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Questions and Answers
What is the electron configuration for sodium (Na)?
What is the electron configuration for sodium (Na)?
2,8,1
How many electrons can the p-sublevel hold?
How many electrons can the p-sublevel hold?
6 electrons
According to the Aufbau principle, how do electrons fill atomic orbitals?
According to the Aufbau principle, how do electrons fill atomic orbitals?
Electrons occupy the lowest available energy state first.
What distinguishes valence electrons from core electrons?
What distinguishes valence electrons from core electrons?
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What is the maximum number of electrons in the 4s sublevel?
What is the maximum number of electrons in the 4s sublevel?
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Which is filled first, the 4s or the 3d sublevel, and why?
Which is filled first, the 4s or the 3d sublevel, and why?
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List the electron configuration for neon (Ne).
List the electron configuration for neon (Ne).
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What is the total number of electrons in argon (Ar)?
What is the total number of electrons in argon (Ar)?
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How many orbitals are present in the d-sublevel?
How many orbitals are present in the d-sublevel?
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What is the significance of valence shells and electrons?
What is the significance of valence shells and electrons?
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What does the electronic configuration 1s2, 2s2, 2p6, 3s2, 3p6 indicate about the element?
What does the electronic configuration 1s2, 2s2, 2p6, 3s2, 3p6 indicate about the element?
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According to Hund's rule, how should electrons be distributed in degenerate orbitals?
According to Hund's rule, how should electrons be distributed in degenerate orbitals?
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Explain the Pauli Exclusion Principle with an example from the provided configurations.
Explain the Pauli Exclusion Principle with an example from the provided configurations.
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How is the electronic configuration of a cation formed based on the principal quantum number?
How is the electronic configuration of a cation formed based on the principal quantum number?
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What distinguishes the electron configuration of Cu (29) from that of Ni (28)?
What distinguishes the electron configuration of Cu (29) from that of Ni (28)?
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What is the electron configuration of Nd (60), and what does the notation [Xe] represent?
What is the electron configuration of Nd (60), and what does the notation [Xe] represent?
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Identify the relationship between the electronic configurations of Cl and Cl-.
Identify the relationship between the electronic configurations of Cl and Cl-.
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How do transition metals like V (23) differ in their electron configurations compared to main group elements?
How do transition metals like V (23) differ in their electron configurations compared to main group elements?
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What impact does the Hund’s rule have on the stability of an atom's electron configuration?
What impact does the Hund’s rule have on the stability of an atom's electron configuration?
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Study Notes
Electronic Configuration of Atoms
- Electronic configuration: Represents the number of electrons in each main energy level (shells) of an atom.
- The number of electrons in each shell determines the atom's reactivity and chemical properties.
- Aufbau Principle: Electrons fill the lowest available energy levels first during electronic configuration.
- Valence Shell: The outermost shell of an atom.
- Valence Electrons: Electrons occupying the valence shell, responsible for chemical bonding.
- s-sublevel: Holds a maximum of 2 electrons in 1 orbital.
- p-sublevel: Holds a maximum of 6 electrons in 3 orbitals (px, py, pz).
- d-sublevel: Holds a maximum of 10 electrons in 5 orbitals.
- f-sublevel: Holds a maximum of 14 electrons in 7 orbitals.
- 4s sublevel: Is lower in energy than the 3d sublevel and is filled first.
- Hund's Rule: When electrons occupy orbitals with equal energy, they fill them singly before pairing up.
- Pauli Exclusion Principle: No more than two electrons occupy an orbital with opposite spins.
- Cations: Positively charged ions formed by losing electrons from the valence shell, following the order np, ns, (n-1)d.
- Anions: Negatively charged ions formed by gaining electrons to achieve the electronic configuration of the next noble gas atom.
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Description
This quiz covers key concepts of electronic configuration in atoms, including the Aufbau Principle, valence shell, and the various sublevels. Understand how the arrangement of electrons affects an atom's reactivity and chemical properties. Test your knowledge on filling orders and rules governing electron placements.
