October 2, 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

Homework Formula Practice Worksheet

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

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

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

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

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 

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

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

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

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

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

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

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

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

Predicting Ionic Charges Groups : 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+

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

Writing Ionic Compound Formulas Example: Barium nitrate 1. Write the formulas for the cation and anion, including CHARGES! Ba 2+ NO 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

Writing Ionic Compound Formulas Example: Ammonium sulfate 1. Write the formulas for the cation and anion, including CHARGES! NH 4 + SO 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

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

Writing Ionic Compound Formulas Example: Aluminum sulfide 1. Write the formulas for the cation and anion, including CHARGES! Al 3+ S 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

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

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

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

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

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

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

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

Made of StarDust Video

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

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

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

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

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

 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

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

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)......

Bond Length and Bond Energy

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.

Resonance in Benzene, C 6 H 6

Practice

QUIZ Ionic and metallic bonding