{"id":34904,"date":"2022-11-21T10:41:40","date_gmt":"2022-11-21T05:11:40","guid":{"rendered":"https:\/\/tsboardsolutions.com\/?p=34904"},"modified":"2022-11-23T16:18:57","modified_gmt":"2022-11-23T10:48:57","slug":"ts-inter-2nd-year-physics-notes-chapter-14","status":"publish","type":"post","link":"https:\/\/tsboardsolutions.com\/ts-inter-2nd-year-physics-notes-chapter-14\/","title":{"rendered":"TS Inter 2nd Year Physics Notes Chapter 14 Nuclei"},"content":{"rendered":"

Here students can locate TS Inter 2nd Year Physics Notes<\/a> 14th Lesson Nuclei to prepare for their exam.<\/p>\n

TS Inter 2nd Year Physics Notes 14th Lesson Nuclei<\/h2>\n

\u2192 Nearly 99.9% of mass of atom is concentrated in a small volume called Nucleus.<\/p>\n

\u2192 Radius of atom is nearly 10,000 times more than radius of nucleus.<\/p>\n

\u2192 Volume of nucleus is nearly 10-12<\/sup> times less than volume of atom.<\/p>\n

\u2192 Atomic mass unit (1u): 1 \/12th mass of 12<\/sup>6<\/sub>C atom is taken as “atomic mass unit”.
\n1.u = \\(\\frac{1.992647 \\times 10^{-26}}{12}\\) = 1.660539 x 10-27<\/sup><\/p>\n

Energy equivalent of 1u = 931.5 MeV.<\/p>\n

\u2192 Isotopes: The nuclei having the same atomic number (Z) but different mass number (A) are called “isotopes”. Ex: 8<\/sub>O16<\/sup>, 8<\/sub>O17<\/sup>, 8<\/sub>O18<\/sup>.<\/p>\n

\u2192 Isobars: The nuclei having the same mass number (A) but different atomic numbers (Z) are called “isobars”. Ex: 14<\/sup>6<\/sub>C, 14<\/sup>7<\/sub>N<\/p>\n

\u2192 Isotones : The nuclei having same neutron number (N) but different atomic number (Z) are called “isotones”. Ex: 80<\/sub>Hg198<\/sup>, 79<\/sub>197<\/sup>Au.<\/p>\n

\u2192 Isomers : Nuclei having the same atomic number (Z) and mass number (A) but with different nuclear properties such as radio-active decay and magnetic moments are called “isomers”.
\nEx: I35<\/sub>80<\/sup> Brm<\/sup>, 80<\/sup>35<\/sub>Brg<\/sup> . Here ‘m’ denotes metastable state and ‘g’ denotes ground state.<\/p>\n

\u2192 Positive charge of nucleus is due to protons.<\/p>\n

\u2192 Toted charge of electrons in an atom is (- Ze) and that of protons is (+ Ze). Where Z is atomic number.<\/p>\n

\u2192 Neutron is a chargeless particle. Mass of neutron and mass of proton are almost equal.<\/p>\n

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\u2192 A free neutron is unstable when it is outside the nucleus. Its mean life period is 1000 sec.<\/p>\n

\u2192 Inside nucleus neutron is stable.<\/p>\n

\u2192 Number of neutrons in an atom is (A – Z) where A is mass number and Z is “atomic number”.<\/p>\n

\u2192 Volume of nucleus is proportional to mass number V \u221d A (OR) \\(\\frac{4}{3}\\)\u03c0R3<\/sup> \u221d A \u21d2 R = R0<\/sub>A1\/3<\/sup>\u00a0where RQ is a constant. R0<\/sub> = 1.2 \u00d7 10-15<\/sup> m.<\/p>\n

\u2192 Density of nuclear matter is almost cons-tant. It is independent of mass number A.<\/p>\n

\u2192 Density of nuclear matter \u03c1n<\/sub> = 2.3 \u00d7 1017<\/sup> kg\/m3<\/sup>.<\/p>\n

\u2192 Einstein mass .energy equation: From theory of relativity mass is treated as another form of energy. Relation between mass and energy is E = mc2<\/sup>. Where c = Velocity of light = 3 \u00d7 108<\/sup> m\/s.<\/p>\n

\u2192 In a nuclear reaction Law of conservation of energy states that the initial energy and, final energy are equal provided the energy associated with mass is also taken into account.<\/p>\n

\u2192 Mass defect: In every nucleus the theore-tical mass (MT<\/sub>) is always less than practical mass (M). The difference of mass of nucleus and its constituents is known as “mass defect”. Mass defect \u0394m = [Zmp<\/sub> + (A – Z) mn<\/sub>] – M.<\/p>\n

\u2192 Binding energy : When a certain number of protons and neutrons are brought together to form a nucleus the certain amount of energy Eb<\/sub> is released.
\nThe energy released while forming a nucleus is called “Binding energy Eb<\/sub>“. Binding energy = \u0394mc2<\/sup>.
\nNote : We have to supply an amount of energy equals to Eb<\/sub> from outside to divide a nucleus into its constituents.<\/p>\n

\u2192 Nuclear force:<\/p>\n