The shape of AsCl4 (arsenic tetrachloride) is tetrahedral. This is due to the arrangement of the bonding pairs of electrons around the central arsenic atom.
In AsCl4, the arsenic atom is surrounded by four chlorine atoms. According to VSEPR (Valence Shell Electron Pair Repulsion) theory, the electron pairs (including bonding pairs) will arrange themselves in space to minimize repulsion between them. Since there are four bonded pairs and no lone pairs on the arsenic atom, the optimal arrangement is a tetrahedral geometry.
In a tetrahedral shape, the bond angles between the chlorine atoms are approximately 109.5 degrees, creating a three-dimensional structure that allows for the maximum distance between the bonded atoms. This configuration is typical for molecules with a central atom bonded to four other atoms with no lone pairs.