2. Unit 3-Nomenclature

3. Nomenclature More than four million chemical compounds are currently known-memorizing common names for all these would be impossible Nomenclature-a system for naming compounds in which the name tells something about the composition of the compound NaOH Soda Lye CaSO 4 Plaster of Paris Milk of Magnesia Mg(OH) 2 N 2 O CaCO 3 Chalk NaHCO 3 Baking Soda Solution:

4. Naming Compounds Binary Compounds Binary compounds are compounds composed of two elements. Two Broad Classes of Binary compounds 1.Compounds that contain a metal and a nonmetal (Type I and Type II)“ionic compounds” 2. Compounds that contain two nonmetals (Type III) “molecular compounds”

5. Rules for Naming Type I Ionic Compounds 1. The cation is named first; the anion is named second 2.The cation takes it’s name from the name of the element (NAME THE CATION) 3.The anion takes the first part of the element name ( the root) and then add –ide Let’s PRACTICE: NaClMgCl 2 SrI 2 KFCsBrNa 2 S CaOLiHMgBr 2 AlCl 3 BaSZnCl 2 Ag 2 ORb 3 NCaS sodium chloride potassium floride calcium oxide aluminum chloride

6. Type II Binary Ionic Compounds This type of metal has more than one type of cation (these are the transition metals). EXAMPLES: Cr 2+ Cu 2+ Pb 2+ Cr 3+ Cu + Pb 4+ Fe 2+ Sn 2+ Ni 2+ Fe 3+ Sn 4+ Ni 3+ Chemists deal with this situation by using a Roman Numeral to specify the charge of the cation by including it in the name. 1 I 2 II 3 III 4 IV 5 V 6 VI

7. Rules for Naming Type II Ionic Compounds 1. Cation is named first; anion is named second 2. Because cation can assume more than one charge, the charge is specified by a Roman numeral in parentheses 3. The anion takes the first part of the element name (the root) and then add –ide Let’s PRACTICE : CuI 2 MnO 2 TiO 2 FeSCrOCrF 3 AuCl 3 SnI 4 Ni 2 O 3 Fe 2 O 3 CuClPbS 2 Cu 2 OFeBr 3 V3N5V3N5 copper (II) iodide iron (II) sulfide gold (III) chloride iron (III) oxide copper (I) oxide

8. REVIEW: Naming Compounds Binary Compounds Binary compounds are compounds composed of two elements. Two Broad Classes of Binary compounds 1.Compounds that contain a metal and a nonmetal (Type I and Type II)“ionic compounds” 2. Compounds that contain two nonmetals (Type III) “molecular compounds” DO NOT WRITE THIS YOU ALREADY HAVE IT IN YOUR NOTES

9. Rules for Naming Type III Binary Compounds 1. First element is named first, full name is used (2 nonmetals) 2. Second element is named as though it were anion, so it ends in -ide 3. Prefixes* are used to denote the # of atoms present * the prefix mono- is not used with the first element. Prefixes mono-1 di-2 tri-3 tetra-4 penta-5 hexa-6 hepta-7 octa-8 nona-9 deca-10 CONOCCl 4 CO 2 SF 6 BF 3 N2O5N2O5 P 4 O 10 H2OH2O P2O3P2O3 S 2 Cl 2 NH 3 Let’s PRACTICE : carbon monoxide carbon dioxide diphosphorus trioxide dinitrogen pentoxide nitrogen monoxide

10. College Prep Students must memorize all of the following polyatomic ions! Students must know the name, formula and the charge of the ion. You will use the other ions but you will have a chart to look them up! Honors Students must memorize all of the following polyatomic ions! Students must know the name, formula and the charge of the ion. Copyright © Houghton Mifflin Company.All rights reserved. 5–95–9 Honors Students must memorize all of the following polyatomic ions! Students must know the name, formula and the charge of the ion. NAMING COMPOUNDS WITH POLYATOMIC IONS Polyatomic ion- charged entities composed of several atoms bound together Polyatomic ions are assigned special names that you must memorize in order to name the compounds containing them(you must also know the charge of the ions)

11. Honors Students must memorize all of the following polyatomic ions! Students must know the name, formula and the charge of the ion. NH 4 + ammoniumOH - hydroxide NO 3 - nitratePO 4 3- phosphate NO 2 - nitriteCO 3 2- carbonate SO 4 2- sulfateClO 3 - chlorate SO 3 2- sulfiteC 2 H 3 O 2 - acetate Copyright © Houghton Mifflin Company.All rights reserved. 5–10 Honors Students must memorize all of the following polyatomic ions! Students must know the name, formula and the charge of the ion.

12. Naming Compounds with Polyatomic Ions Rules for Naming Compounds that contain Polyatomic Ions 1.If the polyatomic ion is paired with a Type I or Type II metal you follow the rules for naming binary compounds that also contain these metals and then you simply add the name of the polyatomic ion. 2.If there are two polyatomic ions simply name them in the order they appear. Let’s PRACTICE: Na 2 SO 3 Ca(NO 3 ) 2 Zn(CN) 2 Mn(OH) 2 MgSO 4 KMnO 4 NH 4 ClNaClO 3 Sn(C 2 H 3 O 2 ) 4 Cu 2 CrO 4 BaBrO 3 AgNO 2 NH 4 OHPbSO 4 Ca 3 (PO 4 ) 2 sodium sulfite manganese (II) hydroxide ammonium chloride copper (I) chromate

13. See if you can write-out the chemical formula for some of the ingredients in RED- Instant Noodle Soup (disregard the circled ingredients)

14. Naming Acids: The acid is considered as one or more H + ions attached to an anion.

15. Here are the names of a few acids that you need to memorize: HCl (hydrochloric acid) HNO 3 (nitric acid) CH 3 COOH or HC 2 H 3 O 2 (acetic acid) H 2 SO 4 (sulfuric acid)

16. Review: Naming Compounds No Polyatomic ion or ions present? YesNo Name the compound using procedures similar to those for naming binary compounds This is a compound for which naming procedures have not yet been considered. Is the metal a Type I or a Type II ?

17. Naming Acids Practice Let’s Practice HF HNO 3 HCl HBr H 2 SO 4 H 3 PO 4 HI HCN H 2 S HNO 2 H 2 SO 3 HC 2 H 3 O 2

18. Writing Formulas when given the name of the compounds using the Criss-Cross Method

19. Al Cl Example: Aluminum Chloride Step 1: Step 2: Step 3: Criss-Cross Rule for writing formulas from names Al Cl 3+1- write symbols & charge of elements criss-cross the numbers with the charges as subsrcipts combine as formula unit (“1” is never shown) 31 AlCl 3

20. Cu S Example: Copper (I)sulfide Step 1: Step 2: Step 3: Criss-Cross Rule for writing formulas from names Cu S 1+2- write symbols & charge of elements criss-cross the numbers with the charges as subsrcipts combine as formula unit (“1” is never shown) 12 Cu 2 S

21. NH 4 PO 4 Example: Ammonium Phosphate Step 1: Step 2: Step 3: Criss-Cross Rule for writing formulas from names NH 4 PO 4 1+ 3- write symbols & charge of elements criss-cross the numbers with the charges as subsrcipts combine as formula unit (“1” is never shown) 1 3 (NH 4 ) 3 PO 4 ( )

22. Rules for Parentheses Parentheses are used only when the following two conditions are met: 1.There is a radical (polyatomic ion) present and… 2.There are two or more of that radical in the formula. Examples: NaNO 3 NO 3 1- is a radical, but there is only one of it. Mg(NO 3 ) 2 NO 3 1- is a radical and there are two of them (NH 4 ) 2 SO 4 NH 4 1+ is a radical and there are two of them; SO 4 2- is a radical but there is only one of it. Mg(OH) 2 OH 1- is a radical and there are two of it. Al 2 (CO 3 ) 3 CO 3 2- is a radical and there are three of them. NaOH OH 1- is a radical but there is only one of it.