The oxidation number of potassium in KClO3 is +1. This is because the overall charge of the compound is 0, and the oxidation number of oxygen is usually -2. Therefore, the oxidation number of potassium can be calculated by setting up the equation: x + (-2) + (-2) + (-2) = 0. Solving for x gives a value of +1.
The oxidation number of nitrogen in NH4+ is -3. This is because the overall charge of the compound is +1, and the oxidation number of hydrogen is usually +1. Therefore, the oxidation number of nitrogen can be calculated by setting up the equation: (-3) + 4(+1) = +1. Solving for x gives a value of -3.
The oxidation number of chromium in Cr2O72- is +6. This is because the overall charge of the compound is -2, and the oxidation number of oxygen is usually -2. Therefore, the oxidation number of chromium can be calculated by setting up the equation: 2x + 7(-2) = -2. Solving for x gives a value of +6.
The oxidation number of manganese in MnO42- is +7. This is because the overall charge of the compound is -2, and the oxidation number of oxygen is usually -2. Therefore, the oxidation number of manganese can be calculated by setting up the equation: x + 4(-2) = -2. Solving for x gives a value of +7.
To determine the oxidation numbers of a compound, you can follow a few steps. First, identify the elements in the compound and their known oxidation numbers. Then, set up an equation using the overall charge of the compound and the known oxidation numbers. Finally, solve for the unknown oxidation numbers by balancing the equation. Keep in mind that some elements, like hydrogen and oxygen, have common oxidation numbers that can be used as a guide. Additionally, the sum of all oxidation numbers in a neutral compound should equal 0, while in an ion, it should equal the overall charge of the ion.