Electronic Configuration of Atoms
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Questions and Answers

What is the electron configuration for sodium (Na)?

2,8,1

How many electrons can the p-sublevel hold?

6 electrons

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?

<p>Valence electrons are in the outermost shell; core electrons are in inner shells.</p> Signup and view all the answers

What is the maximum number of electrons in the 4s sublevel?

<p>2 electrons</p> Signup and view all the answers

Which is filled first, the 4s or the 3d sublevel, and why?

<p>The 4s sublevel is filled first because it is lower in energy.</p> Signup and view all the answers

List the electron configuration for neon (Ne).

<p>2,8</p> Signup and view all the answers

What is the total number of electrons in argon (Ar)?

<p>18 electrons</p> Signup and view all the answers

How many orbitals are present in the d-sublevel?

<p>5 orbitals</p> Signup and view all the answers

What is the significance of valence shells and electrons?

<p>They determine an atom's chemical properties and bonding behavior.</p> Signup and view all the answers

What does the electronic configuration 1s2, 2s2, 2p6, 3s2, 3p6 indicate about the element?

<p>This configuration indicates that the element has a total of 18 electrons, which corresponds to the element Argon (Ar).</p> Signup and view all the answers

According to Hund's rule, how should electrons be distributed in degenerate orbitals?

<p>Electrons should occupy each degenerate orbital singly before pairing up in orbitals.</p> Signup and view all the answers

Explain the Pauli Exclusion Principle with an example from the provided configurations.

<p>The Pauli Exclusion Principle states that no two electrons can occupy the same orbital with the same spin; for instance, 1s2 indicates that two electrons fill the 1s orbital with opposite spins.</p> Signup and view all the answers

How is the electronic configuration of a cation formed based on the principal quantum number?

<p>Electrons are removed from the outermost shell in the order of np, ns, followed by (n-1)d orbitals.</p> Signup and view all the answers

What distinguishes the electron configuration of Cu (29) from that of Ni (28)?

<p>Cu has an electron configuration of 1s2, 2s2, 2p6, 3s2, 3p6, 4s1, 3d10, while Ni is 1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d8.</p> Signup and view all the answers

What is the electron configuration of Nd (60), and what does the notation [Xe] represent?

<p>Nd has the configuration [Xe] 4f4, 6s2, indicating it has 4 f electrons and 2 s electrons in the 6th shell, with [Xe] signifying the core electron configuration of Xenon.</p> Signup and view all the answers

Identify the relationship between the electronic configurations of Cl and Cl-.

<p>Cl has the configuration 1s2, 2s2, 2p6, 3s2, 3p5, while Cl- is 1s2, 2s2, 2p6, 3s2, 3p6, indicating Cl- has gained one electron.</p> Signup and view all the answers

How do transition metals like V (23) differ in their electron configurations compared to main group elements?

<p>Transition metals like V have partially filled d orbitals, with configuration 1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d3, affecting their chemical properties.</p> Signup and view all the answers

What impact does the Hund’s rule have on the stability of an atom's electron configuration?

<p>Following Hund's rule leads to a more stable configuration as it minimizes electron repulsion by preventing pairing in degenerate orbitals until necessary.</p> Signup and view all the answers

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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PF1009 2024 4 Electronic Configuration of Atoms PDF

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.

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