Besides the central atom, what are the differences between \(\mathrm{CO}_{2}\) and \(\mathrm{SiO}_{2} ?\)

Carbon (C) and Silicon (Si) are both elements found in group 14 of the periodic table. However, they have different properties due to their electron configurations and position in the carbon group. Carbon has the electron configuration 1s2 2s2 2p2, while Silicon has 1s2 2s2 2p6 3s2 3p2. Thus, Carbon and Silicon form different types of bonds with Oxygen.

In carbon dioxide (\(\mathrm{CO}_2\)), the carbon forms two double bonds with the oxygen atoms, resulting in a linear molecular shape with a bond angle of 180°. The molecule has a molecular formula that shows these double bonds as O=C=O. On the contrary, in silicon dioxide (\(\mathrm{SiO}_2\)), the silicon atom forms single bonds with two oxygen atoms. Each oxygen atom also forms a single bond with another silicon atom, leading to an extended tetrahedral network of Si-O bonds.

In \(\mathrm{CO}_2\), the central carbon atom has no lone pair electrons and forms two double bonds with oxygen atoms, resulting in a linear molecular shape with a bond angle of 180°. Carbon dioxide is a discrete molecule. In \(\mathrm{SiO}_2\), the silicon atom tends to form tetrahedrally coordinated structures by forming single bonds with four oxygen atoms. In this case, the silicon atom sp3 hybridizes, leading to a tetrahedral geometry around the silicon atom. Silicon dioxide forms a continuous three-dimensional network of Si-O bonds, and is not a discrete molecule.

Carbon dioxide (\(\mathrm{CO}_2\)) is a gas at room temperature, and it is composed of discrete molecules. It has low melting and boiling points (-78.5 °C and -57.8 °C), and it cannot conduct electricity. Silicon dioxide (\(\mathrm{SiO}_2\)), on the other hand, exists as a solid at room temperature. It forms a covalent network of tetrahedrally coordinated Si-O bonds, which results in a high melting and boiling point (above 1600 °C) and low electrical conductivity. In summary, the differences between carbon dioxide and silicon dioxide, besides the central atom, are: 1. Bond types: \(\mathrm{CO}_2\) has double bonds while \(\mathrm{SiO}_2\) has single bonds. 2. Molecular shape: \(\mathrm{CO}_2\) is linear, while \(\mathrm{SiO}_2\) has a three-dimensional network. 3. Physical properties: \(\mathrm{CO}_2\) is a gas with low melting and boiling points, while \(\mathrm{SiO}_2\) is a solid with high melting and boiling points.