Physics 102 Atomic And Nuclear Physics Exercises Complete

Phy 102 Atomic And Nuclear Physics Exercisescomplete The Following Ex

Complete the following exercises. 1. Rank the following in order of increased size? A. Proton B. Nucleus C. Electron D. Atom 2. Match the following terms: 1. Mass number 2. Isotopes 3. Nitrogen 4. Atomic number A. The number of protons in the nucleus of an atom. B. The number of protons and neutrons in the nucleus of an atom. C. The name of the element with atomic number 7. D. Atoms with the same number of protons, but different number of neutrons. 3. Your friend says your body is made up of more than 99.9999% empty space. What do you think? 4. An isotope has 46 electrons, 60 neutrons, and 46 protons. Name the isotope. 5. Find the approximate atomic mass of a water molecule (H₂O). Give your answer in atomic mass units rounded to the nearest whole number. 6. Find the approximate atomic mass of carbon dioxide. Give your answer in atomic mass units rounded to the nearest whole number. 7. Consider chlorine-37. a. How many protons are there in the nucleus of Cl-37? b. How many neutrons are there in the nucleus of Cl-37? 8. Why is it impossible to see an individual atom in an optical microscope? 9. Compare alpha, beta, and gamma radiation. 10. Your friend says the helium in your birthday helium balloon comes from radioactive decays. What is your response? 11. Radium-214 decays in an alpha decay. a. What is the mass number of the daughter isotope? b. What is the atomic number of the daughter isotope? c. What element is the daughter product? 12. Iodine-131 has a half-life of 8 days. How many days will it take before 32mg of Iodine-131 has decayed to 1mg? 13. Carbon-14 has a half-life of 5,730 years. If an archaeological sample has only one-fourth of the radioactivity of a similar sample from today, how old is the archaeological sample? Give your answer in years. 14. Can the Carbon-14 isotope be used to date a stone tablet? Explain your answer. 15. Is it feasible to make a car engine powered by nuclear fission? How can energy from nuclear fission be used to power cars indirectly? The remaining questions are multiple-choice questions: 16. Consider an atom. Which contributes most to the size of the atom? A. The electrons B. The neutrons C. The protons D. Both the neutrons and the protons 17. Consider an atom. Which contributes most to the mass of the atom? A. The electrons B. The neutrons C. The protons D. Both the neutrons and the protons 18. What is the name of the center of the atom? A. Nucleus B. Protons C. Neutrons D. Electrons E. Ions 19. What makes an element distinct? A. The number of electrons B. The number of neutrons C. The number of protons D. The number of ions E. The number of nucleons 20. What is different between two isotopes of the same element? A. The number of electrons B. The number of neutrons C. The number of protons D. The number of ions E. The number of nucleons 21. When does a nuclear fission reaction occur? A. When a nucleus is cut in two using a really sharp knife. B. When two nuclei collide and combine to one. C. When a large nucleus spontaneously is divided for no apparent reason. D. When the electric forces within the nucleus are stronger than the nuclear forces. 22. Which processes release the energy in the sun? A. Combustion reactions B. Gravitational forces C. Fusion processes D. Fission processes E. Electrical discharges 23. Which processes release the energy in the nuclear reactors used in power plants? A. Combustion reactions B. Gravitational forces C. Fusion processes D. Fission processes E. Electrical discharges 24. Where does the energy released in nuclear reactions come from? A. The mass of the fuel B. Water C. The sun D. The Earth

Paper For Above instruction

Atomic and nuclear physics are fundamental branches of physics that explore the structure of atoms and the processes involving nuclear reactions. These concepts are vital for understanding natural phenomena, medical applications, energy production, and more. This comprehensive analysis addresses key concepts such as atomic structure, isotopes, nuclear decay, radiation types, and practical implications in energy and dating techniques.

1. Relative Sizes of Atomic Components

The size hierarchy of atomic constituents begins with the electron, which is extremely small compared to the atom itself. Electrons are subatomic particles with negligible size, but they define the electron cloud surrounding the nucleus. The nucleus, composed of protons and neutrons, is significantly smaller in size compared to the entire atom. Protons and neutrons are roughly spherical, but their combined size is dwarfed by the electron cloud. Therefore, in order of increasing size: A proton and B neutron (similar size), C electron, and D atom, with the atom being the largest due to the electron cloud surrounding the nucleus.

2. Matching Terms: Atomic Concepts

Mass number (2, B) represents the total number of protons and neutrons within the nucleus, providing the mass's approximate scale. Isotopes (4, D) are atoms sharing the same number of protons but differing in the number of neutrons, which affects their mass. Nitrogen (3, C) refers to the chemical element with atomic number 7, characterized by 7 protons. Atomic number (1, A) specifically indicates the number of protons in an atom's nucleus, defining the element's identity.

3. The Structure of the Atom and Human Body Composition

The assertion by the friend that the human body is over 99.9999% empty space is largely metaphorical. While atomic nuclei occupy minuscule volume compared to the electron cloud, most of the atom's volume is empty space. Nonetheless, this space is filled with the electron cloud that underpins chemical bonds. The human body, composed of countless atoms, therefore contains predominantly empty space, but the forces within this space are responsible for its solidity and structure.

4. Identifying an Isotope

This isotope has 46 electrons, 46 protons, and 60 neutrons. Since the number of protons equals the atomic number, it is element palladium (Pd). The isotope's mass number is the sum of protons and neutrons: 46 + 60 = 106. Thus, it is Pd-106.

5. Atomic Mass of Water (H₂O)

The atomic masses are approximately 1 unit for hydrogen and 16 units for oxygen. Therefore, the water molecule's atomic mass is 2(1) + 16 = 18 atomic mass units, rounded to the nearest whole number: 18.

6. Atomic Mass of Carbon Dioxide (CO₂)

Carbon has an atomic mass of about 12, and oxygen about 16. Calculating: 12 + 2(16) = 44. Rounded, the atomic mass of CO₂ is approximately 44 amu.

7. Chlorine-37 Characteristics

a. The number of protons in Cl-37 is 17, which is the atomic number of chlorine.

b. The number of neutrons is the difference between mass number and atomic number: 37 - 17 = 20 neutrons.

8. Visibility of Individual Atoms

Optical microscopes rely on visible light, which has a wavelength much larger than an atom (~0.2 nanometers). Therefore, individual atoms are too small to be resolved with visible light, necessitating tools like electron microscopes that use electron beams with much shorter wavelengths.

9. Comparing Radiation Types

Alpha radiation consists of helium nuclei; beta consists of high-energy electrons or positrons; gamma radiation is high-energy electromagnetic radiation. Alpha particles have low penetration but high ionization, beta particles penetrate further with moderate ionization, and gamma rays have high penetration with minimal ionization.

10. Helium from Radioactive Decay

The helium gas in balloons primarily originates from natural sources such as the decay of certain radioactive isotopes in the Earth's crust, especially uranium and thorium decay chains, rather than human-produced radioactive decay. Thus, the helium in balloons is not directly from decay processes but from natural extraction processes.

11. Decay of Radium-214

a. The mass number of the daughter isotope is 214 - 4 = 210, since alpha decay reduces the mass number by 4.

b. The atomic number decreases by 2 in alpha decay: 88 - 2 = 86.

c. The element with atomic number 86 is radon (Rn).

12. Decay Calculation for Iodine-131

Starting with 8 days for one half-life, the decay from 32 mg to 1 mg involves three half-lives (since 32 → 16 → 8 → 4 → 2 → 1).

So, the total is 8 days × 3 = 24 days.

13. Age of Archaeological Sample with Carbon-14

Since the sample has one-fourth of its original radioactivity, it has undergone two half-lives (because after one half-life it would be half, after two half-lives it would be quarter). Multiplying two half-lives by 5730 years per half-life: 2 × 5730 = 11,460 years.

14. Applicability of Carbon-14 Dating to Stone Tablets

Carbon-14 dating is effective for organic materials but not for inorganic stone materials. Therefore, it cannot directly date stone tablets unless they contain organic residues. Alternative methods, such as thermoluminescence, are used for inorganic artifacts.

15. Nuclear Fission for Car Engines

In theory, nuclear fission could power an engine indirectly through nuclear reactors generating electricity, which then powers electric motors. Direct fission-powered engines are impractical due to safety, shielding, and engineering complexities. Use of nuclear energy in transportation is primarily via nuclear-powered ships and potential future nuclear electric vehicles.

Multiple Choice Questions

16. Contributing to the size of the atom

A. The electrons

17. Contributing most to the mass of the atom

D. Both the neutrons and the protons

18. The center of the atom

A. Nucleus

19. What makes an element distinct

C. The number of protons

20. Difference between isotopes of same element

B. The number of neutrons

21. When does nuclear fission occur

C. When a large nucleus spontaneously is divided for no apparent reason.

22. Processes that release energy in the Sun

C. Fusion processes

23. Processes in nuclear power plants

D. Fission processes

24. Source of energy in nuclear reactions

A. The mass of the fuel

References

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