How many electrons will a single atom of sulfur with no charge and no bonds have in its valence shell?

6

Explanation:

Sulfur is an element that can be found on Group 6 and Period 3 on the periodic table with the Atomic Mass 32 and Atomic Number 16.

In an electronic configuration, the maximum number of electrons in a given shell can be obtained using the formula 2n², where n represent the number of valence shell.

Therefore in the first shell when n=1;

the maximum number of electrons it can contain is 2 * 1² = 2

For the second shell, when n = 2

the maximum number of electrons it can contain is 2 * 2² = 2 * 4 = 8

For the third shell, when n = 3

the maximum number of electrons it can contain is 2 * 3² = 2 * 9 = 18

...

Now, in a single atom of sulphur with no charge and no bonds, the Atomic Number is said to be 16

We can therefore determine the number of the electrons in the outermost valence shell to be 6 because, the first shell takes 2 electrons, the second shell takes 8 electrons and the third shell takes 6. All together making 16 electrons.

There are 6 electrons in the outermost shell.

Explanation:

Sulphur is a non-mettalic element which is in the period 3 and group. 6on the periodic table. It has an atomic number of 16 and a Mass number of 32. Atomic number tells you the number of electrons in an electrically neutral atom. It has the electronic configuration of 1s2 2s2 2p6 3s2 3p4.

The orbitals have a formula 2n^2 where n = 0, 1, 2, 3 etc.

In the shells, n = 1 so there are 2 electrons. For n = 2, 2 * (2) ^2 = 8 electrons. So, 16 - (8 + 2) = 6 electrons in the 3 shell (outermost shell)

Therefore from the electronic confriguration above, there are 6 electrons in the outermost shell.