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Write orbital notations for the electron in orbitals with the following quantum numbers. n = 2, l = 1

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प्रश्न

Write orbital notations for the electron in orbitals with the following quantum numbers.

n = 2, l = 1

एक शब्द/वाक्यांश उत्तर
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उत्तर

2p

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पाठ 4: Structure of Atom - Exercises [पृष्ठ ५४]

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बालभारती Chemistry [English] Standard 11 Maharashtra State Board
पाठ 4 Structure of Atom
Exercises | Q 6. (J)(a) | पृष्ठ ५४

संबंधित प्रश्‍न

Using s, p, d notations, describe the orbital with the following quantum numbers n = 4; l =3.


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Define the term Electronic configuration.


State Hund’s rule of maximum multiplicity with a suitable example.


Write orbital notations for the electron in orbitals with the following quantum numbers.

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Write electronic configurations of \[\ce{Fe, Fe2+, Fe3+}\].


Write condensed orbital notation of electronic configuration of the following element:

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Write condensed orbital notation of electronic configuration of the following element:

Oxygen (Z = 8)


Using the concept of quantum numbers, calculate the maximum numbers of electrons present in the ‘M’ shell. Give their distribution in shells, subshells, and orbitals.


The principal quantum number (n) and magnetic quantum number (ml) for the valence electrons of rubidium atom (Z = 37) are ____________ respectively.


How many electrons in 19K have n = 3, l = 1?


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On the basis of above diagram which of the following statements is incorrect?


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The number of radial nodes for 3p orbital is ______.


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(i) \[\ce{Na^{+}, Mg^{2+}}\]

(ii) \[\ce{Al3^{+}, O-}\]

(iii) \[\ce{Na+ , O2-}\]

(iv) \[\ce{N3-, Cl-}\]


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3dxy, 4dxy 3dz2, 3dyz, 4dyz, 4dz2  


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Based upon the above information, arrange the following orbitals in the increasing order of energy.

1s, 2s, 3s, 2p


The electronic configuration of valence shell of Cu is 3d104s1 and not 3d94s2. How is this configuration explained?


What is the difference between the terms orbit and orbital?


Match species given in Column I with the electronic configuration given in Column II.

Column I Column II
(i) \[\ce{Cr}\] (a) [Ar]3d84s0
(ii) \[\ce{Fe^{2+}}\] (b) [Ar]3d104s1
(iii) \[\ce{Ni^{2+}}\] (c) [Ar]3d64s0
(iv) \[\ce{Cu}\] (d) [Ar] 3d54s1
  (e) [Ar]3d64s2

Which one of the following laws will represent the pairing of electrons in a subshell after each orbital is filled with one electron?


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