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प्रश्न
Draw shapes of 2s orbitals.
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उत्तर
Shapes of 1s and 2s orbitals Boundary surface diagrams
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संबंधित प्रश्न
Using s, p, d notations, describe the orbital with the following quantum numbers n = 4; l = 2.
Using s, p, d notations, describe the orbital with the following quantum numbers n = 4; l =3.
Choose the correct option.
“No two electrons in the same atoms can have identical set of four quantum numbers”. This statement is known as -
Define the term Electronic configuration.
State the order of filling atomic orbitals following Aufbau principle.
Explain the anomalous behaviour of chromium.
Write electronic configurations of \[\ce{Fe, Fe2+, Fe3+}\].
Write condensed orbital notation of electronic configuration of the following element:
Carbon (Z = 6)
If n = 3, what are the quantum number l and m?
The principal quantum number (n) and magnetic quantum number (ml) for the valence electrons of rubidium atom (Z = 37) are ____________ respectively.
Which mineral among the following contains vanadium in it?
The three electrons have the following set of quantum numbers:
X = 6, 1, −1, `+1/2`
Y = 6, 0, 0, `+1/2`
Z = 5, 1, 0, `+1/2`
Identify the CORRECT statement.
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 properties of atom could be explained correctly by Thomson Model of atom?
Number of angular nodes for 4d orbital is ______.
Total number of orbitals associated with third shell will be ______.
In which of the following pairs, the ions are iso-electronic?
(i) \[\ce{Na^{+}, Mg^{2+}}\]
(ii) \[\ce{Al3^{+}, O-}\]
(iii) \[\ce{Na+ , O2-}\]
(iv) \[\ce{N3-, Cl-}\]
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.
Which of the following orbitals are degenerate?
3dxy, 4dxy 3dz2, 3dyz, 4dyz, 4dz2
Calculate the total number of angular nodes and radial nodes present in 3p orbital.
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.
4s, 3s, 3p, 4d
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 of the following is the correct plot for the probability density ψ2 (r) as a function of distance 'r' of the electron from the nucleus for 2s orbitals?
In the case of R, S configuration the group having the highest priority is ______.
Which one of the following laws will represent the pairing of electrons in a subshell after each orbital is filled with one electron?
