Consider the Bohr model for the hydrogen atom. $\left( c = 3.00 \times 10 ^ { 8 } \mathrm {~m} / \mathrm { s } , 1 \mathrm { eV } = 1.60 \times 10 ^ { - 19 } \mathrm {~J} \right.$, $\left. h = 6.626 \times 10 ^ { - 34 } \mathrm {~J} \cdot \mathrm { s } \right)$
(a) How much energy (in eV) is needed to cause a transition of an electron from the second excited state to the third excited state?
(b) What wavelength photon just has enough energy to initiate the transition in (a)?

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The Answer of Consider the Bohr model for the hydrogen atom. $\left( c = 3.00 \times 10 ^ { 8 } \mathrm {~m} / \mathrm { s } , 1 \mathrm { eV } = 1.60 \times 10 ^ { - 19 } \mathrm {~J} \right.$, $\left. h = 6.626 \times 10 ^ { - 34 } \mathrm {~J} \cdot \mathrm { s } \right)$
(a) How much energy (in eV) is needed to cause a transition of an electron from the second excited state to the third excited state?
(b) What wavelength photon just has enough energy to initiate the transition in (a)?

Consider the Bohr Model for the Hydrogen Atom (c=3.00×108 m/s,1eV=1.60×10−19 J\left( c = 3.00 \times 10 ^ { 8 } \mathrm {~m} / \mathrm { s } , 1 \mathrm { eV } = 1.60 \times 10 ^ { - 19 } \mathrm {~J} \right.(c=3.00×108 m/s,1eV=1.60×10−19 J

Consider the Bohr Model for the Hydrogen Atom $\left( c = 3.00 \times 10 ^ { 8 } \mathrm {~m} / \mathrm { s } , 1 \mathrm { eV } = 1.60 \times 10 ^ { - 19 } \mathrm {~J} \right.$