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D Divya Prakash Singh
Given quantum numbers : NOT possible, because n cannot be equal to zero.

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D Divya Prakash Singh
The number of orbitals in the  shell is equal to . So, for , there are  orbitals present. As each orbital has one electron with spin . Hence, there will be  electrons with .

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D Divya Prakash Singh
For a given value of ,  can have values from  to . Therefore, for ,  can have values from   to . i.e., . Thus, four subshells are associated with , which are 

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D Divya Prakash Singh
As Krypton (Kr) is a noble gas whose atomic number is 36 and have all orbitals filled. Hence, there are no unpaired electrons in Kr element.

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D Divya Prakash Singh
The electronic configuration of Fe : . Hence, the number of unpaired electrons are 4 (in 3d ).

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D Divya Prakash Singh
The electronic configuration of Cr : . Hence, the number of unpaired electrons are 6 (1 in 4s and 5 in 3d).

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D Divya Prakash Singh
The electronic configuration of Si : . Hence, the number of unpaired electrons are 2 in  orbital.  

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D Divya Prakash Singh
The electronic configuration of P: . Hence, the number of unpaired electrons are 3 in 3p orbital.    

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D Divya Prakash Singh
Nuclear charge is defined as the net positive charge experienced by an electron in the orbital of an atom exerted by the nucleus of the atom. Silicon has a greater nuclear charge  than aluminium . Hence, the effective nuclear charge exerted on the unpaired 3p electron of silicon would be greater as compared to that of aluminium. 

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D Divya Prakash Singh
Nuclear charge is defined as the net positive charge experienced by an electron in the orbital of an atom exerted by the nucleus of the atom. Closer orbitals experience more nuclear charge than outer orbitals. Therefore, (ii) 3d and 3p The 3p orbital is more closer to the nucleus than 3d orbital hence 3p will experience a larger effective nuclear charge compared to 3d.

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D Divya Prakash Singh
Nuclear charge is defined as the net positive charge experienced by an electron in the orbital of an atom exerted by the nucleus of the atom. Closer orbitals experience more nuclear charge than outer orbitals. Therefore, (ii) 4d and 4f The 4d orbital is more closer to the nucleus than 4f orbital hence 4d will experience a larger effective nuclear charge compared to 4f.

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D Divya Prakash Singh
Nuclear charge is defined as the net positive charge experienced by an electron in the orbital of an atom exerted by the nucleus of the atom. Closer orbitals experience more nuclear charge than outer orbitals. Therefore, (i) 2s and 3s The 2s orbital is more closer to the nucleus than 3s orbital hence 2s will experience a larger effective nuclear charge compared to 3s.

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D Divya Prakash Singh
As the p-orbital is farthest from the nucleus hence the electrons in (4p)subshell experiences the lowest effective nuclear charge.  

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D Divya Prakash Singh
Quantum number provides the entire information about an electron of a particular atom. Principal quantum number   Azimuthal quantum number  Magnetic quantum number  Spin quantum number . The orbitals occupied by the electrons are: 1. 4d-orbital  2. 3d-orbital 3. 4p-orbital 4. 3d-orbital 5. 3p-orbital 6. 4p-orbital For the same orbitals, electrons will have the same energy and higher the value...

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D Divya Prakash Singh
We have given the uncertainty in position, i.e., . According to Heisenberg's Uncertainty Principle: Where,  is uncertainty in the position of the electron.  is uncertainty in the momentum of the electron. Then,  Or            The actual momentum of the electron: Therefore, it cannot be defined because the actual magnitude of the momentum is smaller than the uncertainty.
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