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physics
modern physics

Questions and Answers of Modern Physics

What is the maximum kinetic energy of the electron emitted when a 12B nucleus beta decays into a 12C nucleus?
The kinetic energy of an electron emitted from a 32P nucleus that beta decays into a 32S nucleus is observed to be 1.00 MeV. What is the energy of the accompanying neutrino of the decay process?
Show that the disintegration energy for decay is Q = (mp – mD – me)c2 = (Mp – MD – 2me)c2, where the m’s represent the masses of the parent and daughter nuclei and the M’s represent the
The kinetic energy of a positron emitted from the decay of a 13N nucleus into a 13C nucleus is measured to be 1.190 MeV. What is the energy of the accompanying neutrino of the decay process? Neglect
The expressions for the Q values associated with both β– and β+ decay are given in Exercises 20 and 23. Assume that the daughter’s atomic mass MD is the same in both processes. (a) Use the
(a) Assuming the range of the nuclear force to be 1.0 x 10-15m, predict the mass (in kilograms) of the exchange particle related to this force. (b) Convert the answer into the particle’s rest
(a) In an interaction using the virtual particle model, the range of the interaction (1) increases, (2) remains the same, (3) decreases as energy of the exchange particle increases. Why? (b) If the
By what minimum amount of energy is the energy conservation “violated” during a πo exchange process?
How long is the conservation of energy “violated” in a neutral pi–meson exchange process?
Determine what the daughter nuclei would be in each of the following decays. Can any of these decays occur spontaneously? Explain your reasoning in each case.
(a) What is the mass difference between the charged pion and its neutral version? Express your answer in both kilograms and rest energy (MeV). (b) What would be the kinetic energy of a neutral pion
If the (electron) neutrino mass were 6.0 x 10-6 MeV, what is its speed if its total energy is 0.50 MeV?
(a) Using Table 30.3, determine the mass of the Ω- particle in kilograms. (b) Determine its total energy if it were moving at a speed of 0.800c.
(a) Using Table 30.3, estimate the average distance that a τ- particle would travel in the laboratory if it were traveling at 0.95c. (b) What would its kinetic energy be?
(a) The quark combination for an antiproton is (1) uud, (2) udd, (3) uud, (4) udd. (b) Prove that your answer to part (a) gives the correct electric charge for the antiproton.
(a) The quark combination for a antineutron is (1) udd, (2) uud, (3) uud, (4) ddd. (b) Prove that your answer to part (a) gives the correct electric charge for the antineutron.
(a) Show that the neutral pion cannot be composed solely of any pair of quarks in which one is an up quark (or an anti-up quark) and one is a down quark (or an anti-down quark). (b) According to
Suppose the grand unified theory (GUT) was correct and the half-life of a proton was 1.2 x 1035 y. Estimate the decay rate of a liter of water in decays per second and curies. How does this compare
(a) Referring to Exercise 37, what would be the proton decay constant λ? In exercise Suppose the grand unified theory (GUT) was correct and the half-life of a proton was 1.2 x 1035 y. Estimate the
Referring to Exercise 37, estimate the activity of the Earth’s oceans (in curies) due to proton decay. Assume the oceans are 3 km deep covering 75% of the Earth’s surface. In exercise Suppose the
Find the Q value for 11H + 21H ( 32He + y..
Complete the following nuclear reactions and find their Q values (use Appendix V for masses if necessary):
(a) Write down the equation for the beta decay of 14C. (b) What kind of neutrino and beta particle are emitted? (c) Find the maximum neutrino energy. (d) If the neutrino has half its maximum
Show that the Q value for electron capture (EC) is given by Q = (mp – me – mD)c2 = (Mp – MD)c2, where the m’s represent the masses of the parent and daughter nuclei and the M’s represent
At first glance, it would seem that the unstable 7Be nucleus could decay into a stable 7Li nucleus either by capturing an electron or through β+ decay. (a) From an energy point of view, what should
Determine the Q value and the threshold energy for:
Assume that the average kinetic energy of ions in a plasma is the same as the average kinetic energy of the atoms in an ideal gas. If fusion can begin to occur when the ions approach to within about
If the proton is unstable, GUT theory predicts that its primary mode of decay is into a beta particle and a pion. (a) Write down the only decay possible. (b) If the pro-ton is initially free and at
The main mode of decay for the neutral pion is into two y-rays. (a) Write down the decay equation. (b) If the pion is moving (relative to the laboratory) at 0.90c, and assuming the two -rays are
The predominant mode of decay for the charged pions is into a muon and a neutrino. The positive pion results in the neutrino and the negative pion in the antineutrino. (a) Write the decay equations
One method for detecting of antineutrino is to observe the inverse of positron decay, typically in a detector containing huge amounts of water where protons are readily available. (See, for example,
Uranium-238 undergoes alpha decay as follows:(a) Would you expect the Q value to be (1) positive, (2) negative, or (3) zero? Why? (b) Find the Q value.
Determine the temperature of a sample of ideal gas in which the particles have an average kinetic energy equal to the maximum energy of the protons to be produced by the Large Hadron Collider, that
If two colliding protons in the Large Hadron Collider approached head-on, each with an energy of 7 TeV, what would be the minimum distance of separation between their centers? Compare this to the
For the 7-TeV (kinetic energy) protons produced by the Large Hadron Collider, determine (a) The total energy and (b) The momentum of each proton. (c) By how much (in m/s) does their speed differ
Find the threshold energy for the following reaction:
Find the threshold energy for the following reaction:
Is the given reaction endoergic or exoergic? Prove your answer by determining the Q value.
Is the reaction endoergic or exoergic? Prove your answer. (The reaction on page 1003 gives the mass values.)
The frequency of the strong red line in the spectrum of potassium is 3.91 × 1014/s. What is the wavelength of this light in nanometers?
The element cesium was discovered in 1860 by Robert Bunsen and Gustav Kirchhoff, who found two bright blue lines in the spectrum of a substance isolated from a mineral water. One of the spectral
The following are representative wavelengths in the infrared, ultraviolet, and x-ray regions of the electromagnetic spectrum, respectively: 1.0 × 10–6 m, 1.0 × 10–8 m, and 1.0 × 10–10 m.
Calculate the wavelength of light emitted from the hydrogen atom when the electron undergoes a transition from level n = 3 to level n = 1.
What is the difference in energy levels of the sodium atom if emitted light has a wavelength of 589 nm?
Calculate the wavelength (in picometers) associated with an electron traveling at a speed of 2.19 × 106 m/s.
Explain why each of the following sets of quantum numbers is not permissible for an orbital. a. n = 0, l = 1, ml = 0, ms + 1/2 b. n = 2, l = 3, ml = 0, ms 1/2 c. n = 3, l = 2, ml = +3, ms + 1/2 d.
Laser light of a specific frequency falls on a crystal that converts this light into one with double the original frequency. How is the wavelength of this frequencydoubled light related to the
An atom has a line spectrum consisting of a red line and a blue line. Assume that each line corresponds to a transition between two adjacent energy levels. Sketch an energy-level diagram with three
A proton is approximately 2000 times heavier than an electron. How would the speeds of these particles compare if their corresponding wavelengths were about equal?
Give a brief wave description of light. What are two characteristics of light waves?
Calculate the shortest wavelength of visible light (in nanometers) seen in the spectrum of the hydrogen atom. What are the principal quantum numbers for the levels in this transition? Does Figure
Light of wavelength 1.03 × 10–7 m is emitted when an electron in an excited level of a hydrogen atom undergoes a transition to the n = 1 level. What is the region of the spectrum of this light?
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
The root-mean-square speed of an oxygen molecule, O2, at 21oC is 479 m/s. Calculate the de Broglie wavelength for an O2 molecule traveling at this speed. How does this wavelength compare with the
A particular microwave oven delivers 800 watts. (A watt is a unit of power, which is the joules of energy delivered, or used, per second.) If the oven uses microwave radiation of wavelength 12.2 cm,
For each of the following combinations of quantum numbers, make changes that produce an allowed combination. Count 3 for each change of n, 2 for each change of l, and 1 for each change of ml. What is
The term degeneracy means the number of different quantum states of an atom or molecule having the same energy. For example, the degeneracy of the n = 2 level of the hydrogen atom is 4 (a 2s quantum
The energy required to dissociate the Cl2 molecule to Cl atoms is 239 kJ/mol Cl2. If the dissociation of a Cl2 molecule were accomplished by the absorption of a single photon whose energy was exactly
The energy required to dissociate the H2 molecule to H atoms is 432 kJ/mol H2. If the dissociation of an H2 molecule were accomplished by the absorption of a single photon whose energy was exactly
A microwave oven heats by radiating food with microwave radiation, which is absorbed by the food and converted to heat. Suppose an oven’s radiation wavelength is 12.5 cm. A container with 0.250 L
Explain the process of absorption of light by an atom.
Warm objects emit electromagnetic radiation in the infrared region. Heat lamps employ this principle to generate infrared radiation. Water absorbs infrared radiation with wavelengths near 2.80 µm.
Light with a wavelength of 425 nm fell on a potassium surface, and electrons were ejected at a speed of 4.88 × 105 m/s. What energy was expended in removing an electron from the metal? Express the
Light with a wavelength of 405 nm fell on a strontium surface, and electrons were ejected. If the speed of an ejected electron is 3.36 × 105 m/s, what energy was expended in removing the electron
When an electron is accelerated by a voltage difference, the kinetic energy acquired by the electron equals the voltage times the charge on the electron. Thus, one volt imparts a kinetic energy of
When an electron is accelerated by a voltage difference, the kinetic energy acquired by the electron equals the voltage times the charge on the electron. Thus, one volt imparts a kinetic energy of
The atom is sometimes said to be similar to a miniature planetary system, with electrons orbiting the nucleus. What does the uncertainty principle have to say about this view of the atom?
Bohr described the hydrogen atom as an electron orbiting a hydrogen nucleus. Although certain aspects of his theory are still valid, his theory agreed quantitatively with experiment only in the case
Give the possible values of (a) the principal quantum number, (b) the angular momentum quantum number, (c) the magnetic quantum number, and (d) the spin quantum number.
Light, Energy, and the Hydrogen Atoma. Which has the greater wavelength, blue light or red light?b. How do the frequencies of blue light and red light compare?c. How does the energy of blue light
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 R = RH/n3 where RH is
Consider two beams of the same yellow light. Imagine that one beam has its wavelength doubled; the other has its frequency doubled. Which of these two beams is then in the ultraviolet region?
Some infrared radiation has a wavelength that is 1000 times larger than that of a certain visible light. This visible light has a frequency that is 1000 times smaller than that of some X radiation.
One photon of green light has less than twice the energy of two photons of red light. Consider two hypothetical experiments. In one experiment, potassium metal is exposed to one photon of green
An atom in its ground state absorbs a photon (photon 1), then quickly emits another photon (photon 2). One of these photons corresponds to ultraviolet radiation, whereas the other one corresponds to
Three emission lines involving three energy levels in an atom occur at wavelengths x, 1.5x, and 3.0x nanometers. Which wavelength corresponds to the transition from the highest to the lowest of the
Briefly describe the portions of the electromagnetic spectrum, starting with shortest wavelengths and going to longer wavelengths.
An atom emits yellow light when an electron makes the transition from the n = 5 to the n = 1 level. In separate experiments, suppose you bombarded the n = 1 level of this atom with red light, yellow
Which of the following particles has the longest wavelength? a. An electron traveling at x meters per second b. A proton traveling at x meters per second c. A proton traveling at 2x meters per second
Imagine a world in which the rule for the l quantum number is that values start with 1 and go up to n. The rules for the n and ml quantum numbers are unchanged from those of our world. Write the
Given the following energy level diagram for an atom that contains an electron in the n = 3 level, answer the following questions. a. Which transition of the electron will emit light of the lowest
The following shapes each represent an orbital of an atom in a hypothetical universe. The small circle is the location of the nucleus in each orbital.a. If you placed an electron in each orbital,
Radio waves in the AM region have frequencies in the range 530 to 1700 kilocycles per second (530 to 1700 kHz). Calculate the wavelength corresponding to a radio wave of frequency 1.365 × 106/s
Microwaves have frequencies in the range 109 to 1012/s (cycles per second), equivalent to between 1 gigahertz and 1 terahertz. What is the wavelength of microwave radiation whose frequency is 1.258 =
Light with a wavelength of 478 nm lies in the blue region of the visible spectrum. Calculate the frequency of this light.
Calculate the frequency associated with light of wavelength 656 nm. (This corresponds to one of the wavelengths of light emitted by the hydrogen atom.)
At its closest approach, Mars is 56 million km from Earth. How long would it take to send a radio message from a space probe of Mars to Earth when the planets are at this closest distance?
Planck originated the idea that energies can be quantized. What does the term quantized mean? What was Planck trying to explain when he was led to the concept of quantization of energy? Give the
The space probe Pioneer 11 was launched April 5, 1973, and reached Jupiter in December 1974, traveling a distance of 998 million km. How long did it take an electromagnetic signal to travel to Earth
The meter was defined in 1963 as the length equal to 1,650,763.73 wavelengths of the orange-red radiation emitted by the krypton-86 atom (the meter has since been redefined). What is the wavelength
The second is defined as the time it takes for 9,192,631,770 wavelengths of a certain transition of the cesium-133 atom to pass a fixed point. What is the frequency of this electromagnetic radiation?
What is the energy of a photon corresponding to radio waves of frequency 1.365 × 106/s?
What is the energy of a photon corresponding to microwave radiation of frequency 1.258 × 1010/s?
The green line in the atomic spectrum of thallium has a wavelength of 535 nm. Calculate the energy of a photon of this light.
Indium compounds give a blue-violet flame test. The atomic emission responsible for this blue-violet color has a wavelength of 451 nm. Obtain the energy of a single photon of this wavelength.
A particular transition of the rubidium atom emits light whose frequency is 3.84 × 1014 Hz. (Hz is the abbreviation for hertz, which is equivalent to the unit /s, or s–1.) Is this light in the
Barium atoms have a particular transition that emits light of frequency 5.41 × 1014 Hz. (Hz is the abbreviation for hertz, which is equivalent to the unit /s, or s1.) Is this light in the visible
An electron in a hydrogen atom in the level n × 5 undergoes a transition to level n × 3. What is the frequency of the emitted radiation?
In your own words, explain the photoelectric effect. How does the photon concept explain this effect?
Calculate the frequency of electromagnetic radiation emitted by the hydrogen atom in the electron transition from n = 4 to n = 3.

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