Table of contents

1. Intro to General Chemistry3h 48m
2. Atoms & Elements4h 16m
3. Chemical Reactions4h 10m
4. BONUS: Lab Techniques and Procedures1h 38m
5. BONUS: Mathematical Operations and Functions48m
6. Chemical Quantities & Aqueous Reactions3h 53m
7. Gases3h 49m
8. Thermochemistry2h 37m
9. Quantum Mechanics2h 58m
10. Periodic Properties of the Elements3h 9m
11. Bonding & Molecular Structure3h 29m
12. Molecular Shapes & Valence Bond Theory1h 57m
13. Liquids, Solids & Intermolecular Forces2h 23m
14. Solutions3h 1m
15. Chemical Kinetics2h 53m
16. Chemical Equilibrium2h 29m
17. Acid and Base Equilibrium5h 1m
18. Aqueous Equilibrium4h 47m
19. Chemical Thermodynamics1h 50m
20. Electrochemistry2h 42m
21. Nuclear Chemistry2h 36m
22. Organic Chemistry5h 7m
23. Chemistry of the Nonmetals2h 39m
24. Transition Metals and Coordination Compounds3h 16m

21. Nuclear Chemistry

Nuclear Binding Energy

General Chemistry

21. Nuclear Chemistry

Nuclear Binding Energy

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Multiple Choice

Calculate the total binding energy (in MeV) for the isotope 127I, given that the atomic mass is 126.90447 u and the atomic number is 53.

1048 MeV

980 MeV

1150 MeV

1120 MeV

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Verified step by step guidance

Understand the concept of binding energy: Binding energy is the energy required to disassemble a nucleus into its individual protons and neutrons. It is a measure of the stability of a nucleus.

Calculate the mass defect: The mass defect is the difference between the sum of the masses of the protons and neutrons and the actual mass of the nucleus. Use the formula: \( \text{Mass defect} = (Z \times m_p + N \times m_n) - m_{\text{nucleus}} \), where \( Z \) is the atomic number, \( m_p \) is the mass of a proton, \( N \) is the number of neutrons, \( m_n \) is the mass of a neutron, and \( m_{\text{nucleus}} \) is the atomic mass of the isotope.

Determine the number of neutrons: For the isotope \( ^{127}\text{I} \), the number of neutrons \( N \) can be calculated using \( N = A - Z \), where \( A \) is the mass number (127 for iodine) and \( Z \) is the atomic number (53 for iodine).

Convert the mass defect to energy: Use Einstein's equation \( E = \Delta m \times c^2 \) to convert the mass defect from atomic mass units (u) to energy in MeV. The conversion factor is \( 1 \text{ u} = 931.5 \text{ MeV/c}^2 \).

Calculate the total binding energy: The total binding energy is the energy equivalent of the mass defect calculated in the previous step. This will give you the binding energy in MeV for the isotope \( ^{127}\text{I} \).