Advertisements
Advertisements
प्रश्न
Give the names of quantum numbers.
Advertisements
उत्तर
The four quantum numbers are principal quantum number (n), azimuthal or subsidiary quantum number (l), magnetic quantum number (ml), and electron spin quantum number (ms).
APPEARS IN
संबंधित प्रश्न
Using s, p, d notations, describe the orbital with the following quantum numbers n = 3; l =1.
Choose the correct option.
p-orbitals are _________ in shape.
Choose the correct option.
“No two electrons in the same atoms can have identical set of four quantum numbers”. This statement is known as -
State and explain Pauli’s exclusion principle.
State the order of filling atomic orbitals following Aufbau principle.
Write orbital notations for the electron in orbitals with the following quantum numbers.
n = 2, l = 1
Write orbital notations for the electron in orbitals with the following quantum numbers.
n = 4, l = 2
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:
Calcium (Z = 20)
Draw shapes of 2s orbitals.
Draw shapes of 2p orbitals.
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.
Indicate the number of unpaired electrons in \[\ce{Si}\] (Z = 14).
The designation of a subshell with n = 6 and l = 2 is ____________.
Number of angular nodes for 4d orbital is ______.
Total number of orbitals associated with third shell will be ______.
Orbital angular momentum depends on ______.
The pair of ions having same electronic configuration is ______.
Out of the following pairs of electrons, identify the pairs of electrons present in degenerate orbitals:
| (i) | (a) `n = 3, l = 2, m_l = -2, m_s = - 1/2` |
| (b) `n = 3, l = 2, m_l = -1, m_s = - 1/2` | |
| (ii) | (a) `n = 3, l = 1, m_l = 1, m_s = + 1/2` |
| (b) `n = 3, l = 2, m_l = 1, m_s = + 1/2` | |
| (iii) | (a) `n = 4, l = 1, m_l = 1, m_s = + 1/2` |
| (b) `n = 3, l = 2, m_l = 1, m_s = + 1/2` | |
| (iv) | (a) `n = 3, l = 2, m_l = +2, m_s = - 1/2` |
| (b) `n = 3, l = 2, m_l = +2, m_s = + 1/2` |
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
The electronic configuration of valence shell of Cu is 3d104s1 and not 3d94s2. How is this configuration explained?
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 |
Choose the INCORRECT statement
Which of the following element do not follow Aufbau principle?
What are the possible values of magnetic quantum number for p orbital?
