1. 1 Ions Ions: A charged particle formed when a neutral atom or group of atoms gain or lose one or more electrons. Example Na  Na + + e - F + e -  F -

2. 2 Cations Mg  Mg 2+ + 2e - Al  Al 3+ + 3e - Cation: A positively-charged ion. One or more electrons are lost from a neutral atom  oxidation

3. 3 Anions I + e -  I - O + 2e -  O 2- O + 2e -  O 2- S + 2e -  S 2- S + 2e -  S 2- Anion: A negatively-charged ion. Electrons are gained by a neutral atom  reduction

4. 4 Ions Ion charges can be predicted from the Periodic Table Ion charges can be predicted from the Periodic Table Main Group metal (IA-IVA) ion-charges correspond to group number Main Group metal (IA-IVA) ion-charges correspond to group number Sodium (Na) in IA  +1 Sodium (Na) in IA  +1 Main Group non-metal (IIIA-VIIIA) ion-charges correspond to (group# - 8) Main Group non-metal (IIIA-VIIIA) ion-charges correspond to (group# - 8) Fluorine (F) in VIIA  (7-8) = -1 Fluorine (F) in VIIA  (7-8) = -1 All this has to do with electron configuration All this has to do with electron configuration See website as well: http://web.clark.edu/aaliabadi/phSC106_ions%20shee t.htm See website as well: http://web.clark.edu/aaliabadi/phSC106_ions%20shee t.htm http://web.clark.edu/aaliabadi/phSC106_ions%20shee t.htm http://web.clark.edu/aaliabadi/phSC106_ions%20shee t.htm

5. 5 Compounds That Contain Ions  Require metal and non-metal  Form ionic bonds  Called an ionic compound Characteristic Properties 1. Very high melting points 2. Conduct an electric current when melted or when dissolved in water

6. 6 Ionic compound The number of cations and anions must have a net charge of zero. The number of cations and anions must have a net charge of zero.

7. 7 Compounds that Contain Ions Writing Formulas for Ionic Compounds Give the formulas for the compounds that contain the following pairs of ions: (a) K and I (b) Mg and N

8. 8 Naming Ionic Compounds 1. The cation is always named first and the anion second. 2. The cation takes its name from the name of the element. 3. The anion is named by taking the first part of the element name and adding –ide.

9. 9 Naming Ionic Compounds Name the following Type I compounds NaCl NaCl RaBr 2 RaBr 2 Rb 2 O Rb 2 O AlI 3 AlI 3 K 3 N K 3 N Cs 4 Si Cs 4 Si Give the chemical formula for the following Type I compounds Strontium phosphide Strontium phosphide Calcium fluoride Calcium fluoride Beryllium carbide Beryllium carbide Lithium hydride Lithium hydride Barium sulfide Barium sulfide Magnesium telluride Magnesium telluride

10. 10 Naming Ionic Compounds Type II compounds need to be identified by a Roman numeral  (I), (IV), etc. Type II compounds need to be identified by a Roman numeral  (I), (IV), etc. Represents oxidation state of cation Represents oxidation state of cation Not how many cations are present in compound! Not how many cations are present in compound! Example: NaCl  sodium (I) chloride is INCORRECT Example: NaCl  sodium (I) chloride is INCORRECT Example: SnCl 4  tin (IV) chloride is correct Example: SnCl 4  tin (IV) chloride is correct

11. 11 Naming Ionic Compounds Type II Ionic Compounds FeCl 2 and FeCl 3 PbO and PbO 2 MnS and Mn 2 S 7

12. 12 A Mixed Bag PbBr 2 and PbBr 4 PbBr 2 and PbBr 4 Aluminum arsenide Aluminum arsenide FeS and Fe 2 S 3 FeS and Fe 2 S 3 Thallium (III) boride Thallium (III) boride Mercury (II) carbide Mercury (II) carbide Na 2 S Na 2 S CoCl 3 CoCl 3 Cerium (IV) phosphide Cerium (IV) phosphide ScF 3 ScF 3 Gold (I) selenide Gold (I) selenide Vanadium (V) telluride Vanadium (V) telluride

13. 13 Naming Compounds that Contain Polyatomic Ions Polyatomic Ion: An ion that contains more than one atom. They are charged entities composed of several atoms bound together. Consult my website for the list: Consult my website for the list: http://web.clark.edu/aaliabadi/phSC106_ions% 20sheet.htm http://web.clark.edu/aaliabadi/phSC106_ions% 20sheet.htm

14. 14 Caveat Parenthesis required if more than one polyatomic ion present Parenthesis required if more than one polyatomic ion present Ca(ClO) 2 is correct Ca(ClO) 2 is correct Ca(I) 2 is INCORRECT Ca(I) 2 is INCORRECT

15. 15 Naming Compounds that Contain Polyatomic Ions Name or provide the chemical formula for each of the following compounds: (a) Ca(OH) 2 (e) Co(ClO) 2 (b) Sodium phosphate (f) platinum (IV) bicarbonate (c) KMnO 4 (g) Cu(NO 2 ) 2 (d) Ammonium nitrate (h) nickel (III) oxide

16. 16 Naming Compounds that Contain Polyatomic Ions Name or provide each of the following compounds: Name or provide each of the following compounds: (a) calcium carbonate (e) MoO (b) BaSO 4 (f) Iridium (VII) acetate (c) CsClO (g) ZnCl 2 (d) Zirconium sulfite (h) lithium cyanide

17. 17 Naming Acids Acids: A substance that yields hydrogen ions (protons, H + ) when dissolved in water. HCl (aq)  H + (aq) + Cl - (aq) HCl (aq)  H + (aq) + Cl - (aq) H 3 PO 4(aq)  3H + (aq) + PO 4 3- (aq) H 3 PO 4(aq)  3H + (aq) + PO 4 3- (aq)

18. 18 Rules for naming acids If the formula does not contain oxygen the prefix of the acid is hydro and the suffix –ic is attached to the root name for the element. If the formula does not contain oxygen the prefix of the acid is hydro and the suffix –ic is attached to the root name for the element. Ex: HCl = hydrochloric acid, H 2 S = hydrosulfuric acid Ex: HCl = hydrochloric acid, H 2 S = hydrosulfuric acid When the anion contains oxygen, the acid name is formed from the anion name. The suffix –ic or –ous is added. When the anion contains oxygen, the acid name is formed from the anion name. The suffix –ic or –ous is added. When the anion ends in –ate, the suffix –ic is used. When the anion ends in –ate, the suffix –ic is used. H 2 CO 3 = carbonic acid H 2 CO 3 = carbonic acid When the anion ends in –ite, the suffix –ous is used. When the anion ends in –ite, the suffix –ous is used. H 2 SO 3 = sulfurous acid H 2 SO 3 = sulfurous acid

19. 19 Naming Compounds that Contain Only Nonmetals: Type III Compounds containing only nonmetals: Compounds containing only nonmetals: Form covalent bonds Form covalent bonds share electrons share electrons Rules for Naming Type III Binary Compounds 1. The first element in the formula is named first, and the full element name is used. 2. The second element is named as though it were an anion. 3. Prefixes are used to denote the numbers of atoms present. 4. The prefix mono- is never used for naming the first element. 5. Drop the “a” when it is followed by an “o”  Tetraoxide should be tetroxide

20. 20 Naming Compounds that Contain Only Nonmetals: Type III Prefixes Used to Indicate Numbers in Chemical Names Prefix Number Indicated Prefix Number Indicated mono- 1 mono- 1 di- 2 di- 2 tri- 3 tri- 3 tetra- 4 tetra- 4 penta- 5 penta- 5 hexa- 6 hexa- 6 hepta- 7 hepta- 7 octa- 8 octa- 8 nona- 9 nona- 9 deca- 10 deca- 10

21. 21 Practice CCl 4 CCl 4 Silicon dioxide Silicon dioxide NO 2 NO 2 Sulfur trioxide Sulfur trioxide P 2 O 5 P 2 O 5 Iodine pentafluoride Iodine pentafluoride Dinitrogen tetroxide Dinitrogen tetroxide SeI 2 SeI 2 Xenon hexafluoride Xenon hexafluoride

22. 22 The Name Game Extra credit opportunity Extra credit opportunity Mix-and-match Mix-and-match