Final answer:
In determining configuration for hydrogen bonding, the hydrogen atoms share electrons to achieve stability, resulting in a covalent bond with antiparallel spins. Examples include the stable H₂ molecule and the more complex H₂O angle due to electron pair repulsion. Understanding orbital energy levels is essential for determining electron configurations.
Step-by-step explanation:
When determining configuration, particularly with hydrogen, it is essential to understand the electron arrangements and the types of bonds that may form. Hydrogen atoms have one electron each and can share electrons to achieve a stable configuration similar to that of helium. Each hydrogen atom’s electron configuration is described as 1s¹, indicating that its single electron occupies the 1s orbital.
In a molecule such as H₂, the two hydrogen atoms bond covalently, allowing them to have a space-symmetric electron configuration with antiparallel spins, which is energetically favorable. This bond results in a stable molecule with an equilibrium separation of about 0.074 nm and a binding energy of 4.52 eV. The H₂ molecule is a simple example of this sharing, with each atom contributing one electron to the bond.
The behavior of electrons can also be considered in more complex molecules, such as water (H₂O), where the electron pairs form a distorted tetrahedral arrangement due to repulsion, resulting in a bent shape with a 104.5° bond angle. This contrast with a linear molecule like the HBeH is because beryllium only has two electrons to bond with the two electrons from hydrogen.
Understanding the energy order of orbitals (1s, 2s, 2p, 3s, 3p, etc.) and their filling sequences is crucial when determining electron configurations for any atom. The periodic table provides guidance on constructing these configurations by building upon the configuration of hydrogen as the simplest element.