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Mass defect and binding energy
The atomic mass of any other atom is less than the sum of the
masses of the protons, neutrons and electrons present.
Mass defect is a measure of the binding energy of the protons
and neutrons in the nucleus.
The loss in mass and liberation of energy are related by Einstein’s
equation
!E = !mc2
where !E = energy liberated,
!m = loss of mass, and
c = speed of light in a vacuum = 2.998 x 108 m/s
Worked example: Nuclear binding energy
Assuming that the mass defect originates solely from the
interaction of protons and neutrons in the nucleus, estimate the
nuclear binding energy of 73Li given the following data:
Observed atomic mass of 73Li = 7.01600 u
1u = 1.66054 x 10-27 kg
Electron rest mass = 9.10939 x 1031 kg
Proton rest mass = 1.67262 x 1027 kg
Neutron rest mass = 1.67493 x 1027 kg
c = 2.998 x 108 m/s
The actual mass of a 73Li atom
= 7.01600 u x 1.66054 x 1027 kg/u
=1.16503 x 1026 kg
The sum of the masses of the protons, neutrons and electrons in
a 73Li atom
= (3 x 9.10939 x 10-31) + (3 x 1.67262 x 10-27)
+ (4 x 1.67493 x 10-27)
= 1.17203 x 10-26 kg
The difference in mass = !m
= (1.17203 x 10-26 ) - (1.16503 x 10-26 )
= 0.00700 x 10-26 kg
The difference !E = !mc2
= (0.00700 x 10-26 ) x (2.998 x 108)2 kg m2 s-2
= 6.29160 x 10-12 J per atom (J = kg m2 s-2)
This corresponds to 3.79 x 1012 J or 3.79 x 109 kJ per mole of nuclei
3. Estimate the nuclear binding energy of 168O in J per atom,
given that the observed atomic mass is 15.99491 u. Other
data you require are given above.
Exercises:
1. Estimate the nuclear binding energy of 42He given that its
observed atomic mass is 4.002 60 u; other necessary data are
given above.
[Ans. 4:53 x 10-12 J per atom]
2. If the nuclear binding energy of an atom of 94Be is 9.3182 x 10-12 J per atom, calculate the atomic mass of 9
4Be; other
necessary data are given above.
[Ans. 9.012 18 u]
[Ans. 2.045 x 10-11 J per atom]
The average binding energy per nucleon
The average binding energy per nucleon is BE per atom divided
by the sum of protons and neutrons.
For 73Li, binding energy per nucleon
!
=6.29x10
"12
7= 8.98x10
"13J
BE per nucleon values represent the energy released per
nucleon upon the formation of the nucleus from its fundamental
particles.
These values can be used to give a measure of the relative
stabilities of nuclei with respect to decomposition into those
particles.
The nucleus with the greatest
binding energy is 5626Fe and this is
therefore the most stable nucleus.
Nuclei with Z around 60 have the highest
average BE per nucleon.
Variation in average binding energy per nucleon as a function of A.
- stable Fe and Ni are believed to constitute
the bulk of the Earth’s core
Nuclei with A = 4, 12 and 16 have
relatively high BE per nucleon.
Variation in average binding energy per nucleon as a function of A.
- these are used as projectiles in the synthesis
of heavy nuclei
The BE per nucleon decreases
remarkably for A > 100.
Magic Numbers for Nuclear Stability
No. of Protons: 2 8 20 28 50 82 114
No. of Neutrons: 2 8 20 28 50 82 126 184
Distribution of Naturally Occurring Stable Nuclides
Combination Number of Nuclides
Z even - N even 163Z even - N odd 55
Z odd - N even 50
Z odd - N odd 4
Neutron-to-proton ratio and the stability of nuclides
Possible heavy nuclides of high stability
(long radioactive half-lives)
Naturally occurring stable nuclides
(ranging from H to Bi)
Naturally occurring and
artificially made radioactive
nuclides
BE values are important for the application of nuclear reactions as
energy sources.
A reaction involving nuclei will be exothermic if:
. a heavy nucleus is divided into two nuclei of medium mass (so-
called nuclear fission), or
. two light nuclei are combined to give one nucleus of medium
mass (so-called nuclear fusion).
Radioactivity
Nuclear emissions
Nuclear transformations are usually very slow, but even so
spontaneous changes of many heavy nuclides occur.
e.g. 23892U and 232
90Th
3 Types of emission recognized by Rutherford:
1.. Alpha (") decay - involves emission of alpha particles, 42" or
(42He2+)
!
92
238U"
90
234Th+
2
4He + #e.g.
# " decay results in a decrease in the atomic number by 2 units and the
mass number by 4 units.
2. Beta ($#)decay - involves emission of electrons (0-1e or 0
-1!) from
the nucleus (called beta particles).
# " easily captures two electrons; it can be represented as 42He.
e.g.
!
6
14C"
7
14N+#1
0$
$# decay results in an increase in the atomic number by one and leaves
the mass number unchanged.
# a neutron is converted into a proton
3. Gamma (%) emission (high energy X-rays) usually accompanies
other types of nuclear emission.
% emission leaves the atomic number and mass number unchanged.
The decay of some nuclei also involves the emission of other types
of particle:
4. Positron ($+) decay - involves emission of positron (like electron
except that its charge is +)
!
8
15O"
7
15N++1
0#e.g.
$+ decay results in a decrease in the atomic number by one and leaves
the mass number unchanged.
5. Neutrino (&e)- an “electron neutrino” is associated with electron
but is uncharged, possesses near zero mass, accompany
positron emission.
Muon Neutrino (&µ) - associated with muon w/c is a heavier
version (200x in mass) of electron
Two other types of neutrino:
Tau Neutrino (&') - associated with tau w/c is a heavier version
(2500x mass of e-)of electron and muon
The electron, muon and tau, and their corresponding neutrinos
constitute the 6 leptons, which are seen as elementary particles.
The other elementary particles are the 6 “flavors” of quarks:
u (up), d (down), c (charm), s (strange), t (top), b (bottom)
Quarks occur only in combinations of
two quarks : mesons (are bosons; have integer spin;
three quarks: baryons (are fermions; have half-integral
spin)(e.g. proton(uud) and neutron (udd))
five quarks: pentaquarks
6. Antineutrinos - the corresponding antimatter of the neutrinos.
A comparison of the penetrating powers of "-particles, $-
particles, %-radiation and neutrons. Neutrons are especially
penetrating and their use in a nuclear reactor calls for
concrete-wall shields of 2m in thickness.
Nuclear transformations
Many nuclear reactions, as opposed to ordinary chemical
reactions, change the identity of (transmute) the starting
element.
Steps involving the loss of an "- or $-particle may be part of a
decay series.!
92
238U"
90
234Th+
2
4He+
0
0#Examples
!
6
14C"
7
14N+#1
0$
The decay series from 23892U to
20682Pb. Only the last nuclide in
the series, 20682Pb, is stable with
respect to further decay.
Exercise: Three of the nuclides are
not labeled. What are their
identities?