it all depends on the electron configuration if it is positive or negative, you have to look at the transition metals and valence electrons and determine the charge and use the formula n-1
1s^2 2s^2 2p^6 3s^2 3p^6 3d^10
Any element that would need to rid itself of three or more electrons to achieve a noble gas configuration (a transition metal), is extremely unlikely to do so.
Instead, an element will lose its incomplete sublevel (a lone 4s, 5s, etc. electron) that results with 18 electrons in the highest occupied energy level, and all of its orbitals filled. It now has a pseudo noble-gas electron configuration.
Although the formation of an octet is the most stable electron configuration, other electron configurations provide stability. These relatively stable electron arrangements are referred to a pseudo-noble gas configuration. Although the formation of an octet is the most stable electron configuration, other electron configurations provide stability. These relatively stable electron arrangements are referred to a pseudo-noble gas configuration.
Element that have a completely filled valence orbital but differ in all properties of the zeroth group.
For example: Zinc have 30electrons. Hence, 1s2,2s2,2p6,3s2,3p6,3d10,4s2... 4s2 have a completely filled with electron,so,zinc is pseudo inert gas configuration.
"Noble gas configuration" means that in writing out an electron configuration for an atom, rather than writing out the occupation of each and every orbital specifically, you instead lump all of the core electrons together and designate it with the symbol of the corresponding noble gas on the Periodic Table (in brackets).
For example, the noble gas configuration of nitrogen is [He]2s22p3
yes, Cu+ has a pseudo-noble-gas electron configuration
nitrogen will get noble gas configuration by adding three more electrons.
If alkali metals loses one electron, they achieve the electronic configuration of the nearest noble gases.
Due to their electron configuration, the atoms in a noble gas hardly attract each other.
Silicon has 4 valence electrons. No noble gases will have 4 valence electrons.
Although the formation of an octet is the most stable electron configuration, other electron configurations provide stability. These relatively stable electron arrangements are referred to a pseudo-noble gas configuration. Although the formation of an octet is the most stable electron configuration, other electron configurations provide stability. These relatively stable electron arrangements are referred to a pseudo-noble gas configuration.
no. it doesn't
[noble gas]ns2 np6
By acquiring noble gas configuration elements become stable .
Silver needs 7 more electrons to reach a "pseudo-noble gas" configuration.
yes, Cu+ has a pseudo-noble-gas electron configuration
The pseudo noble-gas electron configuration has the outer three orbitals filled, the s, p and d- s2p6d10 (18 electrons total) and so is fairly stable. Elements that attain this electron configuration are at the right side of the transition metals (d-block). Br-, I-, Se2-
[Ne]3s23p4
it only fills the S sublevel
Noble gases have a stable electron configuration. So they are less reactive.
All of the noble gasses have full outer electron shells - rendering them extremely nonreactive. Their electron configuration is what places them in the group on the periodic table that we have designated "noble gases".
The group of elements that have a stable electron configuration are the noble gases.