Question

In: Physics

How much higher in energy is this electron with respect to the ground state of H

 

Part A

Suppose an electron is in the n=6 energy level of a H atom.

How much higher in energy is this electron with respect to the ground state of H

Part B

 How much additional energy is required to just remove this excited electron from the H atom?

Solutions

Expert Solution

1) according bore's formula for energy

E =RH[(1/ni2) - (1/nf2)]

here RH is constant =2.179 x10-18 J

ni =intial level =1 and nf =final level =6

  E =(2.179 x10-18 J )[(1/1) -(1/36)] = 2.1185 x10-18 J =2.1185 x10-18 x(6.241509·1018 eV) =13.22 eV

energy difference is 13.22 eV

2)additional energy required to remove the electron is ionization energy

  E =-Z2RH (1/n2)

here Z= atomic number of hydrogen =1 and n=6

   E =-2.179 x10-18 J (1/36) =6.0528 x10-20 J =6.0528 x10-20 x6.241509·1018 eV) =0.38 eV


Related Solutions

You have .900 mol of H atoms in the ground state. How much energy is required...
You have .900 mol of H atoms in the ground state. How much energy is required to transition all of the atoms from the ground state to n=4
The hydrogen atom electron is in the ground state. The electron absorbs energy and makes a...
The hydrogen atom electron is in the ground state. The electron absorbs energy and makes a transition to the n=3 state. Then it returns to the ground state by emitting two photons when going to n=2 and then n=1 states. A. What are the wavelengths of these photons? B. What will be the wavelength if only one photon is emitted? C. What is the maximum number of electrons with ml=3 in the shell with n=5? D. How many electrons with...
The ground state energy of an oscillating electron is 1.24 eV
The ground state energy of an oscillating electron is 1.24 eV. How much energy must be added to the electron to move it to the second excited state? The fourth excited state?
An electron is in the ground state of an infinite square well. The energy of the...
An electron is in the ground state of an infinite square well. The energy of the ground state is E1 = 1.35 eV. (a) What wavelength of electromagnetic radiation would be needed to excite the electron to the n = 4 state? nm (b) What is the width of the square well? nm
An electron at ground state, absorbs the energy of a photon that has a frequency of...
An electron at ground state, absorbs the energy of a photon that has a frequency of 3.1573 x 1015/s, and jumps to the higher level. The same electron makes two more consecutive jumps. First, the electron jumps to another energy level by emitting a photon with a wavelength of 434.1 nm. This electron jumps immediately to the third energy level. Find the energy and the frequency of the photon which are the result of the third jump
The binding energy of an electron in the ground state in a hydrogen atom is about:...
The binding energy of an electron in the ground state in a hydrogen atom is about: A. 13.6 eV B. 3.4 eV C. 10.2 eV D. 1.0 eV E. 27.2 eV
A hydrogen electron in the ground state absorbs a 92.3157 nm photon to reach a higher...
A hydrogen electron in the ground state absorbs a 92.3157 nm photon to reach a higher excited state (a), and then emits two photons, one with 1.75777 x 10^-20 J of energy to reach an intermediate state (b), and one with wavelength 1005.22nm as it falls back to a lower excited state (c). Determine the three energy levels (a,b,c) of this particular electron.
Consider a hydrogen atom in the ground state. What is the energy of its electron? E=...
Consider a hydrogen atom in the ground state. What is the energy of its electron? E= J Consider a hydrogen atom in an excited state of 2s^1. What is the energy of its electron? E= J
Calculate the energy (in kJ/mol) required to remove the electron in the ground state for each...
Calculate the energy (in kJ/mol) required to remove the electron in the ground state for each of the following one-electron species using the Bohr model. (The Rydberg constant for hydrogen is approximately ?2.178 ? 10?18 J.) (a) H = ? kJ/mol (b) B^4+ = ? kJ/mol (c) Li^2+ = ? kJ/mol (d) Mn^24+ = ? kJ/mol
How much energy would be needed to remove three electrons from a ground state beryllium atom?
The following are all ionization energies for beryllium.     1st Ionization     2nd Ionization     3rd Ionization     4th IonizationEnergy (kJ/mol)89917571484521000How much energy would be needed to remove three electrons from a ground state beryllium atom?
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT