Aluminum oxide is an ionic compound, which has a strong ionic bond between the atoms of the aluminum metal and the oxygen atoms. Aluminium atoms have a steric number of three, and the oxygen atom has a valence electron of six. The lewis structure of aluminium oxide molecule has the following features.
Aluminum oxide has a trigonal planar shape, with three central atoms, and the valence electrons of the atoms are distributed over the outermost shells. It has a 120-degree bond angle. Al2O3 is used in refractories, ceramics, and aluminosilicate glasses.
This compound has been studied theoretically and experimentally. It is important to understand the properties of the different types of aluminium oxide molecules.
Aluminium atoms have an electronegativity of three, and they have three valence electrons in their outermost shells. They then transfer their outer electrons to the oxygen atoms, which have two electrons each. After this, the oxygen atoms acquire a -2 charge.
The Lewis structure of the Al2O3 molecule is a sp2 hybridized molecule. It has the following features: a trigonal planar shape, a total of 24 valence electrons, and a trigonal ionic bond between the atoms. It also has a polar nature.
The Lewis structure is drawn using the octet rule. To draw the sp2 hybridized molecule of aluminium oxide, there are some rules to follow.
First, a symmetric structure is more stable than an asymmetric one. Secondly, the presence of eight electrons in the outermost orbital is an indication that an atom is stable.