\begin{tabular}{l} EXAMPLES: \( \begin{array}{ll}\text { Na } & \text { No chatge }=\operatorname{atom} ightarrow \text { sodium atom_- } \\ \mathrm{Na}^{*} & \text { charge and an "A metal } ightarrow \text { sodum ion_ } \\ \mathrm{Cu} & \text { No charge }=\text { atom } ightarrow \text { Copper atom } \\ \mathrm{Cu} & \text { charge and a "B" metal } ightarrow \text { copper(I) ion }\end{array} \) \\ \hline \end{tabular} (2) Ca2+ 3. K 4. K= 5. Birium atom 6. Banum ion 7. Ee? 8. Fer 9. Iran (IV) ton 10. ifon (III) ion 11. magnesium ion 12. magencatuts atora: A2: Naming Nommetal Atoms and lons (Monatomic and Polvatomic ions): EXAMPLES: O No charge = atom oxygen atom O O2. charge =ion oxide ion NO2Polyatomic ion-Use polyatomic ion table (more than one element in a "charged" group nitrite ion 13. O 14. N3. 15. N 16. PO43. 17. P3 18. OH 19. PO33 20. CO32 21. HCO3 - 22. SO42 23. SO32 ** Name Formula (-ide ending means ion is from PT (exception hydroxide OHis a polyatomic ion) /-ate or-ite means it's a Polyatomic ion- use table) 24. Sulfide ion 25. Sulfate ion 26. Chlorine atom 27. Chloride ion 28. Phosphide ion 29. Phosphate ion 30. Nitrate ion 31. Nitrite ion Part B: Naming lonic Compounds (Metal ion/Nonmetal ion) Ionic compounds are made up of a metal ion (+) and a nonmetal ion(-) The motals (tions), "A" and "B" metals, The nonmetals (- ions) Remember from part A that there are The two types of nonmetals are Monatomic ions and Polyatomic ions (Use table provided). B1. Given the Molecular Formula, Name the lonic Compound - To do this, you will first Name the Metal ion and then name the nonmetal - After you have the named in part A of this lab. put the names together for the metal ion and name of the nonmetal ion both the metal and the for the compound leaving out the words "ion" on Example: MgCl2 Metal ion: Magnesium ion I Nonmetal: Chloride ion Put names together Magnesium Chloride 32. NaF 34. CaSO4 35. Cu2S3 36. MnO2 37. Fe(NO2)3 38. LiBr 39. Cu3N 40.FeBr 41. KCl 42. Pb(SO4)2 43. Be(HCO3)2 44. Na2CO3 45. Al(OH)3 B2. Given the Name of the lonic Compound, Determine the Molecular Formula: Since Ionic compounds are neutral compounds, the sum of the (+) and () charges must add to zero. One method to achieve this is the use the Criss Cross / Reduce method: 1. Using the periodic table, write the symbol of the metal with is charge, and the symbol of the nonmetal with its charge. 2. Apply Criss Cross/ Reduce Method: Move the value of the charge (not the sign of the charge + or ) of the metal to the subscript of the nonmetal and the value of the charge of the nonmetal to the subscript of the metal as illustrated below: Example : Write the Formula for: copper (ii) fluoride 1. Write the symbol of each ion from the given name: copper (II) is Cu2 fluoride is F1. 2. CrissCross/ Reduce: Take the value of 2 from Cu and put it as a subscript on F to make F2. Next, take the value of 1 from F and put as a subscript on Cu1. The Formula is then Cu1F2 Reducing is not required. Example: Write the Formula for. Potassium Phosphide 1. Symbols with Charges: K+P3 2. Criss Cross/Reduce: K3P (reducing not required) Example: Write the Formula for: manganese (IV) carbonate 1. Symbols with charges 2. Use Criss cross/Reduce: Mn4 and CO22Mn2(CO2) t and then reduce (is possible here) Mn (COO) 46. lead (II) oxide 47. cobalt (III) hydroxide 48. iron (II) carbonate 49. sodium sulfate 50. calcium phosphide 51. aluminum iodide 52. lead (II) nitride 53. aluminum nitride