\(\mathrm{SiO}_{2}\)

In \(\mathrm{SiO}_{2}\), there are two types of atoms: Silicon (Si) and Oxygen (O). Silicon has 4 valence electrons and Oxygen has 6 valence electrons.

To determine the type of bond between Silicon and Oxygen atoms, we need to analyze the electronegativity difference between them. The electronegativity difference between Si (1.90) and O (3.44) is 1.54, which suggests that the bond between them is polar covalent.

To understand the molecular structure, we will use a Lewis structure approach. First, count the total number of valence electrons: Silicon: 4 valence electrons Oxygen: 2 atoms × 6 valence electrons = 12 valence electrons Total valence electrons: 4 + 12 = 16 Next, arrange the atoms according to their connectivity and distribute the valence electrons: - Place Si in the center and surround it with two O atoms. - Each bond between Si and O needs 2 electrons. Therefore, form two Si-O bonds. This will use 4 electrons. - Distribute the remaining 12 electrons among the two O atoms to satisfy the octet rule, which means 6 electrons on each O atom. Thus, the Lewis structure of \(\mathrm{SiO}_{2}\) is as follows: ``` O || Si - O ```

The molecular weight is calculated using the atomic weight of the individual atoms. Silicon: 28.085 g/mol Oxygen: 16 g/mol Molecular weight of \(\mathrm{SiO}_{2}\): (1 × 28.085) + (2 × 16) = 28.085 + 32 = 60.085 g/mol

\(\mathrm{SiO}_{2}\), also known as Silica, is a covalent network solid with a high melting point due to its strong Si-O bonds and three-dimensional structure. It is an important component in the production of glass, ceramics, and other industrial materials. It is also commonly found in the Earth's crust in the form of quartz and sand.