If compound MX_4 is non-polar and has no lone | vedclass

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(D) For a molecule $MX_4$ to be non-polar with no lone pair on the central atom,it must have a highly symmetric geometry such that the dipole moments

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All of these

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(D) For a molecule $MX_4$ to be non-polar with no lone pair on the central atom,it must have a highly symmetric geometry such that the dipole moments cancel out.$1$. If the geometry is tetrahedral ($sp^3$ hybridization),the bond angle is $109^o28'$.$2$. If the geometry is square planar ($dsp^2$ hybridization),the bond angle is $90^o$.$3$. If the geometry is linear ($sp^3d^2$ or similar symmetric arrangements),the bond angle can be $180^o$.Therefore,all the given bond angles are possible depending on the specific geometry of the $MX_4$ molecule.

Label	Order	Property
$i.$	$NH_3 > H_2O > SO_2$	Bond angle
$ii.$	$H_2O > NH_3 > H_2S$	Dipole moment
$iii.$	$N_2 > O_2 > H_2$	Bond enthalpy
$iv.$	$NO^{+} > O_2 > O_2^{2-}$	Bond order

If compound $MX_4$ is non-polar and has no lone pair at the central atom,then the bond angle $\angle XMX$ in the compound may be:

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Calculate the formal charge on the $C$ atom in the thiocyanate ion $(SCN^-)$ as shown in the structure.

Observe the following sets:
Label Order Property
$i.$ $NH_3 > H_2O > SO_2$ Bond angle
$ii.$ $H_2O > NH_3 > H_2S$ Dipole moment
$iii.$ $N_2 > O_2 > H_2$ Bond enthalpy
$iv.$ $NO^{+} > O_2 > O_2^{2-}$ Bond order

Which of the above sets are correctly matched?

Identify the correct statement among the following options.

Sulphuric acid $(H_2SO_4)$ provides an example of:

Which of the following does not undergo Lewis acid-base reaction?

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