Using the Bohr model, determine the energy in joules of the photon produced when electron in a Het ion moves from the orbit with n = 5 to the orbit with n = 2.

According to the Bohr model for the hydrogen atom, the energy necessary to excite an electron from n = 2 to n = 3 is ________ the energy necessary to excite an electron from n = 3 to n = 4.

What is the maximum number of electrons that all the orbitals with a principle quantum number of 4 could hold? What about a principle quantum number of 5?

Use the graphs of the hydrogen 2s and 2p orbitals (probability density) to explain why the energy of the 2s orbital is lower even though it has a higher expectation value for the radius

Using the Bohr model, determine the energy of an electron with n = 8 in a hydrogen atom.

When a hydrogen atom absorbs a photon of electromagnetic radiation (EMR), the internal energy of the atom increases and one or more electrons may be energized into an excited state. The release of this extra energy as the excited state electron transitions back to a lower energy state results in the emission of a photon. These energy changes are responsible for the emission spectrum of hydrogen (shown below) and are described by the Bohr equation. delta?=−2.178×10−18 J(1?2final−1?2initial)ΔE=−2.178×10−18 J(1nfinal2−1ninitial2) *refer to attached image before proceeding* To ionize a hydrogen atom (forming a hydrogen ion), requires that the energy absorbed is sufficient to send the energized electron an infinite distance away from the nucleus (as shown by the ionization line in the image above). In other words, nfinal is equal to infinity.   Calculate the energy required to ionize a ground state hydrogen atom. Report your answer in kilojoules. delta E= ____kJ   What is the longest…

What are the allowed values of ml quantum number if the n quantum number has a value of 2?

Give the possible values for ml if n=4 and l=2. What type of orbital is associated with these quantum numbers? Howmany orbitals are associated with these quantum numbers?

We enphasized that the Bohr Planetary Model along with the Balmer equation provides precisely correct answers only for hydrogen and other elements, such as Li+2, with only a single electron.  In a single sentence, identify a property in a multi-electron atom that may be responsible for the failure of the Balmer equation to correctly predict the energy of electrons.

Why are there 8 in most electron shells but only two in the first one?