1. Nomenclature
Naming Compounds

2. Ionic Compounds Metal bonding with non-metal
One atom gains electrons, one atom loses electrons
Exist as ions with full highest energy levels.
Are held together in a giant crystal by the electrostatic attraction of the opposite charges.
The metal is named first; the nonmetal gets “ide” at the end of it’s name.
Ex. CaCl2 Calcium chloride

4. There is no real bond between the ions
There is no real bond between the ions. There is just strong attraction between the opposite charges. - - + + - + + - - + - - + + -

5. Metals
Non-Metals
Rule #1

6. Try these Metal & Non-metal
K2Se
MgO
Cs3P
SrF2
Rb3N
FrI
BeS

7. Try these Metal & Non-metal
K2Se Potassium Selenide
MgO Magnesium Oxide
Cs3P Cesium Phosphide
SrF2 Strontium Fluoride
Rb3N Rubidium Nitride
FrI Francium Iodide
BeS Beryllium Sulfide

8. Try these Metal & Non-metal
K2Se Potassium Selenide
MgO Magnesium Oxide
Cs3P Cesium Phosphide
SrF2 Strontium Fluoride
Rb3N Rubidium Nitride
FrI Francium Iodide
BeS Beryllium Sulfide

9. Writing Ionic Formulas
Determine the charge on each ion.
Find the lowest common multiple that will balance the charge.
ex. Calcium Chloride
Ca Cl-
+2 x2=-2 (to balance the charge)
CaCl2

10. Try these Metal & Non-metal
Sodium phosphide
Magnesium telluride
Lithium chloride
Barium carbide
Strontium arsenide

11. Try these Metal & Non-metal
Sodium Phosphide
Na P-3 x3
Na3P

12. Try these Metal & Non-metal
Magnesium Telluride
Mg Te-2
MgTe

13. Try these Metal & Non-metal
Lithium Chloride
Li Cl-
LiCl

14. Try these Metal & Non-metal
Barium Carbide
Ba C-4 X2
Ba2C

15. Try these Metal & Non-metal
Strontium Arsenide
Sr As-3
X x2
Sr3As2

16. Ionic Compounds part II
The transition metal is named first with a Roman numeral to indicate the charge on the ion; the nonmetal gets “ide” at the end of its name.

17. Transition Metals

18. Non- metals
Rule #2
Transition Metals

19. Non- metals
Rule #2
Transition Metals

20. What is the name of CuO ? We know that oxygen has a charge of –2.
Therefore, copper must have a charge of +2.
We must indicate the charge of the transition metal.
Copper (II) oxide

21. Try these: Transition Metal & Non-metal
Fe3N2
NiBr3
CoCl2
HgI
SnS2

22. Try these: Transition Metal & Non-metal
Fe3N2
Iron was multiplied by 3 and nitrogen (-3) was multiplied by 2 (-6) so that the charges would balance.
The charge on Iron must have been +2.
Iron (II) nitride

23. Try these: Transition Metal & Non-metal
NiBr3
The charge (from the periodic table) on Br is –1.
Br was multiplied by 3 (hence the subscript), so the charge on Nickel MUST be +3.
Nickel (III) Bromide

24. Try these: Transition Metal & Non-metal
CoCl2
The charge (from the periodic table) on Cl is –1.
Chlorine was multiplied by 2 (hence the subscript), so the charge on Cobalt MUST be +2.
Cobalt (II) Chloride

25. Try these: Transition Metal & Non-metal
HgI
The charge (from the periodic table) on I is –1.
Iodine was not multiplied by anything (no subscript), so the charge on Mercury MUST be +1.
Mercury (I) Iodide

26. Try these: Transition Metal & Non-metal
MnO2
The charge (from the periodic table) on O is –2.
Oxygen was multiplied by 2 (hence the subscript), so the charge on Manganese MUST be +4.
Manganese (IV) Oxide

27. Formula writing with transition metals
Simple!
ex. Nickel (II) Iodide
The charge on the nickel ion is obviously +2.
The charge on iodide is always -1.
Therefore, the formula is: NiI2

28. Ionic Compounds part III
Bonding with a Polyatomic ion
The metal is named first; the polyatomic anion is named second (a polyatomic cation is named first).
Ex. Li3PO4 Lithium phosphate

29. Polyatomic Ions that we use in science 10:
OH-1
SO4-2
NO3-1
CO3-2
PO4-3
NH4+1
ClO3-1
hydroxide
sulfate
nitrate
carbonate
phosphate
ammonium
chlorate

30. Try these: Polyatomic Ion
NaOH
K2SO4
Ba(NO3)2
CuCO3
Li3PO4
NH4Cl

31. Try these: NaOH K2SO4 Ba(NO3)2 CuCO3 Li3PO4 NH4ClO3 Sodium Hydroxide
Potassium Sulfate
Barium Nitrate
Copper(II) Carbonate
Lithium Phosphate
Ammonium Chlorate

32. Writing Formulas Calcium sulfate Potassium carbonate
Ammonium hydroxide
Iron (III) chlorate
Copper (I) phosphate
Zinc sulfate

33. Ionic Bonding vs Molecular Bonding
Makes "Compounds” vs Makes "Molecules"
Transfers electrons vs Shares electrons
Metals & Nonmetals vs Made of Nonmetals
Positive & Negative vs Neutral
Weak Bond vs Strong bond
NaCl KOH CaCl2 vs H2O CO2 NH3 CH4

34. Molecular Compounds Non-metals bond with non-metals.
Prefixes
Mono Di
Tri
Tetra
Penta
Hexa
Hepta
Octa
Nona
Deca
Non-metals bond with
non-metals.
Atoms share electrons.
The number of each atom present is indicated by a prefix.
Add “ide” to the end of the second atom’s name.

35. Non- metals
Rule #3

36. ex.
N2O dinitrogen monoxide
NO nitrogen monoxide
N2O3 dinitrogen trioxide
NO2 nitrogen dioxide *
N2O4 dinitrogen tetroxide
N2O5 dinitrogen pentoxide

37. * When the first atom is singular, the prefix “mono” is not used.
ex.
N2O dinitrogen monoxide
NO nitrogen monoxide
N2O3 dinitrogen trioxide
NO2 nitrogen dioxide *
N2O4 dinitrogen tetroxide
N2O5 dinitrogen pentoxide
* When the first atom is singular, the prefix “mono” is not used.

38. Try These: Non-metal & Non-metal
SO3
XeF6
KrF2
BrCl5
SCl4
PF3
As4O10
N2O3
sulfur trioxide
xenon hexafluoride
krypton difluoride
bromine pentachloride
sulfur tetrachloride
phosphorus trifluoride
tetrarsenic decoxide
dinitrogen trioxide

39. Writing Formulas
Write each atom’s symbol with a subscript equal to the prefix.
Ex.
Hexaphosphorus tribromide P6Br3
Pentatellurium mononitride Te5N

40. Try these dinitrogen pentasulfide carbon monoxide heptasulfur trioxide
xenon hexafluoride
trisulfur hexafluoride
phosphorus pentachloride
nitrogen monoxide
dibismuth trichloride

41. Try these dinitrogen pentasulfide N2S5 carbon monoxide C0
heptasulfur trioxide S7O3
xenon hexafluoride XeF6
trisulfur hexafluoride S3F6
phosphorus pentachloride PCl5
nitrogen monoxide NO
dibismuth trichloride Bi2Cl3