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Questions and Answers
What did Rutherford propose about the nucleus of an atom?
What did Rutherford propose about the nucleus of an atom?
Rutherford proposed that the nucleus contains most of the atom's mass and positive charge in a very small volume.
How did Rutherford describe the arrangement of electrons in his atomic model?
How did Rutherford describe the arrangement of electrons in his atomic model?
Rutherford described electrons as revolving around the nucleus in circular paths called orbits.
What force keeps the electrons and nucleus together in the Rutherford model?
What force keeps the electrons and nucleus together in the Rutherford model?
The electrons are held to the nucleus by a strong electrostatic force of attraction.
What limitation of the Rutherford atomic model was pointed out by Maxwell's theory?
What limitation of the Rutherford atomic model was pointed out by Maxwell's theory?
What was a significant drawback of the Rutherford atomic model regarding the electrons?
What was a significant drawback of the Rutherford atomic model regarding the electrons?
According to calculations related to Rutherford's model, how quickly would an electron collapse into the nucleus?
According to calculations related to Rutherford's model, how quickly would an electron collapse into the nucleus?
What did both Thomson's and Rutherford's atomic models fail to address?
What did both Thomson's and Rutherford's atomic models fail to address?
How did the early atomic models contribute to the development of quantum mechanics?
How did the early atomic models contribute to the development of quantum mechanics?
What is the relationship between atomic mass (A), atomic number (Z), and the number of neutrons (N)?
What is the relationship between atomic mass (A), atomic number (Z), and the number of neutrons (N)?
Define isotopes and give an example.
Define isotopes and give an example.
What distinguishes isotones from isotopes?
What distinguishes isotones from isotopes?
Explain what isobars are and provide an example.
Explain what isobars are and provide an example.
What is the primary role of the nuclear force in an atomic nucleus?
What is the primary role of the nuclear force in an atomic nucleus?
How does the strength of the nuclear force compare to other fundamental forces?
How does the strength of the nuclear force compare to other fundamental forces?
What are the three types of nucleon interactions mentioned in the context of nuclear force?
What are the three types of nucleon interactions mentioned in the context of nuclear force?
What does the term 'atomic number' (Z) represent in nuclear physics?
What does the term 'atomic number' (Z) represent in nuclear physics?
What property of nuclear force allows it to bind protons together despite their repulsive nature?
What property of nuclear force allows it to bind protons together despite their repulsive nature?
At what distance does the nuclear force become practically non-existent?
At what distance does the nuclear force become practically non-existent?
How does the nuclear force behave at distances less than 0.7 Fermi?
How does the nuclear force behave at distances less than 0.7 Fermi?
What are the two subatomic particles that comprise the nucleus of an atom?
What are the two subatomic particles that comprise the nucleus of an atom?
What are the two processes through which nuclear energy is released?
What are the two processes through which nuclear energy is released?
What role does the repulsive component of nuclear force play in the size of the nucleus?
What role does the repulsive component of nuclear force play in the size of the nucleus?
How does nuclear fusion differ from nuclear fission?
How does nuclear fusion differ from nuclear fission?
What effect does the Coulomb resistance have on the nuclear force?
What effect does the Coulomb resistance have on the nuclear force?
What is mass defect and how is it calculated?
What is mass defect and how is it calculated?
How does the concept of binding energy relate to mass defect?
How does the concept of binding energy relate to mass defect?
List two applications of nuclear technology in medicine.
List two applications of nuclear technology in medicine.
Explain the role of neutron activation analysis in scientific investigations.
Explain the role of neutron activation analysis in scientific investigations.
What is the significance of mass defect in nuclear physics?
What is the significance of mass defect in nuclear physics?
Identify one agricultural use of nuclear technology.
Identify one agricultural use of nuclear technology.
Describe a role of nuclear technology in engineering projects.
Describe a role of nuclear technology in engineering projects.
What types of particles does binding energy concern in a nuclear context?
What types of particles does binding energy concern in a nuclear context?
What is the mass defect of the helium nucleus based on the given information?
What is the mass defect of the helium nucleus based on the given information?
Calculate the binding energy of a helium nucleus in MeV.
Calculate the binding energy of a helium nucleus in MeV.
What is the binding energy per nucleon for a helium nucleus?
What is the binding energy per nucleon for a helium nucleus?
What is the mass defect of the Li⁷ nucleus given the provided data?
What is the mass defect of the Li⁷ nucleus given the provided data?
What is the binding energy of the Li⁷ nucleus in Joules?
What is the binding energy of the Li⁷ nucleus in Joules?
What is the frequency of the photon emitted when a Hydrogen atom transitions from the first excited state to the ground state?
What is the frequency of the photon emitted when a Hydrogen atom transitions from the first excited state to the ground state?
Identify the number of protons and neutrons in the Aluminum nucleus 27₁₃Al.
Identify the number of protons and neutrons in the Aluminum nucleus 27₁₃Al.
What is the energy of an electron in the first Bohr's orbit for a hydrogen atom?
What is the energy of an electron in the first Bohr's orbit for a hydrogen atom?
What is the energy of the photon emitted during the transition from n = 4 to n = 2 in a hydrogen atom?
What is the energy of the photon emitted during the transition from n = 4 to n = 2 in a hydrogen atom?
Calculate the wavelength of the Hα line resulting from the transition from n = 3 to n = 2.
Calculate the wavelength of the Hα line resulting from the transition from n = 3 to n = 2.
What is the radius of the first orbit of the hydrogen atom according to Bohr's model?
What is the radius of the first orbit of the hydrogen atom according to Bohr's model?
Determine the binding energy per nucleon for helium.
Determine the binding energy per nucleon for helium.
What is the frequency of the photon emitted when a hydrogen atom transitions from -15 eV to -3.4 eV?
What is the frequency of the photon emitted when a hydrogen atom transitions from -15 eV to -3.4 eV?
Calculate the mass defect of uranium using the data provided.
Calculate the mass defect of uranium using the data provided.
What is the second line wavelength of the Lyman series if the first line is at 1200 Å?
What is the second line wavelength of the Lyman series if the first line is at 1200 Å?
What is the binding energy of the iron nucleus in MeV?
What is the binding energy of the iron nucleus in MeV?
Flashcards
Rutherford Atomic Model
Rutherford Atomic Model
A model of the atom with a positively charged nucleus at the center, surrounded by negatively charged electrons orbiting in circular paths.
Nucleus (atom)
Nucleus (atom)
The small, dense, positively charged central part of an atom.
Electron Orbits
Electron Orbits
The circular paths followed by electrons around the nucleus, as described in the Rutherford model.
Atomic Stability Problem
Atomic Stability Problem
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Electromagnetic Radiation
Electromagnetic Radiation
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Limitations of Rutherford's Model
Limitations of Rutherford's Model
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Electron's energy loss
Electron's energy loss
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Maxwell's theory
Maxwell's theory
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Atomic Number (Z)
Atomic Number (Z)
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Atomic Mass (A)
Atomic Mass (A)
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Isotopes
Isotopes
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Isotones
Isotones
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Isobars
Isobars
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Nuclear Force
Nuclear Force
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Neutrons (N)
Neutrons (N)
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Nucleus
Nucleus
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Nuclear Force Attraction
Nuclear Force Attraction
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Nuclear Force Repulsion
Nuclear Force Repulsion
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Range of Nuclear Force
Range of Nuclear Force
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Nuclear Energy
Nuclear Energy
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Nuclear Fission
Nuclear Fission
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Nuclear Fusion
Nuclear Fusion
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Mass Defect
Mass Defect
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Binding Energy
Binding Energy
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Mass Defect Formula
Mass Defect Formula
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ΔM
ΔM
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MA
MA
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mp
mp
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mn
mn
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Z
Z
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Binding Energy per Nucleon
Binding Energy per Nucleon
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Helium Nucleus Mass Defect
Helium Nucleus Mass Defect
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Lithium-7 Nucleus Mass Defect
Lithium-7 Nucleus Mass Defect
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Mass Number
Mass Number
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Atomic Number
Atomic Number
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Bohr's Orbit
Bohr's Orbit
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Hydrogen atom's ground state energy
Hydrogen atom's ground state energy
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Photon energy during transition
Photon energy during transition
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Balmer series
Balmer series
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Lyman series
Lyman series
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Frequency of emitted photon
Frequency of emitted photon
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First Bohr orbit radius
First Bohr orbit radius
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Study Notes
Dalton's Atomic Theory
- All matter composed of atoms
- Atoms indivisible
- Each element consists of one type of atom
- Atoms of different elements have different masses
- Atoms combine in simple whole number ratios to form compounds
Thomson's Atomic Model
- Proposed in 1900
- Atoms composed of positive sphere with negatively charged electrons embedded
- Electrons much lighter than protons
- Atoms electrically neutral
Limitations of Thomson's Model
- Couldn't explain stability of atom
- Couldn't explain scattering of alpha particles
Rutherford's Atomic Model
- Experiment involved bombarding gold foil with alpha particles
- Most alpha particles passed straight through
- Some alpha particles deflected at large angles
- Nucleus is small, dense, positively charged, and contains most of the atom's mass
- Electrons orbit the nucleus
Limitations of Rutherford's Model
- Couldn't explain stability of atom (electrons should radiate energy and spiral into nucleus)
Bohr's Atomic Model
- Electrons orbit nucleus in specific energy levels (orbits)
- Atoms stable due to electrons fixed in fixed orbits
- Electrons gain or lose energy by moving between orbits
Limitations of Bohr's Model
- Violated Heisenberg Uncertainty Principle
- Poor spectral predictions for larger atoms
- Failed to explain Zeeman and Stark effects
Quantum Mechanical Model
- Treats electrons as waves
- Electrons don't orbit in fixed paths
- Probability of finding an electron in an area rather than a definite path
- Explains all aspects of atomic structure
Nucleus of an Atom
- Central region of an atom containing most of the mass
- Protons and neutrons (nucleons) in nucleus
- Atomic number (Z) = number of protons
- Mass number (A) = number of protons and neutrons
Atomic Mass (A)
- Sum of protons and neutrons in the nucleus
Isotopes
- Atoms of the same element with different numbers of neutrons, same atomic number, but different mass numbers
Isobars
- Atoms of different elements but with same mass number
Isotones
- Atoms with the same number of neutrons, but different atomic numbers
Nuclear Force
- Strong force binding protons and neutrons in the nucleus
- Overcomes electrostatic repulsion between protons at short range
- Repulsive at very short distances
Nuclear Energy
- Energy stored in the nucleus
- Released by nuclear fission (splitting) or fusion (combining)
- Used in nuclear power plants and weapons
Mass Defect
- Difference between actual atomic mass and sum of individual constituent masses
- Energy released in nuclear reactions is due to conversion of mass to energy
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