Ionic Bonding

October 1, 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 BOHR MODEL HANDOUT!!! Turn in any late work and 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 DO NOW 10/1/13 Download the NearPod App if you have an android or an apple device if you haven’t already In your DO NOW form: The half-life of Zn-71 is 2.4 minutes. If one had 100.0 g at the beginning, how many grams would be left after 7.2 minutes has elapsed?

DO Now Review 9/30 The half-life of Zn-71 is 2.4 minutes. If one had 100.0 g at the beginning, how many grams would be left after 7.2 minutes has elapsed? 7.2 / 2.4 = 3 half-lives(1/2)3 = 0.125 (the amount remaining after 3 half-lives)100.0 g x 0.125 = 12.5 g remaining

Homework Nuclear Decay and Mole test Corrections** ( Parent signature, up to 4 extra points, cannot get over 100 points) DUE TOMORROW FOR CREDIT!!

Upcoming Dates 10/2/2013 – TEST CORRECTIONS DUE Ionic/Metallic Bonding Quiz 10/4/2013 – Mid-Quarter Test 10/7/2013 – Bonding/Forces/Nomenclature Test

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

Tutoring Tuesday 2:30-3:30 in room 529 Thursday 2:30-3:30 in room 710 Test Make-ups/Test Retakes/Extra Credit Wednesday first 20 mins of lunch

Metallic Bonding review http://www.youtube.com/watch?v=eVv3TpaQ2-A&list=TLP_eZDcVGRlnvRTDbWCxec32uOhW9UX62

Anticipation Guide Complete the BEFORE READING of the anticipation guide if you have not already

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

Bonds Forces that hold groups of atoms together and make them function as a unit. Ionic bonds – transfer of electrons Covalent bonds – sharing of electrons

The Octet Rule – Ionic Compounds Ionic compounds form so that each atom, by gaining or losing electrons, has an octet of electrons in its highest occupied energy level. Metals lose electrons to form positively-charged cations Nonmetals gains electrons to form negatively-charged anions

Ionic Bonding: The Formation of Sodium Chloride Sodium has 1 valence electron Chlorine has 7 valence electrons An electron transferred gives each an octet Na: 1s22s22p63s1 Cl: 1s22s22p63s23p5

Ionic Bonding: The Formation of Sodium Chloride This transfer forms ions, each with an octet: Na+ 1s22s22p6 Cl- 1s22s22p63s23p6

Ionic Bonding: The Formation of Sodium Chloride The resulting ions come together due to electrostatic attraction (opposites attract): Na+ Cl- The net charge on the compound must equal zero

Examples of Ionic compounds Mg2+Cl-2 Magnesium chloride: Magnesium loses two electrons and each chlorine gains one electron Na+2O2- Sodium oxide: Each sodium loses one electron and the oxygen gains two electrons Al3+2S2-3 Aluminum sulfide: Each aluminum loses two electrons (six total) and each sulfur gains two electrons (six total)

Metal Monatomic Cations Ion name Lithium Li+ Sodium Na+ Potassium K+ Magnesium Mg2+ Calcium Ca2+ Barium Ba2+ Aluminum Al3+

Nonmetal Monatomic Anions Ion Name Fluorine F- Fluoride Chlorine Cl- Chloride Bromine Br- Bromide Iodine I- Iodide Oxygen O2- Oxide Sulfur S2- Sulfide Nitrogen N3- Nitride Phosphorus P3- Phosphide

Sodium Chloride Crystal Lattice Ionic compounds form solid crystals at ordinary temperatures. Ionic compounds organize in a characteristic crystal lattice of alternating positive and negative ions. All salts are ionic compounds and form crystals.

Properties of Ionic Compounds Structure: Crystalline solids Melting point: Generally high Boiling Point: Electrical Conductivity: Excellent conductors, molten and aqueous Solubility in water: Generally soluble

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 a polyatomic ion. Ba2+ ( ) NO3- 2 Not balanced!

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!

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!

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!

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!

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!

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!

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

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

Bohr Model Homework / Test If you did your homework you can move onto the next handout – guided notes will also play in the process If you did not – you have 20 minutes to complete your test/homework now.

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 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