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Ionic Nomenclature

2. D.1 Intro: Elements, Compounds and Nomenclature
Chemical nomenclature: the organized system used to name substances and write their chemical formulas.
Chemical formula: represents the number of each kind of atom bonded together in a substance.
Subscript: indicates the number of atoms or ions present in the formula.

3. D.1 Intro: Elements, Compounds and Nomenclature
Example (formula for water):

4. D.2 The History of Chemical Nomenclature
Lavoisier’s system of nomenclature is sometimes called the Classical System.
This system of naming is used to the present day.
Common Name
Systematic Name
fixed air
carbon dioxide
cinnabar
mercuric sulfide

5. D.2 The History of Chemical Nomenclature
Chemical formulas of compounds…
are written using two or more symbols side by side.
use subscripts to make the formulas more compact.
Example: carbon dioxide
Dalton formula:
Berzelius formula: CO2

6. D.2 The History of Chemical Nomenclature
Many elements form several compounds with another given element.
Lavoisier’s Classical System was modified to include suffixes to name these compounds:
Examples:
ferric oxide Fe2O3
ferrous oxide FeO
(More will be said on this in Section D.6.)

7. D.2 The History of Chemical Nomenclature
Examples:
Chemical
Formula
Classical
System
Stock
FeCl2
ferrous chloride
iron(II) chloride
FeCl3
ferric chloride
iron(III) chloride
FeO
ferrous oxide
iron(II) oxide
Fe2O3
ferric oxide
iron(III) oxide

8. D.3 Classification of Compounds
Ionic compounds are formed when oppositely charged ions are attracted to each other.
Strong electrostatic attractions.
High melting point and boiling point solids.
Capable of dissolving in water.

9. D.3 Classification of Compounds
Cations are positively-charged ions.
Examples:
Na+, K+, Ca2+, Al3+, Fe3+
Anions are negatively-charged ions.
Examples:
Cl–, F–, S2–, Se2–, P3–

10. D.3 Classification of Compounds
Molecular compounds are pure substances composed of atom groupings called molecules.
strong covalent bonds between atoms
atoms share electrons
each atom has a noble-gas electron arrangement
possess weak bonds between molecules
low melting point and boiling point gases, liquids and solids

11. D.4 Binary Ionic Compounds
Molecular Formula:
Chemical formula for molecular substances.
The actual number of each kind of atom present in the molecule.
Empirical Formula:
Indicates the simplest whole number ratio of atoms or ions in the compound.

12. D.4 Binary Ionic Compounds
Naming Binary Ionic Compounds
When naming any ionic compounds, simply write the name of the positive ion followed by the name of the negative ion.
The rules for naming simple ions were given in Unit B.

13. D.4 Binary Ionic Compounds
Name the cation by writing the full name of the metallic element.
Na+ is a sodium ion
Zn2+ is a zinc ion
Al3+ is an aluminum ion.
Name the anion by abbreviating the full name of the nonmetallic element and adding –ide.
Cl– is a chloride ion
S2– is a sulfide ion
P3– is a phosphide ion

14. D.4 Binary Ionic Compounds
Examples:
NaCl {from Na+Cl–}
sodium chloride
Sodium chloride is table salt.
CaCl2 {from Ca2+(Cl–)2}
calcium chloride
Calcium chloride is a drying agent also used to melt ice.

15. D.4 Binary Ionic Compounds
Writing Chemical Formulas for Binary Ionic Compounds
When given the name of the ionic compound, first write the symbols for the ions involved.
Next, determine the lowest whole number ratio of ions that will provide an overall net charge of zero.
(Criss-Cross)

16. D.4 Binary Ionic Compounds
Examples:

17. D.4 Binary Ionic Compounds
Examples:

18. D.4 Binary Ionic Compounds
Examples: