1. Ionic Bonding

2. 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 g at the beginning, how many grams would be left after 7.2 minutes has elapsed?

3. DO Now Review 9/30
The half-life of Zn-71 is 2.4 minutes. If one had 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 = (the amount remaining after 3 half-lives)100.0 g x = 12.5 g remaining

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

5. 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

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

7. 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

8. Metallic Bonding review

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

10. 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

11. 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

12. 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

13. 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

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

15. 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

16. 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)

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

18. 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

19. 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.

20. 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

21. 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!

22. 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!

23. 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!

24. 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!

25. 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!

26. 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!

27. 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!

28. 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

29. 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

30. 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.

31. 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

32. 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