Kerala KEAM 5 June 2024 Solved Paper

The number of angular nodes and radial nodes in an orbital can be determined by the following formulas:1. Angular nodes: The number of angular nodes is equal to $l$, where $l$ is the azimuthal quantum number. For a 'd' orbital, $l = 2$. Therefore, the number of angular nodes is:$$Angular nodes = l = 2$$2. Radial nodes: The number of radial nodes is given by the formula:$$Radial nodes = n - l - 1$$where $n$ is the principal quantum number. For the '4d' orbital, $n = 4$ and $l = 2$. So, the number of radial nodes is:$$Radial nodes = 4 - 2 - 1 = 1$$Thus, the number of angular nodes is 2, and the number of radial nodes is 1.Therefore, the correct answer is:$$\boxed{A) 2, 1}$$ Quick Tip: The number of angular nodes in an orbital is equal to the value of $l$, while the number of radial nodes is given by the formula $n - l - 1$, where $n$ is the principal quantum number.