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Characteristics of p- Block Elements

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Question

give reason
a] elemental silicon does not form graphite like structure

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Solution

Silicon does not form graphite like structure as size of silicon is larger than carbon . Due to the small size of carbon , it will form large chains. Carbon shows catenation .i.e. self linking property. But silicon does not show much catenation .

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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. 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. Explain the following:
(i) Gallium has higher ionization enthalpy than aluminum.
(ii) Boron does not exist as

B^{3 +}

ion.
(iii) Aluminum forms

[A l F_{6}]^{3 -}

ion but boron does not form

[B F_{6}]^{3 -}

P b X_{2}

is more stable than

P b X_{4}

P b^{4 +}

acts as an oxidizing agent, but

S n^{2 +}

acts as a reducing agent.
(vi) Electron gain enthalpy of chlorine is more negative as compared to fluorine.
(vii)

T I (N O_{3})_{3}

acts as an oxidizing agent.
(viii) Carbon shows catenation property but lead does not.
(ix)

B F_{3}

does not hydrolyze.
(x) Why does the element silicon, not form a graphite-like structure whereas carbon does?

Diamond and graphite are allotropes of carbon.

Reason: Some elements can have different structural forms called allotropes.

Q. Which of the following is not an element ?
(a) graphite
(b) germanium
(c) silica
(d) silicon

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