Which solid will have the weakest intermolecu | vedclass

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(B) The strength of intermolecular forces is directly related to the melting point of the solid. Among the given options,$Ice$ $(H_2O)$ is a molecular

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Phosphorus

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(B) The strength of intermolecular forces is directly related to the melting point of the solid. Among the given options,$Ice$ $(H_2O)$ is a molecular solid held by hydrogen bonds,but it has a relatively low melting point compared to the others. However,comparing the types: $Sodium \ fluoride$ $(NaF)$ is an ionic solid (strong electrostatic forces),$Phosphorus$ $(P_4)$ and $Naphthalene$ $(C_{10}H_8)$ are molecular solids held by weak van der Waals forces. Among molecular solids,$Ice$ has hydrogen bonding,which is stronger than the London dispersion forces present in $Phosphorus$ and $Naphthalene$. $Phosphorus$ $(P_4)$ consists of discrete molecules held by very weak van der Waals forces,making it the solid with the weakest intermolecular forces among the choices.

$I$. Ion-ion	$a$. $1/r$
$II$. Dipole-dipole	$b$. $1/r^{2}$
$III$. London dispersion	$c$. $1/r^{3}$
	$d$. $1/r^{6}$

Which solid will have the weakest intermolecular forces?

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The number of network solids and ionic solids in the list given below is respectively $H_2O$ (ice),$AlN$,$Cu$,$CaF_2$,diamond,$MgO$,$CCl_4$,$ZnS$,$Ag$,$NaCl$,$SiO_2$.

Graphite is a soft solid lubricant extremely difficult to melt. The reason for this anomalous behaviour is that graphite

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$I$. Ion-ion $a$. $1/r$
$II$. Dipole-dipole $b$. $1/r^{2}$
$III$. London dispersion $c$. $1/r^{3}$
$d$. $1/r^{6}$

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Which of the following does not conduct electricity?

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