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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Problem Details

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 contained two double bonds

e. The formal charges could not sum to zero if BeCl 2 contained two double bonds

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Based on our data, we think this problem is relevant for Professor Culbertson's class at K- STATE.