitrogen pentoxide N 2 O 5 ammonium perchlorate NH 4 Cl. O 4 47

if this helps, use it. if it doesn’t, don’t! 48