I need help with 2 and 4 Thanks Students should Describe the relationship betwee

Question

I need help with 2 and 4 Thanks Students should Describe the relationship between energy (E), frequency (v) and wavelength (X) of electromagnetic radiations. Calculate either energy (E), frequency (v) or wavelength (lambda), given any one of them. Rank electromagnetic radiations according to energy, frequency and/or wavelength. Calculate. Describe Bohr's Model and calculate energy difference between energy levels in hydrogen atom. Use appropriate quantum numbers in atomic orbitals. Sample quiz/exam questions Arrange the following colors of light in order of increasing energy. violet infrared green blue microwave What is the energy, frequency and wavelength of photons involved in a transition from n = 2 to n = 4 levels in a hydrogen atom? Will photons be absorbed or emitted? Without any calculations, select all transition that will result in emission of photons and then rank these transition according to the wavelength of photons emitted. n = 1 to n = 3 n = 6 to n = 2 n = 10 to n = 100 n = infinity to n = 1000 n = 10 to n = infinity n = 2 to n = 1 When Vernier readings (degree) were plotted on y-axis, and wavelengths of line-spectra (nm) for Hg-Iamp were plotted on x-axis, the best-fit-line equation obtained from Excel was y = 0.204x+ 131.5 Predict where (the Vernier reading) you may find the faint purple line in Hg-lamp, which was very challenging to find in this lab. Which obital (or obitals) has the lowest energy for H atom? How about O atom? 2s 3p 3d 2p

Explanation / Answer

2. a.

E= hv

Where

v =c/lamda

Therefore

E = hc/lamda       

Where E = energy, v= frequency, h= plancks constant, and lamda = wavelength

b.

E= hv

h= E/v

v= E/h

c.

Electromagnetic radiations in the order of decreasing wavelength ( highest to lowest)

Radio waves –highest wavelength, > micro wave> Infra red > Red> violet > UV> X-ray > gamma rays

Electromagnetic radiations in the order of increasing frequency ( lowest to highest)

Frequency = 1/ wavelength ( inversely proportional)

Radio waves –lowest frequency< micro wave< Infra red < Red< violet < UV< X-ray < gamma rays

Electromagnetic radiations in the order of increasing energy ( lowest to highest)

E= hv ( energy is directly proportional to v)

Radio waves –lowest energy< micro wave< Infra red < Red< violet < UV< X-ray < gamma rays

d.

The Rutherford–Bohr model or Bohr model, introduced by Niels Bohr and Ernest Rutherford depicts the atom as a small, positively charged nucleus surrounded by electrons that travel in circular orbits around the nucleus. The postulates of Bohr model of atom are 1)only certain special orbits known as discrete orbits for electrons are allowed inside an atom and 2) while revolving in discrete orbits the electrons do not radiate energy .The model's key success lay in explaining the Rydberg formula for the spectral emission lines of atomic hydrogen.

The electronic transitions between the quantized energy levels of the Bohr atom will give rise to discrete line spectra. For the Balmer series of hydrogen, light is emitted when an electron makes a transition from energy levels with n 3 to the n = 2 energy level. The energy of light emitted corresponds to the energy level difference between the final and initial levels (note that Z=1 for H):

E = E photon = Efinal –E initial = hv photon = hc/   

= { -e4me(1/n2final)} –{--e4me/8 o2h2(1/n2initial)

= - e4me/8 o2h2{1/n2final - 1/n2initial}

Where e, me, o, and h are fundamental constants, this equation expresses the difference between hydrogen atom energy levels in terms of the principal quantum numbers of those levels. This energy level difference corresponds to the energy of the light that is emitted or absorbed when the electron changes its energy.

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