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Multiple Bond Formation

Silicon exist...

Question

Silicon exists only in the diamond structure due to tendency to form $p π - p π$ bonds to itself.

A

True

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B

False

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Solution

The correct option is B False
Silicon can not form $p π - p π$ bond with itself. It exists in diamond cubic structure and forms sigma bonds with itself in $s p^{3}$ hybridization

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Q. Assertion :STATEMENT 1: Silicon exists only in diamond-like structure while carbon exists both in diamond and graphite forms. Reason: STATEMENT 2: Carbon can show pronounced

p π - p π

bonding while silicon shows negligible extent of

p π - p π

Q. Consider the following statements:
I: In diamond, each carbon atom is linked tetrahedrally to four other carbon atoms by

s p^{3}

bonds.
II: Graphite has planar hexagonal layers of carbon atoms held together by weak van der Waal's forces.
III: Silicon exists only in diamond structure due to its tendency to form

p π - p π

bonds to itself.

Q. Assertion: Both rhombic and monoclinic sulphur exist as

S_{8}

but oxygen exists as

O_{2} .

Reason: Oxygen form

p π - p π

multiple bond due to small size and small bond length but

p π - p π

bonding is not possible in sulphur due to its larger atomic size than oxygen.

Q. Assertion :Silicon is not expected to form an allotrope with graphite like structures. Reason: There is feasibility to

p - p π

bond in silicon.

Q. Nitrogen has unique ability to form

P π - P π

multiple bonds with itself and with other elements due to:

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