Why does the most proper Lewis structure of BeCl 2 contain two single Be-Cl bonds instead of two double Be=Cl bonds?
a. The formal charges of the atoms would be maximized, rather than minimized as required by the formal charge rule, if BeCl 2 contained two double bonds
b. Neither Be nor Cl could satisfy the octet rule if BeCl 2 contained two double bonds
c. Be would be surrounded by more than eight electrons if BeCl 2 had two double bonds
d. The Cl atoms would be surrounded by more than eight electrons each if BeCl 2 contained two double bonds
e. The formal charges could not sum to zero if BeCl 2 contained two double bonds
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