Questions and Answers
Why do atoms emit light energy according to the Bohr model?
Because an electron has fallen to a lower energy state.
Why does arsenic produce a blue flame when heated, while calcium produces an orange-red flame?
Because the energy level difference between orbits is greater in arsenic than in calcium.
According to Schrodinger, the accuracy with which we can measure the momentum of an electron increases _______
none of the above
What can quantum numbers tell us?
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What is Hund's Rule?
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Which two elements have the same ground state electron configuration?
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The ______ subshell contains seven orbitals.
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What does the angular quantum number (l) designate?
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What does n = principal represent?
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What does ml represent?
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What does ms represent?
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What cannot exist?
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At max, an f-orbital can hold _______ electrons, a d-orbital can hold ______ electrons, and a p-orbital can hold _______ electrons.
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What is the element that has a valence configuration of 5s^2?
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How many quantum numbers are necessary to designate a particular electron in an atom?
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Which of the following is the correct quantum numbers to designate a p orbital?
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Discuss one example of Rutherford's model violating the laws of physics and how the Bohr model improved on Rutherford's model.
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Explain two major differences between the classical models of Bohr and Rutherford and the quantum mechanical view of the atom.
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Calculate the wavelength of an atom of silicon moving at a velocity of 3.0E4 m/s.
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How did the Bohr model explain the emission spectra produced by atoms?
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Which of the following is not true about the Bohr model of the atom?
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Which of the following best summarizes the quantum mechanical view of an electron?
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Electrons occupying the same energy level and orbital type share which of the following sets of quantum numbers and values?
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The _____ subshell contains 3 orbitals.
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The second energy shell can accommodate a maximum of _____ orbitals and ______ electrons.
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What information do electron configurations provide about an atom?
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What is the Aufbau rule?
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What are ground state rules?
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In a ground state cobalt atom, Co, the _____ subshell is partially filled.
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How many different principal quantum numbers can be found in the ground state electron configuration of oxygen?
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Explain why atoms were expected to emit continuous spectra of energy at all times and how the Bohr model of the atom explained the unexpected spectral lines produced by atoms.
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Discuss two faults of the Bohr model.
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Study Notes
Bohr Model and Light Emission
- Atoms emit light energy when electrons drop to lower energy states.
- Arsenic produces blue flames and calcium produces orange-red flames due to greater energy level differences in arsenic.
Quantum Mechanics Concepts
- Accuracy of momentum measurements for electrons is uncertain, with the response indicating non-applicability.
- Quantum numbers indicate the probable location of electrons and describe properties of orbitals.
Key Principles and Rules
- Hund's Rule states that orbitals of equal energy are singly occupied before being doubly occupied, maintaining consistent electron spin.
- No two elements can have the same ground state electron configuration.
- The f subshell has seven orbitals, while the p subshell has three orbitals.
Quantum Number Components
- Angular quantum number (l) dictates the shape of orbitals.
- Principal quantum number (n) designates energy level and distance from the nucleus.
- Magnetic quantum number (ml) shows orbital orientation, while spin quantum number (ms) indicates the direction of spin.
Electron Capacity in Orbitals
- Maximum electron capacities: f-orbital holds 14, d-orbital holds 10, and p-orbital holds 6 electrons.
Valence Configurations
- The element barium (Ba) has a valence configuration of 5s².
- Four quantum numbers are necessary to define a specific electron in an atom.
Quantum Number Designation
- The quantum numbers for a p orbital are designated as 2 (n), 1 (l), 1 (ml).
Rutherford and Bohr Models
- Rutherford's model violates Coulomb's law due to predictions that electrons would spiral into the nucleus.
- Bohr's model addresses these issues by establishing stable orbits where electrons do not radiate energy, emitting light only when transitioning between set energy levels.
Comparative Models of Atom
- The quantum mechanical model allows electrons to exhibit both wave-like and particle-like properties.
- It focuses on understanding the behavior of electrons collectively, rather than addressing specific electrons.
Emission Spectra Explanation
- Spectral lines result from electron transitions from higher to lower energy orbits.
- The Bohr model cannot adequately explain different spectra across elements.
Quantum Mechanical View
- Electrons are best described as exhibiting both wave and particle characteristics.
- Electrons within the same energy level and type share quantum numbers n and l.
Electron Configuration Characteristics
- Electron configurations reveal electron locations within an atom.
- Aufbau principle dictates that electrons fill the lowest energy levels first, while ground state rules align with this filling sequence and spin orientation.
Ground State of Cobalt and Oxygen
- Ground state cobalt (Co) has a partially filled 3d subshell.
- In its ground state, oxygen has two distinct principal quantum numbers.
Emission Spectra Expectations
- Early expectations suggested continuous spectra due to accelerating electrons drawing near the nucleus.
- Bohr's model countered this by proposing electrons reside in stable orbits, only emitting energy when transitioning between orbits.
Faults of the Bohr Model
- Bohr's model fails to explain the behavior of complex atoms beyond hydrogen.
- The model's assumption of stable orbits conflicts with the principle that electrons should continuously radiate energy.
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Test your knowledge on key chemistry concepts with these flashcards. Learn about atomic behavior, energy levels, and flame tests as explained by the Bohr model and other theories. Perfect for last-minute studying before your exam!