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2025年6月21日 · Answer: Oxygen primarily exhibits oxidation states of −2 (most common in oxides), −1 (in peroxides), +1 (in O2 F2 ), and +2 (in OF2 ). It does not show higher positive oxidation states like …
2021年11月2日 · Oxygen being highly electronegative, it mostly shows an oxidation state of – 2 only. Other members of the family like sulphur, have vacant d-orbitals, thereby giving four and six halffilled …
Oxygen usually shows −2 state due to its high electronegativity and the preference to gain or share two electrons. Sulphur exhibits +2, +4, and +6 oxidation states through excitation and hybridisation …
Other elements of this family show +2, +4 or +6 oxidation state because they are not as electronegative as oxygen. Due to an increase in the number of electron shells down the group electronegativity …
Since oxygen atom does not have 2d orbitals, no electorn promotion is possible in this case. Therefore, oxygen cannot show `+4 " and " +6` oxidation states in compounds.
Flashcards: Oxygen and Sulphur of Chemistry helps you revise the topic with practice questions, key-concepts and engaging question answer. Access them on EduRev.
### Step 1: Understanding Oxidation States Oxygen typically has an oxidation state of -2 in most of its compounds. However, it can exhibit other oxidation states under certain conditions.
-Oxygen fluorides are strong oxidising agents with high energy and can release their energy either instantaneously or at a controlled rate. Thus, these compounds attracted much attention as potential …
Oxygen can show an oxidation state of -2 (in oxides), -1 (in peroxides) +1 (in O2F2) and +2 (in OF2).
That means two bonds. Other elements in the same group have d subshell available as well, and it means that they can form more than two bonds.
