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.
The outer shell of Hellium is full, 1s2.
The outer shell of neon is full, 2s2, 2p6
The outer shells of the rest of the noble gases are not full but all have ns2, np6 outer shells, the octet.
noble gases are stable because they have 8 electrons so they do not need or give away any valance electrons
It won't react with any of the other elements.
Noble gas configurations are stable because their outermost energy level is completely filled up. This means that they don't normally react with other elements.
because there are no electrons
Beryllium would have that configuration
4
A cesium atom has 1 valence electron. It is an alkali metal, and all alkali metals have 1 valence electron. The electron configuration for cesium is (Rn)7s1. The single electron in the 7s sublevel is its valence electron.
With an e- configuration of [Ne] 3s23p5, the atom will be found in Group VII A, meaning that there are 7 valence electrons.
7s1 because the definition of valence electrons are the outermost s and p electrons therefore in this case there is only an outermost s electron and therefore the answer is 7s1. NOTE:IT DOES NOT INCLUDE THE D AND THE F ELECTRONS!!!!Other valence configuration examples include;Nitrogen : 2s2 2p3Chlorine : 3s2 2p5Zinc: 4s2Bromine: 4s2 4p5
The valence electrons are the outermost (highest energy) s and p sublevels. There are 5 valence electrons in a phosphorus atom, and it is in period 3, so its valence electron configuration is 3s23p3.
Krypton has 8 valence electrons.The electron configuration is: [Ar]3d10.4s2.4p6.
The answer is nitrogen. Nitrogen is one example of an element that has the same valence electron configuration as phosphorus.Ê
Magnesium (Mg) has atomic number 12, so the electron configuration is1s2 2s2 2p6 3s2. The VALENCE electron configuration would simply be 3s2.
The electron configuration of phosphorus is [Ne]3s2.3p3.
The answer is nitrogen. Nitrogen is one example of an element that has the same valence electron configuration as phosphorus.Ê
Beryllium would have that configuration
[Ne]3s23p4
Nitrogen
sulfer
4s2 4p4
Fr is in the 1st period. It removes an electron to get noble gas configuration. Fr+ does not have valence electrons.Francium has 1 electron in its outermost energy level. It donates its outermost electron to stabilize its electron configuration. Francium(I) has no valence electrons.