Elemental silicon does not form graphite like structure as carbon does. Give reason.

Open in App

Solution

It is because $S i$ cannot form $p π - p π$ bond like carbon in graphite due to larger atomic size.

Suggest Corrections

Similar questions

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

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 -}

ion.
(iv)

P b X_{2}

is more stable than

P b X_{4}

(v)

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?

Q. Explain the following:

A Gallium has higher ionization enthalpy than Aluminium.

B Boron does not exist as $B^{3+}$ ion

C Aluminium forms $[AlF_6]^{3-}$- ion but Boron does not form $[BF_6]^{3-}$- ion.

D $PbX_2$ is more stable than $PbX_4$.

E $Pb^{4+}$ acts as an oxidizing agent but $Sn^{2+}$ acts as a reducing agent.

F Electron gain enthalpy of chlorine is more negative as compared to fluorine.

G $Tl (NO_3)_3$ acts as an oxidizing agent.

H Carbon shows catenation property but lead does not.

I $BF_3$ does not hydrolyze.

J Why does the element silicon not form a graphite-like structure whereas carbon does.

Q. No form of elemental silicon is comparable to graphite. Give reason.

Silicon is also tetravalent like carbon but why it does not combine with so many elements to form thousands of covalent compunds just like carbon does ?

Join BYJU'S Learning Program

Elemental silicon does not form graphite like structure as carbon does. Give reason.

It is because Si cannot form pπ−pπ bond like carbon in graphite due to larger atomic size.

It is because $S i$ cannot form $p π - p π$ bond like carbon in graphite due to larger atomic size.