Already have an account? Get multiple benefits of using own account!
Login in your account..!
Remember me
Don't have an account? Create your account in less than a minutes,
Forgot password? how can I recover my password now!
Enter right registered email to receive password!
Q. Example of octahedral complexes?
Let us now turn our attention to the complexes having transition metal ion with d2 or d3 electrons. With these configurations, there are enough of vacant orbitals available to accept the pairs of elements from four or six ligands to form tetrahedral, square planar or octahedral compound. The magnetic moment of the complex will be the same as free ion value as shown in the diagram given below:
When the number of d electrons is greater than three and up to six as in d2, d6 systems, there is still a possibility of forming octahedral complexes using d2sp3 hybridised orbitals by forcing some of the electrons to pair up.
What is the diagonal relationship between Beryllium and Aluminium
Desiccants (drying agents) can often be regenerated by heating. A desiccant that is commonly regenerated is CaSO 4 ?2H 2 O:
Organic Compounds - Organic Chemistry The term 'organic' signifies life. Hence, every molecule that was prepared directly or indirectly from living organisms, animals and plant
,Potassium-42 is a radioisotope that nutritionists use to determine whether the body is effectively using potassium at the cellular level. The half-life of potassium-42 is 12.4 hou
Processing of Cereals Owing to the low moisture content, cereals and pulses are relatively stable during storage; and processing is not so much for preservation. However, proc
what is atomic mass?
do bases react with lab glassware?
What is the reliablitiy of redox titrations?
The number of electrons that can be accommodated in dz 2 orbital: (1) 10 (2) 1 (3) 4 (4) 2 Ans: 2
#question.i
Get guaranteed satisfaction & time on delivery in every assignment order you paid with us! We ensure premium quality solution document along with free turntin report!
whatsapp: +91-977-207-8620
Phone: +91-977-207-8620
Email: [email protected]
All rights reserved! Copyrights ©2019-2020 ExpertsMind IT Educational Pvt Ltd