1. 6.3 Naming Compounds and Writing Formulas
Chapter 6
Chemical Bonds

2. What are we going to learn?
How to write the name and formula of ionic and covalently bonded compounds

3. Naming Ionic Compounds
Ionic compound name: distinguishes the compound from other ionic compounds containing the same elements
Name = words (ex: calcium chloride)

4. Ionic compound formula: describes the ratio of the ions in the compound
Formula = numbers of elements (ex: CaCl2)

5. Binary Compounds
If a compound is made from only two elements is a binary compound
(Ex: salt is a binary compound made of sodium and chlorine - sodium chloride)

6. What’s in a Name?
To name a binary compound: list the name of the cation (+ ion) followed by the name of the anion (- ion)

7. Cations – First in Naming
Cation: simply the name of the metal (no changes)
Ex: sodium atom and sodium ion

8. This works for groups 1A, 2A and Aluminum
Group 1A has a 1+ charge
Group 2A has a 2+ charge
Aluminum (Group 3A) has a 3+ charge

9. Transition metals with more than one possible charge have a different naming strategy
Name of the ion contains a Roman numeral to indicate the charge
Ex: copper (II) ion

10. Anions – The Followers
Anion: use name of the nonmetal with the suffix –ide replacing –ine
(ex: chlorine atom and chloride ion)
Nonmetals are on the right side of the periodic table
Ex: sodium chloride
(cation) (anion)

11. Formulas
If you know the name of an ionic compound, you can write its chemical formula
Chemical formula includes chemical symbols of the elements and numbers (indicating amounts of each element)

12. How do you write a formula?
Write the symbol of the cation first
Follow with the symbol of the anion
Use subscripts to show the ratio of the ions in the compound

13. Polyatomic Ions
A covalently bonded group of atoms that has a positive or negative charge and acts as a unit
Ex: nitrate (NO)3-, sulfate (SO4)2-, phosphate (PO4)3-

15. Molecular Compounds
Name and formula of a molecular compound describe the type and number of atoms in a molecule of the compound
These elements are usually on the right side of the periodic table
Elements in the compound share electrons

16. The molecules in the top row bond by sharing electrons.
The compounds in the bottom row join in polar covalent bonds.

17. Naming a Molecular Compound
Most metallic element name appears first (most left in the periodic table)
Name of the second element is changed to end in the suffix -ide
Ex: carbon dioxide

18. Prefixes indicate amount of atoms in the molecule
Ex: di shows that there are two carbon atoms in the molecule

19. Molecular Formula
Write the symbols for the elements in the order the elements appear in the name
Prefixes in the compound name indicate the number of atoms of each element in the molecule
Prefixes appear as subscripts in the formula

21. Writing Chemical Formulas for Binary Compounds Practice
1 - Write the symbols for the elements. 2 - Look up element ion charges and write them as superscripts to the right of the elemental symbols. 3 - Use the correct combination of ions to produce a compound with a net charge of zero. Multiple ions are indicated with subscripts.
lithium oxide
potassium chloride
calcium oxide
barium bromide

22. Writing Chemical Formulas for Binary Compounds Practice
1 - Write the symbols for the elements. 2 - Look up element ion charges and write them as superscripts to the right of the elemental symbols. 3 - Use the correct combination of ions to produce a compound with a net charge of zero. Multiple ions are indicated with subscripts.
lithium oxide Li2O
potassium chloride KCl
calcium oxide CaO
barium bromide BaBr2

23. Writing Chemical Formulas for Binary Compounds with Polyatomic Ions
lithium carbonate
calcium nitrate
ammonium sulfide
sodium sulfate

24. Writing Chemical Formulas for Binary Compounds with Polyatomic Ions
lithium carbonate Li2CO3
calcium nitrate Ca(NO3) 2
ammonium sulfide (NH4) 2S
sodium sulfate Na2SO4

25. Writing Chemical Formulas for Transition Metals Practice
Lead (IV) carbonate
Copper (II) nitrate
Iron (III) oxide
Tin (IV) fluoride

26. Writing Chemical Formulas for Transition Metals Practice
Lead (IV) carbonate Pb(CO3)2
Copper (II) nitrate Cu(NO3)2
Iron (III) oxide Fe2O3
Tin (IV) fluoride SnF4

27. Writing Chemical Names for Transition Metals Practice
Fe(NO3)2
CuF2
NiS
FeCl2

28. Writing Chemical Names for Transition Metals Practice
Fe(NO3) iron (II) nitrate
CuF copper (II) fluoride
NiS nickel (II) sulfide
FeCl2 iron (II) chloride

29. Writing Chemical Formulas Practice
zinc carbonate
barium oxide
cadmium fluoride
magnesium sulfide
lithium phosphate

30. Writing Chemical Formulas Practice
zinc carbonate ZnCO3
barium oxide BaO
cadmium fluoride CdF2
magnesium sulfide MgS
lithium phosphate Li3PO4

31. Writing Chemical Names Practice
FeF2
FeF3
Hg2Br2
HgBr2

32. Writing Chemical Names Practice
FeF iron (II) fluoride
FeF iron (III)fluoride
Hg2Br2 mercury (I) bromide
HgBr2 mercury (II) bromide

33. Writing Chemical Names Practice
BaSO4
FeF2
CuCO3
CaS
MgO
KCl

34. Writing Chemical Names Practice
BaSO4 barium sulfate
FeF2 iron (II) fluoride
CuCO3 copper (II) carbonate
CaS calcium sulfide
MgO magnesium oxide
KCl potassium chloride

35. NO
N2O
NO2
N2O5
N2O3

36. NO nitrogen monoxide
N2O dinitrogen monoxide
NO nitrogen dioxide
N2O5 dinitrogen pentoxide
N2O dinitrogen trioxide