DConte said:I have never come across this term before in my few years of chemistry. At first, i thought it meant molecular shape, such as "trigonal planar" or linear. But apparently, that is not the case. Apparently, it is in some form of AX2E (2 being a subscript), but that's all i can find on the matter. Does anyone have experience on this?
The AX2E molecular shape is a type of molecular geometry where there are two bonded atoms (A) and one lone pair of electrons (E) attached to a central atom (X). This results in a bent or V-shaped structure.
To determine the molecular shape of an AX2E molecule, you first need to draw the Lewis structure. Then, you can use the VSEPR theory and the number of bonding and lone pairs of electrons to predict the molecular shape. In this case, the presence of two bonded atoms and one lone pair of electrons results in a bent shape.
The bond angle in an AX2E molecule is approximately 120 degrees. This is because the lone pair of electrons repels the bonded atoms, causing them to spread out and form a V-shape with a bond angle of 120 degrees.
Some examples of molecules with an AX2E shape include sulfur dioxide (SO2), water (H2O), and hydrogen sulfide (H2S). In these molecules, the central atom (S or O) is bonded to two other atoms (S or H) and has one lone pair of electrons.
Molecules with an AX2E shape have polar covalent bonds, meaning there is an unequal distribution of electrons due to the difference in electronegativity between the central atom and the bonded atoms. This results in a dipole moment, making these molecules polar. They also have a bent shape, making them asymmetrical and allowing for intermolecular forces like dipole-dipole interactions.