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H, Li, and Be all form duplets in Lewis structures to achieve the noble gas configuration of He. B also has an incomplete octet of 6 electrons (like in the compound BF3) because F is unlikely to share more electrons with boron due to its high electronegativity.
Kaylee Sepulveda 3C wrote:Usually, the elements that do this are B, Al, Li, and H. B and Al will usually form compounds where they only have six electrons instead of a complete octet.
Why does B and Al exhibit this behaviour (where they don't form a complete octet)?
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