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Tuesday!!!!! 12/13/11

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.

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Tuesday!!!!! 12/13/11

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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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