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Questions and Answers
What does the Aufbau principle describe in relation to electron configurations?
What does the Aufbau principle describe in relation to electron configurations?
How are unpaired electrons represented in orbital diagrams?
How are unpaired electrons represented in orbital diagrams?
Which rule states that electrons must occupy each orbital singly before pairing?
Which rule states that electrons must occupy each orbital singly before pairing?
What is represented by the quantum numbers of an electron?
What is represented by the quantum numbers of an electron?
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What is the significance of degenerate orbitals within a subshell?
What is the significance of degenerate orbitals within a subshell?
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Which of the following does NOT describe the quantum model of the atom?
Which of the following does NOT describe the quantum model of the atom?
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In which part of the periodic table can the energies of subshells be determined?
In which part of the periodic table can the energies of subshells be determined?
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What is the highest energy occupied orbital in the ground state electron configuration for antimony (Sb)?
What is the highest energy occupied orbital in the ground state electron configuration for antimony (Sb)?
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How many of the electrons in the ground-state electron configuration for antimony (Sb) occupy s orbitals?
How many of the electrons in the ground-state electron configuration for antimony (Sb) occupy s orbitals?
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How many unpaired electrons are in the ground state electron configuration for an iron atom?
How many unpaired electrons are in the ground state electron configuration for an iron atom?
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How many unpaired electrons are in the ground state electron configuration for Fe3+?
How many unpaired electrons are in the ground state electron configuration for Fe3+?
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What type of ion is formed when an atom gains one or more electrons?
What type of ion is formed when an atom gains one or more electrons?
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Which of the following statements about core electrons is true?
Which of the following statements about core electrons is true?
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Which subshell's electrons are removed first when forming cations from s- and p-block elements?
Which subshell's electrons are removed first when forming cations from s- and p-block elements?
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What notation is used to represent an abbreviated electron configuration?
What notation is used to represent an abbreviated electron configuration?
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What determines the principal quantum number for s and p block elements?
What determines the principal quantum number for s and p block elements?
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In which order do electrons fill orbitals according to the Aufbau principle?
In which order do electrons fill orbitals according to the Aufbau principle?
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How many electrons can occupy a single orbital?
How many electrons can occupy a single orbital?
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What is the correct electron configuration for a beryllium atom with an atomic number of 4?
What is the correct electron configuration for a beryllium atom with an atomic number of 4?
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When a violation of the Aufbau principle occurs during electron assembly, what is indicated?
When a violation of the Aufbau principle occurs during electron assembly, what is indicated?
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What happens when you attempt to place more than two electrons in a single orbital?
What happens when you attempt to place more than two electrons in a single orbital?
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What characterizes the 2p and 3p orbitals in terms of energy?
What characterizes the 2p and 3p orbitals in terms of energy?
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What is the significance of the Lewis valence electron dot structure in electron assembly?
What is the significance of the Lewis valence electron dot structure in electron assembly?
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Study Notes
Tip of the Day
- Keep track of questions while reviewing class material.
- Create a dedicated "questions page" in a notebook or using sticky notes.
Chapter Eight: The Quantum Model of the Atom (CHEM 1211K)
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Objectives:
- Describe and apply the dual nature of light.
- Calculate energy, frequency, or wavelength of a sample of light.
- Use the Bohr model to explain light emission and absorption in gaseous atoms.
- Calculate the energy or wavelength of a specific electronic transition in a hydrogen atom.
- Use quantum numbers to characterize the energies, spatial distributions, and spins of atomic electrons.
- Visualize and describe spatial distributions and energies of atomic electrons using the quantum model.
- Sketch electronic energy levels of an atom.
- Add electrons to atomic orbital energy diagrams.
- Determine electron configurations for elements using shells, subshells, and orbitals.
Orbital Diagrams (8.6)
- Electrons are represented by arrows pointing up or down to indicate spin (↑ ms = ½, ↓ ms = -½ ).
- Aufbau principle: Fill orbitals starting with the lowest energy level and moving up.
- Hund's rule: Maximize total spin. Fill each orbital in a subshell singly before pairing electrons. (e.g., in a 2p subshell, fill each of the three 2p orbitals with one electron before pairing them)
In-Class Question 1
- A d subshell containing 7 electrons has 3 unpaired electrons.
Electron Configurations (8.7)
- Electron configuration shows the orbitals electrons occupy in an atom.
- Examples of electron configurations are given for N and Ne.
Orbital Diagrams (8.6)
- Energy-level diagrams show relative energies of subshells.
- Orbitals within a subshell are degenerate (same energy).
Electron Configurations (8.7)
- s and p block elements: n = row number.
- d block elements: n = row number - 1.
- f block elements: n = row number - 2.
Electron Arrangement App (Figure 8.27)
- There is an interactive diagram for visualizing and understanding electron configurations.
In-Class Question 2
- The highest energy occupied orbital for antimony (Sb) is 5p.
In-Class Question 3
- Number of electrons in s orbitals for antimony (Sb) = 10.
Electron Configurations (8.7)
- Use noble gas notation for abbreviated electron configurations, showing the filled inner shells in brackets.
Electron Configurations (8.7)
- Core electrons are inner electrons close to the nucleus, with very low energy, and unaffected by chemical processes.
- Valence electrons are outer electrons shown when using noble gas shorthand notation. These are important in chemical properties.
Electron Configurations (8.7)
- Cations form when atoms lose electrons.
- Most common s and p block cations have noble gas configurations.
Electron Configurations (8.7)
- Atoms lose highest-energy electrons first.
- For s and p block atoms, this is the highest energy s or p electron. Electrons are removed starting with those in the highest energy s or p levels first.
- In d block atoms, s electrons are removed before d electrons though in this case it's not perfectly general and d electrons can be removed before s electrons.
Electron Configurations (8.7)
- Anions form when atoms gain electrons.
- Most common s and p block anions have noble gas configurations.
In-Class Question 4
- An iron (Fe) atom has 4 unpaired electrons in its ground state.
In-Class Question 5
- A Fe³⁺ ion has 5 unpaired electrons.
In-Class Question 6
- K⁺ is the species that cannot have the abbreviated electron configuration [Kr].
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Description
Dive into Chapter Eight of CHEM 1211K, where you'll explore the quantum model of the atom. This quiz covers light's dual nature, energy calculations, and electron configurations. Test your understanding of atomic theories and visualizations with this essential review.
