Math

QuestionElectronic Structure and Chemical Bonding Predicting the arrangement of electron groups around the central atom o...
Answer the questions in the table below about the shape of the difluoroiodide (IF2)\left(\mathrm{IF}_{2}^{-}\right)anion. \begin{tabular}{|l|l|} \hline How many electron groups are around the central iodine atom? \\ Note: one "electron group" means one lone pair, one single bohd, \\ one double bond, or one triple bond. \end{tabular}

Studdy Solution

STEP 1

Assumptions
1. We are analyzing the difluoroiodide anion, IF2\mathrm{IF}_{2}^{-}.
2. The central atom is iodine (I).
3. An "electron group" refers to a lone pair, single bond, double bond, or triple bond.
4. We need to determine the number of electron groups around the central iodine atom.

STEP 2

Identify the valence electrons for iodine.
Iodine is in group 17 of the periodic table, so it has 7 valence electrons.

STEP 3

Consider the additional electron due to the negative charge.
The negative charge on the anion IF2\mathrm{IF}_{2}^{-} indicates an additional electron, bringing the total to 8 valence electrons for iodine.

STEP 4

Determine the bonding with fluorine atoms.
Each fluorine atom forms a single bond with iodine. Since there are two fluorine atoms, iodine forms two single bonds.

STEP 5

Calculate the remaining electrons after bonding.
Each single bond uses 2 electrons. Therefore, 2 bonds use 2×2=42 \times 2 = 4 electrons. Subtract these from the total valence electrons.
Remaining electrons = 8 (total valence electrons) - 4 (used in bonds) = 4 electrons.

STEP 6

Determine the number of lone pairs on iodine.
The remaining 4 electrons form 2 lone pairs on the iodine atom.

STEP 7

Count the total number of electron groups around iodine.
The electron groups include: - 2 single bonds with fluorine atoms. - 2 lone pairs.
Total electron groups = 2 (bonds) + 2 (lone pairs) = 4 electron groups.
The number of electron groups around the central iodine atom is 4.

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