2. October 2, 2013 -When the bell rings voices are at zero, working on the DO NOW -Pick up daily handouts -Pick up turned back docs -Turn in your TEST CORRECTIONS and any late work, any progress reports. -DO NOT TURN ANYTHING IN UNLESS STATED ABOVE -HAVE OUT YOUR REFERENCE TABLE -Start on the Do Now in your Do Now form -PICK UP 1 WHITE BOARD AND 1 MARKER – DO NOT USE THEM YET – LEAVE YOUR MARKER CAPPED DO NOW 10/2/13 Finish your anticipation guide (after reading – use what we learned yesterday and anything in the provided reading) WRITE “ANTICIPATION GUIDE” in your DO NOW FORM

3. Homework Formula Practice Worksheet

4. Notebook Check Friday 10/4/13 Electron Configuration/Lewis Structure Notes (periodic table colored in) Ionic Formula Writing Handout (today)

5. Upcoming Dates 10/2/2013 Bonding Quiz 10/4/2013 Mid-Quarter Test 10/4/2013 Take home test Periodic Trends

6. Tutoring Saturday 12pm-1pmSaturday 12pm-1pm University City Regional Library 301 East W.T. Harris Boulevard Charlotte, NC 28262

7. Objectives SWBAT - Explain how covalent bonding in compounds determines its characteristics - Determine that a bond is predominately covalent by the location of the atoms on the Periodic Table - Write covalent formulas - Predict ionic charge based on valence electrons

8. Ions  Cation: A positive ion  Mg 2+, NH 4 +  Anion: A negative ion  Cl , SO 4 2   Cation: A positive ion  Mg 2+, NH 4 +  Anion: A negative ion  Cl , SO 4 2 

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

10. Predicting Ionic Charges Group 2: Loses 2 electrons to form 2+ ions Be 2+ Mg 2+ Ca 2+ Sr 2+ Ba 2+

11. Predicting Ionic Charges Group 13: Loses 3 Loses 3 electrons to form 3+ ions B 3+ Al 3+ Ga 3+

12. Predicting Ionic Charges Group 14: Lose 4 Lose 4 electrons or gain 4 electrons? Neither! Group 13 elements rarely form ions.

13. Predicting Ionic Charges Group 15: Gains 3 Gains 3 electrons to form 3- ions N 3- P 3- As 3- Nitride Phosphide Arsenide

14. Predicting Ionic Charges Group 16: Gains 2 Gains 2 electrons to form 2- ions O 2- S 2- Se 2- Oxide Sulfide Selenide

15. Predicting Ionic Charges Group 17: Gains 1 Gains 1 electron to form 1- ions F 1- Cl 1- Br 1- Fluoride Chloride Bromide I 1- Iodide

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

17. Predicting Ionic Charges Groups 3 - 12: Many transition elements Many transition elements have more than one possible oxidation state. have more than one possible oxidation state. Iron(II) = Fe 2+ Iron(III) = Fe 3+

18. Predicting Ionic Charges Groups 3 - 12: Some transition elements Some transition elements have only one possible oxidation state. have only one possible oxidation state. Zinc = Zn 2+ Silver = Ag +

19. Writing Ionic Compound Formulas Example: Barium nitrate 1. Write the formulas for the cation and anion, including CHARGES! Ba 2+ NO 3 - 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. Not balanced! ( ) 2

20. Writing Ionic Compound Formulas Example: Ammonium sulfate 1. Write the formulas for the cation and anion, including CHARGES! NH 4 + SO 4 2- 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. Not balanced! ( ) 2

21. Writing Ionic Compound Formulas Example: Iron(III) chloride 1. Write the formulas for the cation and anion, including CHARGES! Fe 3+ Cl - 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. Not balanced! 3

22. Writing Ionic Compound Formulas Example: Aluminum sulfide 1. Write the formulas for the cation and anion, including CHARGES! Al 3+ S 2- 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. Not balanced! 23

23. Writing Ionic Compound Formulas Example: Magnesium carbonate 1. Write the formulas for the cation and anion, including CHARGES! Mg 2+ CO 3 2- 2. Check to see if charges are balanced. They are balanced!

24. Writing Ionic Compound Formulas Example: Zinc hydroxide 1. Write the formulas for the cation and anion, including CHARGES! Zn 2+ OH - 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. Not balanced! ( ) 2

25. Writing Ionic Compound Formulas Example: Aluminum phosphate 1. Write the formulas for the cation and anion, including CHARGES! Al 3+ PO 4 3- 2. Check to see if charges are balanced. They ARE balanced!

26. Naming Ionic Compounds  Cation first, then anion  Monatomic cation = name of the element  Ca 2+ = calcium ion  Monatomic anion = root + -ide  Cl  = chloride  CaCl 2 = calcium chloride  Cation first, then anion  Monatomic cation = name of the element  Ca 2+ = calcium ion  Monatomic anion = root + -ide  Cl  = chloride  CaCl 2 = calcium chloride

27. Naming Ionic Compounds (continued)  some metal forms more than one cation  use Roman numeral in name  PbCl 2  Pb 2+ is cation  PbCl 2 = lead(II) chloride  some metal forms more than one cation  use Roman numeral in name  PbCl 2  Pb 2+ is cation  PbCl 2 = lead(II) chloride Metals with multiple oxidation states

28. Objectives SWBAT - Explain how ionic bonding in compounds determines its characteristics - Determine that a bond is predominately ionic by the location of the atoms on the Periodic Table - Write ionic formulas - Predict ionic charge based on valence electrons

29. Exit Ticket 1.In an ionic bond, ions come together due to ___________________ 2.Write the Ionic Formula Compound for the following 1.Barium Nitrate 3.Name the Following Ionic Compound 1.CaCl 2

30. Made of StarDust Video

31. Covalent Bonding Bonding models for methane, CH 4. Models are NOT reality. Each has its own strengths and limitations.

32. The Octet Rule and Covalent Compounds  Covalent compounds tend to form so that each atom, by sharing electrons, has an octet of electrons in its highest occupied energy level.  Covalent compounds involve atoms of nonmetals only.  The term “molecule” is used exclusively for covalent bonding

33. The Octet Rule: The Diatomic Fluorine Molecule F F 1s 2s 2p seven Each has seven valence electrons FF

34. The Octet Rule: The Diatomic Oxygen Molecule O O 1s 2s 2p six Each has six valence electrons O O

35. The Octet Rule: The Diatomic Nitrogen Molecule N N 1s 2s 2p five Each has five valence electrons N N

36.  Lewis structures show how valence electrons are arranged among atoms in a molecule.  Lewis structures Reflect the central idea that stability of a compound relates to noble gas electron configuration.  Shared electrons pairs are covalent bonds and can be represented by two dots (:) or by a single line ( - ) Lewis Structures

37. The HONC Rule HH Hydrogen (and Halogens) form one covalent bond O Oxygen (and sulfur) form two covalent bonds One double bond, or two single bonds N Nitrogen (and phosphorus) form three covalent bonds One triple bond, or three single bonds, or one double bond and a single bond C Carbon (and silicon) form four covalent bonds. Two double bonds, or four single bonds, or a triple and a single, or a double and two singles

38. C H H H Cl........ Completing a Lewis Structure -CH 3 Cl  Add up available valence electrons:  C = 4, H = (3)(1), Cl = 7 Total = 14  Join peripheral atoms to the central atom with electron pairs.  Complete octets on atoms other than hydrogen with remaining electrons  Make carbon the central atom (it wants the most bonds, 4)......

39. Bond Length and Bond Energy

40. Resonance Occurs when more than one valid Lewis structure can be written for a particular molecule. These are resonance structures. The actual structure is an average of the resonance structures.

41. Resonance in Benzene, C 6 H 6

42. Practice

43. QUIZ Ionic and metallic bonding