1. Ch. 6 Chemical Names and Formulas
Distinguish between chemical formulas, molecular formulas, and formula units
Distinguish between ionic and molecular compounds
Define cation and anion and relate them to metal and nonmetal
Define polyatomic ion and give the names and formulas of the most common polyatomic ions
Apply the rules for naming and writing formulas for ionic compounds
Apply the rules for naming and writing formulas for molecular compounds
Name and write the formulas for common acids

2. Types of Chemical Formulas
Distinguish between chemical formulas, molecular formulas, and formula units
Chemical Formulas
Show the kinds and number of atoms in the smallest representative unit of a substance
Types of Chemical Formulas
Monatomic formulas
Single atom, formula is their atomic symbol (He, Ne)
Diatomic formulas
Two atoms
There are 7 (H2, F2, N2, O2, Cl2, Br2, I2)

3. Distinguish between chemical formulas, molecular formulas, and formula units
Shows the kinds and numbers of atoms in a molecule of a compound (covalent)
Ex:
H2O (water, two hydrogen atoms, one oxygen atom)
NH3 (ammonia, one nitrogen atom, three hydrogen atoms)

4. Distinguish between chemical formulas, molecular formulas, and formula units
Ionic Compounds
The chemical formula does not represent a molecule
Ionic solids are positive and negative ions arranged in continuous arrays
The formula unit represents the lowest number ratio of ions in the compound

5. Distinguish between ionic and molecular compounds
Ionic Compounds
Made up of cations and anions
Cations: positive ions, metals
Anions: negative ions, nonmetals
Ex: NaCl
Na+ (cation)
Cl- (anion)

6. Define cation and anion and relate them to metal and nonmetal
Monatomic Cations (one atom)
Element
Cation
Charge
Aluminum
Al3+ 3+
Barium
Ba2+ 2+
Hydrogen H+ 1+
Silver
Ag+
Sodium
Na+

7. Define cation and anion and relate them to metal and nonmetal
Monatomic Anions (name ends in -ide)
Element
Anion
Charge
Chloride
Cl- 1-
Oxide
O2- 2-
Nitride
N3- 3-

8. Define cation and anion and relate them to metal and nonmetal
Oxidation State
when an atom loses electrons, it is said to be oxidized
Oxidation of an atom may have nothing to do with oxygen, some metals have more than one oxidation state

9. Define cation and anion and relate them to metal and nonmetal
Formula
Charge
Classical Name
Iron (II)
Fe2+ 2+
Ferrous
Iron (III)
Fe3+ 3+
Ferric
Chromium (II)
Cr2+
Chromous
Chromium (III)
Cr3+
Chromic
Tin (II)
Sn2+
Stannous
Tin (IV)
Sn4+ 4+
Stannic

10. Define polyatomic ion and give the names and formulas of the most common polyatomic ions
Polyatomic Cations (more than one atom)
Cation
Formula
Charge
Ammonium
NH4+ 1+
Mercury (I)
Hg22+ 2+

11. Define polyatomic ion and give the names and formulas of the most common polyatomic ions
Polyatomic Anions: name ends in -ite or -ate
Anion
Formula
Charge
Carbonate
CO32- 2-
Bicarbonate
HCO3- 1-
Nitrite
NO2-
Nitrate
NO3-
Sulfate
SO42-

12. Apply the rules for naming and writing formulas for ionic compounds
Binary Ionic Compounds – Name Ends in “ide”.
Two types of atoms (different elements)
May have more than one atom of each element
Balance cations with anions
Ex: Sodium chloride Na+ + Cl- NaCl
Iron (III) oxide _Fe3+ + _O2- Fe2O3

13. Apply the rules for naming and writing formulas for ionic compounds
Ternary Ionic Compounds – Name of the “polyatomic anion”
Three types of atoms (different elements)
Ex: Sodium carbonate
Na+ + CO32- Na2CO3

14. Apply the rules for naming and writing formulas for ionic compounds
Quaternary Ionic Compounds – Name of the “polyatomic anion”.
Four types of atoms (different elements)
Ex: Ammonium sulfate
NH4+ + SO42- (NH4)2SO4

15. Apply the rules for naming and writing formulas for ionic compounds
Ionic Naming Rules
the cation is always named first
name does not change
the anion is named second
anion is monatomic add –ide
anion is polyatomic add –ate or –ite (check chart)
LiCl Lithium chloride
Sn(NO3)4 Tin (IV) nitrate
Stop go to Ionic Naming handout

16. Binary Molecular Compounds
Apply the rules for naming and writing formulas for molecular compounds
Binary Molecular Compounds
Composed of two nonmetallic elements
Ionic charges are not used to assign formulas or names
Elements often combine in a number of different ways

17. Binary Molecular Compounds
Apply the rules for naming and writing formulas for molecular compounds
Binary Molecular Compounds
Carbon and Oxygen
Formula
Form
Carbon dioxide
CO2
Gas
Carbon monoxide CO
Poison Gas
Carbonate
CO32-
Anion
Oxalate
C2O22-

18. Binary Molecular Compounds
Apply the rules for naming and writing formulas for molecular compounds
Binary Molecular Compounds
Prefixes tell how many atoms of each element are present in each molecule
Prefix
Number
Mono- 1
Hexa- 6
Di- 2
Hepta- 7
Tri- 3
Octa- 8
Tetra- 4
Nona- 9
Penta- 5
Deca- 10

19. Binary Molecule Compounds
Apply the rules for naming and writing formulas for molecular compounds
Binary Molecule Compounds
If there is a single atom of the first element in the name, omit the mono-
Ex: Carbon dioxide, not monocarbon dioxide
The second element in the name ends with -ide
Sometimes a vowel gets dropped when the prefix is added
Ex: monoxide not monooxide

20. Apply the rules for naming and writing formulas for molecular compounds
Naming Common Acids
Formula: anions connected to as many hydrogen ions as required to make electrically neutral
Acid formed from halogens (F, Cl, Br) use the prefix hydro-
EX: HCl hydochloric acid; HF hydrofluoric acid
Acid names
drop the -ate or -ide from the anion and add -ic acid -OR-
drop the -ite and add -ous

21. Apply the rules for naming and writing formulas for molecular compounds
Acid
Formula
Anion
Hydrogen Ions
Hydrochloric acid
HCl
Cl-
1 H+
Hydrofluoric acid HF F-
Sulfuric acid
H2SO4
SO42-
2 H+
Sulfurous acid
H2SO3
SO32-
Nitric Acid
HNO3
NO3-
Acetic Acid
HC2H3O2
C2H3O2-
Phosphoric acid
H3PO4
PO43-
3 H+
Carbonic Acid
H2CO3
CO32-

22. second atom gets prefix and –ide at the end CO2 carbon dioxide
Apply the rules for naming and writing formulas for molecular compounds
Covalent Naming Rules
if first atom is monatomic do not add a prefix, if polyatomic add a prefix
second atom gets prefix and –ide at the end
CO2 carbon dioxide
Cl2O dichlorine monoxide

23. Use your chart and pg. 147 for help with naming
Apply the rules for naming and writing formulas for ionic and molecular compounds
PRACTICE PROBLEMS
Pg , 56, 58, 61, 62, 64-66
Use your chart and pg. 147 for help with naming