Why half filled and fully filled orbitals are most stable?
The orbitals in which the sub-shell is exactly half-filled or completely filled are more stable because of the symmetrical distribution of electrons. Exchange energy: The electrons which are there in degenerate orbitals have a parallel spin and tend to exchange their position. Therefore, its stability is maximum.
Is fully filled orbitals more stable than half filled?
Full filled orbitals are more stable than half filled orbitals. Half filled orbitals are more stable than any other type of configuration( except full filled, of course). Half-filled orbitals and Full-filled orbitals are more stable because they are symmetrical in nature and they have less exchange energy.
What orbitals are most stable?
Explanation: Half-filled and fully filled orbitals are most stable.
Why are d5 and d10 more stable?
Answer: this is because of a phenomenon known as exchange energy . The greater the exchange energy , the more stable the atom is . So the d10 type of electronic configuration is more stable than the d5 type of electronic configuration .
What is the difference between stable and unstable electronic configuration?
Stable electronic configuration: Atoms having octet (8 electrons) or duplet 2 electrons in outermost shell is stable electronic configuration 2 electrons in K shell the valence shell. Unstable electronic configuration: “Atoms of the element which do not have their valence shells completely filled.”
Why fully filled subshells are more stable?
The reason for their stability are symmetry and exchange energy. The half-filled and fully-filled orbitals are more symmetrical than any other configuration and symmetry leads to greater stability. The electrons present in the different orbitals of the same sub-shell can exchange their positions.
Why is a full shell more stable?
A complete octet is very stable because all orbitals will be full. Atoms with greater stability have less energy, so a reaction that increases the stability of the atoms will release energy in the form of heat or light. A stable arrangement is attended when the atom is surrounded by eight electrons.
Why half filled and completely filled orbital electronic configuration are more stable in comparison to incompletely filled orbital electronic configuration?
The exactly half-filled and fully filled orbitals have greater stability than other configurations. The reason for their stability are symmetry and exchange energy. The electrons present in the different orbitals of the same sub-shell can exchange their positions.
Which is more stable d10 or d5?
d10 orbital is more stable than d5 orbital. According to HUND’S STABILITY RULE , FULFILLED ORBITAL IS MORE STABLE THAN HALF FILLED ORBITAL AND HALF FILLED ORBITAL IS MORE STABLE THAN UNFILLED ORBITAL(which neither have half filled electron nor fullfilled electron in the orbital).
Which electron configurations are the most stable and why?
The most stable electron configuration is that of a noble gas, due to the fact that its valence shell is filled. For helium, that means two valence electrons (a duet) in the 1s sublevel, and for the rest it means eight valence electrons (an octet) in the outermost s and p sublevels.
What makes an electron stable?
Atoms are stable when they have eight valence electrons (two in the case of hydrogen). This is called having an octet. You can see that each hydrogen atom now has a duet of valence electrons, making them stable, and the oxygen atom now has an octet of valence electrons, making it stable.
Why are the half-filled and fully filled orbitals more stable?
The exchange energy is maximized when orbitals are half filled and completely filled. I understand the concept of half-filled orbitals. They are more stable because they have single electrons with one directional spin But what’s about fully filled orbitals because each orbital has two electrons with opposite spins.
Is the energy of an electron in an orbital stable?
There is nothing especially stable about half filled or fully filled orbitals. The energy of an electron in an orbital depends on the attraction of the nuclear charge and the electrostatic interaction of the electrons. There is another, quantum mechanical, interaction between electrons known as exchange energy.
What happens when two electrons have the same spin?
Two or more electrons with the same spin can exchange their position with the degenerate orbitals. The spinning of electrons introduces a new type of quantum mechanical interaction called Exchange energy, Eex.
Why are the 4s and 3d orbitals degenerate?
For chromium, it turns out the 4s and 3d orbitals are virtually degenerate. This means that the energy required to pair two electrons in the 4s orbital is more than the energy required to move up and put an electron in the 3d orbital. No need to invoke electron exchange energy here.