Assign oxidation numbers to each element in the following compounds. (f) H2PtCl6

Verified step by step guidance

1. Step 1: Understand the compound structure. H2PtCl6 is a coordination compound where Pt is the central metal atom surrounded by 6 Cl ligands and 2 H atoms.
2. Step 2: Assign oxidation numbers to hydrogen. In most compounds, hydrogen has an oxidation number of +1. Since there are 2 hydrogen atoms, the total contribution from hydrogen is +2.
3. Step 3: Assign oxidation numbers to chlorine. Chlorine typically has an oxidation number of -1. Since there are 6 chlorine atoms, the total contribution from chlorine is -6.
4. Step 4: Use the rule that the sum of oxidation numbers in a neutral compound is zero. Set up the equation: 2(+1) + x + 6(-1) = 0, where x is the oxidation number of Pt.
5. Step 5: Solve the equation for x to find the oxidation number of Pt.

Key Concepts

Oxidation Number

An oxidation number is a theoretical charge assigned to an atom in a compound, reflecting its degree of oxidation or reduction. It helps in understanding electron transfer in redox reactions. The oxidation number can be positive, negative, or zero, depending on the atom's bonding and electron sharing with other atoms.

Rules for Assigning Oxidation Numbers

There are specific rules for assigning oxidation numbers, such as: the oxidation number of an element in its standard state is zero, the oxidation number of a monatomic ion equals its charge, and in compounds, hydrogen typically has an oxidation number of +1 while oxygen usually has -2. These rules guide the determination of oxidation states in complex compounds.

Complex Ions and Coordination Compounds

Complex ions consist of a central metal atom bonded to surrounding ligands, which can be neutral molecules or ions. In coordination compounds like H2PtCl6, the oxidation state of the central metal (platinum) is influenced by the charges of the ligands. Understanding the structure and bonding in these compounds is essential for accurately assigning oxidation numbers.