In S2Cl2, each sulfur atom has an oxidation number of 0, and each chlorine atom has an oxidation number of -1.
The oxidation number of Cl in PtCl4^2- is -1. This can be determined by considering that the overall charge of the complex ion is 2-, and each Cl atom has an oxidation number of -1.
The oxidation number of Cl in Cl4 is -1. Since there are four Cl atoms, the total charge contributed by Cl is -4, making the oxidation number of each Cl atom -1.
The oxidation number of Sn in SnCl2 is +2. This is because Cl is more electronegative than Sn, so each Cl atom has an oxidation number of -1, leaving Sn with an oxidation number of +2 to balance the charges.
Chlorine typically has an oxidation number of -1 in its compounds, but to determine the oxidation number of Cl in Cl3, you would divide the total charge (+3) by the three atoms, resulting in an oxidation state of +1 for each Cl atom.
In S2Cl2, each sulfur atom has an oxidation number of 0, and each chlorine atom has an oxidation number of -1.
The oxidation number of Cl in PtCl4^2- is -1. This can be determined by considering that the overall charge of the complex ion is 2-, and each Cl atom has an oxidation number of -1.
The oxidation number of Cl in Cl4 is -1. Since there are four Cl atoms, the total charge contributed by Cl is -4, making the oxidation number of each Cl atom -1.
The oxidation number of Sn in SnCl2 is +2. This is because Cl is more electronegative than Sn, so each Cl atom has an oxidation number of -1, leaving Sn with an oxidation number of +2 to balance the charges.
Chlorine typically has an oxidation number of -1 in its compounds, but to determine the oxidation number of Cl in Cl3, you would divide the total charge (+3) by the three atoms, resulting in an oxidation state of +1 for each Cl atom.
The oxidation number of S in S2Cl2 is +1. Each Cl atom has an oxidation number of -1, and since the molecule is neutral, the overall oxidation numbers of S must balance out to zero. Thus, the oxidation number of S in this compound is +1.
The oxidation number of C in CCl4 is +4, while the oxidation number of Cl is -1. Each Cl atom in CCl4 has an oxidation number of -1, and since there are four Cl atoms, the total negative charge from Cl is -4. The sum of the oxidation numbers in a neutral compound is zero, so the oxidation number of C must be +4 to balance the charge.
The oxidation number for Cl in ClO3- is +5. This is because the overall charge of the ion is -1, and each oxygen atom has an oxidation number of -2.
The oxidation number of Cl in Cl2 is 0 because in a diatomic molecule, each atom shares the electrons equally, resulting in no charge difference.
In HgCl2, mercury's oxidation number is 2+ and chlorine's is 1-.
In TiCl4, the oxidation number of titanium (Ti) is +4 since each chlorine atom (Cl) has an oxidation number of -1. Overall, the sum of the oxidation numbers in TiCl4 equals zero, indicating a neutral compound.
The oxidation number of chlorine in ClO4 is +7. Each oxygen atom has an oxidation number of -2 and the overall charge of the ion is -1, which means the oxidation number of chlorine must be +7 to balance the charge.