Question

What is the oxidation state of hydrogen in $H_{2}O$ and $H_2{O}_2$ respectively?

Answer 1

Hint: In basic words, the oxidation number is the number assigned to the components in a chemical combination. The oxidation number is the total number of electrons that atoms in a molecule can share, lose, or acquire while establishing chemical interactions with atoms of another element.

Complete answer:
The oxidation state is also known as the oxidation number. However, depending on whether we are considering the electronegativity of the atoms or not, these phrases might have a different meaning. In coordination chemistry, the word oxidation number is widely employed. In general, the oxidation state or number aids in the description of electron transmission. However, students should be aware that this is not the same as a formal charge, which dictates atom configuration. In redox processes, the oxidation number/state is also utilised to determine the changes that occur. In the meanwhile, it's quite similar to valence electrons. In $H_{2}O$ and $H_2{O}_2$ , the oxidation state of hydrogen is +1.
The degree of oxidation of an atom in a chemical compound is indicated by its oxidation state. The degree of oxidation of an atom is proportional to its oxidation state; the degree of reduction is proportional to its oxidation state. Because each hydrogen in hydrogen peroxide gives up a single electron to oxygen, each hydrogen nevertheless retains an oxidation number of +1. Because each oxygen gets just one electron from its neighbouring hydrogen, oxygen has an oxidation number of -1. Hydrogen has an oxidation number of +1 in water because it has lost one electron. Because the single oxygen atom has received a total of two electrons, one from each hydrogen, oxygen has an oxidation number of +2.

Note:
The higher the charge, the more difficult it is to remove an electron, resulting in a larger ionisation energy. As a result, the removal of 10 electrons is very speculative. Similarly, when the negative charge increases, adding an electron becomes more difficult. Larger than three oxidation states, whether positive or negative, are nearly inconceivable. Regardless of the assumption, it aids in comprehending the changes that occur when an atom undergoes a chemical transition.