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Using s, p, d notations, describe the orbital with the following quantum numbers n = 3; l =1.

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प्रश्न

Using s, p, d notations, describe the orbital with the following quantum numbers n = 3; l =1.

एका वाक्यात उत्तर
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उत्तर

For n = 3 and l = 1

The orbital is 3p.

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पाठ 2: Structure of Atom - EXERCISES [पृष्ठ ७०]

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एनसीईआरटी Chemistry Part 1 and 2 [English] Class 11
पाठ 2 Structure of Atom
EXERCISES | Q 2.29 - (b) | पृष्ठ ७०

संबंधित प्रश्‍न

Choose the correct option.

“No two electrons in the same atoms can have identical set of four quantum numbers”. This statement is known as -


Explain the anomalous behaviour of copper.


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

n = 2, l = 1


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


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

Lithium (Z = 3)


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

Chlorine (Z = 17)


Explain in brief, the significance of the azimuthal quantum number.


If n = 3, what are the quantum number l and m?


The designation of a subshell with n = 6 and l = 2 is ____________.


Which one of the following orders is CORRECT in case of energy of the given subshells?

P: n = 4; l = 3

Q: n = 5; I = 1

R: n = 5; l = 0

S: n = 4; l = 2


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


Which of the following has a greater number of electrons than neutrons?

(Mass number of Mg, C, O and Na is 24, 12, 16 and 23 respectively).


The probability density plots of 1s and 2s orbitals are given in Figure:


The density of dots in a region represents the probability density of finding electrons in the region.

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


Which of the following statements concerning the quantum numbers are correct?

(i) Angular quantum number determines the three dimensional shape of the orbital.

(ii) The principal quantum number determines the orientation and energy of the orbital.

(iii) Magnetic quantum number determines the size of the orbital.

(iv) Spin quantum number of an electron determines the orientation of the spin of electron relative to the chosen axis.


Nickel atom can lose two electrons to form \[\ce{Ni^{2+}}\] ion. The atomic number of nickel is 28. From which orbital will nickel lose two electrons.


The arrangement of orbitals on the basis of energy is based upon their (n + l) value. Lower the value of (n + l), lower is the energy. For orbitals having same values of (n + l), the orbital with lower value of n will have lower energy.

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

1s, 2s, 3s, 2p


Match the following species with their corresponding ground state electronic configuration.

Atom / Ion Electronic configuration
(i) \[\ce{Cu}\] (a) 1s2 2s2 2p6 3s2 3p6 3d10
(ii) \[\ce{Cu^{2+}}\] (b) 1s2 2s2 2p6 3s2 3p6 3d10 4s2
(iii) \[\ce{Zn^{2+}}\] (c) 1s2 2s2 2p6 3s2 3p6 3d10 4s1
(iv) \[\ce{Cr^{3+}}\] (d) 1s2 2s2 2p6 3s2 3p6 3d9
  (e) 1s2 2s2 2p6 3s2 3p6 3d3

Match the quantum numbers with the information provided by these.

Quantum number Information provided
(i) Principal quantum number (a) orientation of the orbital
(ii) Azimuthal quantum number (b) energy and size of orbital
(iii) Magnetic quantum number (c) spin of electron
(iv) Spin quantum number (d) shape of the orbital

In assigning R - S configuration, which among the following groups has highest priority?


Which of the following element do not follow Aufbau principle?


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