Chem

It is possible to determine the ionization energy for hydrogen using the Bohr equation. Calculate the ionization energy for an atom of hydrogen, making the assumption that ionization is the transition from n=1 to n=infinity.
I don't know how to solve this problem.

A. -2.18 x 10-18 J
B. +2 .18 x 10-18 J
C. +4.59 x 10-18 J
D. -4.59 x 10-18 J
E. +4.36 x 10-18 J

  1. 👍 3
  2. 👎 2
  3. 👁 4,604
  1. 1/wavelength = R(1/1^2 - 0)
    Note: that last term is 1/n^2 but if n = infinity then 1/infinity is zero.
    R = Rydberg constant = 1.0973E7
    Solve for wavelength in meters then E =hc/wavelength to solve for energy in joules. You may want to change that to electron volts.

    1. 👍 2
    2. 👎 0
  2. 1/W(WAVELENGTH)=1.097*10^9[1-0]
    W=9.09*10^-8m
    E=hc/w
    6.63*10^-34*3*10^8/9.09*10^-8
    =2.18*10^-18 J B IS THE ANSWER

    1. 👍 2
    2. 👎 6
  3. It is possible to determine the ionization energy for hydrogen using the Bohr equation. Calculate the ionization energy (in kJ) for a mole of hydrogen atoms, making the assumption that ionization is the transition from n=1 to n= infinity.

    1. 👍 0
    2. 👎 1

Respond to this Question

First Name

Your Response

Similar Questions

  1. chemistry

    calculate the lattice energy of sodium oxide (Na2O) from the following data: Ionization energy of Na(g): 495 kJ/mol Electron affinity of O2 for 2e: 603 kJ/mol Energy to vaporize Na(s): 109 kJ/mol O2(g) bond energy: 499 kJ/mol

  2. chemistry final-urgent

    Choose the element with the highest ionization energy element: Na, Mg, Al, P, S In my book: ionization energy increase from left to right and bottom to top. Na

  3. Chemistry 151

    Of the following transitions in the Bohr hydrogen atom, the ____ transition results in the emission of the highest-energy photon. a.n=1, n=6 b.n=6, n=1 c.n=6,n=3 d.n=3,n=6 e.n=1,n=4

  4. Chemistry

    Calculate the energy change associated with the transition of an electron from the n=2 shell to the n=5 shell in a Bohr hydrogen atom.

  1. Chemistry

    Calculate the maximum wavelength of light capable of removing an electron for a hydrogen atom from the energy state of n=4 if it requires an energy of at least 1.36 x10^-19 J to do this. I just want to know how to find the second

  2. Chemistry

    Suppose that a PES experiment is performed in which mercury vapor is irradiated with ultraviolet light of wavelength 58.4 nm. Energy of a photon of this light is 21.2 eV. Write an equation that shows the process corresponding to

  3. Chemistry!! - bobpursley please

    Calculate the maximum wavelength of light capable of removing an electron for a hydrogen atom from the energy state characterized by the following when n=4 =__________nm Responses Chemistry!! - bobpursley, Wednesday, October 22,

  4. Chemistry

    Which trends are observed when the elements in Period 3 on the Periodic Table are considered in order of increasing atomic number? (1) The atomic radius decreases, and the first ionization energy generally increases. (2) The

  1. chemistry

    What is the difference between the ionization energy of inner-shell electrons and the ionization energy of outer-shell electrons? A. The ionization energy of inner-shell electrons is less than the ionization energy of outer-shell

  2. chemistry

    The following reaction can be written as the sum of two reactions, one of which relates to ionization energy and one of which relates to electron affinity: Li(g)+F(g)→Li+(g)+F−(g) What is the reaction that corresponds to the

  3. chem

    According to the Bohr theory of the hydrogen atom, what is the minimum energy (in J) needed to ionize a hydrogen atom from the n = 2 state?

  4. Chemistry

    When an electron makes a transition from the n=3 to the n=2 hydrogen atom bohr orbit, the energy difference between these two orbits (3.0x10^-19 J) is given off in a photon of light. The relationship ... between the energy of a

You can view more similar questions or ask a new question.