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An element ‘M’ with electronic configuration 2 8 3 combines separately with Cl-, SO 4 -2 anions. Write the chemical formulae of the compounds formed. Predict with the suitable reason the nature of the bond formed by element ‘M’ in general. How will the electrical conductivity of the compounds formed vary with respect to ‘M’?
Answer:
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The element M having electronic configuration 2,8,3 has 3 electrons in the outermost shell.
With Cl- :
When the element M combines with Cl-, it will lose 3 outermost shell electrons in order to attain a stable electronic configuration of (2,8). Since 1 Cl- can accept only 1 electron, M will combine with 3 Cl- to form MCl3.
With SO 4 2- :
When the element M combines with SO 4 2- , it will lose 3 outermost shell electrons in order to attain a stable configuration of (2,8). SO 4 2- can accept only electrons, so 2 M will combine with 3 SO 4 2- and form M2(SO 4 ) 3 .
In order to form these compounds, an exchange of electrons takes place. M is losing electrons, whereas Cl- or SO 4 2- are gaining electrons. Therefore, the nature of bond formed between them will be ionic bond.
Both MCl 3 and M 2 (SO 4 ) 3 will conduct electricity only in dissolved state or molten state. But they will not conduct electricity in solid state because of the unavailability of free ions.
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