Atomic Structure Orbitals
Electrons occupy outer space in the structure of the atom. However they are not arranged randomly, but orderly.
Introduction to atomic structure orbitals
Electrons are moving in three dimensional space.The space in which they are moving is called as orbitals .The same is also called as sub-shell.I like to share this Werner Heisenberg Atomic Theory with you all through my article.
As they are not fixed in a position, they are not said to be at a fixed place in the orbitals. They are like waves. So the electrons in orbitals are exhibiting uncertainty. This is called as principle of uncertainity and is the probability of finding an electron at a place in an orbital is given by Heisenberg's equation. Schrödinger, Pauling, Mulliken were also others who contributed to it by the application of quantum mechanics.
Types of Atomic Orbitals
There are orbitals called s,p,d,f and so on.
The s orbital is spherical in structure, the p orbital is dumble shaped and so on.
The s orbital is lowest in energy and the level goes on increasing from p, d, f and so on.
So the first orbital to be filled is 's' followed by p, d, f etc...,
These atomic orbitals have different capacities to accommodate electrons. It is given by the formula 2[2l+1] where s, p, d, f have l=0,1,2,3 respectively.
Thus the s orbital has capacity of 2.
Both these electrons would have opposite spins.
Similarly the p orbital would have the capacity of 6 and the d orbital 10.
These orbitals are arranged in the shells like K, L, M, N etc..,
The number of electrons to be occupied by these shells is given by the formula 2n2 where n is 1,2,3, for K,LM,N etc.
Electronic configuration of atoms too can be shown as electronic configuration of the noble gas followed by the remaining valence electrons in specific orbitals.Please express your views of this topic Ionic Compound Formula by commenting on blog.
e.g.Na with atomic number 11= [Ne] 3s1
Mg with atomic number 12= [Ne] 3s2
K with atomic number 19 =[Ar] 4s1
Ca with atomic number 20 =[Ar] 4s2
Reactivity and Orbital Structure.
As a principle, in a bond formation reaction, an atom would try to give out that electron which is possessing highest energy. In a nitrogen atom, the orbital from which electron would be utilised to form a bond is p orbital.
The orbitals may also mix up and rarrange to form hybridized orbitals.
e.g. Carbon in CH4 is having four sp3 hybridized orbitals with tetrahedral structure.
Introduction to atomic structure orbitals
Electrons are moving in three dimensional space.The space in which they are moving is called as orbitals .The same is also called as sub-shell.I like to share this Werner Heisenberg Atomic Theory with you all through my article.
As they are not fixed in a position, they are not said to be at a fixed place in the orbitals. They are like waves. So the electrons in orbitals are exhibiting uncertainty. This is called as principle of uncertainity and is the probability of finding an electron at a place in an orbital is given by Heisenberg's equation. Schrödinger, Pauling, Mulliken were also others who contributed to it by the application of quantum mechanics.
Types of Atomic Orbitals
There are orbitals called s,p,d,f and so on.
The s orbital is spherical in structure, the p orbital is dumble shaped and so on.
The s orbital is lowest in energy and the level goes on increasing from p, d, f and so on.
So the first orbital to be filled is 's' followed by p, d, f etc...,
These atomic orbitals have different capacities to accommodate electrons. It is given by the formula 2[2l+1] where s, p, d, f have l=0,1,2,3 respectively.
Thus the s orbital has capacity of 2.
Both these electrons would have opposite spins.
Similarly the p orbital would have the capacity of 6 and the d orbital 10.
These orbitals are arranged in the shells like K, L, M, N etc..,
The number of electrons to be occupied by these shells is given by the formula 2n2 where n is 1,2,3, for K,LM,N etc.
Electronic configuration of atoms too can be shown as electronic configuration of the noble gas followed by the remaining valence electrons in specific orbitals.Please express your views of this topic Ionic Compound Formula by commenting on blog.
e.g.Na with atomic number 11= [Ne] 3s1
Mg with atomic number 12= [Ne] 3s2
K with atomic number 19 =[Ar] 4s1
Ca with atomic number 20 =[Ar] 4s2
Reactivity and Orbital Structure.
As a principle, in a bond formation reaction, an atom would try to give out that electron which is possessing highest energy. In a nitrogen atom, the orbital from which electron would be utilised to form a bond is p orbital.
The orbitals may also mix up and rarrange to form hybridized orbitals.
e.g. Carbon in CH4 is having four sp3 hybridized orbitals with tetrahedral structure.