Final answer:
The energy of the highest frequency radiation emitted by boron in the visible region can be calculated using Planck's equation.
Step-by-step explanation:
To answer the student's question, we must first identify the highest frequency radiation emitted by boron in the visible region, use Planck's equation to calculate the energy of the radiation, find the wavelength of this radiation, determine the electronic configuration of boron, and calculate the frequency of the emitted radiation.
(a) We use Planck's equation, E = hf, where h is Planck's constant (6.626 x 10-34 J·s) and f is the frequency. The visible region ends at violet, with frequencies around 7.5 x 1014 Hz. (b) We convert this frequency to wavelength using λ = c/f, where c is the speed of light (3 x 108 m/s), to find the wavelength of the violet light. (c) The electronic configuration of boron is 1s2 2s2 2p1. (d) To calculate the frequency of the radiation, we can use the frequency corresponding to violet light, as it would be close to the highest frequency radiation that boron can emit in the visible spectrum.
The energy of the radiation in kJ/mol can be found by first calculating the energy in joules (E = hf) and then converting it to kJ/mol using Avogadro's number since 1 mole of photons will contain 6.022 x 1023 photons.