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Chapter 8: Problem 90

Calculate the formal charge on the indicated atom in each of the following molecules or ions: (a) the central oxygen atom in \(\mathrm{O}_{3},\) (b) phosphorus in \(\mathrm{PF}_{6}^{-},(\mathbf{c})\) nitrogen in \(\mathrm{NO}_{2}\) (d) iodine in ICl_\(\mathrm{ICl}_{3},\) (e) chlorine in \(\mathrm{HClO}_{4}\) (hydrogen is bonded to \(\mathrm{O} )\)

Short Answer

Expert verified
The formal charges on each of the indicated atoms are as follows: a) O3 (central oxygen atom): \(0\) b) PF6- (phosphorus): \(-1\) c) NO2 (nitrogen): \(0\) d) ICl3 (iodine): \(+2\) e) HClO4 (chlorine): \(+3\)

Step by step solution

01

Determine Valence Electrons

Determine the number of valence electrons for each atom of interest: a) O (central oxygen): 6 valence electrons b) P (phosphorus): 5 valence electrons c) N (nitrogen): 5 valence electrons d) I (iodine): 7 valence electrons e) Cl (chlorine): 7 valence electrons
02

Identify Electrons Assigned to Atom

Determine the number of electrons assigned to each atom of interest. a) O3 (central oxygen): 2 lone pairs (4 electrons) + 2 half bonding pairs (2 electrons) = 6 electrons b) PF6- (phosphorus): 6 half bonding pairs (6 electrons) = 6 electrons c) NO2 (nitrogen): 1 lone pair (2 electrons) + 3 half bonding pairs (3 electrons) = 5 electrons d) ICl3 (iodine): 1 lone pair (2 electrons) + 3 half bonding pairs (3 electrons) = 5 electrons e) HClO4 (chlorine): 4 half bonding pairs (4 electrons) = 4 electrons
03

Calculate Formal Charge for each Atom

Calculate the formal charge of each atom by subtracting the assigned electrons from the valence electrons. a) O3 (central oxygen): Formal charge = 6 - 6 = 0 b) PF6- (phosphorus): Formal charge = 5 - 6 = -1 c) NO2 (nitrogen): Formal charge = 5 - 5 = 0 d) ICl3 (iodine): Formal charge = 7 - 5 = +2 e) HClO4 (chlorine): Formal charge = 7 - 4 = +3 The formal charges on each of the indicated atoms are as follows: a) O3 (central oxygen atom): 0 b) PF6- (phosphorus): -1 c) NO2 (nitrogen): 0 d) ICl3 (iodine): +2 e) HClO4 (chlorine): +3

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Most popular questions from this chapter

By referring only to the periodic table, select (a) the most electronegative element in group \(6 \mathrm{A} ;(\mathbf{b})\) the least electronegative element in the group Al, Si, P; (c) the most electronegative element in the group \(\mathrm{Ga}, \mathrm{P}, \mathrm{Cl}, \mathrm{Na} ;(\mathbf{d})\) the element in the group \(\mathrm{K}\) \(\mathrm{C}, \mathrm{Zn}, \mathrm{F}\) that is most likely to form an ionic compound with Ba.

The hypochlorite ion, \(\mathrm{ClO}^{-},\) is the active ingredient in bleach. The perchlorate ion, \(\mathrm{ClO}_{4}^{-},\) is a main component of rocket propellants. Draw Lewis structures for both ions (a) What is the formal charge of Cl in the hypochlorite ion? (b) What is the formal charge of Cl in the perchlorate ion, assuming the Cl-O bonds are all single bonds? (c) What is the oxidation number of Cl in the hypochlorite ion? (d) What is the oxidation number of \(C l\) in the perchlorate ion, assuming the \(C l-O\) bonds are all single bonds? (e) In a redox reaction, which ion would you expect to be more easily reduced?

Energy is required to remove two electrons from Ca to form \(\mathrm{Ca}^{2+},\) and energy is required to add two electrons to \(\mathrm{O}\) to form \(\mathrm{O}^{2-} .\) Yet \(\mathrm{CaO}\) is stable relative to the free elements. Which statement is the best explanation? (a) The lattice energy of CaO is large enough to overcome these processes. (b) CaO is a covalent compound, and these processes are irrelevant. (c) CaO has a higher molar mass than either Ca or O. (d) The enthalpy of formation of CaO is small. (e) CaO is stable to atmospheric conditions.

Ammonia reacts with boron trifluoride to form a stable compound, as we saw in Section 8.7 . (a) Draw the Lewis structure of the ammonia-boron trifluoride reaction product. (b) The B-N bond is obviously more polar than the \(\mathrm{C}-\mathrm{C}\) bond. Draw the charge distribution you expect on the \(\mathrm{B}-\mathrm{N}\) bond within the molecule (using the delta plus and delta minus symbols mentioned in Section 8.4\()\) . ( ) Boron trichloride also reacts with ammonia in a similar way to the trifluoride. Predict whether the \(B-N\) bond in the trichloride reaction product would be more or less polar than the \(B-N\) bond in the trifluoride product, and justify your reasoning.

The substance chlorine monoxide, ClO(g), is important in atmospheric processes that lead to depletion of the ozone layer. The ClO molecule has an experimental dipole moment of \(1.24 \mathrm{D},\) and the \(\mathrm{Cl}-\) O bond length is 1.60 \(\mathrm{A}\) . (a) Determine the magnitude of the charges on the Cl and O atoms in units of the electronic charge, \(e\) (b) Based on the electronegativities of the elements, which atom would you expect to have a partial negative charge in the Clo molecule? (c) Using formal charges as a guide, propose the dominant Lewis structure for the molecule. (d) The anion \(\mathrm{ClO}^{-}\) exists. What is the formal charge on the Cl for the best Lewis structure for \(\mathrm{ClO}^{-}\) ?
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