Question

Arrange S, P, As in order of increasing ionisation energy
(a) S < P < As (b) P < S < As
(c) As < S < P (d) As < P < S

Answer 1

Among the following the increasing order of Ionisation energy is as followed

As < S < P

1) We know Ionisation energy is inversely proportional to size of atom so As being the biggest among these has lowest I.E

2) Among P and S the last shell of P has half filled electrons which make it more stable and hence more energy is required to remove an electron from its last shell as compared to S so P has greater Ionisation energy than S.

3) So option (c) is the right answer

Answer 2

As < S < P  is the correct order.

Explanation:

• Ionisation energy is defined as the amount of energy needed to pull out one electron from an atom to make it a single charged cation.

• The ionisation energy has a particular trend along the periodic table.

• As we move right along the periodic table, the ionization energy decrease because of the more number of electrons pushing the others easily, with minor exceptions.

As we move down the periodic table, the ionization energy always decrease because of the addition of more shell and increase of distance between the last shell and nucleus.

• In phosphorus and arsenic we can see that the electronic configuration is identical, being in same group 15, which is ns2 np3.

• The electronic configuration of sulphur is ns2 np4.

• Arsenic being in next period has the less ionisation energy from rest.

• But phosphorous having half filled p orbital, is more stable than sulphur, hence having more ionisation enthalpy.

For more information about ionisation enthalpy,

https://brainly.in/question/6571176

The first ionization energy of sodium boron nitrogen and oxygen atoms follows the order

https://brainly.in/question/11934521

Define ionization energy. Name the

factors on which ionisation energy

depends? How does it vary down the

group and across a period?​