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Ionic Compounds

Ionic Compounds. Lewis Dot Diagrams Chemical Interactions Occur between the Valence Electrons. Dots : represent valence electrons. When atoms combine to make molecules, they form chemical bonds. Valence electron interaction. Forming Chemical Bonds. Octet Rule Atoms will form bonds by:

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Ionic Compounds

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  1. Ionic Compounds

  2. Lewis Dot DiagramsChemical Interactions Occur between the Valence Electrons Dots: represent valence electrons

  3. When atoms combine to make molecules, they form chemical bonds. Valence electron interaction

  4. Forming Chemical Bonds • Octet RuleAtoms will form bonds by: • Sharing • Giving or • Taking electrons to complete their octet Higher energy farther away from nucleus

  5. Atoms form ions to have stable electron configurations (similar to noble gases) hh

  6. Ionic Bonds • Ionic Bonds form when one atom (nonmetal) gains electrons and the other atom (metal) loses electrons in order to gain stability.

  7. Ionic Bonds form between a metal (cation) and a nonmetal (anion).

  8. To form an ion, lithium will most likely: • Gain 1 electron • Gain 2 electrons • Lose 1 electron • Lose 2 electrons

  9. Forming Chemical Bonds • Lithium • Better to lose 1 electron or to gain 7 electrons? X

  10. Therefore, as an ion lithium will have what charge? • 1+ • 2+ • 1- • 2-

  11. Ionic Bonds • Atoms gain or lose its electrons + NaCl - salt

  12. Chemical Interactions Occur between the Valence Electrons Lewis structures are simpler to do & see

  13. Formation of MgCl2

  14. Formation of Na2S

  15. Write down the chemical formula for Aluminum Flouride

  16. Formation of AlF3

  17. Today is a practice Day! • We need to be able to name ions given chemical formula • We need to be able to determine the chemical formula given the name

  18. Valence Electrons Noble Gas Structure = Octet 1,2 3,4,5,6,7,8

  19. IONIC BONDS / Cations and Anions Cation – positive ions Transition Metals use Roman Numerals to tell you the ox # Anion – negative ions

  20. Oxidation Numbers • Oxidation Numbers - indicated # of e’ lost, gained or shared. Ex. Oxidation number of chlorine is -1

  21. Halogens will have an oxidation number of: • +1 • +2 • -1 • -2

  22. Alkaline earth metals will have an oxidation number of: • +1 • +2 • -1 • -2

  23. We will name binary compounds together • Using pages 156- 158 • Describe how to name cations and anions when they are by themselves

  24. Naming Binary Ionic Compounds • Write the name of the ionic compound, Ca2N3. • Write the name of the ionic compound, K2O.

  25. What is the name of BeBr2? • Boron bromine • Beryllium bromine • Bromide beryllide • Beryllium bromide • Beryllide bromide

  26. Metals with Variable Charges • Many transition metals can form more than one type of cation. • For this reason, you must show the oxidation number in the name using Roman Numerals

  27. Naming Binary Ionic Compounds with Transition Metal Cations • Write the name of the ionic compound, Cu2O.. • Write the name of the ionic compound, NiS.

  28. What is the name for SnBr2? • Bromide Tin • Tin Bromide • Tin (I) Bromide • Tin (II) Bromide • Tin (III) Bromide • Tin (IV) Bromide

  29. What is the name for FeI3? • Iron iodide • Iron (I) iodide • Iron (II) iodide • Iron (III) iodide

  30. What is the name for MnS? • Manganese sulfide • Manganese (I) sulfide • Manganese (II) sulfide • Manganese (III) sulfide

  31. Exceptions: • Some of the transition metals have only one ionic charge: • Do not need to use roman numerals for these: • Silver is always 1+ (Ag1+) • Cadmium and Zinc are always 2+ (Cd2+ and Zn2+)

  32. Writing Formulas for Binary Ionic Compounds • Write the formula for barium iodide. • Write the formula for sodium oxide. • Write the formula for aluminum nitride. • Write the formula for copper (I) sulfide.

  33. Criss-Cross Method for Writing Formulas- You can write the oxidationnumber and criss-cross them as subscripts.- Note – if not in lowest termsyou must reduce the subscripts(ex. Magnesium oxide) Al3+ S2- 2 3 = Al2S3

  34. What is the formula for aluminum bromide? • AlBr • AlBr2 • Al3Br • Br3Al • AlBr3

  35. What is the formula for magnesium oxide? • MgO • Mg2O2 • MgO2 • Mg2O • OMg

  36. Write the formula for titanium (II) chloride. • TiCl • Ti2Cl • TiCl2 • Ti2Cl2

  37. Write the formula for tin (IV) oxide. • SnO • SnO4 • SnO2 • Sn4O • Sn2O

  38. POLYATOMIC IONS • Not all compounds are made of only 2 types of atoms • poly – “many” Memorize the polyatomic ions from p. 170.

  39. Tricks for Polyatomic Naming Perchlorate per+root+ate ClO4-1 chlorate root+ate ClO3-1 chlorite root+ite ClO2-1 Hypochlorite hypo+root+ite ClO-1 Prefixes and suffixes designate number of oxygens

  40. Naming Polyatomic Ionic Compounds • Polyatomic ionic compounds are named just like binary ionic compounds. • Exception: be sure to enclose the polyatomic ion in parentheses before writing the subscript (only necessary if subscript is not 1). • Ex. Barium hydroxide = Ba(OH)2

  41. Write the formula for Calcium Nitrate. • CaNO2 • Ca(NO2)2 • Ca2NO3 • Ca2NO2 • Ca(NO3)2

  42. Write the formula for Magnesium Phosphate. • MgPO4 • Mg3(PO4)2 • Mg4(PO3)2 • MgPO3 • Mg(PO4)2

  43. Naming Ionic Compounds

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