Question map
The number of angular and radial nodes for 4d orbital is respectively
Explanation
In atomic chemistry, the number of nodes in an orbital is determined by its quantum numbers. For a 4d orbital, the principal quantum number (n) is 4 and the azimuthal quantum number (l) is 2, as l=2 corresponds to d-orbitals. The number of angular nodes is equal to the azimuthal quantum number (l), which for a 4d orbital is 2. The number of radial nodes is calculated using the formula (n - l - 1). Substituting the values for a 4d orbital (4 - 2 - 1) results in 1 radial node. Therefore, the 4d orbital has 2 angular nodes and 1 radial node respectively. This distinction is crucial as radial nodes represent spherical surfaces where the probability of finding an electron is zero, while angular nodes represent planar or conical surfaces.
SIMILAR QUESTIONS
Which of the following pairs are correctly matched ?
(Period) | (Wars)
1. AD 1767-69 | First Anglo Maratha War
2. AD 1790-92 | Third Mysore War
3. AD 1824-26 | First Anglo-Burmese War
4. AD 1845-46 | Second Sikh War