Interpretation:
The
Concept introduction:
Wavelength is the separation between two progressive crests or troughs.
The energy of a photon can be expressed as
Here,
The emission energy of photon (E) when it moves from the first excited state to ground state can be calculated as
The relationship between meter and nanometer can be expressed as:
To convert meter to nanometer, conversion factor is
The relationship between number of moles and number of atoms can be expressed as
To convert number of atoms to number of moles, conversion factor is
The relationship between kilojoules and joules can be expressed as
To convert kilojoules to joules, conversion factor is
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Chemistry
- It requires 799 kJ of energy to break one mole of carbon-oxygen double bonds in carbon dioxide. What wavelength of light does this correspond to per bond? Is there any transition in the hydrogen atom that has at least this quantity of energy to one photon?arrow_forward6.96 When a helium atom absorbs light at 58.44 nm, an electron is promoted from the 1s orbital to a 2p orbital. Given that the ionization energy of (ground state) helium is 2372 kJ/ mol, find the longest wavelength of light that could eject an electron from the excited state helium atom.arrow_forwardHow many electrons in an atom can have the following quantum designation? (a) 1s (b) 4d, m l =0(c) n=5,l=2arrow_forward
- Investigating Energy Levels Consider the hypothetical atom X that has one electron like the H atom but has different energy levels. The energies of an electron in an X atom are described by the equation E=RHn3 where RH is the same as for hydrogen (2.179 1018 J). Answer the following questions, without calculating energy values. a How would the ground-state energy levels of X and H compare? b Would the energy of an electron in the n = 2 level of H be higher or lower than that of an electron in the n = 2 level of X? Explain your answer. c How do the spacings of the energy levels of X and H compare? d Which would involve the emission of a higher frequency of light, the transition of an electron in an H atom from the n = 5 to the n = 3 level or a similar transition in an X atom? e Which atom, X or H, would require more energy to completely remove its electron? f A photon corresponding to a particular frequency of blue light produces a transition from the n = 2 to the n = 5 level of a hydrogen atom. Could this photon produce the same transition (n = 12 to n = 5) in an atom of X? Explain.arrow_forwardGive the maximum number of electrons in an atom that can have these quantum numbers: a. n = 4 b. n = 5, ml = + l c. n = 5,ms = +12 d. n = 3, l = 2 e. n = 2, l = 1arrow_forwardWhat is the maximum number of electrons that can be identified with each of the following sets of quantum numbers? In some cases, the answer may be none In such cases, explain why none is the correct answer. (a) n = 4, = 3, m = 1 (b) n = 6, = 1, m = 1, ms = 1/2 (c) n= 3, = 3, m = 3arrow_forward
- According to a relationship developed by Niels Bohr, for an atom or ion that has a single electron, the total energy, En, of an electron in a stable orbit of quantum number n is En = [Z2/n2] (2.179 1018 J) where Z is the atomic number. Calculate the ionization energy for the electron in a ground-state He+ ion.arrow_forwardAn energy of 3.3 1019 J/atom is required to cause a cesium atom on a metal surface to lose an electron. Calculate the longest possible wavelength of light that can ionize a cesium atom. In what region of the electromagnetic spectrum is that radiation found?arrow_forward
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