Why does the best Lewis structure of BeBr₂ contain two single Be–Br bonds instead of two double Be=Br bonds?

• A. If BeBr₂ had two double bonds, Be would be surrounded with more than eight electrons.
• B. If BeBr₂ contained two double bonds, the sum of formal charges would not be equal to zero.
• C. If BeBr₂ contained two double bonds, the formal charges of Be and Br atoms would be maximized instead of minimized as required by the formal charge rules.
• D. If BeBr₂ contained two double bonds, both Be and Br will violate the octet rule.
• E. If BeBr₂ contained two double bonds, each of the Cl atoms would be surrounded by more than eight electrons.

Answer: (C)