what is the oxidation number of S in this molecule? ### Chemical Structures and Compounds#### SSF₂ and S₂F₄ Diagrams1. **SSF₂**: This molecular formula indicates a compound consisting of sulfur and fluorine atoms. The structure is not depicted in the image.2. **S₂F₄ Structure**: - The chemical structure shows a compound with two sulfur (S) atoms and four fluorine (F) atoms. - The diagram illustrates the molecular bonding between these atoms: - One sulfur atom is bonded to three fluorine atoms. - The second sulfur atom is bonded to a single fluorine atom and linked to the first sulfur atom. - The bonds between sulfur and fluorine indicate the angles and spatial arrangement: - Straight lines represent bonds projecting in the plane of the paper. - The solid wedge represents a bond coming out of the plane towards the viewer. - The hashed wedge indicates a bond going behind the plane away from the viewer.This structure helps visualize the three-dimensional arrangement of atoms in the S₂F₄ molecule, which is crucial for understanding its chemical properties and reactions. This image shows the Lewis structure of sulfur tetrafluoride (SF₂). The diagram represents the molecular structure including atom arrangements and bonding.### Explanation:1. **Central Atoms**: - The central sulfur (S) atom at the bottom is bonded to two fluorine (F) atoms. - The top sulfur (S) atom is double-bonded to the central sulfur atom.2. **Bonding**: - Single bonds are depicted by a single line (─) between the sulfur and each fluorine atom. - A double bond, represented by two lines (═), connects the two sulfur atoms.3. **Lone Pairs**: - Each fluorine atom has three pairs of dots around it, indicating three lone pairs of electrons. - The top sulfur atom has one pair of dots, showing one lone pair of electrons. - The central sulfur atom has one lone pair as well, shown by the two dots at the bottom.This diagram is a visual representation used to understand the electron-sharing and position of atoms within sulfur tetrafluoride.

Oxidation number or oxidation state is the hypothetical charge which an atom will have if all its bonds to attached atoms are ionic. Consider a molecule AB, we know the oxidation state of B = -2 but we don't know the oxidation state of A, we can calculate it as follows: Let oxidation state of A = x Sum of charge on molecule = 0, because the molecule is neutral x + (-2) = 0 x = +2 Oxidation state of A = +2