Given below are two statements :Statement (I) | vedclass

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(A) Statement $(I)$ is correct because,in the periodic table,the first ionisation enthalpy generally increases from left to right across a period due

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Statement $I$ is correct but Statement $II$ is incorrect

Vedclass · Answer

(A) Statement $(I)$ is correct because,in the periodic table,the first ionisation enthalpy generally increases from left to right across a period due to the increase in effective nuclear charge and decrease in atomic size. Thus,group $14$ elements have higher first ionisation enthalpy than group $13$ elements.Statement $(II)$ is incorrect because group $14$ elements (like carbon and silicon) form strong covalent bonds in their elemental state,leading to much higher melting and boiling points compared to the corresponding group $13$ elements.

$B$	$801$
$Al$	$577$
$Ga$	$579$
$In$	$558$
$Tl$	$589$

Similar Questions

The correct order of first ionisation enthalpy of the given elements is:

Which of the following elements has the highest metallic character?
Element $- IP$

The first ionization enthalpy values (in $kJ\,mol^{-1}$) of group $13$ elements are :

$B$ $801$

$Al$ $577$

$Ga$ $579$

$In$ $558$

$Tl$ $589$

How would you explain this deviation from the general trend?

In which of the following arrangements is the order not correct according to the property indicated against it?

Identify the element having the highest ionization enthalpy.

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