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Chapter 8: Problem 34

Use Lewis symbols and Lewis structures to diagram the formation of \(\mathrm{PF}_{3}\) from \(\mathrm{P}\) and \(\mathrm{F}\) atoms, showing valence- shell electrons. (a) How many valence electrons does P have initially? (b) How many valence electrons does each F have initially? ( c) How many valence electrons surround the Pin the PF_ \(_{3}\) molecule? (d) How many valence electrons surround each \(\mathrm{F}\) in the \(\mathrm{PF}_{3}\) molecule? (e) How many bonding pairs of electrons are in the \(\mathrm{PF}_{3}\) molecule?

Short Answer

Expert verified
In summary, the Lewis structure of \(\mathrm{PF}_{3}\) is formed by combining a phosphorus (P) atom with 3 fluorine (F) atoms, sharing electrons to create covalent bonds. Initially, P has 5 valence electrons, and each F atom has 7 valence electrons. In the \(\mathrm{PF}_{3}\) molecule, 8 valence electrons surround the P atom, and 8 valence electrons surround each F atom. The molecule has 3 bonding pairs of electrons, represented by the single covalent bonds between P and F atoms.

Step by step solution

01

Determine the Lewis symbols for P and F atoms

First, we need to determine the Lewis symbols for the P and F atoms. The Lewis symbol represents the symbol of an element and its valence electrons as dots surrounding the symbol. P has 5 valence electrons (it is in group 15 of the periodic table), and F has 7 valence electrons (it is in group 17). Therefore, their Lewis symbols are: P: :P⋅⋅ F: :F: Notice that there's a pair of dots on the left side of both P and F.
02

Draw the Lewis structure for \(\mathrm{PF}_3\)

To draw the Lewis structure for \(\mathrm{PF}_{3}\), we first need to combine the P atom with 3 F atoms. The 3 F atoms will each share one of their unpaired electrons with the P atom to form a covalent bond, as shown below: :F: | .:P:---:F: | :F:
03

Answer the questions based on the Lewis structure

Now that we have the Lewis structure of \(\mathrm{PF}_3\), we can answer the questions: (a) P has 5 valence electrons initially, as mentioned in Step 1. (b) Each F atom has 7 valence electrons initially, as mentioned in Step 1. (c) In the \(\mathrm{PF}_{3}\) molecule, P atom is surrounded by 8 valence electrons (2 lone pairs and 6 shared electrons). (d) Each F atom in \(\mathrm{PF}_3\) is surrounded by 8 valence electrons (6 from their lone pairs and 2 from the shared pair with P). (e) There are 3 bonding pairs of electrons in the \(\mathrm{PF}_3\) molecule, as seen in the Lewis structure with the 3 single covalent bonds between P and F atoms.

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Most popular questions from this chapter

Under special conditions, sulfur reacts with anhydrous liquid ammonia to form a binary compound of sulfur and nitrogen. The compound is found to consist of 69.6\(\% \mathrm{S}\) and 30.4\(\% \mathrm{N} .\) Measurements of its molecular mass yield a value of 184.3 \(\mathrm{g} / \mathrm{mol}\) . The compound occasionally detonates on being struck or when heated rapidly. The sulfur and nitrogen atoms of the molecule are joined in a ring. All the bonds in the ring are of the same length. (a) Calculate the empirical and molecular formulas for the substance. (b) Write Lewis structures for the molecule, based on the information you are given. (Hint: You should find a relatively small number of dominant Lewis structures.) (c) Predict the bond distances between the atoms in the ring. (Note: The \(S-S\) distance in the \(S_{8}\) ring is 2.05 A.) ( d.) The enthalpy of formation of the compound is estimated to be 480 \(\mathrm{kJ} / \mathrm{mol}^{-1} . \Delta H_{f}^{9}\) of \(\mathrm{S}(g)\) is 222.8 \(\mathrm{kJ} / \mathrm{mol} .\) Estimate the average bond enthalpy in the compound.

A new compound is made that has a \(\mathrm{C}-\mathrm{C}\) bond length of 1.15 \(\mathrm{A} .\) Is this bond likely to be a single, double, or triple \(\mathrm{C}-\mathrm{Cbond} ?\)

Ammonium chloride, \(\mathrm{NH}_{4} \mathrm{Cl},\) is a very soluble salt in water. (a) Draw the Lewis structures of the ammonium and chloride ions. (b) Is there an \(\mathrm{N}-\) Cl bond in solid ammonium chloride? (c) If you dissolve 14 gof ammonium chloride in 500.0 \(\mathrm{mL}\) of water, what is the molar concentration of the solution? (d) How many grams of silver nitrate do you need to add to the solution in part (c) to precipitate all of the chloride as silver chloride?

True or false: (a) The \(\mathrm{C}-\) Cbonds in benzene are all the same length and correspond to typical single \(\mathrm{C}-\mathrm{Cbond}\) lengths. (b) The \(\mathrm{C}-\mathrm{C}\) bond in acetylene, HCCH, is longer than the average \(\mathrm{C}-\mathrm{C}\) bond length in benzene.

(a) Construct a Lewis structure for \(\mathrm{O}_{2}\) in which each atom achieves an octet of electrons. (b) How many bonding electrons are in the structure? (c) Would you expect the \(\mathrm{O}-\mathrm{O}\) bond in \(\mathrm{O}_{2}\) to be shorter or longer than the \(\mathrm{O}-\mathrm{O}\) bond in compounds that contain an \(\mathrm{O}-\mathrm{O}\) single bond? Explain.
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