2
Question
Explain the following:
A) CO2 is a gas whereas SiO2 is a solid.
B)Silicon forms [SiF6]2− ion whereas the corresponding fluoro compound of carbon is not known.
A) CO2 is a gas whereas SiO2 is a solid.
B)Silicon forms [SiF6]2− ion whereas the corresponding fluoro compound of carbon is not known.
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Solution
a)
• CO2 is a linear and nonpolar molecule.
• It has a very weak intermolecular forces of attraction (i.e. Van Der Waals forces) and therefore exists in gaseous form.
• SiO2 is a covalent three-dimensional network solid is whether each Silicon atom is covalently bonded in a tetrahedral manner to 4 oxygen atoms.
• Each O Atom in turn is covalently bonded to another Si as shown in the diagram:
• Like C, Si cannot form pπ−pπ bonding with other atoms and therefore forms 4 covalent bonds with O atoms
• Thus, the entire structure may be considered as a giant molecule forming a solid structure.
b)
•Valence shell of C atom does not have any vacant d-orbitals and therefore cannot expand its octet by increasing its covalency beyond4 covalent bonds.
• Si has an empty 3d orbital and can accept lone pairs of electrons to expand its covalency beyond 4 bonds.
• Thus, Si can accept electrons from F− ion to form 6 bond and exist as[SiF6]2−. Valence shell of C atom does not have any vacant d-orbitals and therefore cannot expand its octet by increasing its covalency beyond 4 covalent bonds.
Si has an empty 3d orbital and can accept lone pairs of electrons to expand its covalency beyond 4 bonds.
•Valence shell of C atom does not have any vacant d-orbitals and therefore cannot expand its octet by increasing its covalency beyond 4 covalent bonds.
• Si has an empty 3d orbital and can accept lone pairs of electrons to expand its covalency beyond 4 bonds.
• Thus, Si can accept electrons from F− ion to form 6 bond and exist as [SiF6]2−. Thus, Si can accept electrons from F− ion to form 6 bond and exist as [SiF6]2−.
• Also, the smaller size of C cannot accommodate the six F atoms around it.
• Due to all these factors, C is unable to form [CF6]2− anion.
• CO2 is a linear and nonpolar molecule.
• It has a very weak intermolecular forces of attraction (i.e. Van Der Waals forces) and therefore exists in gaseous form.
• SiO2 is a covalent three-dimensional network solid is whether each Silicon atom is covalently bonded in a tetrahedral manner to 4 oxygen atoms.
• Each O Atom in turn is covalently bonded to another Si as shown in the diagram:
• Like C, Si cannot form pπ−pπ bonding with other atoms and therefore forms 4 covalent bonds with O atoms
• Thus, the entire structure may be considered as a giant molecule forming a solid structure.
b)
•Valence shell of C atom does not have any vacant d-orbitals and therefore cannot expand its octet by increasing its covalency beyond4 covalent bonds.
• Si has an empty 3d orbital and can accept lone pairs of electrons to expand its covalency beyond 4 bonds.
• Thus, Si can accept electrons from F− ion to form 6 bond and exist as[SiF6]2−. Valence shell of C atom does not have any vacant d-orbitals and therefore cannot expand its octet by increasing its covalency beyond 4 covalent bonds.Si has an empty 3d orbital and can accept lone pairs of electrons to expand its covalency beyond 4 bonds.
•Valence shell of C atom does not have any vacant d-orbitals and therefore cannot expand its octet by increasing its covalency beyond 4 covalent bonds. • Si has an empty 3d orbital and can accept lone pairs of electrons to expand its covalency beyond 4 bonds. • Thus, Si can accept electrons from F− ion to form 6 bond and exist as [SiF6]2−. Thus, Si can accept electrons from F− ion to form 6 bond and exist as [SiF6]2−.
• Also, the smaller size of C cannot accommodate the six F atoms around it.
• Due to all these factors, C is unable to form [CF6]2− anion.
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