The outer shell is involved in the bonding and it cannot really be described as an atomic outer shell any more.
In the very simplest terms, Lewis model, electrons are shared with other atoms. In CH4 for example the carbon hydrogen bonds have 2 electrons each which could be considered to be 1 from the carbon and one from each hydrogen. Carbon then has 8 and hydrogen 2.
There are two approaches that have a quantum mechanical slant. Valence bond theory is closest to chemists views on chemical bonds involving localised electron pairs, In VB theory hybrid atomic orbitals are postulated that optimise overlap of orbitals on the one atom with another. In methane the carbon is sp3 hybridised giving 4 tetrahedral lobes, which overlap nicely with the 1s orbitals on the hydrogens.
It always change when forming bonds. It takes nobel gas configuration normally
This electron configuration is changed for ions.
It accepts one electron.
Alkali metals and alkaline earth metals will form ions (by losing 1 and 2 electrons respectively) with noble gas electron configuration.
Every halogen has the capacity to accept one electron from a sodium atom and to thereby achieve a noble gas electron configuration of eight valance electrons. The halogens are fluorine, chlorine, bromine, iodine, and astatine.
For Mg to acquire the same electron configuration as Neon, it must lose 2 of its valence electrons. It thus obtains a 2+ charge. The 2 electrons that it loses can go to an accepting atom, such as O, S, Cl, etc. to form an ionic bond, where the accepting atom has a negative charge.
Lithium(Li) gains 1 electron to become stable.
It accepts one electron.
It accepts one electron.
It accepts one electron.
study island answer- It gives up two electrons
Argon
The ions of elements nitrogen (N3-), oxygen (O2-), and fluorine (F-) will have the same electron configuration as a sodium ion (Na+), which is the same as the electron configuration of the noble gas neon.
A fluorine atom gains one atom in order to achieve the same electron configuration as neon. In doing so, the fluorine atom forms a fluoride ion with a 1- charge with the formula F-. As a negatively charged ion, it can form ionic bonds with various positively charged ions.
Adding one electron gives the chloride ion which has an octet (it achieves the same electron configuration as argon.
Alkali metals and alkaline earth metals will form ions (by losing 1 and 2 electrons respectively) with noble gas electron configuration.
Rhodium (Rh) forms a 3 plus ion that has the electron configuration Kr4d6. Rhodium has oxidation states of 2,3 and 4, so it can loan out 2, 3 or 4 electrons depending on the circumstances of a chemical reaction.
Chlorine (Cl)
The atomic number of Sodium is 11 (2,8,1), so there is one electron in the outer-most shell. As soon as sodium looses this outer-most one electron, it acquires the stable most structure with a 2,8. That';s why sodium ion is stabler than sodium metal. The electronic configuration of a sodium ion is 2,8. Same thing happens with Chlorine. The electronic configuration of chlorine is 2,8,7. Chlorine needs just one electron to stabilize itself with a configuration of 2,8,8. When the chlorine atom gains one electron, it forms the chlorine ion which has the configuration 2,8,8 which is stable.