Nuclei
13.1 INTRODUCTION
In the previous chapter, we have learnt that in every atom, the positive charge and mass are densely concentrated at the centre of the atom forming its nucleus. The overall dimensions of a nucleus are much smaller than those of an atom. Experiments on scattering of $\alpha$-particles demonstrated that the radius of a nucleus was smaller than the radius of an atom by a factor of about $10^{4}$. This means the volume of a nucleus is about $10^{-12}$ times the volume of the atom. In other words, an atom is almost empty. If an atom is enlarged to the size of a classroom, the nucleus would be of the size of pinhead. Nevertheless, the nucleus contains most (more than 99.9%) of the mass of an atom.
Does the nucleus have a structure, just as the atom does? If so, what are the constituents of the nucleus? How are these held together? In this chapter, we shall look for answers to such questions. We shall discuss various properties of nuclei such as their size, mass and stability, and also associated nuclear phenomena such as radioactivity, fission and fusion.
13.2 ATOMIC MASSES AND COMPOSITION OF NUCLEUS
The mass of an atom is very small, compared to a kilogram; for example, the mass of a carbon atom, $ ^{12} \mathrm{C}$, is $1.992647 \times 10^{-26} \mathrm{~kg}$. Kilogram is not a very convenient unit to measure such small quantities. Therefore, a different mass unit is used for expressing atomic masses. This unit is the atomic mass unit $(\mathrm{u})$, defined as $1 / 12^{\mathrm{th}}$ of the mass of the carbon $( ^{12} \mathrm{C})$ atom. According to this definition
$$ \begin{align*} 1 \mathrm{u} & =\frac{\text { mass of one } ^{12} \mathrm{C} \text { atom }}{12} \\ & =\frac{1.992647 \times 10^{-26} \mathrm{~kg}}{12} \\ & =1.660539 \times 10^{-27} \mathrm{~kg} \tag{13.1} \end{align*} $$
The atomic masses of various elements expressed in atomic mass unit $(\mathrm{u})$ are close to being integral multiples of the mass of a hydrogen atom. There are, however, many striking exceptions to this rule. For example, the atomic mass of chlorine atom is $35.46 \mathrm{u}$.
Accurate measurement of atomic masses is carried out with a mass spectrometer, The measurement of atomic masses reveals the existence of different types of atoms of the same element, which exhibit the same chemical properties, but differ in mass. Such atomic species of the same element differing in mass are called isotopes. (In Greek, isotope means the same place, i.e. they occur in the same place in the periodic table of elements.) It was found that practically every element consists of a mixture of several isotopes. The relative abundance of different isotopes differs from element to element. Chlorine, for example, has two isotopes having masses $34.98 \mathrm{u}$ and $36.98 \mathrm{u}$, which are nearly integral multiples of the mass of a hydrogen atom. The relative abundances of these isotopes are 75.4 and 24.6 per cent, respectively. Thus, the average mass of a chlorine atom is obtained by the weighted average of the masses of the two isotopes, which works out to be
$$ \begin{aligned} & =\frac{75.4 \times 34.98+24.6 \times 36.98}{100} \\ & =35.47 \mathrm{u} \end{aligned} $$
which agrees with the atomic mass of chlorine.
Even the lightest element, hydrogen has three isotopes having masses $1.0078 \mathrm{u}, 2.0141 \mathrm{u}$, and $3.0160 \mathrm{u}$. The nucleus of the lightest atom of hydrogen, which has a relative abundance of $99.985 %$, is called the proton. The mass of a proton is
$$ \begin{equation*} m_{p}=1.00727 \mathrm{u}=1.67262 \times 10^{-27} \mathrm{~kg} \tag{13.2} \end{equation*} $$
This is equal to the mass of the hydrogen atom $(=1.00783 \mathrm{u})$, minus the mass of a single electron $(m_{e}=0.00055 \mathrm{u})$. The other two isotopes of hydrogen are called deuterium and tritium. Tritium nuclei, being unstable, do not occur naturally and are produced artificially in laboratories.
The positive charge in the nucleus is that of the protons. A proton carries one unit of fundamental charge and is stable. It was earlier thought that the nucleus may contain electrons, but this was ruled out later using arguments based on quantum theory. All the electrons of an atom are outside the nucleus. We know that the number of these electrons outside the nucleus of the atom is $Z$, the atomic number. The total charge of the atomic electrons is thus $(-Z e)$, and since the atom is neutral, the charge of the nucleus is $(+Z e)$. The number of protons in the nucleus of the atom is, therefore, exactly $Z$, the atomic number.
DISCOVERY OF NEUTRON
Since the nuclei of deuterium and tritium are isotopes of hydrogen, they must contain only one proton each. But the masses of the nuclei of hydrogen, deuterium and tritium are in the ratio of 1:2:3. Therefore, the nuclei of deuterium and tritium must contain, in addition to a proton, some neutral matter. The amount of neutral matter present in the nuclei of these isotopes, expressed in units of mass of a proton, is approximately equal to one and two, respectively. This fact indicates that the nuclei of atoms contain, in addition to protons, neutral matter in multiples of a basic unit. This hypothesis was verified in 1932 by James Chadwick who observed emission of neutral radiation when beryllium nuclei were bombarded with alpha-particles ( $\alpha$-particles are helium nuclei, to be discussed in a later section). It was found that this neutral radiation could knock out protons from light nuclei such as those of helium, carbon and nitrogen. The only neutral radiation known at that time was photons (electromagnetic radiation). Application of the principles of conservation of energy and momentum showed that if the neutral radiation consisted of photons, the energy of photons would have to be much higher than is available from the bombardment of beryllium nuclei with $\alpha$-particles. The clue to this puzzle, which Chadwick satisfactorily solved, was to assume that the neutral radiation consists of a new type of neutral particles called neutrons. From conservation of energy and momentum, he was able to determine the mass of new particle ‘as very nearly the same as mass of proton’.
The mass of a neutron is now known to a high degree of accuracy. It is
$$ \begin{equation*} m_{\mathrm{n}}=1.00866 \mathrm{u}=1.6749 \times 10^{-27} \mathrm{~kg} \tag{13.3} \end{equation*} $$
Chadwick was awarded the 1935 Nobel Prize in Physics for his discovery of the neutron.
A free neutron, unlike a free proton, is unstable. It decays into a proton, an electron and a antineutrino (another elementary particle), and has a mean life of about 1000s. It is, however, stable inside the nucleus.
The composition of a nucleus can now be described using the following terms and symbols:
$Z$ - atomic number $=$ number of protons
$N$ - neutron number $=$ number of neutrons
$A$ - mass number $=Z+N$
$=$ total number of protons and neutrons [13.4(c)]
One also uses the term nucleon for a proton or a neutron. Thus the number of nucleons in an atom is its mass number $\mathrm{A}$.
Nuclear species or nuclides are shown by the notation $ _{Z}^{A} \mathrm{X}$
$ _{Z}^{A} \mathrm{X}$ where $X$
is the chemical symbol of the species. For example, the nucleus of gold is denoted by $ _{79}^{197} \mathrm{Au}$. It contains 197 nucleons, of which 79 are protons and the rest 118 are neutrons.
The composition of isotopes of an element can now be readily explained. The nuclei of isotopes of a given element contain the same number of protons, but differ from each other in their number of neutrons. Deuterium, $ _{1}^{2} \mathrm{H}$,
which is an isotope of hydrogen, contains one proton and one neutron. Its other isotope tritium, $ _{1}^{3} \mathrm{H}$, contains one proton and two neutrons. The element gold has 32 isotopes, ranging from $A=173$ to $A=204$. We have already mentioned that chemical properties of elements depend on their electronic structure. As the atoms of isotopes have identical electronic structure they have identical chemical behaviour and are placed in the same location in the periodic table.
All nuclides with same mass number $A$ are called isobars. For example, the nuclides $ _{1}^{3} \mathrm{H}$ and
$ _{2}^{3} \mathrm{He}$ are isobars. Nuclides with same neutron number $N$ but different atomic number $Z$, for example
$ _{80}^{198} \mathrm{Hg}$ and
$ _{79}^{197} \mathrm{Au}$, are called isotones.
13.3 SIZE OF THE NUCLEUS
As we have seen in Chapter 12, Rutherford was the pioneer who postulated and established the existence of the atomic nucleus. At Rutherford’s suggestion, Geiger and Marsden performed their classic experiment: on the scattering of $\alpha$-particles from thin gold foils. Their experiments revealed that the distance of closest approach to a gold nucleus of an $\alpha$-particle of kinetic energy $5.5 \mathrm{MeV}$ is about $4.0 \times 10^{-14} \mathrm{~m}$. The scattering of $\alpha$-particle by the gold sheet could be understood by Rutherford by assuming that the coulomb repulsive force was solely responsible for scattering. Since the positive charge is confined to the nucleus, the actual size of the nucleus has to be less than $4.0 \times 10^{-14} \mathrm{~m}$.
If we use $\alpha$-particles of higher energies than $5.5 \mathrm{MeV}$, the distance of closest approach to the gold nucleus will be smaller and at some point the scattering will begin to be affected by the short range nuclear forces, and differ from Rutherford’s calculations. Rutherford’s calculations are based on pure coulomb repulsion between the positive charges of the $\alpha$ particle and the gold nucleus. From the distance at which deviations set in, nuclear sizes can be inferred.
By performing scattering experiments in which fast electrons, instead of $\alpha$-particles, are projectiles that bombard targets made up of various elements, the sizes of nuclei of various elements have been accurately measured.
It has been found that a nucleus of mass number $A$ has a radius
$$ \begin{equation*} R=R_{0} A^{1 / 3} \tag{13.5} \end{equation*} $$
where $R_{0}=1.2 \times 10^{-15} \mathrm{~m}(=1.2 \mathrm{fm} ; 1 \mathrm{fm}=10^{-15} \mathrm{~m})$. This means the volume of the nucleus, which is proportional to $R^{3}$ is proportional to $A$. Thus the density of nucleus is a constant, independent of $A$, for all nuclei. Different nuclei are like a drop of liquid of constant density. The density of nuclear matter is approximately $2.3 \times 10^{17} \mathrm{~kg} \mathrm{~m}^{-3}$. This density is very large compared to ordinary matter, say water, which is $10^{3} \mathrm{~kg} \mathrm{~m}^{-3}$. This is understandable, as we have already seen that most of the atom is empty. Ordinary matter consisting of atoms has a large amount of empty space.
Example 13.1 Given the mass of iron nucleus as 55.85u and $\mathrm{A}=56$, find the nuclear density?
Solution
$m_{\mathrm{Fe}}=55.85, \mathrm{u}=9.27 \times 10^{-26} \mathrm{~kg}$
Nuclear density $=\frac{\text { mass }}{\text { volume }}=\frac{9.27 \times 10^{-26}}{(4 \pi / 3)(1.2 \times 10^{-15})^{3}} \times \frac{1}{56}$
$$ =2.29 \times 10^{17} \mathrm{~kg} \mathrm{~m}^{-3} $$
The density of matter in neutron stars (an astrophysical object) is comparable to this density. This shows that matter in these objects has been compressed to such an extent that they resemble a big nucleus.
13.4 MASS-ENERGY AND NUCLEAR BINDING ENERGY
13.4.1 Mass - Energy
Einstein showed from his theory of special relativity that it is necessary to treat mass as another form of energy. Before the advent of this theory of special relativity it was presumed that mass and energy were conserved separately in a reaction. However, Einstein showed that mass is another form of energy and one can convert mass-energy into other forms of energy, say kinetic energy and vice-versa.
Einstein gave the famous mass-energy equivalence relation
$E=m c^{2}$
Here the energy equivalent of mass $m$ is related by the above equation and $c$ is the velocity of light in vacuum and is approximately equal to $3 \times 10^{8} \mathrm{~m} \mathrm{~s}^{-1}$.
Example 13.2 Calculate the energy equivalent of $1 \mathrm{~g}$ of substance.
Solution
$$ \text { Energy, } \begin{aligned} E & =10^{-3} \times(3 \times 10^{8})^{2} \mathrm{~J} \ E & =10^{-3} \times 9 \times 10^{16}=9 \times 10^{13} \mathrm{~J} \end{aligned} $$
Thus, if one gram of matter is converted to energy, there is a release of enormous amount of energy.
Experimental verification of the Einstein’s mass-energy relation has been achieved in the study of nuclear reactions amongst nucleons, nuclei, electrons and other more recently discovered particles. In a reaction the conservation law of energy states that the initial energy and the final energy are equal provided the energy associated with mass is also included. This concept is important in understanding nuclear masses and the interaction of nuclei with one another. They form the subject matter of the next few sections.
13.4.2 Nuclear binding energy
In Section 13.2 we have seen that the nucleus is made up of neutrons and protons. Therefore it may be expected that the mass of the nucleus is equal to the total mass of its individual protons and neutrons. However,
the nuclear mass $M$ is found to be always less than this. For example, let us consider $ _{8}^{16} \mathrm{O}$; a nucleus which has 8 neutrons and 8 protons. We have
Mass of 8 neutrons $=8 \times 1.00866 \mathrm{u}$
Mass of 8 protons $=8 \times 1.00727 \mathrm{u}$
Mass of 8 electrons $=8 \times 0.00055 \mathrm{u}$
Therefore the expected mass of $ _{8}^{16} \mathrm{O}$ nucleus
$=8 \times 2.01593 \mathrm{u}=16.12744 \mathrm{u}$.
The atomic mass of $ _{8}^{16} \mathrm{O}$
found from mass spectroscopy experiments is seen to be $15.99493 \mathrm{u}$. Substracting the mass of 8 electrons $(8 \times 0.00055 \mathrm{u})$ from this, we get the experimental mass of $ _{8}^{16} \mathrm{O}$ nucleus to be $15.99053 \mathrm{u}$.
Thus, we find that the mass of the $ _{8}^{16} \mathrm{O}$ nucleus is less than the total mass of its constituents by 0.13691 . The difference in mass of a nucleus and its constituents, $\Delta M$, is called the mass defect, and is given by
$$ \begin{equation*} \Delta M=\left[Z m_{p}+(A-Z) m_{n}\right]-M \tag{13.7} \end{equation*} $$
What is the meaning of the mass defect? It is here that Einstein’s equivalence of mass and energy plays a role. Since the mass of the oxygen nucleus is less that the sum of the masses of its constituents (8 protons and 8 neutrons, in the unbound state), the equivalent energy of the oxygen nucleus is less than that of the sum of the equivalent energies of its constituents. If one wants to break the oxygen nucleus into 8 protons and 8 neutrons, this extra energy $\Delta M c^{2}$, has to supplied. This energy required $E_{\mathrm{b}}$ is related to the mass defect by
$$ \begin{equation*} E_{b}=\Delta M c^{2} \tag{13.8} \end{equation*} $$
Example 13.3 Find the energy equivalent of one atomic mass unit, first in Joules and then in MeV. Using this, express the mass defect of $ _{8}^{16} \mathrm{O}$ in $\mathrm{MeV} / \mathrm{c}^{2}$.
Solution
$1 \mathrm{u}=1.6605 \times 10^{-27} \mathrm{~kg}$
To convert it into energy units, we multiply it by $c^{2}$ and find that energy equivalent $=1.6605 \times 10^{-27} \times(2.9979 \times 10^{8})^{2} \mathrm{~kg} \mathrm{~m}^{2} / \mathrm{s}^{2}$
$=1.4924 \times 10^{-10} \mathrm{~J}$
$$ \begin{aligned} & =\frac{1.4924 \times 10^{-10}}{1.602 \times 10^{-19}} \mathrm{eV} \ & =0.9315 \times 10^{9} \mathrm{eV} \ & =931.5 \mathrm{MeV} \end{aligned} $$
or, $1 \mathrm{u}=931.5 \mathrm{MeV} / \mathrm{c}^{2}$
For $ _{8}^{16} \mathrm{O}, \quad \Delta M=0.13691 \mathrm{u}=0.13691 \times 931.5 \mathrm{MeV} / \mathrm{c}^{2}$
$$ =127.5 \mathrm{MeV} / \mathrm{c}^{2} $$
The energy needed to separate $ _{8}^{16} \mathrm{O}$ into its constituents is thus $127.5 \mathrm{MeV} / \mathrm{c}^{2}$.
in the process. The energy $E_{b}$ is called the binding energy of the nucleus. If we separate a nucleus into its nucleons, we would have to supply a total energy equal to $E_{b}$, to those particles. Although we cannot tear apart a nucleus in this way, the nuclear binding energy is still a convenient measure of how well a nucleus is held together. A more useful measure of the binding between the constituents of the nucleus is the binding energy per nucleon, $E_{b n}$, which is the ratio of the binding energy $E_{b}$ of a nucleus to the number of the nucleons, $A$, in that nucleus:
$$ \begin{equation*} E_{b n}=E_{b} / A \tag{13.9} \end{equation*} $$
We can think of binding energy per nucleon as the average energy per nucleon needed to separate a nucleus into its individual nucleons.
Figure 13.1 is a plot of the
FIGURE 13.1 The binding energy per nucleon as a function of mass number. binding energy per nucleon $E_{b n}$ versus the mass number $A$ for a large number of nuclei. We notice the following main features of the plot:
(i) the binding energy per nucleon, $E_{b n}$, is practically constant, i.e. practically independent of the atomic number for nuclei of middle mass number $(30<\mathrm{A}<170)$. The curve has a maximum of about $8.75 \mathrm{MeV}$ for $A=56$ and has a value of $7.6 \mathrm{MeV}$ for $A=238$.
(ii) $E_{b n}$ is lower for both light nuclei $(A<30)$ and heavy nuclei $(A>170)$.
We can draw some conclusions from these two observations:
(i) The force is attractive and sufficiently strong to produce a binding energy of a few MeV per nucleon.
(ii) The constancy of the binding energy in the range $30<\mathrm{A}<170$ is a consequence of the fact that the nuclear force is short-ranged. Consider a particular nucleon inside a sufficiently large nucleus. It will be under the influence of only some of its neighbours, which come within the range of the nuclear force. If any other nucleon is at a distance more than the range of the nuclear force from the particular nucleon it will have no influence on the binding energy of the nucleon under consideration. If a nucleon can have a maximum of $p$ neighbours within the range of nuclear force, its binding energy would be proportional to $p$. Let the binding energy of the nucleus be $p k$, where $k$ is a constant having the dimensions of energy. If we increase $A$ by adding nucleons they will not change the binding energy of a nucleon inside. Since most of the nucleons in a large nucleus reside inside it and not on the surface, the change in binding energy per nucleon would be small. The binding energy per nucleon is a constant and is approximately equal to $p k$. The property that a given nucleon influences only nucleons close to it is also referred to as saturation property of the nuclear force.
(iii) A very heavy nucleus, say $A=240$, has lower binding energy per nucleon compared to that of a nucleus with $A=120$. Thus if a nucleus $A=240$ breaks into two $A=120$ nuclei, nucleons get more tightly bound. This implies energy would be released in the process. It has very important implications for energy production through fission, to be discussed later in Section 13.7.1.
(iv) Consider two very light nuclei $(A \leq 10)$ joining to form a heavier nucleus. The binding energy per nucleon of the fused heavier nuclei is more than the binding energy per nucleon of the lighter nuclei. This means that the final system is more tightly bound than the initial system. Again energy would be released in such a process of fusion. This is the energy source of sun, to be discussed later in Section 13.7.2.
13.5 NUCLEAR FORCE
The force that determines the motion of atomic electrons is the familiar Coulomb force. In Section 13.4, we have seen that for average mass nuclei the binding energy per nucleon is approximately $8 \mathrm{MeV}$, which is much larger than the binding energy in atoms. Therefore, to bind a nucleus together there must be a strong attractive force of a totally different kind. It must be strong enough to overcome the repulsion between the (positively charged) protons and to bind both protons and neutrons into the tiny nuclear volume. We have already seen that the constancy of binding energy per nucleon can be understood in terms of its short-range. Many features of the nuclear binding force are summarised below. These are obtained from a variety of experiments carried out during 1930 to 1950.
(i) The nuclear force is much stronger than the Coulomb force acting between charges or the gravitational forces between masses. The nuclear binding force has to dominate over the Coulomb repulsive force between protons inside the nucleus. This happens only because the nuclear force is much stronger than the coulomb force. The gravitational force is much weaker than even Coulomb force.
(ii) The nuclear force between two nucleons falls rapidly to zero as their distance is more than a few femtometres. This leads to saturation of forces in a medium or a large-sized nucleus, which is the reason for the constancy of the binding energy per nucleon.
A rough plot of the potential energy between two nucleons as a function of distance is shown in the Fig. 13.2. The
FIGURE 13.2 Potential energy of a pair of nucleons as a function of their separation. For a separation greater than $r_{0}$, the force is attractive and for separations less than $r_{0}$, the force is strongly repulsive.
potential energy is a minimum at a distance $r_{0}$ of about $0.8 \mathrm{fm}$. This means that the force is attractive for distances larger than $0.8 \mathrm{fm}$ and repulsive if they are separated by distances less than $0.8 \mathrm{fm}$. (iii) The nuclear force between neutron-neutron, proton-neutron and proton-proton is approximately the same. The nuclear force does not depend on the electric charge.
Unlike Coulomb’s law or the Newton’s law of gravitation there is no simple mathematical form of the nuclear force.
13.6 RADIOACTIVITY
A. H. Becquerel discovered radioactivity in 1896 purely by accident. While studying the fluorescence and phosphorescence of compounds irradiated with visible light, Becquerel observed an interesting phenomenon. After illuminating some pieces of uranium-potassium sulphate with visible light, he wrapped them in black paper and separated the package from a photographic plate by a piece of silver. When, after several hours of exposure, the photographic plate was developed, it showed blackening due to something that must have been emitted by the compound and was able to penetrate both black paper and the silver.
Experiments performed subsequently showed that radioactivity was a nuclear phenomenon in which an unstable nucleus undergoes a decay. This is referred to as radioactive decay. Three types of radioactive decay occur in nature :
(i) $\quad \alpha$-decay in which a helium nucleus $ _{2}^{4} \mathrm{He}$ is emitted;
(ii) $\beta$-decay in which electrons or positrons (particles with the same mass as electrons, but with a charge exactly opposite to that of electron) are emitted;
(iii) $\gamma$-decay in which high energy (hundreds of $\mathrm{keV}$ or more) photons are emitted.
Each of these decay will be considered in subsequent sub-sections.
13.7 NUCLEAR ENERGY
The curve of binding energy per nucleon $E_{b n}$, given in Fig. 13.1, has a long flat middle region between $A=30$ and $A=170$. In this region the binding energy per nucleon is nearly constant $(8.0 \mathrm{MeV})$. For the lighter nuclei region, $A<30$, and for the heavier nuclei region, $A>170$, the binding energy per nucleon is less than $8.0 \mathrm{MeV}$, as we have noted earlier. Now, the greater the binding energy, the less is the total mass of a bound system, such as a nucleus. Consequently, if nuclei with less total binding energy transform to nuclei with greater binding energy, there will be a net energy release. This is what happens when a heavy nucleus decays into two or more intermediate mass fragments (fission) or when light nuclei fuse into a havier nucleus (fusion.)
Exothermic chemical reactions underlie conventional energy sources such as coal or petroleum. Here the energies involved are in the range of electron volts. On the other hand, in a nuclear reaction, the energy release is of the order of $\mathrm{MeV}$. Thus for the same quantity of matter, nuclear sources produce a million times more energy than a chemical source. Fission of $1 \mathrm{~kg}$ of uranium, for example, generates $10^{14} \mathrm{~J}$ of energy; compare it with burning of $1 \mathrm{~kg}$ of coal that gives $10^{7} \mathrm{~J}$.
13.7.1 Fission
New possibilities emerge when we go beyond natural radioactive decays and study nuclear reactions by bombarding nuclei with other nuclear particles such as proton, neutron, $\alpha$-particle, etc.
A most important neutron-induced nuclear reaction is fission. An example of fission is when a uranium isotope $ _{92}^{235} \mathrm{U}$ bombarded with a neutron breaks into two intermediate mass nuclear fragments
$ _{0}^{1} \mathrm{n}+ _{92}^{235} \mathrm{U} \rightarrow _{92}^{236} \mathrm{U} \rightarrow _{56}^{144} \mathrm{Ba}+ _{36}^{89} \mathrm{Kr}+3 _{0}^{1} \mathrm{n}$
The same reaction can produce other pairs of intermediate mass fragments
$ _{0}^{1} \mathrm{n}+ _{92}^{235} \mathrm{U} \rightarrow _{92}^{236} \mathrm{U} \rightarrow _{51}^{133} \mathrm{Sb}+ _{41}^{99} \mathrm{Nb}+4 _{0}^{1} \mathrm{n}$
Or, as another example,
$ _{0}^{1} \mathrm{n}+ _{92}^{235} \mathrm{U} \rightarrow _{54}^{140} \mathrm{Xe}+ _{38}^{94} \mathrm{Sr}+2 _{0}^{1} \mathrm{n}$
The fragment products are radioactive nuclei; they emit $\beta$ particles in succession to achieve stable end products.
The energy released (the $Q$ value ) in the fission reaction of nuclei like uranium is of the order of $200 \mathrm{MeV}$ per fissioning nucleus. This is estimated as follows:
Let us take a nucleus with $A=240$ breaking into two fragments each of $A=120$. Then
$E_{b n}$ for $A=240$ nucleus is about $7.6 \mathrm{MeV}$,
$E_{b n}$ for the two $A=120$ fragment nuclei is about $8.5 \mathrm{MeV}$.
$\therefore$ Gain in binding energy for nucleon is about $0.9 \mathrm{MeV}$.
Hence the total gain in binding energy is $240 \times 0.9$ or $216 \mathrm{MeV}$.
The disintegration energy in fission events first appears as the kinetic energy of the fragments and neutrons. Eventually it is transferred to the surrounding matter appearing as heat. The source of energy in nuclear reactors, which produce electricity, is nuclear fission. The enormous energy released in an atom bomb comes from uncontrolled nuclear fission.
13.7.2 Nuclear fusion - energy generation in stars
When two light nuclei fuse to form a larger nucleus, energy is released, since the larger nucleus is more tightly bound, as seen from the binding energy curve in Fig. 13.1. Some examples of such energy liberating nuclear fusion reactions are :
$$ \begin{align*} & _{1}^{1} \mathrm{H}+ _{1}^{1} \mathrm{H} \rightarrow _{1}^{2} \mathrm{H}+e^{+}+v+0.42 \mathrm{MeV} \tag{a}\\ & _{1}^{2} \mathrm{H}+ _{1}^{2} \mathrm{H} \rightarrow _{2}^{3} \mathrm{He}+n+3.27 \mathrm{MeV} \tag{b}\\ & _{1}^{2} \mathrm{H}+ _{1}^{2} \mathrm{H} \rightarrow _{1}^{3} \mathrm{H}+ _{1}^{1} \mathrm{H}+4.03 \mathrm{MeV} \tag{c} \end{align*} $$
In the first reaction, two protons combine to form a deuteron and a positron with a release of $0.42 \mathrm{MeV}$ energy. In reaction [13.13(b)], two deuterons combine to form the light isotope of helium. In reaction (13.13c), two deuterons combine to form a triton and a proton. For fusion to take place, the two nuclei must come close enough so that attractive short-range nuclear force is able to affect them. However, since they are both positively charged particles, they experience coulomb repulsion. They, therefore, must have enough energy to overcome this coulomb barrier. The height of the barrier depends on the charges and radii of the two interacting nuclei. It can be shown, for example, that the barrier height for two protons is $\sim 400 \mathrm{keV}$, and is higher for nuclei with higher charges. We can estimate the temperature at which two protons in a proton gas would (averagely) have enough energy to overcome the coulomb barrier:
$(3 / 2) k T=K \simeq 400 \mathrm{keV}$, which gives $\mathrm{T} \sim 3 \times 10^{9} \mathrm{~K}$.
When fusion is achieved by raising the temperature of the system so that particles have enough kinetic energy to overcome the coulomb repulsive behaviour, it is called thermonuclear fusion.
Thermonuclear fusion is the source of energy output in the interior of stars. The interior of the sun has a temperature of $1.5 \times 10^{7} \mathrm{~K}$, which is considerably less than the estimated temperature required for fusion of particles of average energy. Clearly, fusion in the sun involves protons whose energies are much above the average energy.
The fusion reaction in the sun is a multi-step process in which the hydrogen is burned into helium. Thus, the fuel in the sun is the hydrogen in its core. The proton-proton ( $\mathrm{p}, \mathrm{p}$) cycle by which this occurs is represented by the following sets of reactions:
$$ \begin{align*} & _{1}^{1} \mathrm{H}+ _{1}^{1} \mathrm{H} \rightarrow _{1}^{2} \mathrm{H}+e^{+}+v+0.42 \mathrm{MeV} \tag{i}\\ & e^{+}+e^{-} \rightarrow \gamma+\gamma+1.02 \mathrm{MeV} \tag{ii}\\ & _{1}^{2} \mathrm{H}+ _{1}^{1} \mathrm{H} \rightarrow _{2}^{3} \mathrm{He}^{+} \gamma+5.49 \mathrm{MeV} \tag{iii}\\ & _{2}^{3} \mathrm{He}+ _{2}^{3} \mathrm{He} \rightarrow _{2}^{4} \mathrm{He}+ _{1}^{1} \mathrm{H}+ _{1}^{1} \mathrm{H}+12.86 \mathrm{MeV} \text { (iv) } \tag{13.14} \end{align*} $$
For the fourth reaction to occur, the first three reactions must occur twice, in which case two light helium nuclei unite to form ordinary helium nucleus. If we consider the combination 2(i) +2 (ii) +2 (iii) $+$ (iv), the net effect is
$4 _{1}^{1} \mathrm{H}+2 e^{-} \rightarrow _{2}^{4} \mathrm{He}+2 v+6 \gamma+26.7 \mathrm{MeV}$
or $(4 _{1}^{1} \mathrm{H}+4 e^{-}) \rightarrow( _{2}^{4} \mathrm{He}+2 e^{-})+2 \nu+6 \gamma+26.7 \mathrm{MeV}$
Thus, four hydrogen atoms combine to form an $ _{2}^{4} \mathrm{He}$ atom with a release of $26.7 \mathrm{MeV}$ of energy.
Helium is not the only element that can be synthesized in the interior of a star. As the hydrogen in the core gets depleted and becomes helium, the core starts to cool. The star begins to collapse under its own gravity which increases the temperature of the core. If this temperature increases to about $10^{8} \mathrm{~K}$, fusion takes place again, this time of helium nuclei into carbon. This kind of process can generate through fusion higher and higher mass number elements. But elements more massive than those near the peak of the binding energy curve in Fig. 13.1 cannot be so produced.
The age of the sun is about $5 \times 10^{9} \mathrm{y}$ and it is estimated that there is enough hydrogen in the sun to keep it going for another 5 billion years. After that, the hydrogen burning will stop and the sun will begin to cool and will start to collapse under gravity, which will raise the core temperature. The outer envelope of the sun will expand, turning it into the so called red giant.
13.7.3 Controlled thermonuclear fusion
The natural thermonuclear fusion process in a star is replicated in a thermonuclear fusion device. In controlled fusion reactors, the aim is to generate steady power by heating the nuclear fuel to a temperature in the range of $10^{8} \mathrm{~K}$. At these temperatures, the fuel is a mixture of positive ions and electrons (plasma). The challenge is to confine this plasma, since no container can stand such a high temperature. Several countries around the world including India are developing techniques in this connection. If successful, fusion reactors will hopefully supply almost unlimited power to humanity.
Example 13.4 Answer the following questions:
(a) Are the equations of nuclear reactions (such as those given in Section 13.7) ‘balanced’ in the sense a chemical equation (e.g., $2 \mathrm{H} _{2}+\mathrm{O} _{2} \rightarrow 2 \mathrm{H} _{2} \mathrm{O}$ ) is? If not, in what sense are they balanced on both sides?
(b) If both the number of protons and the number of neutrons are conserved in each nuclear reaction, in what way is mass converted into energy (or vice-versa) in a nuclear reaction?
(c) A general impression exists that mass-energy interconversion takes place only in nuclear reaction and never in chemical reaction. This is strictly speaking, incorrect. Explain.
Solution
(a) A chemical equation is balanced in the sense that the number of atoms of each element is the same on both sides of the equation. A chemical reaction merely alters the original combinations of atoms. In a nuclear reaction, elements may be transmuted. Thus, the number of atoms of each element is not necessarily conserved in a nuclear reaction. However, the number of protons and the number of neutrons are both separately conserved in a nuclear reaction. [Actually, even this is not strictly true in the realm of very high energies - what is strictly conserved is the total charge and total ‘baryon number’. We need not pursue this matter here.] In nuclear reactions (e.g., Eq. 13.10), the number of protons and the number of neutrons are the same on the two sides of the equation.
(b) We know that the binding energy of a nucleus gives a negative contribution to the mass of the nucleus (mass defect). Now, since proton number and neutron number are conserved in a nuclear reaction, the total rest mass of neutrons and protons is the same on either side of a reaction. But the total binding energy of nuclei on the left side need not be the same as that on the right hand side. The difference in these binding energies appears as energy released or absorbed in a nuclear reaction. Since binding energy contributes to mass, we say that the difference in the total mass of nuclei on the two sides get converted into energy or vice-versa. It is in these sense that a nuclear reaction is an example of massenergy interconversion.
(c) From the point of view of mass-energy interconversion, a chemical reaction is similar to a nuclear reaction in principle. The energy released or absorbed in a chemical reaction can be traced to the difference in chemical (not nuclear) binding energies of atoms and molecules on the two sides of a reaction. Since, strictly speaking, chemical binding energy also gives a negative contribution (mass defect) to the total mass of an atom or molecule, we can equally well say that the difference in the total mass of atoms or molecules, on the two sides of the chemical reaction gets converted into energy or vice-versa. However, the mass defects involved in a chemical reaction are almost a million times smaller than those in a nuclear reaction. This is the reason for the general impression, (which is incorrect) that mass-energy interconversion does not take place in a chemical reaction.
SUMMARY
1. An atom has a nucleus. The nucleus is positively charged. The radius of the nucleus is smaller than the radius of an atom by a factor of $10^{4}$. More than $99.9 %$ mass of the atom is concentrated in the nucleus.
2. On the atomic scale, mass is measured in atomic mass units (u). By definition, 1 atomic mass unit $(1 \mathrm{u})$ is $1 / 12^{\text {th }}$ mass of one atom of $ ^{12} \mathrm{C}$; $1 \mathrm{u}=1.660563 \times 10^{-27} \mathrm{~kg}$.
3. A nucleus contains a neutral particle called neutron. Its mass is almost the same as that of proton
4. The atomic number $Z$ is the number of protons in the atomic nucleus of an element. The mass number $A$ is the total number of protons and neutrons in the atomic nucleus; $A=Z+N$; Here $N$ denotes the number of neutrons in the nucleus.
A nuclear species or a nuclide is represented as $ _{Z}^{A} \mathrm{X}$, where $\mathrm{X}$ is the chemical symbol of the species.
Nuclides with the same atomic number $Z$, but different neutron number $N$ are called isotopes. Nuclides with the same $A$ are isobars and those with the same $N$ are isotones.
Most elements are mixtures of two or more isotopes. The atomic mass of an element is a weighted average of the masses of its isotopes and calculated in accordance to the relative abundances of the isotopes.
5. A nucleus can be considered to be spherical in shape and assigned a radius. Electron scattering experiments allow determination of the nuclear radius; it is found that radii of nuclei fit the formula
$R=R_{0} A^{1 / 3}$,
where $R_{0}=$ a constant $=1.2 \mathrm{fm}$. This implies that the nuclear density is independent of $A$. It is of the order of $10^{17} \mathrm{~kg} / \mathrm{m}^{3}$.
6. Neutrons and protons are bound in a nucleus by the short-range strong nuclear force. The nuclear force does not distinguish between neutron and proton.
7. The nuclear mass $M$ is always less than the total mass, $\Sigma m$, of its constituents. The difference in mass of a nucleus and its constituents is called the mass defect,
$\Delta M=(Z m_{p}+(A-Z) m_{n})-M$
Using Einstein’s mass energy relation, we express this mass difference in terms of energy as
$\Delta E_{b}=\Delta M c^{2}$
The energy $\Delta E_{b}$ represents the binding energy of the nucleus. In the mass number range $A=30$ to 170 , the binding energy per nucleon is nearly constant, about $8 \mathrm{MeV} /$ nucleon.
8. Energies associated with nuclear processes are about a million times larger than chemical process.
9. The $Q$-value of a nuclear process is
$Q=$ final kinetic energy - initial kinetic energy.
Due to conservation of mass-energy, this is also,
$Q=$ (sum of initial masses - sum of final masses) $c^{2}$
10. Radioactivity is the phenomenon in which nuclei of a given species transform by giving out $\alpha$ or $\beta$ or $\gamma$ rays; $\alpha$-rays are helium nuclei; $\beta$-rays are electrons. $\gamma$-rays are electromagnetic radiation of wavelengths shorter than $X$-rays.
11. Energy is released when less tightly bound nuclei are transmuted into more tightly bound nuclei. In fission, a heavy nucleus like $ _{92}^{235} \mathrm{U}$ breaks into two smaller fragments, e.g., $ _{92}^{235} \mathrm{U}+ _{0}^{1} \mathrm{n} \rightarrow _{51}^{133} \mathrm{Sb}+ _{41}^{99} \mathrm{Nb}+4 _{0}^{1} \mathrm{n}$
12. In fusion, lighter nuclei combine to form a larger nucleus. Fusion of hydrogen nuclei into helium nuclei is the source of energy of all stars including our sun.
| Physical Quantity | Symbol | Dimensions | Units | Remarks |
|---|---|---|---|---|
| Atomic mass unit | $[\mathrm{M}]$ | u | Unit of mass for expressing atomic or nuclear masses. One atomic mass unit equals $1 / 12^{\text {th }}$ of the mass of $ ^{12} \mathrm{C}$ atom. |
|
| Disintegration or decay constant |
$\lambda$ | $\left[\mathrm{T}^{-1}\right]$ | $\mathrm{s}^{-1}$ | |
| Half-life | $T_{1 / 2}$ | $[\mathrm{~T}]$ | $\mathrm{s}$ | Time taken for the decay of one-half of the initial number of nuclei present in a radioactive sample. |
| Mean life | $\tau$ | $[\mathrm{T}]$ | $\mathrm{s}$ | Time at which number of nuclei has been reduced to $\mathrm{e}^{-1}$ of its initial value |
| Activity of a radio- active sample |
$R$ | $\left[\mathrm{~T}^{-1}\right]$ | $\mathrm{Bq}$ | Measure of the activity of a radioactive source. |
POINTS TO PONDER
1. The density of nuclear matter is independent of the size of the nucleus. The mass density of the atom does not follow this rule.
2. The radius of a nucleus determined by electron scattering is found to be slightly different from that determined by alpha-particle scattering. This is because electron scattering senses the charge distribution of the nucleus, whereas alpha and similar particles sense the nuclear matter.
3. After Einstein showed the equivalence of mass and energy, $E=m c^{2}$, we cannot any longer speak of separate laws of conservation of mass and conservation of energy, but we have to speak of a unified law of conservation of mass and energy. The most convincing evidence that this principle operates in nature comes from nuclear physics. It is central to our understanding of nuclear energy and harnessing it as a source of power. Using the principle, $Q$ of a nuclear process (decay or reaction) can be expressed also in terms of initial and final masses.
4. The nature of the binding energy (per nucleon) curve shows that exothermic nuclear reactions are possible, when two light nuclei fuse or when a heavy nucleus undergoes fission into nuclei with intermediate mass.
5. For fusion, the light nuclei must have sufficient initial energy to overcome the coulomb potential barrier. That is why fusion requires very high temperatures.
6. Although the binding energy (per nucleon) curve is smooth and slowly varying, it shows peaks at nuclides like $ ^{4} \mathrm{He}, ^{16} \mathrm{O}$ etc. This is considered as evidence of atom-like shell structure in nuclei.
7. Electrons and positron are a particle-antiparticle pair. They are identical in mass; their charges are equal in magnitude and opposite. (It is found that when an electron and a positron come together, they annihilate each other giving energy in the form of gamma-ray photons.)
8. Radioactivity is an indication of the instability of nuclei. Stability requires the ratio of neutron to proton to be around 1:1 for light nuclei. This ratio increases to about 3:2 for heavy nuclei. (More neutrons are required to overcome the effect of repulsion among the protons.) Nuclei which are away from the stability ratio, i.e., nuclei which have an excess of neutrons or protons are unstable. In fact, only about $10 %$ of knon isotopes (of all elements), are stable. Others have been either artificially produced in the laboratory by bombarding $\alpha, \mathrm{p}, \mathrm{d}, \mathrm{n}$ or other particles on targets of stable nuclear species or identified in astronomical observations of matter in the universe.
EXERCISES
You may find the following data useful in solving the exercises:
$$ \begin{aligned} &e=1.6 \times 10^{-19}\text{C} & & N= 6.023 \times 10 ^{23} \text{per mole}\\ &\frac{1}{(4 \pi \varepsilon _0)}=9 \times 10 ^9 \text{N} m ^2/C ^2 && k=1.381 \times 10 ^{-23} \text{J} k ^{-1} \\ &1 \text{MeV}=1.6 \times 10 ^{-13} \text{J} && 1 \text{u} = 931.5 \text{MeV}/c ^2 \\ &1 \text{ year} = 3.154 \times 10 ^7 \text{s} \\ & \text{m}_H=4.002603 \text{ u} && \text{m}_n=1.007825 \text{u} \\ & m( ^4_2\text{He})=4.002603 u && \text{m}_e=0.000548 \text{u} \end{aligned} $$
13.1 Obtain the binding energy (in $\mathrm{MeV}$ ) of a nitrogen nucleus $( _{7} ^{14} \mathrm{~N})$, given $m( _{7} ^{14} \mathrm{~N})=14.00307 \mathrm{u}$
Answer Atomic mass of nitrogen $({ }_{7} \mathrm{~N} ^{14}), m=14.00307 \mathrm{u}$ A nucleus of nitrogen ${ }_{7} \mathrm{~N} ^{14}$ contains 7 protons and 7 neutrons. Hence, the mass defect of this nucleus, $\Delta m=7 m_{H}+7 m_{n}-m$ Where, Mass of a proton, $m_{H}=1.007825 \mathrm{u}$ Mass of a neutron, $m_{n}=1.008665 \mathrm{u}$ $\therefore \Delta m=7 \times 1.007825+7 \times 1.008665-14.00307$
$=7.054775+7.06055-14.00307$ $=0.11236 \mathrm{u}$ But $1 \mathrm{u}=931.5 \mathrm{MeV} / \mathrm{c} ^{2}$ $\therefore \Delta m=0.11236 \times 931.5 \mathrm{MeV} / c ^{2}$ Hence, the binding energy of the nucleus is given as: $E_{b}=\Delta m c ^{2}$ Where, $c=$ Speed of light $\therefore E_{b}=0.11236 \times 931.5(\frac{\mathrm{MeV}}{c ^{2}}) \times c ^{2}$ $=104.66334 \mathrm{MeV}$ Hence, the binding energy of a nitrogen nucleus is $104.66334 \mathrm{MeV}$.Show Answer
$$ m( _{26} ^{56} \mathrm{Fe})=55.934939 \mathrm{u} \quad m( _{83} ^{209} \mathrm{Bi})=208.980388 \mathrm{u} $$
Answer Atomic mass of ${ } _{26} ^{56} \mathrm{Fe}, m _{1}=55.934939 \mathrm{u}$ ${ } _{26} ^{56} \mathrm{Fe}$ nucleus has 26 protons and $(56-26)=30$ neutrons Hence, the mass defect of the nucleus, $\Delta m=26 \times m _{H}+30 \times m _{n}-m _{1}$ Where, Mass of a proton, $m _{H}=1.007825 \mathrm{u}$ Mass of a neutron, $m _{n}=1.008665 \mathrm{u}$ $\therefore \Delta m=26 \times 1.007825+30 \times 1.008665-55.934939$ $=26.20345+30.25995-55.934939$ $=0.528461 \mathrm{u}$ But $1 \mathrm{u}=931.5 \mathrm{MeV} / \mathrm{c} ^{2}$ $\therefore \Delta m=0.528461 \times 931.5 \mathrm{MeV} / c ^{2}$ The binding energy of this nucleus is given as: $E _{b 1}=\Delta m c ^{2}$ Where, $c=$ Speed of light $\therefore E _{b 1}=0.528461 \times 931.5(\frac{\mathrm{MeV}}{c ^{2}}) \times c ^{2}$ $=492.26 \mathrm{MeV}$ Average binding energy per nucleon $=\frac{492.26}{56}=8.79 \mathrm{MeV}$ Atomic mass of ${ } ^{\frac{209}{83} \mathrm{Bi}}, m _{2}=208.980388 \mathrm{u}$ ${ } _{83} ^{2099} \mathrm{Bi}$ nucleus has 83 protons and $(209-83) 126$ neutrons. Hence, the mass defect of this nucleus is given as: $\Delta m ^{\prime}=83 \times m _{H}+126 \times m _{n}-m _{2}$ Where, Mass of a proton, $m _{H}=1.007825 \mathrm{u}$ Mass of a neutron, $m _{n}=1.008665 \mathrm{u}$ $\therefore \Delta m ^{\prime}=83 \times 1.007825+126 \times 1.008665-208.980388$ $=83.649475+127.091790-208.980388$
$=1.760877 \mathrm{u}$ But $1 \mathrm{u}=931.5 \mathrm{MeV} / \mathrm{c} ^{2}$ $\therefore \Delta m ^{\prime}=1.760877 \times 931.5 \mathrm{MeV} / c ^{2}$ Hence, the binding energy of this nucleus is given as: $E _{b 2}=\Delta m ^{\prime} c ^{2}$ $=1.760877 \times 931.5(\frac{\mathrm{MeV}}{c ^{2}}) \times c ^{2}$ $=1640.26 \mathrm{MeV}$ Average bindingenergy per nucleon $=\frac{1640.26}{209}=7.848 \mathrm{MeV}$Show Answer
Answer Mass of a copper coin, $m ^{\prime}=3 \mathrm{~g}$ Atomic mass of ${ } _{29} \mathrm{Cu} ^{63}$ atom, $m=62.92960 \mathrm{u}$ The total number of ${ } _{29} \mathrm{Cu} ^{63}$ atoms in the coin,$N=\frac{N _{\mathrm{A}} \times m ^{\prime}}{\text { Mass number }}$ Where, $\mathrm{N} _{\mathrm{A}}=$ Avogadro’s number $=6.023 \times 10 ^{23}$ atoms $/ \mathrm{g}$ Mass number $=63 \mathrm{~g}$
$\therefore N=\frac{6.023 \times 10 ^{23} \times 3}{63}=2.868 \times 10 ^{22}$ atoms ${ } _{29} \mathrm{Cu} ^{63}$ nucleus has 29 protons and $(63-29) 34$ neutrons $\therefore$ Mass defect of this nucleus, $\Delta m ^{\prime}=29 \times m _{H}+34 \times m _{n}-m$ Where, Mass of a proton, $m _{H}=1.007825 \mathrm{u}$ Mass of a neutron, $m _{n}=1.008665 \mathrm{u}$ $\therefore \Delta m ^{\prime}=29 \times 1.007825+34 \times 1.008665-62.9296$ $=0.591935 \mathrm{u}$ Mass defect of all the atoms present in the coin, $\Delta m=0.591935 \times 2.868 \times 10 ^{22}$ $=1.69766958 \times 10 ^{22} \mathrm{u}$ But $1 \mathrm{u}=931.5 \mathrm{MeV} / \mathrm{c} ^{2}$ $\therefore \Delta m=1.69766958 \times 10 ^{22} \times 931.5 \mathrm{MeV} / c ^{2}$ Hence, the binding energy of the nuclei of the coin is given as: $E _{b}=\Delta m c ^{2}$ $=1.69766958 \times 10 ^{22} \times 931.5(\frac{\mathrm{MeV}}{c ^{2}}) \times c ^{2}$ $=1.581 \times 10 ^{25} \mathrm{MeV}$ But $1 \mathrm{MeV}=1.6 \times 10 ^{-13} \mathrm{~J}$ $E _{b}=1.581 \times 10 ^{25} \times 1.6 \times 10 ^{-13}$ $=2.5296 \times 10 ^{12} \mathrm{~J}$ This much energy is required to separate all the neutrons and protons from the given coin.Show Answer
Answer Nuclear radius of the gold isotope ${ } _{79} \mathrm{Au} ^{197}=R _{\mathrm{Au}}$ Nuclear radius of the silver isotope ${ } _{47} \mathrm{Ag} ^{107}=R _{\mathrm{Ag}}$ Mass number of gold, $A _{\mathrm{Au}}=197$ Mass number of silver, $A _{\mathrm{Ag}}=107$ The ratio of the radii of the two nuclei is related with their mass numbers as: $$
\begin{aligned}
\frac{R _{\mathrm{Au}}}{R _{\mathrm{Ag}}} & =(\frac{R _{\mathrm{Au}}}{R _{\mathrm{Ag}}}) ^{\frac{1}{3}} \
& =(\frac{197}{107}) ^{\frac{1}{3}}=1.2256
\end{aligned}
$$ Hence, the ratio of the nuclear radii of the gold and silver isotopes is about 1.23.Show Answer
where the masses refer to the respective nuclei. Determine from the given data the $Q$-value of the following reactions and state whether the reactions are exothermic or endothermic.
(i) $ _{1} ^{1} \mathrm{H}+ _{1} ^{3} \mathrm{H} \rightarrow _{1} ^{2} \mathrm{H}+ _{1} ^{2} \mathrm{H}$
(ii) $ _{6} ^{12} \mathrm{C}+ _{6} ^{12} \mathrm{C} \rightarrow _{10} ^{20} \mathrm{Ne}+ _{2} ^{4} \mathrm{He}$
Atomic masses are given to be
$m( _{1} ^{2} \mathrm{H})=2.014102 \mathrm{u}$
$m( _{1} ^{3} \mathrm{H})=3.016049 \mathrm{u}$
$m( _{6} ^{12} \mathrm{C})=12.000000 \mathrm{u}$
$m( _{10} ^{20} \mathrm{Ne})=19.992439 \mathrm{u}$
Answer Alpha particle decay of ${ } ^{226} \mathrm{Ra}$ emits a helium nucleus. As a result, its mass number reduces to $(226-4) 222$ and its atomic number reduces to $(88-2) 86$. This is shown in the following nuclear reaction. ${ } _{88} ^{226} \mathrm{Ra} \longrightarrow{ } _{86} ^{222} \mathrm{Ra}+{ } _{2} ^{4} \mathrm{He}$ $Q$-value of emitted $\alpha$-particle $=($ Sum of initial mass - Sum of final mass $) c ^{2}$ Where, $c=$ Speed of light It is given that: $m({ } _{88} ^{226} \mathrm{Ra})=226.02540 \mathrm{u}$ $m({ } _{86} ^{222} \mathrm{Rn})=222.01750 \mathrm{u}$ $m({ } _{2} ^{4} \mathrm{He})=4.002603 \mathrm{u}$ $Q$-value $=[226.02540-(222.01750+4.002603)] \mathrm{u} c ^{2}$ $=0.005297 \mathrm{u} c ^{2}$ But $1 \mathrm{u}=931.5 \mathrm{MeV} / \mathrm{c} ^{2}$ $\therefore Q=0.005297 \times 931.5 \approx 4.94 \mathrm{MeV}$ Kinetic energy of the $\alpha$-particle $=(\frac{\text { Mass number after decay }}{\text { Mass number before decay }}) \times Q$ $=\frac{222}{226} \times 4.94=4.85 \mathrm{MeV}$ Alpha particle decay of $({ } _{86} ^{220} \mathrm{Rn})$ is shown by the following nuclear reaction. ${ } _{86} ^{220} \mathrm{Rn} \longrightarrow{ } _{84} ^{216} \mathrm{Po}+{ } _{2} ^{4} \mathrm{He}$ It is given that: Mass of $({ } _{86} ^{220} \mathrm{Rn})=220.01137 \mathrm{u}$ Mass of $({ } ^{24}{ } ^{216} \mathrm{Po})=216.00189 \mathrm{u}$ $\therefore Q$-value $=[220.01137-(216.00189+4.00260)] \times 931.5$ $\approx 641 \mathrm{MeV}$ Kinetic energy of the $\alpha$-particle $=(\frac{220-4}{220}) \times 6.41$ $=6.29 \mathrm{MeV}$Show Answer
Answer The fission of ${ } _{26} ^{56} \mathrm{Fe}$ can be given as: $$
{ } _{13} ^{56} \mathrm{Fe} \longrightarrow 2{ } _{13} ^{28} \mathrm{Al}
$$ It is given that: Atomic mass of $m({ } _{26} ^{56} \mathrm{Fe})=55.93494 \mathrm{u}$ Atomic mass of $m({ } _{13} ^{28} \mathrm{Al})=27.98191 \mathrm{u}$ The $Q$-value of this nuclear reaction is given as: $$
\begin{aligned}
Q & =\left[m({ } _{26} ^{56} \mathrm{Fe})-2 m({ } _{13} ^{28} \mathrm{Al})\right] c ^{2} \
& =[55.93494-2 \times 27.98191] c ^{2} \
& =(-0.02888 c ^{2}) \mathrm{u}
\end{aligned}
$$ But $1 \mathrm{u}=931.5 \mathrm{MeV} / \mathrm{c} ^{2}$ $\therefore Q=-0.02888 \times 931.5=-26.902 \mathrm{MeV}$ The $Q$-value of the fission is negative. Therefore, the fission is not possible energetically. For an energetically-possible fission reaction, the $Q$-value must be positive.Show Answer
Answer Average energy released per fission of ${ } _{94} ^{239} \mathrm{Pu}, E _{a v}=180 \mathrm{MeV}$ Amount of pure ${ } _{94} \mathrm{Pu} ^{239}, m=1 \mathrm{~kg}=1000 \mathrm{~g}$ $\mathrm{N} _{\mathrm{A}}=$ Avogadro number $=6.023 \times 10 ^{23}$ Mass number of ${ } _{94} ^{239} \mathrm{Pu}=239 \mathrm{~g}$ 1 mole of ${ } _{94} \mathrm{Pu} ^{239}$ contains $\mathrm{N} _{\mathrm{A}}$ atoms. $\therefore m$ g of ${ } _{94} \mathrm{Pu} ^{239}$ contains $(\frac{\mathrm{N} _{\mathrm{A}}}{\text { Mass number }} \times m)$ atoms $=\frac{6.023 \times 10 ^{23}}{239} \times 1000=2.52 \times 10 ^{24}$ atoms $\therefore$ Total energy released during the fission of $1 \mathrm{~kg}$ of ${ } _{94} ^{239} \mathrm{Pu}$ is calculated as: $$
\begin{aligned}
E & =E _{\alpha v} \times 2.52 \times 10 ^{24} \
& =180 \times 2.52 \times 10 ^{24}=4.536 \times 10 ^{26} \mathrm{MeV}
\end{aligned}
$$ Hence, $4.536 \times 10 ^{26} \mathrm{MeV}$ is released if all the atoms in $1 \mathrm{~kg}$ of pure ${ } _{94} \mathrm{Pu} ^{239}$ undergo fission.Show Answer
$$ _{1} ^{2} \mathrm{H}+ _{1} ^{2} \mathrm{H} \rightarrow _{2} ^{3} \mathrm{He}+\mathrm{n}+3.27 \mathrm{MeV} $$
Answer The given fusion reaction is: ${ } _{1} ^{2} \mathrm{H}+{ } _{1} ^{2} \mathrm{H} \longrightarrow{ } _{2} ^{3} \mathrm{He}+\mathrm{n}+3.27 \mathrm{MeV}$ Amount of deuterium, $m=2 \mathrm{~kg}$ 1 mole, i.e., $2 \mathrm{~g}$ of deuterium contains $6.023 \times 10 ^{23}$ atoms. $\therefore 2.0 \mathrm{~kg}$ of deuterium contains $=\frac{6.023 \times 10 ^{23}}{2} \times 2000=6.023 \times 10 ^{26}$ atoms It can be inferred from the given reaction that when two atoms of deuterium fuse, 3.27 $\mathrm{MeV}$ energy is released. $\therefore$ Total energy per nucleus released in the fusion reaction: $$
\begin{aligned}
E & =\frac{3.27}{2} \times 6.023 \times 10 ^{26} \mathrm{MeV} \
& =\frac{3.27}{2} \times 6.023 \times 10 ^{26} \times 1.6 \times 10 ^{-19} \times 10 ^{6} \
& =1.576 \times 10 ^{14} \mathrm{~J}
\end{aligned}
$$ Power of the electric lamp, $P=100 \mathrm{~W}=100 \mathrm{~J} / \mathrm{s}$ Hence, the energy consumed by the lamp per second $=100 \mathrm{~J}$ The total time for which the electric lamp will glow is calculated as: $$
\begin{aligned}
& \frac{1.576 \times 10 ^{14}}{100} \mathrm{~s} \
& \frac{1.576 \times 10 ^{14}}{100 \times 60 \times 60 \times 24 \times 365} \approx 4.9 \times 10 ^{4} \text { years }
\end{aligned}
$$Show Answer
Answer When two deuterons collide head-on, the distance between their centres, $d$ is given as: Radius of $1 ^{\text {st }}$ deuteron + Radius of $2 ^{\text {nd }}$ deuteron Radius of a deuteron nucleus $=2 \mathrm{fm}=2 \times 10 ^{-15} \mathrm{~m}$ $\therefore d=2 \times 10 ^{-15}+2 \times 10 ^{-15}=4 \times 10 ^{-15} \mathrm{~m}$ Charge on a deuteron nucleus $=$ Charge on an electron $=e=1.6 \times 10 ^{-19} \mathrm{C}$ Potential energy of the two-deuteron system: $$
V=\frac{e ^{2}}{4 \pi \epsilon _{0} d}
$$ Where, $$
\epsilon _{0}=\text { Permittivity of free space }
$$ $$
\frac{1}{4 \pi \epsilon _{0}}=9 \times 10 ^{9} \mathrm{~N} \mathrm{~m} ^{2} \mathrm{C} ^{-2}
$$ $\therefore V=\frac{9 \times 10 ^{9} \times(1.6 \times 10 ^{-19}) ^{2}}{4 \times 10 ^{-15}} \mathrm{~J}$ $$
=\frac{9 \times 10 ^{9} \times(1.6 \times 10 ^{-19}) ^{2}}{4 \times 10 ^{-15} \times(1.6 \times 10 ^{-19})} \mathrm{eV}
$$ $$
=360 \mathrm{keV}
$$ Hence, the height of the potential barrier of the two-deuteron system is $360 \mathrm{keV}$.Show Answer
Show Answer
Answer
We have the expression for nuclear radius as:
$R=R _{0} A ^{1} \beta ^{3}$
Where,
$R _{0}=$ Constant.
$A=$ Mass number of the nucleus
Nuclear matter density, $\rho=\frac{\text { Mass of the nucleus }}{\text { Volume of the nucleus }}$
Let $m$ be the average mass of the nucleus.
Hence, mass of the nucleus $=m A$
$\therefore \rho=\frac{m A}{\frac{4}{3} \pi R ^{3}}=\frac{3 m A}{4 \pi(R _{0} A ^{\frac{1}{3}}) ^{3}}=\frac{3 m A}{4 \pi R _{0} ^{3} A}=\frac{3 m}{4 \pi R _{0} ^{3}}$
Hence, the nuclear matter density is independent of $A$. It is nearly constant.
