Question

select the electron groupings that results in a bent molecule? -e- -e= -e- -e= -e= -e- -e- -e- -e

Explanation:

Step1: Recall VSEPR theory

VSEPR (Valence - Shell Electron - Pair Repulsion) theory is used to predict molecular geometries. A bent molecular geometry occurs when there are two bonding pairs and one or more lone pairs around the central atom.

Step2: Analyze each option

• For the option \(-\ddot{E}-\), if \(E\) has two lone pairs (\(\ddot{E}\)) and two single bonds (the two \(-\) represent bonding pairs), according to VSEPR, the electron - group geometry is tetrahedral (if there were four bonding pairs) or trigonal planar (if there were three electron groups). But with two bonding pairs and two lone pairs, the molecular geometry is bent.
• For \(-\ddot{E}=\), if \(E\) has one lone pair (\(\ddot{E}\)), one double bond (\(=\)) and one single bond (\(-\)), the electron - group geometry is trigonal planar. The molecular geometry is bent (because of the lone pair repelling the bonding pairs).
• For \(-\ddot{E}-\) (assuming it's similar to the first case of two bonding and two non - bonding pairs), it also gives a bent geometry.

Answer:

\(-\ddot{E}-\), \(-\ddot{E}=\)