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Ionic Compound Formulas

Ionic Compound Formulas. www.lab-initio.com. Ions. Cation : A positive ion Mg 2+ , NH 4 + Anion: A negative ion Cl - , SO 4 2 -. Predicting Ionic Charges. Group 1 :. Lose 1 electron to form 1+ ions. H +. Li +. Na +. K +. Predicting Ionic Charges. Group 2 :.

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Ionic Compound Formulas

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  1. Ionic Compound Formulas www.lab-initio.com

  2. Ions • Cation: A positive ion • Mg2+, NH4+ • Anion: A negative ion • Cl-, SO42-

  3. Predicting Ionic Charges Group 1: Lose 1 electron to form 1+ ions H+ Li+ Na+ K+

  4. Predicting Ionic Charges Group 2: Loses 2 electrons to form 2+ ions Be2+ Mg2+ Ca2+ Ba2+ Sr2+

  5. Predicting Ionic Charges Loses 3 electrons to form 3+ ions Group 13: B3+ Al3+ Ga3+

  6. Predicting Ionic Charges Lose 4 electrons or gain 4 electrons? Group 14: Neither!Group 14 elements rarely form ions. If they do, they lose 4 electrons.

  7. Predicting Ionic Charges Nitride N3- Gains 3 electrons to form 3- ions Group 15: Phosphide P3- As3- Arsenide

  8. Predicting Ionic Charges Oxide O2- Group 16: Gains 2 electrons to form 2- ions S2- Sulfide Se2- Selenide

  9. Predicting Ionic Charges Group 17: Gains 1 electron to form 1- ions F1- Fluoride Cl1- Chloride Br1- Bromide I1- Iodide

  10. Predicting Ionic Charges Group 18: Stable Noble gases do not form ions!

  11. Predicting Ionic Charges Many transition elements have more than one possible oxidation state. Groups 3 - 12: Iron(II) = Fe2+ Iron(III) = Fe3+

  12. Predicting Ionic Charges Some transition elements have only one possible oxidation state. Groups 3 - 12: Zinc =Zn2+ Silver = Ag+

  13. Naming Ionic Compounds • Cation first, then anion • Metal cation = name of the metal • Ca2+ = calcium ion • Nonmetal anion=root + -ide • Cl-=chloride • CaCl2 = calcium chloride

  14. Naming Ionic Compounds(continued) Metals with multiple oxidation states • some metal forms more than one cation • use Roman numeral in name • PbCl2 • Pb2+ is cation • PbCl2 = lead(II) chloride Use this method for all metals except those in Groups 1 and 2.

  15. Naming Polyatomic Ionic Compounds • Cation first, then anion • Polyatomic cation = name of the polyatomic ion • NH4+ = ammonium ion • Metal cation = name of the metal • Ca2+ = calcium ion • some metal forms more than one cation • use Roman numeral in name

  16. Naming Ionic Compounds • Cation first, then anion • Polyatomic anion=name of the polyatomic ion • ClO-=hypochlorite • Nonmetal anion=root + -ide • Cl-=chloride

  17. Naming Ionic Compounds • Cationfirst, then anion • Examples: • CaCO3 • NH4Cl • Cu2SO4 • Mg(OH)2 • (NH4)3PO4 • Al2(C2O4)3

  18. Naming Ionic Compounds • Cationfirst, then anion • Examples: • CaCO3 calcium carbonate • NH4Cl ammonium chloride • Cu2SO4 copper (I) sulfate • Mg(OH)2magnesium hydroxide • (NH4)3PO4 ammonium phosphate • Al2(C2O4)3aluminum oxalate

  19. Writing Ionic Compound Formulas Example: Barium nitrate 1. Write the formulas for the cation and anion, including CHARGES! 2. Check to see if charges are balanced. 3. Balance charges , if necessary, using subscripts.Use parentheses if you need more than one of apolyatomic ion. Ba2+ ( ) NO3- 2 Ba(NO3)2 Not balanced!

  20. Writing Ionic Compound Formulas Example:Ammonium sulfate 1. Write the formulas for the cation and anion, including CHARGES! 2. Check to see if charges are balanced. 3. Balance charges , if necessary, using subscripts. Use parentheses if you need more than one of a polyatomic ion. ( ) NH4+ SO42- 2 (NH4)2SO4 Not balanced!

  21. Writing Ionic Compound Formulas Example: Iron(III) chloride 1. Write the formulas for the cation and anion, including CHARGES! 2. Check to see if charges are balanced. 3. Balance charges , if necessary, using subscripts. Use parentheses if you need more than one of a polyatomic ion. Fe3+ Cl- 3 FeCl3 Not balanced!

  22. Writing Ionic Compound Formulas Example:radium chloride 1. Write the formulas for the cation and anion, including CHARGES! 2. Check to see if charges are balanced. 3. Balance charges , if necessary, using subscripts. Use parentheses if you need more than one of a polyatomic ion. Ra2+ Cl- 3 FeCl3 Not balanced!

  23. Writing Ionic Compound Formulas Example: Aluminum sulfide 1. Write the formulas for the cation and anion, including CHARGES! 2. Check to see if charges are balanced. 3. Balance charges , if necessary, using subscripts. Use parentheses if you need more than one of a polyatomic ion. Al3+ S2- 2 3 Al2S3 Not balanced!

  24. Writing Ionic Compound Formulas Example: Magnesium carbonate 1. Write the formulas for the cation and anion, including CHARGES! 2. Check to see if charges are balanced. MgCO3 Mg2+ CO32- They are balanced!

  25. Writing Ionic Compound Formulas Example: Zinc hydroxide 1. Write the formulas for the cation and anion, including CHARGES! 2. Check to see if charges are balanced. 3. Balance charges , if necessary, using subscripts. Use parentheses if you need more than one of a polyatomic ion. Zn2+ ( ) OH- Zn(OH)2 2 Not balanced!

  26. Writing Ionic Compound Formulas Example: Aluminum phosphate 1. Write the formulas for the cation and anion, including CHARGES! 2. Check to see if charges are balanced. Al3+ PO43- AlPO4 They ARE balanced!

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