This noble gas is argon (Ar).
A sulfide ion, S2-, has 18 electrons. A neutral sulfur atom has 16 electrons, the same as the number of protons, which is the atomic number. Since electrons have a negative charge, a sulfur atom must gain two extra electrons in order to form the sulfide ion with a charge of 2-.
An atom of sulfur-36 can gain two electrons to become a sulfide ion with a -2 charge. When it gains these two electrons, it achieves a stable electron configuration, similar to the noble gas configuration of argon, resulting in a charge of -2.
A sulfur atom has 6 valence electrons, while a sulfide ion has 8 valence electrons because it gains two electrons to achieve a stable electron configuration.
An atom with atomic number n needs to gain enough electrons to have the same number of electrons as the nearest noble gas in the periodic table. This would typically involve gaining 8 electrons to achieve the stable electronic configuration of a noble gas.
There is a neutral charge on an atom when the number of protons is equal to the number of electrons. This is most common in the Noble gases, such as Neon (atomic number 10, the second Noble Gas), where there are 10 protons and 10 electrons, with the negative charge on the electrons balancing out the positive charge of the protons exactly.
A sulfur atom gains 2 electrons when it becomes a sulfide ion.
A sulfide ion, S2-, has 18 electrons. A neutral sulfur atom has 16 electrons, the same as the number of protons, which is the atomic number. Since electrons have a negative charge, a sulfur atom must gain two extra electrons in order to form the sulfide ion with a charge of 2-.
The sulfur atom only has 6 electrons in its outer shell, and following the octet rule, it wants to get to the closest noble gas. The elements want to have a full outer level, so it will gain 2 electrons to get to 8. So the Sulfur atom now becomes a Sulfide ion.
An atom of sulfur-36 can gain two electrons to become a sulfide ion with a -2 charge. When it gains these two electrons, it achieves a stable electron configuration, similar to the noble gas configuration of argon, resulting in a charge of -2.
The noble gas neon has ten protons and an equal number of electrons.
It means that the atom or ion has the same number of electrons as a noble gas, thus adopting the stable electron configuration of the noble gas. This typically involves attaining a full valence shell of electrons. This concept is used in chemistry to describe similarities in chemical behavior between the atom or ion and the noble gas.
A sulfur atom has 6 valence electrons, while a sulfide ion has 8 valence electrons because it gains two electrons to achieve a stable electron configuration.
subtract the group number from the atomic number
Helium has only two electrons. It is the first noble gas in the periodic table and has a full outer electron shell.
The sulfide ion (S²⁻) has 16 protons and 18 electrons. This is because the element sulfur (S) normally has 16 protons and 16 electrons, but by gaining two extra electrons to achieve a stable electron configuration, it becomes the sulfide ion with 18 electrons.
The Alkaline Earth metal which comes just after the noble gas
An atom with atomic number n needs to gain enough electrons to have the same number of electrons as the nearest noble gas in the periodic table. This would typically involve gaining 8 electrons to achieve the stable electronic configuration of a noble gas.