We use cookies to give you the best experience possible. By continuing we’ll assume you’re on board with our cookie policy

Solved Problems on the Particle Nature of Matter Essay Sample

  • Pages: 5
  • Word count: 1,334
  • Rewriting Possibility: 99% (excellent)
  • Category: atomic

Get Full Essay

Get access to this section to get all help you need with your essay and educational issues.

Get Access

Introduction of TOPIC

Charles Asman, Adam Monahan and Malcolm McMillan Department of Physics and Astronomy University of British Columbia, Vancouver, British Columbia, Canada Fall 1999; revised 2011 by Malcolm McMillan Given here are solutions to 5 problems on the particle nature of matter. The solutions were used as a learning-tool for students in the introductory undergraduate course Physics 200 Relativity and Quanta given by Malcolm McMillan at UBC during the 1998 and 1999 Winter Sessions. The solutions were prepared in collaboration with Charles Asman and Adam Monaham who were graduate students in the Department of Physics at the time. The problems are from Chapter 3 The Particle Nature of Matter of the course text Modern Physics by Raymond A. Serway, Clement J. Moses and Curt A. Moyer, Saunders College Publishing, 2nd ed., (1997).

Coulomb’s Constant and the Elementary Charge When solving numerical problems on the particle nature of matter it is useful to note that the product of Coulomb’s constant k = 8.9876 × 109 m2 / C2 (1) and the square of the elementary charge e = 1.6022 × 10−19 C is ke2 = 1.4400 eV nm = 1.4400 keV pm = 1.4400 MeV fm where eV = 1.6022 × 10−19 J (4) (3) (2)

Breakdown of the Rutherford Scattering Formula: Radius of a Nucleus Problem 3.9, page 39 It is observed that α particles with kinetic energies of 13.9 MeV or higher, incident on copper foils, do not −4 obey Rutherford’s (sin φ/2) scattering formula. • Use this observation to estimate the radius of the nucleus of a copper atom. Assume that the nucleus remains fixed in a head-on collision with an α particle. Solution Rutherford’s (sin φ/2) scattering formula governs the scattering of an α particle by an atomic nucleus when the interaction between the α particle and the nucleus is due entirely to the Coulomb force. −4

At the distance d of closest approach in a head-on collision, the kinetic energy of the α particle is zero and therefore, by conservation of energy, the incident kinetic energy K of the α particle is equal to the potential energy of the system: k(Ze)(2e) K= (5) d where Z is the atomic number of the nucleus. Rutherford’s formula breaks down when the α particle is close enough to the nucleus to be influenced by the strong nuclear force. The distance d calculated with the lowest kinetic energy K at which the Rutherford’s formula breaks down is an estimate of the radius of the nucleus. For copper, Z = 29 and K = 13.9 MeV, so d = 6.00 fm. The value of the radius calculated using 1.3A1/3 fm with A = 64 is 5.2 fm.

Bohr’s Model of the Atom: Radii and Speeds Problem 3.14, page 39 • Use text Eq. (3.35): rn = a0 n2 52.9n2 n = = pm me ke2 Z Z Z 2 2 to calculate the radius of the first, second and third Bohr orbits of hydrogen; a0 = 2 /(me ke2 ) = 52.9 pm is the Bohr radius of hydrogen. That is, a0 = r1 when Z = 1. • Determine the electron’s speed in the same three orbits. Is a relativistic correction necessary? Explain. Solution Eq. (6) gives the radius rn of the nth Bohr orbit of a single electron orbiting a fixed nucleus of c

harge +Ze. For hydrogen (Z = 1), Eq. (6) yields r1 r2 r3 It follows using text Eq. (3.24): me vr = n

Sorry, but full essay samples are available only for registered users

Choose a Membership Plan
that the speed vn of an electron in the nth Bohr orbit is vn = so v1 v2 v3 = = = 7.30 × 10−3 c 3.65 × 10−3 c 2.43 × 10−3 c (12) (13) (14) nme a0 = 7.30 × 10−3 c n (11) (10) = = = 52.9 pm 212 pm 476 pm (7) (8) (9)

These speeds are all very much less than c so relativistic corrections are small. Energy corrections are of the order of µeV.

Bohr’s Model of the Atom: Photon Emission Problem 3.24, page 140

A hydrogen atom originally at rest in the n = 3 state decays to the ground state with the emission of a photon. • Calculate the wavelength of the emitted photon. • Estimate the recoil momentum of the atom. Where does this energy come from? Solution Text Eq. (3.33): 1 =R λ where R= 1 1 2 − n2 nf i (15)

ke2 = 1.0973 × 107 m−1 = 1/91.13 nm 2a0 hc gives the wavelength λ of the photon emitted when a hydrogen atom initially at rest in the ni state decays to the nf state. It follows that in the decay from n = 3 state to the ground state (n = 1), the wavelength λ of the emitted photon is 9 = 103 nm. (17) λ= 8R The energy E and magnitude p of the momentum of the emitted photon are E= p= hc = 12.0 eV λ (18)

E = 12.0 eV/c. (19) c Momentum is conserved in the process and therefore p is also the magnitude of the momentum of the recoiling hydrogen atom. The kinetic energy K of the recoiling hydrogen atom is K= p2 = 77.2 neV. 2mH (20)

Eq. (17) assumes that all the transition energy is carried off by the photon and that K = 0. Comparison of Eqs. (18) and (20) shows that this is a reasonable assumption.

Bohr’s Model of the Atom: Muonic Atom Problem 3.33, page 141 A muon is a particle with a charge equal to that of an electron and a mass equal to 207 times the mass of the electron. Muonic lead is formed when 208 Pb captures a muon to replace an electron. Assume that the muon moves in such a small orbit that it sees a nuclear charge Z=82. • According to Bohr’s theory, what are the radius and energy of the ground state of muonic lead? Use the concept of reduced mass in solving the problem. Solution Eq. (6) gives the radius of the nth Bohr orbit and text Eq. (3.36): En = − ke2 2a0 Z2 n2 =− 13.58Z 2 n2 eV (21)

gives the energy of the nth Bohr level for a single electron orbiting a fixed nucleus of charge +Ze.

The model may be extended further when the electron is replaced by a particle of mass m and charge e. In this case, Eqs. (6) and (21) are replaced by rn = me µ µ me µ= 52.9n2 Z 13.58Z 2 n2 mmN m + mN pm (22)

En = − where




where mN is the mass of the nucleus; µ is the reduced mass of the orbiting particle and the nucleus. A negative muon has charge e and mass m = 207me . Muonic lead is formed when 208 Pb captures a negative muon to replace an electron. Assuming that the muon moves in such a small orbit that it only feels a positive charge corresponding to Z = 82 (i.e., that screening effects caused by the other electrons surrounding the nucleus are negligible), then Eqs. (22) and (23) with n = 1 give the radius r1 and ground state energy E1 of the ground state of muonic lead according to Bohr theory: r1 = 3.1 fm E1 = −19 MeV. Nuclear physics studies indicate that the nuclear radius rnucleus is given approximately by rnucleus = 1.3 A 3 fm = 7.7 fm when A = 207. 1

(25) (26)


The Bohr model prediction (Eq. (25)) is of the right order of magnitude but too small; the assumption that the muon feels a positive charge corresponding to Z = 82 is incorrect. The radius r of the ground state of muonic lead is equal to the nuclear radius R when the effective charge in the Bohr model corresponds to Z = 33. The calculations indicate that muonic atoms can be used to probe the atomic nucleus.

Bohr’s Model of the Atom: Positronium Problem 3.35, page 141 Positronium is a hydrogen-like atom consisting of a positron (a positively charged electron) and an electron revolving around each other. • Using the Bohr model, find the allowed radii (relative to the center of mass of the two particles) and the allowed energies of the system. Use the concept of reduced mass in solving the problem. Solution Eqs. (22) and (23) with m = mN = me and Z = 1 give the Bohr model values for the allowed radii rn and energies En of positronium: rn = 105.8n2 pm (28) En = − 6.79 eV n2 (29)

We can write a custom essay on

Solved Problems on the Particle Nature of Matter E ...
According to Your Specific Requirements.

Order an essay

You May Also Find These Documents Helpful

The History of the Atom

Over the span of hundreds of years science has advanced tremendously improving our understanding of what makes up the world we live in. The atom is one of sciences important findings and has had a changing history of new discoveries, always altering the way we see things. In the early 1800s a man called John Dalton made an atomic theory with predictions about atoms. He stated that atoms are tiny particles that make up elements and that they are indivisible. We now know that there are in fact smaller particles inside the atom, but at this stage it was assumed that the atom was the smallest. He also said that all atoms of a given element are the same and atoms of one element are different from those in every other element. This meant that every different element had its own unique type of atoms. (Dalton also developed the first...

The Decision to Drop the Atomic Bomb...

            Public opinion is still divided over the reasons and the necessity to utilize the newly developed atomic bomb against Japan at the close of World War II.  The reason provided at the time was that it would save over one million lives, many of which would be Americans.  Using that reasoning as a standalone argument is simplistic.  While it is true that there was some military justification for ending the war as soon as possible, there were other non-military reasons to deploy the weapons.  The decision to deploy atomic weapons against Japan was affected by military, economic, racial, and political arguments.             Research into the fissionable material started in the 1930’s.  Two Germans scientists, Hahn and Strassmann, succeeded in splitting the nucleus of a uranium atom in Berlin.  News off this success arrived in the United States in the form of a lecture given by Nobel Laureate Niels Bohr. ...

Atomic Radius and Atomic Structure

1-Describe the periodic trend in atomic radius and relate it to atomic structure 2- Describe the periodic trend in electronegativity and relate it to atomic structure Did you know? There are atoms with no electronegativity because electro negativity refers to the attraction of atoms of electrons in a compound; elements that do not form are assigned no electronegativity values. Atomic Radius ≠ Ionization Energy As you move from left to right on the periodic table, the number of valance electron increase. As the number of E increases P increases. As positive force increases, the electron get tighter and the radius gets smaller. Ionization energy is the energy required to remove an electron. As you move up and down the periodic table, the number of electron shells changes. As the number of shells increases, there is more shielding between the nucleuses the outermost electron increases. Atomic Radius: is half the distances...

Popular Essays


Emma Taylor


Hi there!
Would you like to get such a paper?
How about getting a customized one?