MY CART (5)

Use Coupon: CART20 and get 20% off on all online Study Material

ITEM
DETAILS
MRP
DISCOUNT
FINAL PRICE
Total Price: Rs.

There are no items in this cart.
Continue Shopping
Menu
Grade: 11
        
How can you explain higher stability of Bcl3 as compared to Ticl3
 
7 months ago

Answers : (2)

Arun
21971 Points
							
in a group while coming down from top to bottom , due to increase in size and involvement of d and f orbital , the outermost ns2 electron are not shielded or have ineffective sheilding by d or f orbital , so, the s orbital electron remian paired and there increase a inert pair effect , due to which s orbital electron are not used in bonding and +1 oxidation state become more stable while +3 o.s doesnot stable . 
hence , first element boron show +3 o.s in bcl3 becomes stable while the last element of group thalium doesnot show a stable +3 o.s 
so, bcl3 is stable while ticl3 is unstable . 
 
Regards
Arun (askIITians forum expert)
7 months ago
harshin nechooli
121 Points
							
I think Ti is not thallium and it will be representing Titanium in our periodic table so bro I think you are mistaken
7 months ago
Think You Can Provide A Better Answer ?
Answer & Earn Cool Goodies


Course Features

  • 731 Video Lectures
  • Revision Notes
  • Previous Year Papers
  • Mind Map
  • Study Planner
  • NCERT Solutions
  • Discussion Forum
  • Test paper with Video Solution


Course Features

  • 70 Video Lectures
  • Revision Notes
  • Test paper with Video Solution
  • Mind Map
  • Study Planner
  • NCERT Solutions
  • Discussion Forum
  • Previous Year Exam Questions


Ask Experts

Have any Question? Ask Experts

Post Question

 
 
Answer ‘n’ Earn
Attractive Gift
Vouchers
To Win!!! Click Here for details