Question:
Which of the following species is not stable ?
Which of the following species is not stable ?
Updated On: Apr 17, 2024
- $[Sn(OH)_6]^{2-}$
- $[SiCl_6]^{2-}$
- $[SiF_6]^{2-}$
- $[GeCl_6]^{2-}$
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The Correct Option is B
Solution and Explanation
$\bullet$ Due to presence of d-orbital in Si, Ge and Sn they form species like ${SiF_6^{2-} , [GeCl_6]^{2-} , [Sn(OH)_6]^{2-}}$
$\bullet$ ${SiCl_6^{2-}}$ does not exist because six large chloride ions cannot be accommodated around ${Si^{4+}}$ due to limitation of its size.
$\bullet$ ${SiCl_6^{2-}}$ does not exist because six large chloride ions cannot be accommodated around ${Si^{4+}}$ due to limitation of its size.
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Concepts Used:
P-Block Elements
- P block elements are those in which the last electron enters any of the three p-orbitals of their respective shells. Since a p-subshell has three degenerate p-orbitals each of which can accommodate two electrons, therefore in all there are six groups of p-block elements.
- P block elements are shiny and usually a good conductor of electricity and heat as they have a tendency to lose an electron. You will find some amazing properties of elements in a P-block element like gallium. It’s a metal that can melt in the palm of your hand. Silicon is also one of the most important metalloids of the p-block group as it is an important component of glass.
P block elements consist of:
- Group 13 Elements: Boron family
- Group 14 Elements: Carbon family
- Group 15 Elements: Nitrogen family
- Group 16 Elements: Oxygen family
- Group 17 Elements: Fluorine family
- Group 18 Elements: Neon family