Among the statements (I – IV), the correct ones
are:
(I) Be has smaller atomic radius compared to
Mg.
(II) Be has higher ionization enthalpy than Al.
(III) Charge/radius ratio of Be is greater than
that of Al.
(IV) Both Be and Al form mainly covalent
compounds.
Solution
Be < Mg (atomic radius)
<br><br>Be > Al (I.E<sub>1</sub> greater than Al because of fully filled valence shell of Be)
<br><br> Charge/radius ratio of Be is less than that of Al.
<br><br>Both Be and Al form mainly covalent
compound.
About this question
Subject: Chemistry · Chapter: Periodic Table and Periodicity · Topic: Periodic Trends
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