Draw a plausible Lewis structure for the following series of molecules and ions: (a) \(\mathrm{ClF}_{2}^{-} ;\) (b) \(\mathrm{ClF}_{3}\); (c) \(\mathrm{ClF}_{4}^{-} ;\) (d) ClF \(_{5} .\) Describe the electron group geometry and molecular structure of these species.

First, count total valence electrons present: Chlorine (7 electrons) + 2*Fluorine (7 electrons each) + 1 electron (for the -1 charge) = 22 electrons. Draw a skeleton wherein a Chlorine atom is central and is bonded with two Fluorines. Subtract the electrons used for bonding from total electrons: 22-4 =18. Distribute the remaining electrons on atoms, beginning with outer atoms. Each outer Fluorine atom receives 6 electrons and Chlorine gets the remaining 6 electrons. Now, verify that each atom follows Octet rule (except Hydrogen). The structure following the octet rule is the correct Lewis Structure.

First, count total valence electrons present: Chlorine (7 electrons) + 3*Fluorine (7 electrons each) = 28 electrons. Draw a skeleton where Chlorine atom is central and bonded with three Fluorines. Subtract bonding electrons from total: 28-6 =22. Distribute the remaining electrons on atoms. Each outer Fluorine atom receives 6 electrons and Chlorine gets the remaining 4 electrons. Verify that each atom follows Octet rule.

First, count total valence electrons present: Chlorine (7 electrons) + 4*Fluorine (7 electrons each) +1 electron (for -1 charge) = 36 electrons. Draw a skeleton with Chlorine atom as central and bonded with four Fluorines. Subtract bonding electrons from total: 36-8 = 28. Distribute the remaining electrons on atoms. Each outer Fluorine atom receives 6 electrons and Chlorine gets the remaining 4 electrons.

The total valence electrons present are Chlorine (7 electrons) + 5*Fluorine (7 electrons each) = 42 electrons. Draw a skeleton where Chlorine atom is central and bonded with five Fluorines. Subtract bonding electrons: 42-10 = 32. Distribute the remaining electrons on atoms. Each outer Fluorine atom receives 6 electrons.

Electron group geometry considers both bonding and non-bonding electron pairs, while molecular structure considers only bonding pairs. (a) For \(\mathrm{ClF}_{2}^{-}\), there are 3 electron groups (2 bonding and 1 lone pair) around central Chlorine. So its group geometry is T-shape and electron geometry is Trigonal Planar. (b) For \(\mathrm{ClF}_{3}\), there are 5 electron groups (3 bonding and 2 lone pairs). Hence, its group geometry is T-shape and electron geometry is Trigonal Bipyramidal. (c) For \(\mathrm{ClF}_{4}^{-}\), there are 5 electron groups (4 bonding and 1 lone pair). Hence, its group geometry is Seesaw and electron geometry is Trigonal Bipyramidal. (d) For \(\mathrm{ClF}_{5}\), there are 6 electron groups (all bonding), its group geometry and molecular structure are Octahedral.