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Understanding Ionic Compounds and Their Nomenclature in Chemistry

This lesson focuses on the essential concepts of ionic compounds, including the principles of ionic bonding, the prediction of ionic charges across different groups in the periodic table, and the proper methods for writing formulas and naming ionic compounds. Students will review important terms, such as cations, anions, and the significance of oxidation states, as they prepare for their midterm exams. Emphasis will be placed on practical examples and the application of nomenclature rules, equipping students with the skills needed for independent problem-solving in chemistry.

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Understanding Ionic Compounds and Their Nomenclature in Chemistry

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  1. Tuesday!!!!!12/13/11 Bell Ringer Schedule PAP Chemistry • Bell Ringer • HW Check • Nomenclature notes HOMEWORK: Review for your midterm !!!!! Man cannot discover new oceans unless he has the courage to lose sight of the shore. I CAN……solve chemistry problems by being an independent, creative thinker. • Turn in any field trip papers and money. We can take 2 more students! • Pick up the midterm online review paper off the front demo table and the Paper Midterm Review answer key.

  2. Nomenclature NOVA: Island of Stability….why can’t we just create new elements?

  3. Ions • Cation: A positive ion • Mg2+, NH4+ • Anion: A negative ion • Cl-, SO42- • Ionic Bonding: Force of attraction between oppositely charged ions.

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

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

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

  7. Predicting Ionic Charges Group 14: Lose 4 electrons or gain 4 electrons? Neither! Group 14 elements rarely form ions. +/- 4

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

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

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

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

  12. Predicting Ionic Charges Many transition elements have more than one possible oxidation state. Groups 3 - 12: Iron(III) = Fe3+ Iron(II) = Fe2+ Copper (I) = Cu +1 Copper (II) = Cu +2

  13. Predicting Ionic Charges Some transition elements have only one possible oxidation state. Groups 3 - 12: Zinc = Zn2+ Silver = Ag+ Tin ( II) = Sn +2 Tin (IV) = Sn +4

  14. Latin names • You may see the Latin names for Fe, Cu, and Sn • Iron (II) = Ferrous • Irong (III) = Ferric • Copper (I) = Cupprous • Copper (II) = Cuppric • Tin (II) = Stannous • Tin (IV) = Stannic

  15. 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, using subscripts. Use parentheses if you need more than one of a polyatomic ion. Not balanced!

  16. 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, using subscripts. Use parentheses if you need more than one of a polyatomic ion. Not balanced!

  17. 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 3. Balance charges , if necessary, using subscripts. Use parentheses if you need more than one of a polyatomic ion. Not balanced!

  18. 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!

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

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

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

  22. 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

  23. Naming Ionic Compounds(continued) Metals with multiple oxidation states • - some metal forms more than one cation • - use Roman numeralin name • PbCl2 • Pb2+is cation • PbCl2 = lead(II) chloride

  24. Naming Binary (Covalent) Compounds • -Compounds between two nonmetals • -First element in the formula is named first. • -Second element is named as if it were an anion. • - Use prefixes • - Only use mono on second element - P2O5 = diphosphorus pentoxide CO2 = carbon dioxide CO = carbon monoxide N2O = dinitrogen monoxide

  25. Prefixes • 1 - mon(o) • 2 - di • 3 - tri • 4 - tetr(a) • 5 - pent(a) • 6 - hex(a) • 7 - hept(a) • 8 - oct(a) • 9 - non(a) • 10 - dec(a)

  26. C. Molecular Nomenclature • CCl4 • N2O • SF6 • carbon tetrachloride • dinitrogen monoxide • sulfur hexafluoride

  27. C. Molecular Nomenclature • arsenic trichloride • dinitrogen pentoxide • tetraphosphorus decoxide • AsCl3 • N2O5 • P4O10

  28. Common Acids you SHOULD know • HCl Hydrochloric acid • HBr Hydrobromic acid • HNO3 Nitric Acid • HClO3 Chloric Acid • HClO4 Perchloric Acid • H2SO4 Sulfuric Acid • H3PO4 Phosphoric Acid • HC2H3O2 Acetic Acid (5% Acetic Acid is also known as Vinegar)

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