if it is a noble gas it already has an octet, otherwise, it would need to gain or use electrons to complete an octet and would no longer be neutral or unbounded.
Noble gasses have the complete octet of valence electrons. The are in the family 18 of the periodic table. They are unlikely to react with other elements.
2
six valence electrons.....It only requires two more to complete octet....
yes PCl3 obey octet rule there are 5 electrons in the valence shell of phosphorous it need 3 electron to complete its octet so it form bond with 3 chlorine after bond formation there are 8 electron in its octet it obey octet rule
Li3N because Lithium will give 3 electrons to complete Nitrogen's octet as N has 5 electrons in it's valence shell and needs 3 more to complete it's octet.
Noble gasses have the complete octet of valence electrons. The are in the family 18 of the periodic table. They are unlikely to react with other elements.
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six valence electrons.....It only requires two more to complete octet....
A complete octet of electrons (8) in the outer-most, or valence, shell.
No, it doesn't have a complete octet. Phosphorous is in group 5A, meaning it has 5 valence electrons (5 electrons on its outest shell).
yes PCl3 obey octet rule there are 5 electrons in the valence shell of phosphorous it need 3 electron to complete its octet so it form bond with 3 chlorine after bond formation there are 8 electron in its octet it obey octet rule
8 valence electrons
Li3N because Lithium will give 3 electrons to complete Nitrogen's octet as N has 5 electrons in it's valence shell and needs 3 more to complete it's octet.
The optimum number of electrons in the outermost valence shell for phosphorus atoms is eight, known as an octet. Unbonded phosphorus atoms have 5 valence electrons and undergo chemical bonding in order to gain the other 3, either by covalent bonding or by ionic bonding.
covalent - which means "sharing of valence electrons"
Neon has completely filled valence orbitals, obeys octet rule and is hence stable. Chlorine needs one more electron to complete octet and is hence reactive.
Oxygen tends to gain two electrons to complete its "octet", making it O2- with the electron configuration 1s22s22p6