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Resonance Effect

why silicon-s...

Question

why silicon-silicon bond is weak while carbon-carbon bond is strong?

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Solution

The size of silicon is big as compared to carbon. The bond is long in silicon and can easily break but in case of carbon , the bond is short and strong . Hence , the bonding is carbon is more strong than silicon. Therefore , the carbon shows strong catenation and forms a large number of compounds.

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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. Why carbon can form stable

C = C

bond where as silicon can't form

S i = S i

Q. Assertion :Catenation is the ability of an atom to form bonds with other atoms of the same element. It is exhibited by both carbon and silicon. Reason: Carbon exhibits catenation much more than silicon or any other element due to its smaller size which makes the

C - C

bonds strong while the

S i - S i

bonds are comparatively weaker due to its large size and therefore,

S i

does not have enough bond strength to hold together large molecules.

Q. Assertion :Carbon dioxide is a gas but silicon dioxide is an in-fusible solid. Reason: Carbon dioxide has a linear

π -

bonded structure.

Q. Consider the following statements
I : In diamond, each carbon atom is linked tetrahedrally for 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.

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