Name our Date What is bonding? Unit 8: Ionic Compounds Notes and Practice that hold atoms together to form compounds. Positive Ion Formation tend to valence e-. A charged ion is called a. Ex. Na o will lose o Na + Negative Ion Formation tend to valence e-. A charged ion is called an. Ex. S o will gain o S 2- Ionic Size Cations are always than the atoms from which they formed o Fewer electrons so the protons can pull the electrons closer Anions are always than the atoms from which they form o More electrons and the same number of protons Ionic Bonds atoms will electrons to atoms, causing both to become ions. An is the force of attraction that holds together in. 1
Formulas for Ionic Compounds The chemical formula for an ionic compound is called a and represents the of the ions in a compound. Ionic compounds are (charge = )!! The tell chemists how many of each are present in the compound. o Example: means aluminum atoms and sulfur atoms in one formula unit. ow to write ionic formulas: 1. Write the for each ion and its 2. the charges with o Total charge of must = total charge of o Criss-cross or swap 3. Re-write the without any. o Metal (cation) is ALWAYS and the nonmental (anion) is. Write the formula for 1. Calcium iodide 2. Potassium phosphide Naming Ionic Compounds Name the metal (cation) and name the nonmetal (anion), changing the ending to ide Name the following ionic compounds 1. NaF Transition Metal Ionic Compounds 2. Al2O3 Transition metals form cations. Different results in different and different. A is used to indicate the of a metal that forms multiple cations. o Iron is commonly found as both, which is called and, called. o is called & is called. Write the formula for: 1. Iron (II) Oxide 2. Cobalt (II) Iodide 3. Vandium (III) Oxide
Naming You must write a roman numeral in after the of the to show the charge on the. Exceptions: o is always a ion o is always a ion o and can be a or ion. DON T need Roman Numerals MUST have Roman Numerals MEMORIZE TEM!!!! Name the following compounds 1. NiCl2 4. Co3P2 2. CuS 5. PbO2 3. Cu3N Determine the cation and anion of the formula. YES Does the cation have only one charge? NO Write the name of the cation, then the name of the anion. Write the name of the cation followed by a roman numeral to represent the charge. Next write the name of the anion.
Polyatomic Ion Compounds Polyatomic ions are Charge applies to the Acts as an ion in a compound Polyatomic Ions Name Formula Particle Diagram Name Formula Particle Diagram Ammonium N Nitrate O Carbonate O C O Nitrite Chlorate Cl Phosphate P Cyanide Sulfate S ydroxide Sulfite Formula Writing NEVER subscripts of the atoms the poly NEVER the poly If poly is needed, place parentheses the ion and a subscript Example: N4 + and O 2- Naming Example: NaO
Properties of Ionic Compounds, rigid, - as solids Conduct electricity when (aqueous solution) o A substance will conduct electricity if it has. o Ionic solids have a structure, however, when dissolved in water, the ions and are mobile allowing the conduction of electricity. Ionic solids have melting and boiling points due to the attraction between the (+) and (-) ions. o The the temperature, the the force of attraction. o ions are together than larger ions producing a attraction. Ex: KBr vs. NaCl o charges have a attraction. Ex: NaBr vs. MgO Practice Ionic formulas and names for binary (2 types of atomic) ionic compounds with metals that only form 1 ion 1. LiF 2. lithium chloride 3. BBr3 4. aluminum chloride 5. Li3P 6. beryllium fluoride 7. BeO 8. Aluminum sulfide 9. BCl3 10. lithium nitride 11. Na2S 12. boron oxide 13. AlN 14. Beryllium sulfide
Ionic formulas and names for binary ionic compounds with metals that form multiple ions 15. CuCl2 16. copper (I) chloride 17. Cu2O 18. tin (IV) oxide 19. Cu3N 20. copper (II) nitride 21. SnSe 22. copper (II) oxide 23. PbF4 24. lead (II) fluoride 25. PbS 26. lead (IV) sulfide 27. Pb3N4 28. chromium (VI) phosphide 29. FeF3 30. iron (II) bromide 31. Fe2O3 32. lead (IV) oxide Ionic formulas and names for ionic compounds containing polyatomic ions 33. N4Cl 34. beryllium chlorate 35. LiClO3 36. barium nitrate 37. BeSO4 38. aluminum hydroxide 39. CaSO3 40. calcium sulfate 41. (N4)3N 42. calcium phosphate 43. N4NO3 44. cesium cyanide 45.N4NO2 46. sodium nitrate 47. Sr3(PO4)2 48. sodium nitrite 49. KClO3 50. calcium carbonate Polyatomic Ions Chlorate Cyanide Nitrate ydroxide Sulfate ClO3 - CN - NO3 - O - SO4 2- Carbonate Ammonium Nitrite Phosphate Sulfite CO3 2- N4 + NO2 - PO4 3- SO3 2-