1 / 42

October 2 , 2013 When the bell rings voices are at zero, working on the DO NOW

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

vonda
Download Presentation

October 2 , 2013 When the bell rings voices are at zero, working on the DO NOW

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. 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 inyour 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

  2. Homework Formula Practice Worksheet

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

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

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

  6. 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

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

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

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

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

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

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

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

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

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

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

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

  18. 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 Not balanced!

  19. 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 Not balanced!

  20. 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 Not balanced!

  21. 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 Not balanced!

  22. 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. Mg2+ CO32- They are balanced!

  23. 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- 2 Not balanced!

  24. 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!

  25. Cationfirst, then anion Monatomic cation = name of the element Ca2+ = calcium ion Monatomic anion=root + -ide Cl-=chloride CaCl2 = calcium chloride Naming Ionic Compounds

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

  27. 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

  28. Exit Ticket • In an ionic bond , ions come together due to ___________________ • Write the Ionic Formula Compound for the following • Barium Nitrate • Name the Following Ionic Compound • CaCl2

  29. Made of StarDust Video

  30. CovalentBonding Bonding models for methane, CH4. Models are NOT reality. Each has its own strengths and limitations.

  31. 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

  32. The OctetRule: The Diatomic Fluorine Molecule F 1s 2s 2p Each has seven valence electrons F 1s 2s 2p F F

  33. The OctetRule: The Diatomic Oxygen Molecule O 1s 2s 2p Each has six valence electrons O 1s 2s 2p O O

  34. The OctetRule: The Diatomic Nitrogen Molecule N 1s 2s 2p Each has five valence electrons N 1s 2s 2p N N

  35. 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

  36. Hydrogen (and Halogens) form one covalent bond Oxygen (and sulfur) form two covalent bonds One double bond, or two single bonds Nitrogen (and phosphorus) form three covalent bonds One triple bond, or three single bonds, or one double bond and a single bond 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 The HONCRule

  37. Completing a Lewis Structure -CH3Cl • Make carbon the central atom (it wants the most bonds, 4) • Add up available valence electrons: • C = 4, H = (3)(1), Cl = 7 Total = 14 • Join peripheral atoms • to the central atom with electron pairs. H .. .. .. .. .. H C Cl .. .. • Complete octets on • atoms other than hydrogen with remaining electrons H

  38. Bond Length and Bond Energy

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

  40. Resonance in Benzene, C6H6

  41. Practice

  42. QUIZ • Ionic and metallic bonding

More Related