The radial probability distribution for an electron in an atom a. becomes zero at the nucleus. b. is smallest near the nucleus. c. is largest near the nucleus. d. may be zero at more than one point. e. tends to infinity at large distances from the nucleus.

The radial probability distribution for an electron in an atom may be zero at more than one point.

Step-by-step explanation:

If we count the number of dots in each spherical shell, we obtain the total probability of finding the electron at a given value of r. Because the surface area of each shell increases more rapidly with increasing r than the electron probability density decreases, a plot of electron probability versus r (the radial probability) shows a peak. This peak corresponds to the most probable radius for the electron.

In the attached plots, it is shown electron probability as a function of distance from the nucleus (r) in all directions (radial probability), the most probable radius increases as n increases, but the 2s and 3s orbitals have regions of significant electron probability at small values of r.

step-by-step explanation:

no, her answer is not correct.   we square the lengths of all sides and then determine whether the pythagorean theorem holds here:

9² + 15² = 306.   this is not equal to the square of the longest side ( that square being 395.   answer c is correct.

step-by-step explanation:

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