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Writing and Naming Ionic Compounds

Writing and Naming Ionic Compounds. Chapter 8 Part II. Writing Chemical Formulas. 1) Write the symbol for the elements and their oxidation number , positive ion first (the metal). Ex: For a compound of Magnesium and Chlorine. Mg. +2. -1. Cl. Writing Chemical Formulas.

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Writing and Naming Ionic Compounds

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  1. Writing and Naming Ionic Compounds Chapter 8 Part II

  2. Writing Chemical Formulas 1) Write the symbol for the elements and their oxidation number, positive ion first (the metal). Ex: For a compound of Magnesium and Chlorine Mg +2 -1 Cl

  3. Writing Chemical Formulas 2) Criss-cross the numbers and write them as subscripts without the signs. Mg +2 2 -1 1 Cl

  4. Writing Chemical Formulas 3) If there is a one charge, do not write it. Mg1Cl2 MgCl2

  5. Writing Chemical Formulas 4) If you have subscripts that are multiples, reduce them down. +4 4 -2 2 Pb O 1 2

  6. Naming Non-variable Ionic Compounds For ionic compounds where the metal always has the same oxidation number, 1) Name the metal. Ex: BaBr2 Barium

  7. Naming Non-variable Ionic Compounds For ionic compounds where the metal always has the same oxidation number, 2) Write the name of the non-metal, and change the end to –ide. Ex: BaBr2 Barium ine brom ide

  8. Naming Binary Non-variable Compounds • Name the positive ion • Name the negative ion changing the ending to -ide. • AlBr3 Aluminum bromide 3. No Roman numeral is needed

  9. -ides N – Nitrogen >>> Nitride O – Oxygen >>> Oxide F - Fluorine >>> Fluoride P - Phosphorus >>> Phosphide S - Sulfur >>> Sulfide Cl – Chlorine >>> Chloride Br - Bromine >>> Bromide I – Iodine >>> Iodide

  10. Naming Polyatomic Non-variable Compounds • Name the positive ion • Name the negative ion changing the ending to -ate. AlPO4 Aluminum Phosphate No Roman numeral is needed

  11. Naming Ionic Compounds If there is a polyatomic anion, then you do not change the ending: Ex: Ca(NO3)2 Calcium nitrate

  12. Name These: Na2O _________ MgCl2 _________ Na2CO3 _________ Sodium Oxide Magnesium Chloride Sodium Carbonate

  13. If a positive ion (a metal) can have more than one oxidation number, you have to designate its charge in the name! We do this by putting the charge as a roman numeral in parenthesis between the positive and negative ion. Naming Variable Ionic Compounds

  14. Naming binary compounds of variable metals Why do we need to do that? Name: Fe2O3 FeO These both exist in nature, so we have to show which one we mean.

  15. Naming Ionic Compounds +3 If this is true, then what was iron to begin with? Reverse criss cross to find the charge of the iron: Fe2O3 Name it: -2 Iron ( ) ox ygen ide III

  16. Naming Ionic Compounds +2 -2 Reverse criss cross to find the charge of the iron: If this is not true, the numbers must have been reduced. FeO Name it: -1 Iron ( ) ox ygen ide II

  17. Naming Ionic Compounds Metals that don’t need parentheses: Group I, II and IIIA Zn, Cd (always +2) and Ag (always +1) Which means transition, inner transition and other metals do!

  18. Naming binary compounds of variable metals Determine the oxidation number of the variable metal using the crisscross method Cr2O3 Cr+ O- The oxidation number of the chromium is+3 The name isChromium (III) oxide 2 3

  19. Naming polyatomic compoundsof variable metals Determine the valence of the variable metal using the crisscross method Hg2SO4 Hg+ SO4- The oxidation number of the Mercury is +1 Mercury (I) sulfate 2 1

  20. Naming Ionic Compounds Final flowchart of how to name: Name the positive ion. Does it need a roman numeral? If so, reverse criss cross, if not, ignore. Name the negative ion and: If a nonmetal end in -ide; if not, end normally

  21. Name these: Na2S _______________ CuCl2 _______________ K2SO4 _______________ Pb(NO3)2 _______________ Sodium Sulfide Copper (II) Chloride Potassium Sulfate Lead (II) Nitrate

  22. Finding Chemical Formulas • Determine the charge of each side of the formula. • Aluminum oxide Al+3 O-2 • Potassium Chloride K+1 Cl-1 • Calcium nitrate Ca +2 NO3-1

  23. Writing Chemical Formulas 2.Add the oxidation numbers together. Al+3 O-2 K+1 Cl-1 +3-2 = +1 +1-1 = 0 3.If the total = zero the formula is balanced with one ion eachex: KCl

  24. 4. If the total does not equal zero use the criss-cross method to determine the number of ions needed for each side of the formula. 2 3 Al+3O-2 AlO

  25. Writing Chemical Formulas 5) If using polyatomic ions, use parentheses if there is more than one anion. +2 2 -1 1 ) ( Ca NO3

  26. If the total does not equal zero use the crisscross method to determine the number of ions needed for each side of the formula. 3 2 Al+3SO4-2 AlSO4 ( )

  27. Writing Chemical Formulas Here’s an example of a polyatomic that doesn’t have parentheses. +1 1 -3 3 Na PO4

  28. Practice These: BaCl2 Barium and chlorine Rubidium and nitrogen Lithium and phosphate Iron (III) and nitrate Manganese (IV) and sulfur Rb3N Li3PO4 Fe(NO3)3 MnS2

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