- #1
Dual Op Amp
- 151
- 0
I have looked every where, my encyclopia set, the search engine even a different post on this forum, but I just can't find out why an atom is more stable, when the valence shell is filled with eight electrons.
The octet rule states that atoms tend to gain, lose, or share electrons in order to achieve a full outer shell with 8 electrons. This is because a full valence shell is energetically favorable and leads to a more stable configuration for the atom.
The number of valence electrons determines how likely an atom is to form bonds with other atoms. If the valence shell is not full, the atom will be more reactive and likely to form bonds in order to achieve a full outer shell and become more stable.
Yes, there are some exceptions to the octet rule. For example, atoms in the first row of the periodic table (such as hydrogen and helium) only require 2 electrons in their valence shell to achieve stability. Additionally, elements in the third row and below can have expanded valence shells and hold more than 8 electrons.
The octet rule is based on the number of orbitals and energy levels in the second row of the periodic table. Elements in this row have a total of 8 orbitals, allowing for the maximum number of electrons in the valence shell to be 8. Elements in higher rows have more orbitals available, so they can hold more than 8 electrons in their valence shell.
An atom that is stable (with a full valence shell) will be less reactive because it does not need to gain, lose, or share electrons in order to achieve stability. On the other hand, atoms with incomplete valence shells will be more reactive as they try to gain, lose, or share electrons to achieve a stable configuration.