In the early 1960s, krypton was found to react with fluorine gas in an electrical discharge tube at -183 °C. The compound formed was KrF2. What are the oxidation states of Kr and F in this compound? What is the electron-dot structure and geometry?

Oxidation states indicate the degree of oxidation of an atom in a compound, reflecting the number of electrons lost or gained. In KrF2, fluorine typically has an oxidation state of -1, as it is more electronegative. To find the oxidation state of krypton (Kr), we set up the equation: x + 2(-1) = 0, leading to x = +2 for Kr.

The electron-dot structure, or Lewis structure, represents the valence electrons of atoms within a molecule. For KrF2, the structure shows krypton at the center with two fluorine atoms bonded to it, each contributing three lone pairs of electrons. This visualization helps in understanding bonding and electron distribution in the compound.

Molecular geometry describes the three-dimensional arrangement of atoms in a molecule. For KrF2, the geometry is determined by the VSEPR theory, which predicts a linear shape due to the two bonding pairs and three lone pairs on krypton. This arrangement minimizes electron pair repulsion, resulting in a specific spatial configuration.