The coordination geometry of the complex [Cu NH3 4]SO4 is square planar. In this complex, the central metal ion Cu2+ is surrounded by four ammonia NH3 ligands, which are arranged at the corners of a square plane.To determine the nature of the ligand-metal coordination bond and its bonding energy, we can use UV-Vis spectroscopy. This technique measures the absorption of light by a compound as a function of wavelength. The absorption of light is related to the electronic transitions within the molecule, which can provide information about the nature of the bonding.In the case of [Cu NH3 4]SO4, the complex absorbs light in the visible region, which is responsible for its characteristic blue color. The absorption band in the visible region is due to the d-d transition of the Cu2+ ion. This transition involves the promotion of an electron from a lower energy d-orbital to a higher energy d-orbital.The nature of the ligand-metal coordination bond in this complex can be described as a dative covalent bond, where the lone pair of electrons on the nitrogen atom of the ammonia ligand is donated to the empty d-orbitals of the Cu2+ ion. This type of bond is also known as a coordinate covalent bond.To determine the bonding energy, we can use the wavelength of maximum absorption max from the UV-Vis spectrum. The bonding energy E can be calculated using the following equation:E = h * c / maxwhere h is Planck's constant 6.626 x 10^-34 Js , c is the speed of light 2.998 x 10^8 m/s , and max is the wavelength of maximum absorption in meters.Once the bonding energy is calculated, it can provide information about the strength of the ligand-metal coordination bond in the complex.