To predict the geometry of the given species, we can use the VSEPR (Valence Shell Electron Pair Repulsion) theory, which helps us understand how the presence of electron pairs around a central atom can determine its geometry.
A. ClO2 (Chlorine Dioxide)
Chlorine dioxide has one chlorine atom bonded to two oxygen atoms and has one lone pair of electrons on the chlorine atom. According to VSEPR theory, the presence of the lone pair will affect the shape. With three regions of electron density (two bonded atoms and one lone pair), the molecular geometry is bent or angular with an approximate bond angle of 117 degrees.
B. CO3^2- (Carbonate Ion)
The carbonate ion has a central carbon atom bonded to three oxygen atoms. It has one double bond and two single bonds (which each exhibit resonance). There are no lone pairs on the central atom. With three bonding regions, the geometry is trigonal planar, and the bond angles are approximately 120 degrees.
C. SF5Cl (Sulfur Pentafluoride Chloride)
In SF5Cl, sulfur is bonded to five fluorine atoms and one chlorine atom, resulting in a total of six bonding pairs and no lone pairs. According to VSEPR theory, the presence of six bonding regions around the sulfur atom creates an octahedral geometry. The bond angles are approximately 90 degrees.
D. XeF2 (Xenon Difluoride)
Xenon difluoride has a central xenon atom bonded to two fluorine atoms and three lone pairs of electrons. The presence of the three lone pairs will repel the bonded atoms, leading to a linear shape for the bonded atoms. Thus, the molecular geometry is linear with a bond angle of 180 degrees.