S orbital

Definition

An s orbital is a type of atomic orbital that has a spherical shape and can hold a maximum of two electrons with opposite spins. These orbitals are the lowest energy level and are found in all electron shells, playing a fundamental role in the structure of atoms, particularly in the hydrogen atom where they house the electron closest to the nucleus.

5 Must Know Facts For Your Next Test

1. The s orbital is designated by the letter 's' which stands for 'sharp,' reflecting its early classification based on spectral lines.
2. There is one s orbital in each electron shell, starting from the first shell (n=1) and increasing as you move to higher energy levels.
3. The spherical shape of the s orbital means that the probability of finding an electron is uniform in all directions around the nucleus.
4. In multi-electron atoms, s orbitals are filled before p, d, and f orbitals according to the Aufbau principle, which dictates the order of filling based on increasing energy.
5. The maximum capacity of an s orbital is two electrons, which must have opposite spins due to the Pauli exclusion principle.

Review Questions

• How does the shape of the s orbital affect the distribution of electrons around the nucleus?
  • The spherical shape of the s orbital creates a uniform probability distribution for finding an electron at varying distances from the nucleus. This means that there is no preferred direction for locating the electron within this space; instead, it has an equal likelihood of being found anywhere at a given distance from the nucleus. This characteristic is crucial for understanding how atoms interact with one another during chemical bonding.
• Compare and contrast s orbitals with p orbitals regarding their shapes and electron capacity.
  • S orbitals have a spherical shape and can hold a maximum of two electrons, while p orbitals have a dumbbell shape and can hold up to six electrons across three different orientations. While both types of orbitals are essential for electron configurations in atoms, s orbitals are present in every energy level starting from n=1, whereas p orbitals begin to appear from n=2 onward. This difference influences how elements bond and their overall chemical properties.
• Evaluate the significance of the s orbital in determining the chemical behavior of hydrogen compared to heavier elements.
  • The s orbital is critical in understanding hydrogen's chemical behavior because it holds its single electron closest to the nucleus, making hydrogen highly reactive and capable of forming bonds. In heavier elements, while they also possess s orbitals, these electrons experience greater shielding from inner electrons, resulting in different reactivities and bonding characteristics. This distinction highlights how electron configuration influences both individual elemental properties and broader trends across the periodic table.

Related terms

Atomic orbital: A mathematical function that describes the wave-like behavior of electrons in an atom, defining regions in space where electrons are likely to be found.

Electron configuration: The arrangement of electrons in an atom's orbitals, which follows specific rules like the Aufbau principle and Hund's rule to determine the distribution of electrons.

Quantum numbers: A set of four numbers that describe the unique quantum state of an electron in an atom, including its energy level, shape, orientation, and spin.