Question

From the Bohr equation in the introduction, the calculated energy of an electron in the sixth Bohr orbit of a hydrogen atom is

Answer 1

The calculated energy of an electron in the sixth Bohr orbit of a hydrogen atom is approximately -6.048 x 10^-20 J.

Step-by-step explanation:

The energy of an electron in a specific Bohr orbit in a hydrogen atom can be calculated using the Bohr equation, which is given by E = -13.6 eV / n^2, where E is the energy of the electron and n is the principal quantum number of the orbit. Since the question asks for the energy of an electron in the sixth Bohr orbit, we can substitute n = 6 into the equation to get:

E = -13.6 eV / (6^2) = -13.6 eV / 36 = -0.378 eV.

Converting this energy to joules, we use the conversion factor 1 eV = 1.6 x 10^-19 J:

E = -0.378 eV * (1.6 x 10^-19 J / 1 eV) = -6.048 x 10^-20 J.

Answer 2

= - 0.38 eV

Step-by-step explanation:

Using Bohr's equation for the energy of an electron in the nth orbital,

E = -13.6
`(Z^(2) )/(n^(2) )`

Where E = energy level in electron volt (eV)

Z = atomic number of atom

n = principal state

Given that n = 6

⇒ E = -13.6 ×
`(1^(2) )/(6^(2) )`

= - 0.38 eV

Hope this was helpful.