8 valence electrons
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Oxygen needs 2 more valence electrons to have a full outer shell. Oxygen has 6 valence electrons, and a full outer shell for oxygen is achieved at 8 valence electrons.
The symbol for an element that does not need eight electrons to have a full set of valence electrons is typically found in Group 1 or Group 2 of the periodic table. Examples include lithium (Li) from Group 1 and beryllium (Be) from Group 2. These elements follow the duet rule or satisfy the octet rule in a different way.
Phosphorus has 5 valence electrons and it needs 3 more electrons to complete its octet and achieve stability.
8 valence electrons
Four valence electrons need to be accommodated in the Lewis structure for F2. Each fluorine atom contributes seven valence electrons, totaling to fourteen valence electrons in the molecule.
In a reaction u need two valence electrons to gain or share two valence electrons.
6 valence electrons need to be accommodated in the Lewis structure for OF2. This accounts for the oxygen atom's 6 valence electrons and the fluorine atom's 1 valence electron each.
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Nitrogen has five valence electrons as a neutral atom, but it is shooting for eight. So it needs to gain three more electrons.
Beryllium is element 4, so the "neutral" atom would have 4 protons and 4 electrons. In order to have a "-2" charge, it would need 6 electrons.
Oxygen needs 2 more valence electrons to have a full outer shell. Oxygen has 6 valence electrons, and a full outer shell for oxygen is achieved at 8 valence electrons.
11 electrons makes the third energy level complete. One
My best guess is that Be is "tricked" into thinking that it's valence shell is now full since it's two valence electrons are now being "shared/hogged" by the much more electronegative Fluorine. I would guess that this is a highly polar covalent bond!?! 8-) Where is the senior chemistry teacher (RAM) around when I need her? Cheers, "Lurch" from the club club.
The symbol for an element that does not need eight electrons to have a full set of valence electrons is typically found in Group 1 or Group 2 of the periodic table. Examples include lithium (Li) from Group 1 and beryllium (Be) from Group 2. These elements follow the duet rule or satisfy the octet rule in a different way.
Phosphorus has 5 valence electrons and it needs 3 more electrons to complete its octet and achieve stability.