9. Quantum Mechanics

Which of the electron transitions represents absorption with the greatest frequency?

Which of the following transitions (in a hydrogen atom) represent emission of the shortest wavelength?

If the energy of an electron within the boron atom was calculated as –6.0556 x 10^-18 J, at what energy level would it reside?

An atomic emission of light with a specific amount of energy from an atom confirms that

Consider a hydrogen atom in the ground state. What is the energy of its electron?

How much energy does the electron have initially in the n=4 excited state

Consider a hydrogen atom in the ground state. What is the energy of its electron?

Bohr’s model can be used for hydrogen-like ions—ions that have only one electron, such as He+ and Li2+. The ground-state energies of H, He+, and Li2+ are tabulated as follows:

Atom or ion H He+ Li2+

Ground-state energy -2.18 * 10 - 18 J -8.72 * 10 - 18 J -1.96 * 10 - 17 J

a. Does the ground-state energy of the electron in these atoms/ions increase or decrease as the charge of the nucleus increases?

Which of the following explains why the Bohr model is applicable to a He+ ion but not a neutral He atom?

i. The nuclear charge in He+ is the same as that in the H atom.

ii. One electron in the He atom is attracted to the nucleus while the other is repelled from the nucleus, which complicates the model.

iii. The two electrons in the He atom repel one another, which complicates the model.