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**Problem**: 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 bondsb. Neither Be nor Cl could satisfy the octet rule if BeCl 2 contained two double bondsc. Be would be surrounded by more than eight electrons if BeCl 2 had two double bondsd. 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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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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