Hydrogen fluoride HF is a diatomic molecule consisting of one hydrogen H atom and one fluorine F atom. To determine its electronic configuration and molecular structure, we can use quantum mechanics principles, specifically molecular orbital theory.First, let's look at the electronic configuration of the individual atoms:Hydrogen H has 1 electron: 1sFluorine F has 9 electrons: 1s 2s 2pWhen these two atoms form a covalent bond, they share electrons to achieve a stable configuration. The 1s orbital of hydrogen and the 2p orbital of fluorine are the ones involved in the bond formation, as they have the highest energy and are the most likely to interact.In molecular orbital theory, atomic orbitals combine to form molecular orbitals. In the case of HF, the 1s orbital of hydrogen and the 2p orbital of fluorine will combine to form two molecular orbitals: a bonding orbital and an antibonding * orbital.The bonding orbital is lower in energy and more stable, while the antibonding * orbital is higher in energy and less stable. Electrons will fill the bonding orbital first. Since there are two electrons involved in the bond one from hydrogen and one from fluorine , both electrons will occupy the orbital, resulting in a stable covalent bond.The electronic configuration of the HF molecule can be represented as: 1sH + 2pF As for the molecular structure, hydrogen fluoride has a linear geometry. The bond between the hydrogen and fluorine atoms is polar, with the more electronegative fluorine atom pulling electron density towards itself, resulting in a partial negative charge - on the fluorine and a partial positive charge + on the hydrogen. The bond length is approximately 0.92 .In summary, the electronic configuration of the hydrogen fluoride HF molecule is 1sH + 2pF , and its molecular structure is linear with a polar covalent bond between the hydrogen and fluorine atoms.