How can we find the oxidation no. In any compound?

Question

Answer

The oxidation number of a free element is always 0.

The oxidation number of a monatomic ion equals the charge of the ion.

The oxidation number of H is +1, but it is -1 in when combined with less electronegative elements.

The oxidation number of O in compounds is usually -2, but it is -1 in peroxides.

The oxidation number of a Group 1 element in a compound is +1.

The oxidation number of a Group 2 element in a compound is +2.

The oxidation number of a Group 17 element in a binary compound is -1.

The sum of the oxidation numbers of all of the atoms in a neutral compound is 0.

The sum of the oxidation numbers in a polyatomic ion is equal to the charge of the ion.

Answer

Yes i give a answer so please give a question

Answer

Split the compound in cation and anion. by splitting it, write the electrons required for any atoms over it and keeping in mind that make the compound over all neutral that is zero!

Answer

Introduction:
Determining the oxidation number (also known as oxidation state) of an element in a compound is crucial for understanding its chemical behavior. The oxidation number indicates the electron transfer that occurs when atoms form compounds, helping us identify the charge of an atom in a compound. Here are the steps to find the oxidation number in any compound:

Step 1: Identify the compound and its formula:
Before determining the oxidation number, it is important to know the chemical formula of the compound. This will enable us to identify the types and number of elements involved.

Step 2: Understand the general rules:
There are specific rules to assign oxidation numbers to elements in compounds. Familiarizing yourself with these rules is essential. Some key rules include:

1. The oxidation number of an element in its free or uncombined state is always zero.
2. The oxidation number of a monatomic ion is equal to its charge.
3. The sum of oxidation numbers in a neutral compound is always zero.
4. In most cases, oxygen has an oxidation number of -2, and hydrogen has an oxidation number of +1.
5. The oxidation number of a halogen (Group 17 elements) is typically -1.
6. The sum of oxidation numbers in a polyatomic ion is equal to its charge.

Step 3: Apply the rules:
Once you have the compound's formula and the rules in mind, follow these guidelines to find the oxidation number:

1. Consider the oxidation numbers of known elements: Start by determining the oxidation numbers of elements that have known oxidation numbers based on the rules. For example, in H2O (water), oxygen is typically -2, and hydrogen is +1.

2. Use the sum of oxidation numbers rule: For compounds with no charge, the sum of oxidation numbers must equal zero. Utilize this rule to find the oxidation number of an unknown element. For instance, in NO3- (nitrate ion), the sum of the oxidation numbers (-2 from each oxygen and -1 from the overall charge) must equal -1. Therefore, the nitrogen atom has an oxidation number of +5.

3. Balance oxidation numbers in polyatomic ions: In polyatomic ions, the sum of oxidation numbers equals the charge of the ion. For example, in SO4^2- (sulfate ion), the sum of oxidation numbers (-2 from each oxygen and -2 from the overall charge) must equal -2. Therefore, the sulfur atom has an oxidation number of +6.

Conclusion:
Determining the oxidation number of elements in compounds is a vital skill in chemistry. By following the general rules and applying them to the compound's formula, one can assign oxidation numbers accurately. Remember to consider the known oxidation numbers, use the sum of oxidation numbers rule, and balance oxidation numbers in polyatomic ions. Understanding oxidation numbers enhances comprehension of chemical reactions and the behavior of elements in compounds.

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