Sulphur can exists in several oxidation states.
The oxidation state is the number of electrons in the outer energy shell of electrons, involved in bonding.
So for
Sulphuric Acid (H2SO4) sulphur is in oxid'n state '+6'. It makes two double bonds with two oxygen atoms, ; 4 bonds. It then makes a further two single bonds with the remaining two oxygen atoms, 2 bonds. Hence 4 + 2 = 6 bonds.
The two singly bonded oxygen atoms then combine with the two hydorgen atoms by single bonds(Not involving the sulphur).
Sulphurious Acid (H2SO3) sulphur is in oxid'n state '+4'. It makes one double bonds with one oxygen atom, ; 2 bonds. It then makes a further two single bonds with the remaining two oxygen atoms, 2 bonds. Hence 2 + 2 = 4 bonds.
The two singly bonded oxygen atoms then combine with the two hydorgen atoms by single bonds(Not involving the sulphur).
Atomic sulphur is in oxidation state zero'0' no bonds.
Hydrogen sulphide is in oxidation state '-2' ; Note the minus sign, This is because the electrons are 'donated' in the opposite direction, to the above molecules.
NB Sulphur can also form an oxidation state ( makes two ) '2'
When atoms bond together they make molecules or compounds, depending on if the atom bonds with another atom of the same species or a different chemical
Sulfur chlorides are: SCl2, S2Cl2, S3Cl2, SCl4.
Chemical bonds are formed by the sharing or donating of electrons. The electrons that atoms use to make chemical bonds are the outermost electrons, also known as valence electrons.
Carbon can only make a triple bond with 1 atom.
A hydrogen atom can form one chemical bond. This is because it has one electron in its outer shell and needs one more electron to achieve a stable electron configuration, similar to that of the nearest noble gas, helium. Therefore, hydrogen typically forms a single covalent bond by sharing its electron with another atom.
Electrons.
Valence electrons are used to make bonds. These are the outermost electrons of an atom, which are involved in the formation of chemical bonds with other atoms.
The outer energy shell of electrons. The inner energy shells of electrons do NOT take part in chemical bonding. Not all outer energy shell electrons take part in bonding. Those electrons that DO take part in bonding are described as 'oxidation state'. Taking ammonia as an example. Its formula is NH3 Nitrogen's electronic configuration is is 1s2(inner most shell), 2s2(intermediate shell), 2p5(outer most/valence shell). The '5' is the number of electrons in this shell. Nitrogen combines with 3 hydrogens , using up three of these 5 electrons. The other 2 electrons remain as an unused 'lone pair'. Because it has used three electrons in bonding with hydrogen, then its oxidation state can be described as '+3'.
When atoms bond together they make molecules or compounds, depending on if the atom bonds with another atom of the same species or a different chemical
Sulfur can make 6 bonds because it has 6 valence electrons available for bonding with other atoms. This allows sulfur to form multiple bonds with other elements, increasing its bonding capacity.
A hydrogen bond is a type of chemical bond. A hydrogen atom bonds with either a nitrogen, fluorine, or oxygen atom to make a weak bond.
1 sulfur atom and 2 hydrogen atoms combine to form hydrogen sulfide gas, with the chemical formula H2S.
The number of sulfur atoms in a compound depends on the chemical formula of the compound. For example, in sulfur dioxide (SO2), there is one sulfur atom, while in sulfuric acid (H2SO4), there are one sulfur atom.
The atoms rearrange and the new bonds form to make the new substances.
The sulfate ion is held together by covalent bonds between the sulfur atom and the oxygen atoms. These covalent bonds involve the sharing of electrons between the atoms to form a stable molecular structure.
covalent bonds
It is not a chemical change, unless you heat it sufficiently to make it catch fire.