Atoms with full outer electron shells are more stable. The atoms (elements) with full outer electron shells are the noble (sometimes called inert) gases. These are the elements in Group 18 of the Periodic Table, and you know them as helium, neon, argon, krypton, exnon and radon.
FALSE
the sodium atom has 3 shells where 2 electrons are in the first shell, 8 in the second and 1 in the third shell; which isn't stable..... and its symbol is Na :)
The result is what you use to put in the food. Table salt (or sodium chlorine). It's a very stable compound, as each of the ions have their orbitals completely filled. Recall that in their normal states, Sodium has only one valence electron, and the Clorine is missing one to have its orbitals filled.
It would be phosphorus (I) iodide. However, this is not a stable compound; under normal conditions phosphorus and iodine combine to produce phosphorus (III) iodide (which is also not stable ... it's explosive ... but is considerably more stable than phosphorus (I) iodide is). The electron configuration of the phosphorus in PI3 is [Ne]s2, while that of PI is [Ne]s2p2. The filled s subshell is at least metastable, while a filled s subshell plus a partially filled p subshell is normally not and requires considerable effort to maintain.
The evidence comes from the Noble Gases of the Periodic Table of the Elements. Electron octet rule for stability is based on the noble gases, which are also called the inert gases because they are so stable they rarely react with anything. Chemists have come up with the theory of electron orbitals to explain stability. These are referred to as S orbital, P orbital, D orbital, etc. When the outer most orbital contains an octet the electron orbital resembles the Noble Gases and hence why it is considered stable valence configuration.
Na+ is the formula of the ion formed when sodium achieves a stable electron configuration.
no. they are more stable when they have completely filled or half filled shells
completely filled valence shells
yes that is true, it does make up an atom stable.
filled energy sublevels
A completley filled out electron level makes the atom stable
Helium has 2 valence electrons and has completely filled orbitals / shells and helium is stable.
Metals have a few electrons fairly loosely bound in their outer "shells", while halogens have nearly-complete outer electron "shells". The most stable configuration for an atom is to have completely-filled shells, so it's easy for metals to lose an electron or two and get down to the next "completely filled" shell, while halogens pick up extra electrons to get to the next filled shell.
The outer electron shells of the halogens contain seven electrons, and need one more electron to have eight and become stable.
No reactive elements always have partially filled shells- never full outer shells. Because they are partially filled they are less stable and want to react. If they had full shells they would be very stable.
A half filled sub-shell is more stable than other partially filled shells. As an example use Chromium. It should by logic have the following: Sc = [Ar]4s23d1 Ti = [Ar]4s23d2 V = [Ar]4s23d3 Cr should in theory be Cr = [Ar]4s23d4 but it is not. Half filled shells are more stable so the configuration is Cr = [Ar]4s13d5 two half filled sub levels and then Manganese is Mn = [Ar]4s23d5 one full and one half filled level.
The octet rule is a simple rule of thumb that states that atoms tend to combine in such a way that they each have eight electrons in their valence shells, giving them the same electron configuration as a noble gas. The rule is applicable to the main-group elements. In simple terms, molecules or ions tend to be most stable when the outermost electron shells of their constituent atoms contain eight electrons.ELECTRONS
3, three, tres