Advertisements
Advertisements
प्रश्न
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 |
Advertisements
उत्तर
| Atom / Ion | Electronic configuration |
| (i) \[\ce{Cu}\] | (c) 1s2 2s2 2p6 3s2 3p6 3d10 4s1 |
| (ii) \[\ce{Cu^{2+}}\] | (d) 1s2 2s2 2p6 3s2 3p6 3d9 |
| (iii) \[\ce{Zn^{2+}}\] | (a) 1s2 2s2 2p6 3s2 3p6 3d10 |
| (iv) \[\ce{Cr^{3+}}\] | (e) 1s2 2s2 2p6 3s2 3p6 3d3 |
APPEARS IN
संबंधित प्रश्न
Using s, p, d notations, describe the orbital with the following quantum numbers n = 1, l = 0.
Give the names of quantum numbers.
Define the term Electronic configuration.
Explain the anomalous behaviour of chromium.
Write condensed orbital notation of electronic configuration of the following element:
Carbon (Z = 6)
Write condensed orbital notation of electronic configuration of the following element:
Oxygen (Z = 8)
Write condensed orbital notation of electronic configuration of the following element:
Silicon (Z = 14)
Write condensed orbital notation of electronic configuration of the following element:
Chlorine (Z = 17)
The electronic configuration of oxygen is written as 1s2 2s2 \[\ce{2p^2_{{x}}}\] \[\ce{2p^1_{{y}}}\] \[\ce{2p^1_{{z}}}\] and not as 1s2 2s2 \[\ce{2p^2_{{x}}}\], \[\ce{2p^2_{{y}}}\] \[\ce{2p^0_{{z}}}\], Explain.
Indicate the number of unpaired electrons in \[\ce{Si}\] (Z = 14).
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?
The pair of ions having same electronic configuration is ______.
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.
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.
5f, 6d, 7s, 7p
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 |
In the case of R, S configuration the group having the highest priority is ______.
