Naming ionic compounds

1. Naming ionic compounds Chapter 6.3 Notes

2. Naming Ionic Compounds • Naming Ionic Compounds • The name of an ionic compound must distinguish the compound from other ionic compounds containing the same elements. • The formula of an ionic compound describes the ratio of the ions in the compound.

3. Binary Ionic Compounds • Binary Ionic Compounds • A compound made from only two elements is a binary compound. • The pattern for naming binary ionic compounds is the cation followed by the name of the anion.

4. Binary Ionic Compounds • The name for the cation is the name of the metal without any changes while the name of the anion uses part of the name of the nonmetal with the suffix –ide at the end.

5. Metals With Multiple Ions • Metals With Multiple Ions • When a metal forms more than one ion, the name of the ion contains a Roman numeral to indicate the charge on the ion.

6. Metals With Multiple Ions • Ex.1) Copper(I) Oxide VS. Copper(II) Oxide • The chemical formula for copper(I) oxide is Cu2O because it takes two Cu1+ ions to balance the charge on an O2- ion.

7. Metals With Multiple Ions • The chemical formula for copper(II) oxide is CuO because it takes only one Cu2+ ion to balance the charge on an O2- ion.

8. Polyatomic Ions • Polyatomic Ions • A covalently bonded group of atoms that has a positive or negative charge and acts as a unit is a polyatomic ion. • The prefix poly means many.

9. Polyatomic Ions • Ex. 2) Iron(III) Hydroxide • Chemical formula = Fe(OH)3, The parentheses and subscript 3 indicates that there are three hydroxide ions for each iron (III) ions.

10. Writing Formulas for Ionic Compounds • Writing Formulas for Ionic Compounds • If you know the name of an ionic compound, you can write its formula. • Place the symbol of the cation first, followed by the symbol of the anion.

11. Writing Formulas for Ionic Compounds • Use subscripts to show the ratio of the ions in the compound. • Because all compounds are neutral, the total charges on the cations and anions must add up to zero.

12. Writing Formulas for Ionic Compounds • Ex. 3) Sulfur and Sodium • There must be two sodium ions (Na+) for each sulfide ion (S2-). The formula for sodium sulfide is Na2S. The 2- charge on one sulfide ion is balanced by the 1+ charges on two sodium ions.

13. Ex. 4) Write the formula for the compound calcium chloride

14. Ex. 5) Write the formula for the compound calcium oxide

15. Ex. 6) Write the formula for the compound copper(II) sulfide

16. Ex. 7) Write the formula for the compound sodium sulfate

17. Describing Molecular Compounds • Describing Molecular Compounds • In naming molecular compounds the focus is on the composition of molecules. • The name and formula of a molecular compound describe the type and number of atoms in a molecule of the compound.

18. Describing Molecular Compounds • In naming molecular compounds the most metallic element appears first in the name. These elements are farther to the left and bottom of the periodic table. • You first must add the proper prefix to each element. The prefix tells us how many atoms of each element there are. • The name of the second element ends in ide. Such as Carbon Dioxide.

20. Example 8 Name the compound N2O4. • There are two nitrogen atoms and four oxygen atoms. Therefore the name is dinitrogentetraoxide.

21. Example 9 Name the compound NO2. • There is one nitrogen atom and two oxygen atoms. Therefore the name is mononitrogen dioxide. However the prefix mono- is generally not used, therefore the name is nitrogen dioxide.

22. Example 10 Write the formula for diphosphorustetrafluoride. • Since di- means two and tetra means four the formula is P2F4.