CHEM

posted by .

The electron from a hydrogen atom drops from an excited state into the ground state. When an electron drops into a lower-energy orbital, energy is released in the form of electromagnetic radiation.

Part A: How much energy does the electron have initially in the n=4 excited state?

answer I got = -1.36*10^-19 J

Part B: If the electron from Part A now drops to the ground state, how much energy is released?
Enter your answer numerically in joules.

answer= delta E= _____J

what equation should I use for to answer Part B & how do I plug in to get the correct answer?

  • CHEM -

    How did you get the energy for N = 4? Use the same equation but plug in 1 for N = 1 (that's the ground state). Now subtract the energy in the two states to get the amount (the difference) relesed when the electron falls from n = 4 to n = 1.

  • CHEM -

    I used: E = -(Rhc)/n^2

    R= 1.097*10^7 m^-1
    h= 6.6261*10^-34 J s
    c= 3.00*10^8 m s^-1

    E= -(1.097*10^7)(6.6261*10^-34)(3.00*10^8)/16

    E= -1.36*10^-19 J

    so I just use final minus initial? How so?
    when I do the same as above...but put in 1squared=1, rather than 4squared=16..
    I get: -2.18064951*10^-18

    then should the answer be: -2.18065*10^-18 - -1.36*10^-19? = -2.04*10^-18??

  • CHEM -

    guess it was correct... the real answer, rounded though, came to be: -2.05*10^-18J

    thank you.

  • CHEM -

    Using 2.180 x 10^-18 I found 2.044 x 10^-18 J for the difference in energy levels.

  • CHEM -

    A microwave oven operates at 2.40 . What is the wavelength of the radiation produced by this appliance?

  • CHEM -

    .125m or 125000000nm

  • CHEM -

    Energy is an absolute value, the answer should be 2.05*10^-18J, instead of -2.05*10^-18J.

  • CHEM -

    What is the wavelength lambda of the photon that has been released in Part B?

  • CHEM -

    E=hc/Lambda

    2.05*10^-18=(6.63*10^-34)(3.00*10^8)/x
    x=9.72*10^-8 meters

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. physics

    Please help me answer the question below and also show equations and steps of how you came to your answer. Thank you 1. The electron in a hydrogen tom is in the first excited state, when the electron acquires an additional 2.86eV of …
  2. Physics

    Please help me answer the question below and also show equations and steps of how you came to your answer. Thank you 1. The electron in a hydrogen tom is in the first excited state, when the electron acquires an additional 2.86eV of …
  3. physics

    You are shining ultraviolet light on a gas of an unknown element. You know that an electron starts in a ground state with an energy of -19.10 eV. The electron absorbs a 4.00-eV photon. The electron immediately drops to an intermediate …
  4. chemistry

    The electron from a hydrogen atom drops from an excited state into the ground state. When an electron drops into a lower-energy orbital, energy is released in the form of electromagnetic radiation. Part A: How much energy does the …
  5. Chemistry

    A hydrogen atom electron in an excited state with n = 7 drops to a lower energy state with n = 3. What is the wavelength of the light emitted in this transition
  6. physics

    A monochromatic light beam with energy 204eV is used to excite the Be+3 (H –like atom with Z=4) from its ground state to some excited state m. Neglect the finite nuclear mass correction. a) Find the quantum number m of this excited …
  7. physics

    Hydrogen atom is initially in the ground state. It is excited by a photon bombardment and it then undergoes a transition from n = 3 to n=2 state. a) What is the frequency of the bombarding photon?
  8. Physics

    A hydrogen atom is in its third excited state (n=4). Using Bohr theory of the atom calculate (a) the radius of the orbit, (b) the linear momentum of the electron, (c) the angular momentum of the electron (d) the kinetic energy (e) …
  9. Chemistry

    An electron is excited from the n=1 ground state to the n=3 state in a hydrogen atom. Which of the following statements are true?
  10. Chem

    The brilliant color of fireworks is produced by shells containing lithium carbonate (Li2CO3) that are launched into the night sky and explode. The explosions produce enough energy to vaporize the Li2CO3 and produce excited state lithium …

More Similar Questions