SUMMARY
The oxidation numbers for the compounds discussed are as follows: in KClO3, chlorine (Cl) has an oxidation number of +5, potassium (K) is +1, and oxygen (O) is -2. For the ammonium ion (NH4+), nitrogen (N) has an oxidation number of -3, while hydrogen (H) is +1. In the dichromate ion (Cr2O72-), chromium (Cr) has an oxidation number of +6, and in the manganate ion (MnO42-), manganese (Mn) has an oxidation number of +6. These values are derived from established oxidation number rules, ensuring that the overall charge of the molecule or ion is balanced.
PREREQUISITES
- Understanding of oxidation number rules
- Familiarity with chemical formulas and their components
- Basic knowledge of ionic and molecular compounds
- Ability to perform simple algebraic calculations
NEXT STEPS
- Study the rules for determining oxidation states in various compounds
- Learn about the exceptions to oxidation number rules
- Explore the significance of oxidation numbers in redox reactions
- Investigate the applications of oxidation states in coordination chemistry
USEFUL FOR
Chemistry students, educators, and professionals interested in redox chemistry and the determination of oxidation states in various chemical compounds.