# The basic structural unit of silicates is:A. $Si{{O}^{-}}$ B. $Si{{O}_{4}}^{4-}$C. $Si{{O}_{3}}^{2-}$D. $Si{{O}_{4}}^{2-}$

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Hint: Think about the ores in which silicate compounds are formed and recall the general formula for silicates. They are usually structures made up of silicon and oxygen and arranged in tetrahedral units which are joined together. Silicon is at the center and oxygen atoms are present at the corners of the tetrahedron.

Complete step by step solution:
The general formula for silicates is defined to be ${{[Si{{O}_{(4-x)}}^{(4-2x)-}]}_{n}}$ for $0\le x<2$. From this formula, we can safely rule out options ‘A. $Si{{O}^{-}}$’ and ‘D. $Si{{O}_{4}}^{2-}$’ as the correct answers.
Silicates include orthosilicates, metasilicates, and pyrosilicates with the structural formulae of $Si{{O}_{4}}^{4-}$, $Si{{O}_{3}}^{2-}$, and $S{{i}_{2}}{{O}_{7}}^{6-}$ respectively Usually when referring to silicates, the most standard form of a silicate is referred to, the orthosilicate which is tetrahedrally arranged.
The silicon atom in orthosilicate is $s{{p}^{3}}$hybridized and the 4 oxygen atoms are present at 4 corners of the tetrahedron. Orthosilicate compounds are found in various ores of minerals like granite, feldspar, and others.
The structure of the orthosilicate anion is:

Hence, the answer to this question is ‘B. $Si{{O}_{4}}^{4-}$’

The bond length in the orthosilicate anion is 162pm and the bond angle is $109.5{}^\circ$. This is exactly the bond angle that is predicted for tetrahedral structures that do not have any lone pairs or dipole moments.
Note: Although options ‘B. $Si{{O}_{4}}^{4-}$’ and ‘C. $Si{{O}_{3}}^{2-}$’ are both considered to be silicates, the correct answer is ‘B. $Si{{O}_{4}}^{4-}$’ since $Si{{O}_{3}}^{2-}$ is always explicitly described to be a metasilicate and not just a silicate.