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Predicting Ionic Charges

Predicting Ionic Charges. Group IA :. Lose 1 electron to form 1+ ions. H +. Li +. Na +. K +. Predicting Ionic Charges. Group IIA :. Loses 2 electrons to form 2+ ions. Be 2+. Mg 2+. Ca 2+. Ba 2+. Sr 2+. Predicting Ionic Charges. Group 13 :.

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Predicting Ionic Charges

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  1. Predicting Ionic Charges Group IA: Lose 1 electron to form1+ions H+ Li+ Na+ K+

  2. Predicting Ionic Charges Group IIA: Loses 2 electrons to form2+ions Be2+ Mg2+ Ca2+ Ba2+ Sr2+

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

  4. Predicting Ionic Charges Group IVA: loses 4 electrons or gains 4 electrons

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

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

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

  8. Predicting Ionic Charges Group VIII: StableNoble gasesdo notform ions!

  9. Predicting Ionic Charges Groups 3 – 12: Manytransitionelements have more than one possible oxidation state. Groups 3 - 12: Iron(II) = Fe2+ Iron(III) = Fe3+

  10. Predicting Ionic Charges Groups 3 – 12:Sometransitionelements have only one possible oxidation state. Zinc = Zn2+ Silver = Ag+

  11. 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. Ba2+ NO3- 2 Not balanced! 3. Balance charges , if necessary, usingsubscripts. Use parenthesesif youneed more than oneof apolyatomic ion.

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

  13. Writing Ionic Compound Formulas Example:Iron(III) chloride 1. Write the formulas for the cation and anion, including CHARGES! Fe3+ Cl- 2. Check to see if charges are balanced. 3 3. Balance charges , if necessary,usingsubscripts. Use parenthesesif youneed more than oneof apolyatomic ion. Not balanced!

  14. 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. Al3+ S2- 2 3 3. Balance charges , if necessary,usingsubscripts. Use parenthesesif youneed more than one of a polyatomic ion. Not balanced!

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

  16. 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. Zn2+ OH- 2 3. Balance charges , if necessary, using subscripts. Use parentheses if you need more than one of a polyatomic ion. Not balanced!

  17. 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- They ARE balanced!

  18. Naming Ionic Compounds • 1. Cation first, then anion • 2. Monatomic cation = name of the element • Ca2+ = calciumion • 3. Monatomic anion =root+-ide • Cl- = chloride • CaCl2= calcium chloride

  19. Naming Ionic Compounds(continued) Metals with multiple oxidation states • some metal forms more than onecation • useRoman numeralin name PbCl2 • Pb2+is the lead(II) cation • PbCl2 = lead(II) chloride

  20. Naming Binary Compounds • Compounds between twononmetals • First element in the formula isnamed first. • Second element is named as if it were ananion. • Use prefixes • Only usemonoon second element - P2O5 = diphosphoruspentoxide CO2 = carbondioxide CO = carbonmonoxide N2O = dinitrogenmonoxide

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