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Questions and Answers
What is the main difference between the Bohr model and Rutherford’s model of the atom?
What is the main difference between the Bohr model and Rutherford’s model of the atom?
What does the equation E=hv represent in the context of energy release in atoms?
What does the equation E=hv represent in the context of energy release in atoms?
How are energy levels in an atom typically spaced?
How are energy levels in an atom typically spaced?
Which statement best describes a characteristic of atomic orbitals?
Which statement best describes a characteristic of atomic orbitals?
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What is the significance of the Aufbau principle in electron configuration?
What is the significance of the Aufbau principle in electron configuration?
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How many orbitals are present in a p sublevel?
How many orbitals are present in a p sublevel?
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In which scenario will an atom likely emit red light?
In which scenario will an atom likely emit red light?
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Which rule states that each orbital in a sublevel must be singly occupied before any are doubly occupied?
Which rule states that each orbital in a sublevel must be singly occupied before any are doubly occupied?
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Study Notes
Chapter 5 Study Guide
- Be prepared to label a periodic table with its sublevels.
- Compare and contrast the Bohr model and Rutherford's model.
- Explain energy levels and how they are labeled.
- Explain why energy levels are not equally spaced.
- Explain what happens to an electron when an atom absorbs energy.
- Explain how energy is released by an atom, relating it to photons (E=hv).
- Explain light release by the Bohr model, using terms like energy level, ground state, excited state, and quantum.
- Explain when an atom is more likely to release red versus blue light ( Bohr model limitation: only applies to hydrogen atoms, not more complex atoms).
- Explain the quantum mechanical model and its invention.
- Describe the quantum mechanical model.
- Explain how probability is used in the quantum mechanical model and its relation to atomic orbitals.
- Define terms: atomic orbital, sublevel, energy level, s, p, and d orbitals.
- Explain the commonalities of orbitals within the same sublevel.
- Explain how energy levels affect orbitals.
- Identify and name s, p, and d orbitals.
- Write electron configurations.
- Compare and contrast the Rutherford, Bohr, and Quantum Mechanical Models.
- Identify how many orbitals are in a given sublevel (e.g., 2s, 5f, 6d).
- Organize sublevels from most to least energy.
- Identify elements based on electron configurations.
- Interpret Aufbau diagrams, standard electron configurations, and orbital filling diagrams.
- (Honors only) Know Aufbau rule, Hund's rule, and Pauli exclusion principle. Explain exceptions to these rules in Aufbau diagrams.
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Description
This study guide covers essential concepts from Chapter 5 of chemistry, focusing on atomic structure and models. Topics include the periodic table, Bohr and Rutherford models, energy levels, and the quantum mechanical model. Prepare to understand how these concepts relate to electron behavior and photon emission.
