Which of the following best explains what happens as photons of visible light are absorbed by dye molecules?

A) Certain electrons in the dye molecule move to a higher energy level, with the difference in energy between the lower and higher energy levels being the same as the energy of the absorbed photons.
B) Certain chemical bonds in the dye molecules begin to bend and stretch, with the difference in energy between the lower and higher vibrational states being the same as the energy of the absorbed photons.
C) The dye molecules begin to rotate faster in certain modes, with the difference in energy between the lower and higher rotational states being the same as the energy of the absorbed photons.
D) Certain covalent bonds in the dye molecules begin to break and re-form, with the bond energies of the bonds being the same as the energy of the absorbed photons.

A) Certain electrons in the dye molecule move to a higher energy level, with the difference in energy between the lower and higher energy levels being the same as the energy of the absorbed photons.

Explanation:

The reason behind the photonsWhen UV photon or a photon of visible light  is absorbed by an atom then the summation whole of energy of that particular photon gets all excited to a higher energy level. The following movement of an electron to a higher energy level from a lower energy level is called as a transition. A successful transition occurs only in that condition when the energy of the photons which gets absorbed should be greater than or equal to the difference in energy between the underlying energy levels. also,we know that once the electron is being excited to a higher energy level, it becomes more unstable for a fact we know that electron becomes stable only when iot ios grounded or in groud state. As such, the electron will quickly fall back down to the lower energy level and hence it emits a photon with an energy equal to the difference in energy levels.

this explains best about the phenemenon of phtons of visible light being absorbed by dye molecules

assuming that your periodic table has eighteen columns, you should highlight   the four elements in the third column from the left of the table.

neutral atoms of elements after calcium contain d electrons. the energy of d orbitals of a particular main shell lies between the energy of the s and p orbitals of the next main shell. for example, electrons in the have energy higher than those in the orbital while lower than those of the orbital.

by the aufbau principle, electrons fill orbitals one at a time, starting from those of the lowest energy. the orbital is therefore filled right after orbitals and before orbitals.  

potassium has electron configuration and calcium . the s orbital of a main shell holds a maximum of two electrons. the next element would thus have the electron configuration and satisfy the requirements.

a neutral atom of the element contains three electrons on top of the most recent noble gas element. it should thus be placed in the third column of the periodic table. both scandium and yttrium would satisfy the conditions. an aufbau diagram indicates that the 4f orbital is filled before the 5d. however, it appears that exceptions exists for both lanthanum and actinium. neutral atoms of the two d-block elements also demonstrate the and should be highlighted as well.