1. Ch 7: Ionic Bonding Formula Writing
My Name is Bond. Ionic Bond. Taken NOT shared

2. Review
1) Why do atoms come together? 2) What types of atoms form an ionic bond? 3) What is the relationship between ionic bonding and electronegativity? 4) What happens to the electrons in an ionic bond?

3. Review Answers
Atoms come together to achieve stability by filling their valence shells.
A metal with a nonmetal
Ionic bonds form between atoms with a huge difference in electronegativity:
One atom is so much stronger (more electronegativity), it TAKES the electrons

4. 2 Types of Ions Cation = a positively charged ion (lost e-)
Less electroneg./metal
Anion = a negatively charged ion (gained e-)
More electroneg. /nonmetal

5. Monatomic Ions “Mono” = One “Atomic” = Atom
Monatomic Ion: An ion in which a single atom has a positive or negative charge

6. Charge and the Periodic Table

7. Transition Metals Have multiple charges Positive charge (Cations)
Their charge is indicated by the Roman Numeral following their name
Iron (II) = Fe+2
Iron (III) = Fe+3

8. Ions and Electron Configuration
Atomic Number
Element
Electron Configuration
Valence Electrons
# Electrons
Ion Electron Configuration
Ion Symbol w/ charge
Gained
Lost 3
Lithium
1s22s1 1
1s2
Li+1 4
Beryllium
1s2 2s2 2
Be+2 5
Boron
1s2 2s2 2p1
B+3 7
Nitrogen
1s2 2s2 2p3
1s2 2s2 2p6
N-3 8
Oxygen
1s2 2s2 2p4 6
O-2 9
Fluorine
1s2 2s2 2p5
F-1

9. Polyatomic Ions “Poly” = Many “Atomic” = Atom
An ion containing more than one atom that has collectively lost or gained electrons
Ex. NO3-1

10. Ionic Compounds Attraction between cation and anion
The cation is always written first and gets to keep his name
Subscripts = the number of IONS in the formula. Use ( ) for polyatomic ions.
Overall charge of the compound is zero

11. Examples #1-4: Monatomic & Main Group Ionic Compounds
#1) Sodium Fluoride #2) Magnesium Chloride #3) Beryllium Sulfide #4) Aluminum Oxide

12. Examples #5-6 Monatomic & Transition Metal Compounds
#5) Iron (II) Bromide #6) Silver Nitride

13. Examples #7-9 Main Group Metals with Polyatomic Anion
#7) Lithium Nitrate #8) Calcium Carbonate #9) Aluminum Periodate

14. Examples #10-11: Transition Metal with Polyatomic Anion
#10) Copper (II) Phosphate #11) Iron (III) Dichromate

15. Example #12 An Exception: A Polyatomic Cation!
#12) Ammonium Cyanide

16. Nomenclature Nomenclature = Naming
An ionic bond has 2 ions (a cation and an anion) so its name will always have 2 parts.

17. Rules for Naming Ionic Compounds
The metal cation is always written first
The metal cation gets to keep its name
Ex. Na = Sodium
Ex. Ca = Calcium
ONE EXCEPTION: One polyatomic cation = ammonium (NH4+)

18. Rules for Naming Transition metals need a Roman Numeral Ex. CuO

19. Rules for Naming
A Monatomic anion will keep its name but the ending is changed to “ide”
Ex. Cl-1 = Chloride
Ex. O-2 = Oxide
Ex. N-3 = Nitride
A polyatomic anion will end in “ate,” “ite” etc.
On your Common Ion Sheet or in your memory!

20. Naming Binary Compounds: Main Group Cations
Binary = Made up of 2 types of elements
KBr
2. SrCl2
3. Rb2O

21. Naming Binary Compounds: Transition Metal Cations
4. NiO 5. Ni2O3 6. SnO2

22. Naming: Main Group Cations + Polyatomic Anions
7. Al(NO3)3 8. MgCO3 10. NaC2H3O2

23. Naming: Transition Metal Cation + Polyatomic Anion
9. Cu2SO4 11. Zr3(PO4)2

24. Naming: An exception
12. NH4IO