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What is the significance of the concept of quantization in Bohr's atomic model?
What is the significance of the concept of quantization in Bohr's atomic model?
It means that the energy of the atom can only take on specific discrete values, not a continuous range of values.
What happens to the electron when it moves from a higher energy level to a lower energy level in the Bohr model?
What happens to the electron when it moves from a higher energy level to a lower energy level in the Bohr model?
Light is emitted.
What is the relationship between the energy level and the distance of the electron's orbit from the nucleus in the Bohr model?
What is the relationship between the energy level and the distance of the electron's orbit from the nucleus in the Bohr model?
The higher the energy level, the farther the orbit is from the nucleus.
What is the significance of the principal quantum number (n) in the Bohr model?
What is the significance of the principal quantum number (n) in the Bohr model?
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What is the state of the atom when the electron is in the first orbit?
What is the state of the atom when the electron is in the first orbit?
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What is the significance of the concept of stationary states in the Bohr model?
What is the significance of the concept of stationary states in the Bohr model?
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How does the Bohr model explain the structure of the atom when it undergoes energy transitions?
How does the Bohr model explain the structure of the atom when it undergoes energy transitions?
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What is the major idea behind Bohr's atomic model?
What is the major idea behind Bohr's atomic model?
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What is the reason for the electrical neutrality of an atom?
What is the reason for the electrical neutrality of an atom?
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Who proposed the model of the atom as a sphere of positive matter in which electrons are positioned by electrostatic forces?
Who proposed the model of the atom as a sphere of positive matter in which electrons are positioned by electrostatic forces?
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What is the main principle of Hund's rule in the arrangement of electrons in subshells?
What is the main principle of Hund's rule in the arrangement of electrons in subshells?
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What is the characteristic of the nucleus in Rutherford's model?
What is the characteristic of the nucleus in Rutherford's model?
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What is the dual nature of electron according to De Broglie's postulate and Heisenberg's uncertainty principle?
What is the dual nature of electron according to De Broglie's postulate and Heisenberg's uncertainty principle?
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What is the correct set of quantum numbers for the third electron of the F atom?
What is the correct set of quantum numbers for the third electron of the F atom?
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What is the result of an atom losing or gaining electrons in a chemical reaction?
What is the result of an atom losing or gaining electrons in a chemical reaction?
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What is the difference between a partial orbital diagram and a condensed electron configuration?
What is the difference between a partial orbital diagram and a condensed electron configuration?
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What is the significance of the number of protons in an atom?
What is the significance of the number of protons in an atom?
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What is the purpose of using the element symbol of the previous noble gas in square brackets in a condensed electron configuration?
What is the purpose of using the element symbol of the previous noble gas in square brackets in a condensed electron configuration?
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Why is the arrangement of electrons in (c) more acceptable than (a) and (b) according to Hund's rule?
Why is the arrangement of electrons in (c) more acceptable than (a) and (b) according to Hund's rule?
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What is the significance of the ms value in the set of quantum numbers for an electron?
What is the significance of the ms value in the set of quantum numbers for an electron?
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What is the purpose of using partial orbital diagrams?
What is the purpose of using partial orbital diagrams?
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Why is the electron configuration of Al written as [Ne]3s23p1 in condensed form?
Why is the electron configuration of Al written as [Ne]3s23p1 in condensed form?
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What is the purpose of the spin quantum number (m) in describing electrons in atoms?
What is the purpose of the spin quantum number (m) in describing electrons in atoms?
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What happens to the energy and size of an orbital as the principal quantum number (n) increases?
What happens to the energy and size of an orbital as the principal quantum number (n) increases?
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What is the relationship between the principal quantum number (n) and the angular momentum quantum number (l)?
What is the relationship between the principal quantum number (n) and the angular momentum quantum number (l)?
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How many orbital diagrams are associated with l = 2 (d orbitals)?
How many orbital diagrams are associated with l = 2 (d orbitals)?
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What is the range of values for the magnetic quantum number (ml) for a given value of l?
What is the range of values for the magnetic quantum number (ml) for a given value of l?
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What is the significance of the principal energy level (or shell) in the electron configuration of an atom?
What is the significance of the principal energy level (or shell) in the electron configuration of an atom?
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What is the total number of orbitals in an electron shell?
What is the total number of orbitals in an electron shell?
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What are the four quantum numbers for an electron in a 3p orbital?
What are the four quantum numbers for an electron in a 3p orbital?
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What is the Spin Quantum Number, ms, and what are its possible values?
What is the Spin Quantum Number, ms, and what are its possible values?
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How are electrons represented in an orbital diagram?
How are electrons represented in an orbital diagram?
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What is the maximum number of electrons that can reside in the principal level for which n = 3?
What is the maximum number of electrons that can reside in the principal level for which n = 3?
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Write the four quantum numbers for each of the eight electrons in the ground state of an oxygen atom.
Write the four quantum numbers for each of the eight electrons in the ground state of an oxygen atom.
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Study Notes
Atomic Structure
- An atom is electrically neutral because the number of protons are equal to the number of electrons.
- Atoms do not lose or gain protons in any chemical reaction, but they do lose or gain electrons to become ions.
Nuclear Atomic Model
- Thomson's model: proposed a model of the atom as a sphere of positive matter in which electrons are positioned by electrostatic forces.
- Rutherford's model: atoms have a positive charge concentrated in the nucleus (dense central core within an atom).
- Dual nature of electrons: electron energy is quantized, and electron is both particle and wave.
- De Broglie's postulate: electron has wave-like properties.
- Heisenberg's uncertainty principle: not possible to know the unlimited accuracy both the position and momentum of an electron.
Bohr's Atomic Model
- Bohr's model: energy of the atom is quantized, and the amount of energy in the atom is related to the electron's position in the atom.
- Postulates:
- The single electron in H atom moves around the nucleus in orbits or energy levels.
- The H atom has only certain energy levels, which are called stationary states.
- Each state is associated with a fixed circular orbit of the electron around the nucleus.
- The higher the energy level, the farther the orbit is from the nucleus.
- When the H electron is in the first orbit, the atom is in its lowest energy state, called the ground state.
Quantum Numbers
- Principal quantum number (n): describes the energy level of an electron.
- n can be any integer ≥ 1.
- The larger the value of n, the more energy the orbital has.
- The larger the value of n, the larger the orbital.
- Angular momentum quantum number (l): describes the shape of the orbital.
- l = 0, 1, 2, 3, … n-1.
- Shape of the orbital changes with l.
- Magnetic quantum number (ml): describes the orientation of the orbital.
- ml = -l, …., 0, ….
- The total number of orbitals is 1 + 3 + 5 = 9.
- Spin quantum number (ms): describes the spin of an electron.
- ms = +½ or −½.
- Spin up or spin down.
Electron Configurations and Orbital Diagrams
- Electron spin: a fundamental property of all electrons.
- Orbital diagrams: use a square to represent each orbital and a half-arrow to represent each electron in the orbital.
- By convention, a half-arrow pointing up is used to represent an electron in an orbital with spin up.
- Spins must cancel in an orbital with 2 electrons (paired e-).
Electronic Configurations
- Partial orbital diagrams: show only the highest energy sublevels being filled.
- Condensed electron configurations: have the element symbol of the previous noble gas in square brackets.
- Hund's rule: the most stable arrangement of electrons in subshells is the one with the greatest number of parallel spins.
Checkpoints
- Checkpoint 3: write the four quantum numbers for an electron in a 3p orbital.
- Checkpoint 4: the maximum number of electrons that can reside in the orbitals is 2 × 9 = 18.
- Checkpoint 5: write the four quantum numbers for each of the eight electrons in the ground state of an oxygen atom.
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Description
This quiz is about Hund's rule and electron configuration in atoms, including parallel spins and subshell arrangements.