a. Electron Geometry: The electron geometry of CoCl2 (cobalt(II) chloride) is octahedral. This is because the central cobalt atom is surrounded by six electron regions: two bonding pairs with chlorine atoms and four lone pairs.
b. Molecular Geometry: The molecular geometry of CoCl2 is linear. In this case, the two chlorine atoms are positioned opposite each other around the central cobalt atom, resulting in a linear shape.
c. Bond Angles: The bond angle in CoCl2 is approximately 180 degrees due to its linear structure. The position of the two chlorine atoms relative to the cobalt atom creates this angle.
d. Polarity: CoCl2 is a polar molecule. Although the individual Co-Cl bonds are polar due to the difference in electronegativity between cobalt and chlorine, the linear arrangement of the molecule causes the dipoles to not cancel out completely, resulting in an overall dipole moment.
e. Central Atom Hybridization: The hybridization of the central cobalt atom in CoCl2 is dsp2. This hybridization results from the combination of one d, one s, and two p orbitals to accommodate the bonding and lone pairs around the cobalt atom.