Question

Using the Bohr model, determine the energy, in joules, necessary to ionize a ground-state hydrogen atom. Show your calculations.

a) −2.18×10−18−2.18×10−18 J
b) −1.31×10−18−1.31×10−18 J
c) −8.21×10−19−8.21×10−19 J
d) −5.45×10−19−5.45×10−19 J

Answer 1

The energy necessary to ionize a ground-state hydrogen atom using the Bohr model is -2.18 x 10-18 J.

Step-by-step explanation:

The energy necessary to ionize a ground-state hydrogen atom can be determined using the Bohr model.

The formula to calculate the energy required to ionize an atom is:

Energy = Rydberg constant *(1/n^2 - 1/n^2)

where the Rydberg constant is -2.18 x 10-18 J and n is the principal quantum number for the orbit.

For a hydrogen atom, the ground state has n = 1. Substituting the values into the formula gives:

Energy = (-2.18 x 10-18 J) * (1/1^2 - 1/∞^2)

which simplifies to:

Energy = (-2.18 x 10-18 J) * (1 - 0)

Energy = (-2.18 x 10-18 J)

Therefore, the energy necessary to ionize a ground-state hydrogen atom is -2.18 x 10-18 J.