Question

Assertion: s- orbital electron will be more tightly bound to the nucleus than p- orbital electron.
Reason: Zeff experienced by the electron decreases with increase of azimuthal quantum number(l)​

Answer 1

Answer:

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Explanation:

The net positive charge experienced by the outer electrons is known as effective nuclear charge (Z

eff

e). The Z

eff

experienced b the electrons decreases with increase of azimuthul quantum number (l), that is the s orbital electron will be more tightly bound to the nucleus than p orbital electrons which in turn will be better tightly bound than the d orbital electrons.

Hence the arrangement of sub-shells in the increasing order of effective nuclear charge is:

d<p<s

Answer 2

Both assertion and reason are true and reason is the correct explaination of assertion.

• The closer the orbital comes to the nucleus, the more strongly it is related. As a result, an s-orbital electron will be more strongly bonded to the atom's nucleus than a p-orbital electron.
• With increasing azimuthal quantum number l, effective nuclear charge falls. The effective nuclear charge experienced by an electron in an orbital within a particular shell is in the order s > p > d > f.
• Hence, both assertion and reason are true and reason is the correct explaination of assertion.