For a 4d orbital:
The angular nodes for \( l = 2 \) is \( l = 2 \). The radial nodes are given by \( n - l - 1 \), so for \( n = 4 \) and \( l = 2 \), the radial nodes are \( 4 - 2 - 1 = 1 \). Thus, the total number of nodes is \( 2 + 1 = 3 \).
Which of the following is/are correct with respect to the energy of atomic orbitals of a hydrogen atom?
(A) \( 1s<2s<2p<3d<4s \)
(B) \( 1s<2s = 2p<3s = 3p \)
(C) \( 1s<2s<2p<3s<3p \)
(D) \( 1s<2s<4s<3d \)
Choose the correct answer from the options given below:
The energy of an electron in first Bohr orbit of H-atom is $-13.6$ eV. The magnitude of energy value of electron in the first excited state of Be$^{3+}$ is _____ eV (nearest integer value)