Question

The electron affinities of boron and aluminum are -27 and -42 kj/mol, respectively.
Contrary to the usual periodic trends, the electron affinities of remaining elements in group 13 are between those of B and Al. How do you explain this apparent anomaly?

Answer 1

Answer:

sorry don't know answer ✌️✌️✌️✌️

Answer 2

The electron affinities of boron and aluminum are -27 and -42 kj/mol, respectively the electron affinities of the remaining elements in group 13 are in between of those of B and Al because of the following reasons:-

• Group 13 is also known as Boron Family and includes Boron, Aluminium, Gallium, Indium, and Thallium.
• The size is the basic reason behind the difference in the electron affinity for the elements of group 13.
• Boron with outer electronic configuration as 2s² 2p¹ has a very small size because of which adding more electrons cause repulsion and makes it unstable, that's why Boron has the least electron affinity in the group.
• Rather, Aluminium with outer electronic configuration as 3s² 3p¹ has an optimum size so that electrons can be added.
• Also, Aluminium is the element of the 3rd period and all the 3rd-period elements have greater electron affinity than the 2nd-period elements.
• That's why Aluminium has the highest electron affinity in the group and then it decreases from Gallium, Indium, and Thallium to Boron at last.

Hence, The electron affinities of boron and aluminum are -27 and -42 kj/mol, respectively the electron affinities of the remaining elements in group 13 are in between of those of B and Al.

#SPJ2