Question

Use the Molecule Shape simulator (http://openstaxcollege.org/l/16MolecShape) to build a molecule. Starting with the central atom, click on the double bond to add one double bond. Then add one single bond and one lone pair. Rotate the molecule to observe the complete geometry. Name the electron group geometry and molecular structure and predict the bond angle. Then click the check boxes at the bottom and right of the simulator to check your answers.

Short answer

The electron group geometry – bent.

The bond angle is ${120}^{\circ }$.

Step-by-step solution

definition of molecule

A molecule is a particle made up of two or more atoms that are chemically bonded together; the number of atomic nuclei making up a molecule is a determinate number.

Explanation

We have a center atom with two atoms (one with a double bond and the other with a single bond) and a lone pair surrounding it.

The electron group geometry and molecular structure must be named, and the bond angle must be predicted.

Therefore, The bent geometry of the electron group.

The angle of the connection is.

Molecular structure and predict the bond angle

The electron group geometry is trigonal planar, and there are three zones of high electron density (double bond, single bond, and lone pair).

The structure is twisted because lone pairs take significantly more space than multiple bonds (and single bonds), and we only have one lone pair. (Angular), with a bond angle of$<{120}^{\circ }$.

The bond angle in a simulation is${120}^{\circ }$. (Probably because they neglect the difference of space occupied by different regions of electrons)

Therefore,The bent electron group geometry.

The angle of the connection is$-<{120}^{\wedge }0$.