Electron configuration of sulfur

The Electron configuration of sulfur is 32S, 33S, 34S and 36S. Sulfur is a non-metallic chemical element on the periodic table, which is represented by its symbol S and atomic number 16. It is found creating sulfonals and sulfides in its reduced form, and in volcanic regions in its native form.

It has a brownish, strongly yellowish or orange appearance and usually burns with a blue flame, which indicates the release of sulfur dioxide. It cannot dissolve in water but it can dissolve in benzene and carbon disulfide.

sulfur isotopes.

Sulfur has a total of 25 isotopes of which only 4 are stable, these are: 32S, 33S, 34S and 36S. On the other hand, 35S isotope is created when cosmic radiation strikes argon-40, thus exhibiting a half-life of 87 days, the remaining radioactive isotopes are short-lived.

Electron configuration.

The number of electrons that the sulfur atom has will always be the same number of protons, i.e. it will always be 16.

To know the set of quantum numbers of the final electron of the sulfur atom, we make the diagonal diagram until we cover the 16 electrons, where we obtain the following Electron configuration:

S= 1s22s22p63s23p4

In this case, the first two numbers are obtained by following the 3p4 configuration, where n will correspond to the number located before the sub-level s, p, d, f. In this case n is equal to 3.

The value will directly depend on the sub-level, if: s=0, p=a, d=2, f=3. In this case l=1. To find the two remaining quantum numbers, the procedure is performed where the magnetic values ​​will directly depend on the sublevel, always following the diagonal diagram.

Electron configuration of sulfur in a more simplified way.

To make the configuration, the noble gas of the chemical element before the sulfur and the final layers of the atom must be taken into account.

In this case: in the configuration of sulfur, which is: 1s22s22p63s23p4, the noble gas that comes before sulfur in the periodic table, which in this case is neon, will become the element that will be taken into consideration, which is configured as follows:

Born: 1s22s22p6

In the Electron configuration of sulfur and neon, their first three orbitals are the same:

S: 1s22s22p63s23p4

Born: 1s22s22p6

In this case, what is done is to change the three orbitals in the Electron configuration of sulfur to the symbol of this noble gas, i.e. neon and put it in square brackets, thus leaving the remaining two orbitals that sulfur has.

Example:

S: [Ne] 3s2 3p4

Therefore, following the simplified sulfur configuration, it will be represented as follows:

S: [Ne] 3s2 3p4.

Properties of sulfur

• Its atomic number is 16 and is represented by the symbol S.
• It belongs to group 16 and period 3 of the periodic table.
• They have an oxidation state of -2, which is the sum of the negative and positive charges of an atom, which will indirectly reveal how many electrons the atom has donated or accepted, i.e. say they get an approximation of reduction and oxidation processes.
• Its mass is determined by the total mass of protons and electrons. Its atomic mass is 32.065 u.
• It has a boiling point of 717.87 degrees K and a melting point of 388.36 degrees Kelvin.
• It appears as a solid, crystalline element with a bright yellow hue.
• It is very bad as a conductor of electricity and heat.
• It is part of the non-metallic group of the periodic table.
• In its natural form, it exhibits a solid state.
• It has no shine.
• It is very fragile, so it cannot be flattened or stretched to create tablecloths and threads.