Does a photon of visible light (λ ≈ 400 to 700 nm) have sufficient energy to excite an electron in a hydrogen atom from the n = 1 to the n = 5 energy state? From the n = 2 to the n = 6 energy state?

For the hydrogen atom, which statement is true   The transition from n = 5 to n = 3 involves greater energy than one from n = 4 to n = 2   A transition from n = 2 to some large value of n corresponds to the ionization energy of the H atom   The transition from n = 4 to n = 2 emits radiation of longer wavelength than the transition from n = 5 to n = 1   All transitions from states for which n > 1 to the n = 1 state involve the absorption of energy by the atom

Ionization energy is defined as the minimum energy required to remove an electron from the ground state (n0) to infinity (n∞). Determine the energy of radiation (in Joules) required to ionize the hydrogen electron from the n = 2 energy level.

What is the energy (in J) of a photon required to excite an electron from n = 2 to n = 5 in a He⁺ ion?

What is the wavelength (in nm) of the photon emitted when the electron in a single-electron lithium atom in an excited state makes the transition from the n=7 state to the n=3 state?

calculate the energy change when an electron in the hydrogen atom transitions from n=3 to n=1.

What is the wavelength of the electromagnetic radiation emitted from a hydrogen atom when the electron undergoes the n=5 transition n=3 to ?

what is the energy of light that must be absorbed by hydrogen atom to transition an electron from n=3 to n=7.

What is the wavelength of light emitted when hydrogen atom had electronic transition from n=4 to n=1

What is the energy, in J, of light that must be absorbed by a hydrogen atom to transition an electron from n = 3 to n = 7? Submit an answer to three signficant figures.