This preview shows pages 1–2. Sign up to view the full content.
This preview has intentionally blurred sections. Sign up to view the full version.View Full Document
Unformatted text preview: 1. Sodium nitrate 2. Ammonia 3. Zinc oxide 4. Water 5. Calcium hydride 6. Carbon dioxide 7. Nitrogen 8. Potassium sulfate 9. Barium phosphate 10. Hydrogen peroxide 11. Oxygen difluoride 12. Methane Helpful Hints! Pure (uncombined) elements have an oxidation state of zero In covalent compounds, the more electronegative element will be assigned the negative oxidation state Hydrogen will be negative when combined with a metal, and positive when combined with a nonmetal Conclusions Redox reactions involve the transfer of electrons Oxidation is the loss of electrons Reduction is the gain of electrons Use the reference table to help assign oxidation states to elements Uncombined elements, oxidation state = 0 Hydrogen can be +/- (depends on what it is bonded to) Look at EN values for covalent compounds...
View Full Document
This note was uploaded on 01/01/2012 for the course CHEM 101 taught by Professor Donahue during the Spring '11 term at Long Island U..
- Spring '11