Each compound contains both ionic and covalent bonds. Write ionic Lewis structures for each of them, including the covalent structure for the ion in brackets. Write resonance structures if necessary.
Solution 88E Step 1 of 4 Let’s explain RbIO . 2 In IO 2n, Iodine is linked to two atoms of Oxygen as in figure If we calculate the formal charges For I Valence electrons - lone pair electrons - ½ bondin electrons= 7-4-3=0 For O (single bond) Valence electrons - lone pair electrons - ½ bondin electrons= 6-6-1=-1 For O (double bond) Valence electrons - lone pair electrons - ½ bondin electrons= 6-4-2=0 Thus we have a negative charge that can be extended to the whole structure by pitting in brackets the whole structure and indicating the symbol (-) in the upper right corner We can even consider that we can have a resonance form because of the delocalization of the double bond. Since IO ion has a negative , monovalent charge, it can join Rb ion in order to forman ionic 2 bond and a 1:1 stoichiometry compound having this structure Step 2 of 4 Let’s explain NH Cl. 4 NH 4n, has this Lewis structure Nitrogen forms four covalent bonds with four atoms of H. If we calculate formal charges for N Valence electrons - Lone pair electrons - ½ bonded electrons= 5-0-4=+1 this is the meaning of the positive charge, thus this structure is more correct Because of its positive, monovalent charge, ca form an ionic bond with a Cl ion, thus the stoichiometry of the salt is 1:1 and the Lewis structure will be