The molecule/species with the minimum number of lone pairs is SnCl2. Here's why:

Identification of molecules/species:
a) ICl3 - This molecule consists of one iodine atom and three chlorine atoms.
b) BF4- - This species is a polyatomic ion consisting of one boron atom and four fluorine atoms.
c) SnCl2 - This molecule consists of one tin atom and two chlorine atoms.
d) XeF4 - This molecule consists of one xenon atom and four fluorine atoms.

Explanation:
In order to determine the number of lone pairs, we need to look at the electron configuration of each atom in the molecule/species.

a) ICl3 - Iodine (I) has 7 valence electrons and chlorine (Cl) has 7 valence electrons. In this molecule, each chlorine atom forms a single bond with the iodine atom, resulting in a total of 3 shared electron pairs. Additionally, iodine has 2 lone pairs of electrons. So, ICl3 has 2 lone pairs.

b) BF4- - Boron (B) has 3 valence electrons and fluorine (F) has 7 valence electrons. In this species, boron forms a single bond with each fluorine atom, resulting in a total of 4 shared electron pairs. Since boron does not have any lone pairs, BF4- has 0 lone pairs.

c) SnCl2 - Tin (Sn) has 4 valence electrons and chlorine (Cl) has 7 valence electrons. In this molecule, tin forms a single bond with each chlorine atom, resulting in a total of 2 shared electron pairs. Tin also has 2 lone pairs of electrons. So, SnCl2 has 2 lone pairs.

d) XeF4 - Xenon (Xe) has 8 valence electrons and fluorine (F) has 7 valence electrons. In this molecule, xenon forms a double bond with each fluorine atom, resulting in a total of 8 shared electron pairs. Xenon has 2 lone pairs of electrons. So, XeF4 has 2 lone pairs.

Conclusion:
Among the given options, SnCl2 has the minimum number of lone pairs with 2 lone pairs.