Consider IF6+ Draw the Lewis structure. Is this molecule polar or nonpolar? · Polar · Nonpolar
The Correct Answer and Explanation is :
To determine the polarity and draw the Lewis structure for the IF₆⁺ molecule, follow these steps:
- Count the Valence Electrons:
- Iodine (I) is in Group 17 and has 7 valence electrons.
- Fluorine (F) is in Group 17 and has 7 valence electrons each, and there are 6 fluorine atoms, so 6 × 7 = 42 valence electrons.
- The +1 charge means there is one less electron than usual, so subtract 1 from the total count.
- Total electrons = 7 (I) + 42 (F) – 1 (charge) = 48 electrons.
- Draw the Basic Structure:
- Iodine (I) is the central atom.
- Connect each fluorine atom to iodine with a single bond. Each bond represents 2 electrons, so 6 bonds will use up 12 electrons.
- Place the remaining electrons as lone pairs around the fluorine atoms, giving each fluorine 3 lone pairs (6 electrons per fluorine).
- Check the Octet Rule:
- Iodine can expand its octet since it’s in period 5 and can hold more than 8 electrons. In this case, it will have 12 electrons around it (6 bonds to fluorine atoms).
- Fluorine atoms have 8 electrons (2 from the bond with iodine, and 6 as lone pairs), satisfying the octet rule.
- Formal Charges:
- Iodine has 7 valence electrons, and after bonding with 6 fluorines, it has 12 electrons around it (formal charge = 7 – 12 = -5, but the charge of +1 should be factored in).
- Each fluorine has 7 valence electrons and 6 electrons as lone pairs, so no formal charge for fluorine (formal charge = 7 – 6 – 1 = 0).
- Polarity:
- The molecule has a symmetrical octahedral shape. The bonds between iodine and fluorine are polar, but because the molecule is symmetrical and all the bonds are identical, the dipoles cancel out.
- Thus, the molecule is nonpolar.
Now I will generate the image of the Lewis structure for IF₆⁺.
Here is the Lewis structure for IF₆⁺. The molecule is symmetrical, with iodine at the center and six fluorine atoms arranged in an octahedral shape. Due to this symmetry, the dipoles from the polar bonds cancel each other out, making the molecule nonpolar.
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