chapter 30 nuclear physics. milestones in the development of nuclear physics 1896 – the birth of...
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Milestones in the Development of Nuclear Physics 1896 – the birth of nuclear physics
Becquerel discovered radioactivity in uranium compounds
Rutherford showed the radiation had three types Alpha (He nucleus) Beta (electrons) Gamma (high-energy photons)
More Milestones 1911 Rutherford, Geiger and
Marsden performed scattering experiments Established the nucleus could be
treated as a point mass and a point charge
Most of the atomic mass was contained in the nucleus
Nuclear force was a new type of force
Some Properties of Nuclei All nuclei are composed of protons and
neutrons Exception is ordinary hydrogen with just a
proton The atomic number, Z, equals the
number of protons in the nucleus Sometimes called the charge number
The neutron number, N, is the number of neutrons in the nucleus
More Properties of Nuclei The mass number, A, is the number of
nucleons in the nucleus A = Z + N Nucleon is a generic term used to refer to
either a proton or a neutron The mass number is not the same as the
mass
Symbolism
X is the chemical symbol of the element Example:
Mass number is 56 Atomic number is 26 Contains 26 protons Contains 30 (56-26) neutrons
The Z may be omitted since the element can be used to determine Z
XAZ
5626Fe
More Properties The nuclei of all atoms of a particular
element must contain the same number of protons
They may contain varying numbers of neutrons Isotopes of an element have the same Z but
differing N and A values The natural abundance of isotopes can vary Example: CCCC 14
6
13
6
12
6
11
6
Charge The proton has a single positive
charge, +e The electron has a single negative
charge, -e The neutron has no charge
Makes it difficult to detect e = 1.60217733 x 10-19 C
Mass It is convenient to use atomic mass
units, u, to express masses 1 u = 1.660539 x 10-27 kg Based on definition that the mass of one
atom of C-12 is exactly 12 u Mass can also be expressed in MeV/c2
From ER = m c2
1 u = 931.494 MeV/c2
The Size of the Nucleus
First investigated by Rutherford in scattering experiments
He found an expression for how close an alpha particle moving toward the nucleus can come before being turned around by the Coulomb force
From Conservation of Energy, the kinetic energy of the particle must be completely converted to potential energy
Size of the Nucleus, cont d is called the distance of closest
approach d gives an upper limit for the size of the
nucleus Rutherford determined that
For gold, he found d = 3.2 x 10-14 m For silver, he found d = 2 x 10-14 m
2
2
4 ek Zed
mv
More About Size Rutherford concluded that the positive
charge of the atom was concentrated in a sphere whose radius was no larger than about 10-14 m He called this sphere the nucleus
These small lengths are often expressed in femtometers where 1 fm = 10-15 m Also called a fermi
Size of Nucleus, Final Since the time of Rutherford, many
other experiments have concluded the following Most nuclei are approximately spherical Average radius is
ro = 1.2 x 10-15 m A is the mass number
31
oArr
Density of Nuclei The volume of the nucleus
(assumed to be spherical) is directly proportional to the total number of nucleons
This suggests that all nuclei have nearly the same density
Since r3 would be proportional to A
Nucleons combine to form a nucleus as though they were tightly packed spheres
Nuclear Stability There are very large repulsive electrostatic
forces between protons These forces should cause the nucleus to fly apart
The nuclei are stable because of the presence of another, short-range force, called the nuclear force This is an attractive force that acts between all
nuclear particles The nuclear attractive force is stronger than the
Coulomb repulsive force at the short ranges within the nucleus
Features of the Nuclear Force Attractive force that acts between all nuclear
particles It is the strongest force in nature Very short range
It falls to zero when the separation between particles exceeds about several fermis
Independent of charge The nuclear force on p-p, p-n, n-n are all the same Does not affect electrons
Nuclear Stability, cont Light nuclei are most
stable if N = Z Heavy nuclei are most
stable when N > Z Above about Z = 20 As the number of protons
increases, the Coulomb force increases and so more neutrons are needed to keep the nucleus stable
No nuclei are stable when Z > 83
Magic Numbers Most stable nuclei have even numbers
of A Certain values of N and Z correspond to
unusually high stability These values are called magic numbers
N or Z = 2, 8, 20, 28, 50, 82, 126 For example, He has N = 2 and Z = 2 and is
very stable
Nuclear Spin Protons and neutrons have intrinsic
angular momentum called spin A nucleus has a net intrinsic angular
momentum that arises from the individual spins of the protons and neutrons
This angular momentum must obey the same quantum rules as orbital angular momentum
Nuclear Angular Momentum The magnitude of the nuclear angular
momentum is due to the combination of all nucleons
It is equal to I is called the nuclear spin quantum
number It may be an integer or half-integer
1I I
Possible Orientations of Nuclear Spin Shown is a vector model
giving possible orientations of the spin and its projection on the z axis
This is for the case where I = 3/2
Nuclear Magneton The nuclear angular momentum has a nuclear
magnetic moment associated with it The magnetic moment is measured in terms of
the nuclear magneton, n
Note that n is smaller than B by a factor of about 2000, due to the difference in mass between the electron and the proton
275.05 102n
p
e JTm
Nuclear Magnetic Moment, final The magnetic moment of a free proton is
2.792 8n No general theory of nuclear magnetism explains
this value The neutron also has a magnetic moment,
even though it has no charge The magnetic moment of the neutron is –
1.913 5n The negative sign indicates the neutron’s magnetic
moment is opposite its spin angular momentum
Nuclear Magnetic Resonance (NMR) Because the direction of the magnetic
moment for a particle is quantized, the energies of the particle are also quantized
The spin vector cannot align exactly with the direction of the magnetic field This gives the extreme values of the
energy as ±zB z is the z component of the magnetic moment
NMR, cont These states are
often called spin states
It is possible to observe transitions between two spin states using NMR
The magnetic field splits the states
NMR, final The sample is irradiated with electromagnetic
waves in the radio range of the em spectrum The frequency of the radio waves is adjusted
so that the photon energy matches the separation energy between spin states
There is a net absorption of energy in the system which is detected by experimental control and measuring systems
MRI An MRI (Magnetic
Resonance Imaging) is based on NMR
Because of variations in an external field, protons in different parts of the body have different splittings in energy between spin states
The resonance signal can provide information about the positions of the protons
Binding Energy The total rest energy of the bound
system (the nucleus) is less than the combined rest energy of the separated nucleons This difference in energy is called the
binding energy of the nucleus It can be thought of as the amount of energy
you need to add to the nucleus to break it apart into its components
Binding Energy, cont The binding energy can be calculated:
The masses are expressed in atomic mass units
M(H) is the atomic mass of the neutral hydrogen atom
mn is the mass of the neutron M(X) is the mass of that isotope
Ab n ZE (MeV) = [ZM(H) + Nm - M ( X)] x 931.494 MeV/u
Notes from the Graph The curve peaks in the vicinity of A = 60
Nuclei with mass numbers greater than or less than 60 are not as strongly bound as those near the middle of the periodic table
The binding energy is about 8 MeV per nucleon for nuclei with A > 50 This suggests that the nuclear force saturates A particular nucleon can interact with only a limited
number of other nucleons
Marie Curie 1867 – 1934 Shared Nobel Prize in
1903 for studies in radioactive substances
Prize in physics Shared with Pierre Curie
and Becquerel Won Noble Prize in
1911 for discovery of radium and polonium
Prize in chemistry
Radioactivity Radioactivity is the spontaneous
emission of radiation Discovered by Becquerel in 1896 Many experiments were conducted by
Becquerel and the Curies Experiments suggested that
radioactivity was the result of the decay, or disintegration, of unstable nuclei
Radioactivity – Types Three types of radiation can be emitted
Alpha particles The particles are 4He nuclei
Beta particles The particles are either electrons or positrons
A positron is the antiparticle of the electron It is similar to the electron except its charge is +e
Gamma rays The “rays” are high energy photons
Distinguishing Types of Radiation
The gamma particles carry no charge
The alpha particles are deflected upward
The beta particles are deflected downward
A positron would be deflected upward, but would follow a different trajectory than the due to its mass
Penetrating Ability of Particles Alpha particles
Barely penetrate a piece of paper Beta particles
Can penetrate a few mm of aluminum Gamma rays
Can penetrate several cm of lead
The Decay Constant The rate at which a decay process occurs is
proportional to the radioactive nuclei present in the sample
λ is called the decay constant and determines the rate at which the material will decay
N is the number of undecayed radioactive nuclei present No is the number of undecayed nuclei at time t=0
to
dNN gives N N e
dt
Decay Rate The decay rate, R, of a sample is
defined as the number of decays per second
Ro = No is the decay rate at t = o The decay rate is often referred to as the
activity of the sample
t to o
dNR N e R e
dt
Decay Curve The decay curve follows
the equation N = No e- λt The half-life is also a
useful parameter The half-life is defined as
the time interval during which half of a given number of radioactive nuclei decay
693.02lnT 21
Decay Processes The blue circles are the stable
nuclei seen before Above the line the nuclei are
neutron rich and undergo beta decay (red)
Just below the line are proton rich nuclei that undergo beta (positron) emission or electron capture (green)
Farther below the line the nuclei are very proton rich and undergo alpha decay (yellow)
Alpha Decay When a nucleus emits an alpha particle
it loses two protons and two neutrons N decreases by 2 Z decreases by 2 A decreases by 4
Symbolically X is called the parent nucleus Y is called the daughter nucleus
HeYX 42
4A2Z
AZ
Decay – General Rules When one element changes into another
element, the process is called spontaneous decay or transmutation
The sum of the mass numbers, A, must be the same on both sides of the equation
The sum of the atomic numbers, Z, must be the same on both sides of the equation
The total energy and total momentum of the system must be conserved in the decay
Disintegration Energy The disintegration energy, Q of a
system is defined as
Q = (Mx – My – M) c2
The disintegration energy appears in the form of kinetic energy in the daughter nucleus and the alpha particle
It is sometimes referred to as the Q value of the nuclear decay
Alpha Decay – Example Decay of 226 Ra
If the parent is at rest before the decay, the total kinetic energy of the products is 4.87 MeV
In general, less massive particles carry off more of the kinetic energy
HeRnRa 42
22286
22688
Alpha Decay, Notes Experimental observations of alpha-particle
energies show a number of discrete energies instead of a single value The daughter nucleus may be left in an excited
quantum state So, not all of the energy is available as kinetic
energy A negative Q value indicates that such a
proposed decay does not occur spontaneously
Alpha Decay, Mechanism In alpha decay, the
alpha particle tunnels through a barrier
For higher energy particles, the barrier is narrower and the probability is higher for tunneling across
This higher probability translates into a shorter half-life of the parent
Beta Decay During beta decay, the daughter nucleus has
the same number of nucleons as the parent, but the atomic number is changed by one
Symbolically
Beta decay is not completely described by these equations
eYX
eYXA1Z
AZ
A1Z
AZ
Beta Decay, cont The emission of the electron or positron
is from the nucleus The nucleus contains protons and neutrons The process occurs when a neutron is
transformed into a proton or a proton changes into a neutron
The electron or positron is created in the process of the decay
Energy must be conserved
Beta Decay – Particle Energy The energy released in
the decay process should almost all go to kinetic energy of the particle
Since the decaying nuclei all have the same rest mass, the Q value should be the same for all decays
Experiments showed a range in the amount of kinetic energy of the emitted particles
Neutrino To account for this “missing” energy and
momentum, in 1930 Pauli proposed the existence of another particle
Enrico Fermi later named this particle the neutrino Properties of the neutrino
Zero electrical charge Mass much smaller than the electron, probably not zero but
less than 2.8 eV/c2
Spin of ½ Very weak interaction with matter and so is difficult to detect
Beta Decay – Completed Symbolically
is the symbol for the neutrino is the symbol for the antineutrino
To summarize, in beta decay, the following pairs of particles are emitted
An electron and an antineutrino A positron and a neutrino
eYX
eYXA1Z
AZ
A1Z
AZ
Beta Decay, Final Notes The fundamental process of e- decay is
a neutron changing into a proton, an electron and an antineutrino
In e+, the proton changes into a neutron, positron and neutrino This can only occur within a nucleus It cannot occur for an isolated proton since
its mass is less than the mass of the neutron
Electron Capture Electron capture is a process that competes
with e+ decay In this case, a parent nucleus captures one of
its own orbital electrons and emits a neutrino:
In most cases, a K shell electron is captured, a process often referred to as K capture
YeX A
1Z
0
1
A
Z
Carbon Dating Beta decay of C-14 is used in dating organic
materials
The process depends on the ratio of C-14 to C-12 in the atmosphere which is relatively constant
When an organism dies, the ratio decreases as a result of the beta decay of the C-14
14 146 7C N e
Enrico Fermi 1901 – 1954 Awarded Nobel Prize in
physics in 1938 for producing transunranic elements and discovery of nuclear reactions produced by slow neutrons
Other contributions include: Theory of beta decay Free electron theory of metals Development of first fission
reactor (1942)
Gamma Decay Gamma rays are given off when an
excited nucleus decays to a lower energy state
The decay occurs by emitting a high-energy photon
The X* indicates a nucleus in an excited state
X*X A
Z
A
Z
Gamma Decay – Example Example of a decay sequence
The first decay is a beta emission The second step is a gamma emission
Gamma emission doesn’t change Z, N, or A The emitted photon has an energy of hƒ equal to
E between the two nuclear energy levels
C*C
e*CB126
126
126
125
Nuclear Reactions Structure of nuclei can be changed by
bombarding them with energetic particles The changes are called nuclear reactions
As with nuclear decays, the atomic numbers and mass numbers must balance on both sides of the equation
Nuclear Reactions, cont A target nucleus, X, is bombarded by a
particle a, resulting in a daughter nucleus Y and an outgoing particle b a + X Y + b
The reaction energy Q is defined as the total change in mass-energy resulting from the reaction Q = (Ma + MX – MY – Mb) c2
Q Values for Reactions The Q value determines the type of reaction
An exothermic reaction There is a mass “loss” in the reaction There is a release of energy Q is positive
An endothermic reaction There is a “gain” of mass in the reaction Energy is needed, in the form of kinetic energy of the incoming
particles Q is negative The minimum energy necessary for the reaction to occur is
called the threshold energy
Nuclear Reactions, final If a and b are identical, so that X and Y
are also necessarily identical, the reaction is called a scattering event If the kinetic energy before the event is the
same as after, it is classified as elastic scattering
If the kinetic energies before and after are not the same, it is an inelastic scattering
Conservation Rules for Nuclear Reactions The following must be conserved in any
nuclear reaction Energy Momentum Total charge Total number of nucleons
Types of Nuclear Reactions One important feature of nuclear
reactions is that much more energy is released than with normal chemical reactions
Two types of reactions can occur Fission Fusion
Nuclear Fission A heavy nucleus splits into two smaller nuclei A fissionable nucleus (X) absorbs a slowly
moving neutron (a) and splits into two smaller nuclei (Y1 and Y2), releasing energy and multiple neutrons (several particles b)
With no means of control, a chain reaction explosion occurs
With controls, the fission process is used in nuclear power generating plants
Nuclear Fusion Nuclear fusion occurs when two light nuclei
combine to form a heavier nucleus This is difficult since the nuclei must
overcome the Coulomb repulsion before they are close enough to fuse One way to do this is to cause them to move with
high kinetic energy by raising them to a high temperature
Also need a high density
Fusion in the Sun The centers of stars have high enough
temperatures and densities to generate energy through fusion
The Sun fuses hydrogen Some stars fuse heavier elements
Reactions in cool stars (T < 15 x 106 K) take place through the proton-proton cycle
In stars with hotter cores (T > 15 x 106 K), the carbon-cycle dominates
Proton-Proton Cycle The proton-proton cycle is a
series of three nuclear reactions believed to operate in the Sun
The net result is the joining of four protons to form a helium-4 nucleus
Energy liberated is primarily in the form of em radiation (gamma rays), positrons and neutrinos
HHHeHeHe
or
eHeHeH
Then
HeHH
eHHH
11
11
42
32
32
42
32
11
32
21
11
21
11
11
The Carbon Cycle Hydrogen nuclei can
fuse into nuclei heavier than helium
Multiple steps lead to the release of energy
The net effect is that four hydrogen nuclei combine to form a helium-4 nucleus
The Carbon-12 is returned at the end, it acts as a catalyst
1 12 131 6 7
13 127 6
1 13 141 6 7
1 14 151 7 8
15 158 7
1 15 12 41 7 6 2
H C N
N C e
H C N
H N O
O N e
H N C He
Energy in a Star Depending on its mass, a star transforms energy at the
rate of 1023 to 1033 W The energy from the core is transferred outward through
the surrounding layers Neutrinos carry energy directly through these layers to space Energy carried by photons is absorbed by the gasses in the
layer outside the core and gradually works it way to the surface by convection
This energy is emitted from the surface in the form of em radiation, mainly infrared, visible and ultraviolet
The star is stable as long as its supply of hydrogen in the core lasts