Calculate the oxidation state of the central ion in [CoCl4(NH3)2]-1
To calculate the oxidation state of the central ion in [CoCl4(NH3)2]-1, we need to take into account the charges of the ligands and any known oxidation states for the other elements.
The chloride ligands have a charge of -1 each, and there are four of them, so their total charge is -4.
The ammonia ligands (NH3) are neutral, so they do not contribute any charge.
To find the oxidation state of the central ion (Co), we can use the equation:
Charge of central ion + Charge of ligands = 0
Let x be the oxidation state of Co.
x + (-4) + 0 = -1
x - 4 = -1
x = -1 + 4
x = +3
Therefore, the oxidation state of the central ion (Co) in [CoCl4(NH3)2]-1 is +3.
To determine the oxidation state of the central ion in [CoCl4(NH3)2]-1, we need to assign oxidation states to each atom in the compound:
1. Start by considering the known oxidation states of other atoms. Chlorine (Cl) usually has an oxidation state of -1, and hydrogen (H) usually has an oxidation state of +1.
2. Since the compound is negatively charged (indicated by the -1), the sum of the oxidation states of the individual atoms must equal -1 to balance the charge.
3. Calculate the oxidation state of ammonia (NH3). Hydrogen is +1, so a total of +6 is needed to balance the overall charge of -1. Since there are two ammonia molecules, the nitrogen ion (N) must have an oxidation state of -3 to achieve a total of -6.
4. Now let's consider the chloride ions (Cl). Each chloride ion has an oxidation state of -1, meaning that the sum of the oxidation states of the four chloride ions is -4.
5. Since the overall charge of the compound is -1, the sum of all the oxidation states must equal -1. Therefore, the central cobalt ion (Co) must have a positive oxidation state equivalent to (-1 - (-4)) = +3 to balance the charges.
So, the oxidation state of the central cobalt ion in [CoCl4(NH3)2]-1 is +3.