Intro to Quantum Mechanics I

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S orbital

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Intro to Quantum Mechanics I

Definition

An s orbital is a type of atomic orbital that is spherical in shape and can hold a maximum of two electrons with opposite spins. It represents the lowest energy level in any given principal quantum number and plays a crucial role in the structure of atoms and the arrangement of electrons around the nucleus.

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5 Must Know Facts For Your Next Test

  1. The s orbital can exist in different energy levels corresponding to different principal quantum numbers (n = 1, 2, 3, ...), with each energy level having one s orbital.
  2. The shape of the s orbital remains consistent regardless of its energy level, always maintaining a spherical symmetry around the nucleus.
  3. In multi-electron atoms, the s orbitals are filled before the higher-energy p, d, and f orbitals due to their lower energy state.
  4. The first electron shell (n=1) contains only one s orbital, while the second shell (n=2) contains one 2s orbital as well as three p orbitals.
  5. In terms of energy, the s orbitals are generally lower in energy than p, d, and f orbitals at the same principal quantum number.

Review Questions

  • How do s orbitals differ from other types of atomic orbitals in terms of shape and electron capacity?
    • S orbitals are unique because they have a spherical shape, unlike p orbitals that have a dumbbell shape. Each s orbital can hold up to two electrons with opposite spins, which is a common feature among all atomic orbitals. However, the defining characteristic of s orbitals is their lower energy level compared to p, d, and f orbitals at the same principal quantum number.
  • Discuss how the arrangement of electrons in s orbitals affects an atom's overall electron configuration.
    • The arrangement of electrons in s orbitals significantly influences an atom's electron configuration by determining how electrons fill available energy levels. Since s orbitals are filled first due to their lower energy state, they establish a foundational layer for additional electron filling in p, d, and f orbitals. This initial filling pattern affects chemical reactivity and bonding characteristics of elements.
  • Evaluate the implications of the Pauli Exclusion Principle on the filling of s orbitals within multi-electron atoms.
    • The Pauli Exclusion Principle ensures that no two electrons can occupy the same quantum state within an atom. This principle means that when filling s orbitals in multi-electron atoms, each orbital can contain a maximum of two electrons with opposite spins. Consequently, this restriction influences how electrons fill available energy levels and contributes to the overall stability and chemical behavior of the atom.
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