1. Ionic Bonding and Naming
Chapter 7/9
Ionic Bonding and Naming

2. Sim. And diff between Ionic and Covalent Bonds
Draw Ionic and Covalent Pictures
Naming Ions
Given formula, write the name
Basic (monoatomic cations and anions)
Using polyatomic ions
Using transition metals
Given name, write the formula

3. Ionic vs Covalent Bonding?

4. So why do atoms react with each other?

5. How many valence e- does Na have? Cl?

6. Ionic bond – the attraction between oppositely charged atoms
Na now has a +1 charge
Cl now has a -1 charge
Ionic bond – the attraction between oppositely charged atoms
Caused by taking/giving of electrons
Often between metals and nonmetals

7. Metals vs Nonmetals

8. Why Ionic Bond?
NaCl
MgCl2
FeO3
CuF

9. Caption?

11. Covalent Bonds
Defn: atoms share electrons
Often between nonmetals
H2O

12. Why Covalent?
CH4
C6H12O6
NH3

13. Ionic Or Covalent Bonds?
KCl
CO2
BeF3
CuO
AlF3

14. Ionic-Covalent Bonding Activity

15. Common Names 1) Dry ice 2) Epsom salts (magnesium sulfate)
3) Milk of magnesia (magnesium hydroxide)

16. Chemical Formulas
show the relative #’s of atoms in a chemical compound
C12H22O11
Pb(NO3)4
(NH4)2CrO4

17. Monoatomic Anions? End in -ide F vs F-1 S vs S-2
What is the charge based on?

18. What is the name of….
O-2
Cl-1

19. Monoatomic Cations?

20. Monoatomic Cations Single Positive ions What determines charge?
Na+1 Sodium Ion
Mg+2 Magnesium Ion
Examples:
Ca+2
Ag+1

21. Polyatomic Ions Given name, write formula
Recognize ending is ate or ite
Look up using P-ion sheet
Ex5 Chlorate
Ex6 Bicarbonite

22. Polyatomic Ions Given formula, write name
Recognize multiple capital letters together
Look up on Pion sheet
Ex7 PO4-3___________________ Ex8 NO2-1_____________________

23. Monoatomic and Polyatomic Basic wks

24. Writing Names for Ionic Compounds
Front name – positive (cation – metal)
Back name – negative (anion – nonmetal)
Binary ionic compounds – composed of only 2 types of elements ( M + NM) – end in -ide
NaCl
MgCl2
Al2O3
NaH
Sodium Chloride
Magnesium Chloride
Aluminum Oxide
Sodium Hydride

25. Writing Names Using Polyatomic Ions
Same Rules as basic ones:
Take name of positive ion and negative ion and put them together
Ex13 LiClO3
Ex14 LiClO2

26. Ex15 CaCO3
Ex16 K(HCO2)
Ex17 Mg(NO3)2

27. Writing Formulas for Ionic Compounds
_______ – positive ions
Typically _______________________________
_______ – negative ions
Total Charge of all ions must add up to ____

28. Writing Formulas for Ionic Compounds
Cations – positive ions
Typically metals or polyatomic ions
Anions – negative ions
Typically nonmetals or polyatomic ions
Total Charge of all ions must add up to 0

29. Why does the number of Cl’s change?
NaCl
MgCl2
AlCl3

30. Steps for Writing Binary Ionic compound
1) Write the two ions involved
2) If the charges on the ions are the same, “drop ‘em” and push elements together
3) If the charges are different, “criss cross”
4) Simplify the subscripts if possible (ie. 2 and 4 turns to 1 and 2 or 3 and 9 turns to 1 and 3)
Same charges –
Na+1 Cl-1 -
Mg+2 O-2 -
Different charges-
Na+1 S-2-
Mg+2 Cl-1-
NaCl Sodium Chloride
MgO Magnesium Oxide
Na2S Sodium Sulfide
MgCl Magnesium Chloride

31. Writing Formulas for Ionic Compounds
Ternary Ionic compounds
5) Sodium Nitrate
6) Sodium Carbonate
7) Aluminum Nitrate
Na+1 NO3-1
Na(NO3)
Na+1 CO3-2
Na2(CO3)
Al+3 NO3-1
Al(NO3)3

32. Complete Ex 8-10
8) Aluminum Carbonate 9) Aluminum Phosphate 10) Aluminum Bihypophosphite

33. Practice Worksheet

34. Stock System – use Roman Numerals for naming compounds with metals that have multiple charges (the transitions!)
Name
Symbol
Charge
Stock Name
Copper Cu +1
Cu (I) +2
Cu (II)
Mercury Hg
Hg (I)
Hg (II)
Lead Pb
Pb (II) +4
Pb (IV)
Tin Sn
Sn (II)
Sn (IV)
Iron Fe
Fe (II) +3
Fe (III)

35. Exceptions Ag is always = +1 charge Zn always = +2 charge
DON’T write Ag I
Zn always = +2 charge
DON’T write Zn II

36. CuCl
Cu = +1 Copper (I) chloride
CuCl2
Cu = +2 Copper (II) chloride

37. Practice! 5) Sn3N2 6) AgOH 7) PbCO3 8) Zn(OH)2 9) Fe2(SO4)3
Tin (II) Nitride
Silver Hydroxide
Lead (II) Carbonate
Zinc Hydroxide
Iron (III) Sulfate

38. More Practice!! 10) Cu(HSO2)2 11) CuSO2 12) CuHCO3
Copper (II) Bihyposulfite
Copper (II) Hyposulfite
Copper (I) Bicarbonate

39. Ex13 Nickel (III) acetate
Ex 14 Iron (II) chloride
Ex 15 Iron (III) hydroxide
Ex 16 Manganese (IV) nitrite
Ex 17 Chromium (III) sulfide

40. Practice!
1) LiClO3
2) LiClO2
3) CaCO3
4) Ca(HCO2)2
5) Fe(NO3)3
Lithium Chlorate
Lithium Chlorite
Calcium Carbonate
Calcium Bicarbonite
Iron (III) Nitrate

41. Complete Wks
Complete Wks “Ionic Compound Names and Formulas” wks (1-24)
Complete Mixed bag wks

42. Stations Monoatomic ions (no trans. metal) name to formula
Monoatomic ions (no trans. Metal) formula to name
One mono (no trans metal), one poly, name to formula
One mono (no trans metal), one poly, formula to name
Transition metal and mono ion, name to formula
Transition metal and mono ion, formula to name
Transition metal and poly ion, name to formula
Transition metal and poly ion, formula to name
Both polyatomic ions, name to formula
Both polyatomic ions, formula to name