Consider an atom that has an electron in an excited state. The electron falls to a lower energy level. What effect does that have on the electron?

The answer is A (2-7-4)Because when an atom is excited, an electron jumps from the second outermost shell to the outmost shell

The symbol of this configuration has 2 electrons at the local level, so it can be any element of the 2 main subgroup. The transition is possible from one orbital...

Therefore the O electron configuration will be 1s22s22p4. The configuration notation provides an easy way for scientists to write and communicate how electrons are arranged around the nucleus of an atom.Therefore...

If given Ti2+I would write the noble gas electron configuration like this [Ar] 3d2 4s2And then just take away 2 e- from the last number you wrote 4s2-Your noble gas...

E1= h^2/8mL^2 = (6.63x10^-34)^2/8x9.1x10^-31 x 10^-10 x 10^-10 = 0.6038 x 10^-17J.

(b) inductive effect

Ultraviolet and visible radiation interacts with matter which causes electronic transitions (promotion of electrons from the ground state to a high energy state). The ultraviolet region falls in the range between 190-380 nm,...

The total energy, E of the electron is the sum of kinetic energy and potential energy. Kinetic energy of the electron = ½ mv2 Potential energy = -KZe2 /r Total...

An atom of hydrogen in the exited state absorbs energy as an electron moves from the level with low energy to the level with high energy. For example, an electron...

He+ is the hypothetical atom.