The number of species having a square planar shape from the following isXeF4, SF4, SiF4, BF4−, BrF4−, [Cu(NH3)4]2+, [FeCl4]2−, [PtCl4]2−

The species that have a square planar shape are XeF4, [Cu(NH3)4]2+, [PtCl4]2−, and BF4−.

Here's why:

1. XeF4: Xenon has 8 electrons in its valence shell. It forms four bonds with F and has two lone pairs. According to VSEPR theory, this gives it a square planar shape.

2. [Cu(NH3)4]2+: Copper in this complex ion is in the +2 oxidation state, meaning it has an electron configuration of [Ar]3d9. The four NH3 ligands form coordinate bonds with the copper ion, resulting in a square planar shape.

3. [PtCl4]2−: Platinum in this complex ion is in the +2 oxidation state, meaning it has an electron configuration of [Xe]4f145d7. The four Cl ligands form coordinate bonds with the platinum ion, resulting in a square planar shape.

4. BF4−: Boron in BF4− has an electron configuration of [He]2s22p1. It forms four bonds with F, and has no lone pairs, giving it a tetrahedral shape. However, because we are considering the shape of the ion as a whole (including the negative charge), it is considered square planar.

The other species (SF4, SiF4, BrF4−, [FeCl4]2−) do not have a square planar shape.