Podcast
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?
- Bohr's model includes protons and neutrons.
- Bohr's model explains energy levels while Rutherford's does not. (correct)
- Rutherford's model was the first to use quantum mechanics.
- Rutherford's model depicts electrons in fixed orbits.
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?
- The relationship between energy and frequency. (correct)
- The relationship between energy and wavelength.
- The relationship between energy and speed.
- The relationship between energy and mass.
How are energy levels in an atom typically spaced?
How are energy levels in an atom typically spaced?
- They are equally spaced regardless of the electron configuration.
- They decrease in spacing as they increase in energy.
- They are spaced based on the size of the atom.
- They are spaced according to the quantum mechanical model. (correct)
Which statement best describes a characteristic of atomic orbitals?
Which statement best describes a characteristic of atomic orbitals?
What is the significance of the Aufbau principle in electron configuration?
What is the significance of the Aufbau principle in electron configuration?
How many orbitals are present in a p sublevel?
How many orbitals are present in a p sublevel?
In which scenario will an atom likely emit red light?
In which scenario will an atom likely emit red light?
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?
Flashcards
Quantum Mechanical Model
Quantum Mechanical Model
A model that describes the arrangement of electrons in atoms, based on probability and the idea that electrons occupy specific regions of space called orbitals. It uses mathematical equations to predict the behavior of electrons.
Atomic Orbitals
Atomic Orbitals
Regions of space within an atom where electrons are most likely to be found. Each orbital can hold a maximum of two electrons.
Sublevels
Sublevels
A group of orbitals with similar energy levels and shapes. Within a sublevel, orbitals have the same energy.
Energy Levels
Energy Levels
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Pauli Exclusion Principle
Pauli Exclusion Principle
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Hund's Rule
Hund's Rule
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Aufbau Principle
Aufbau Principle
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Aufbau Diagram
Aufbau Diagram
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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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