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Chapter 8: Problem 34

Using Lewis symbols and Lewis structures, diagram the formation of \(\mathrm{BF}_{3}\) from \(\mathrm{B}\) and \(\mathrm{F}\) atoms, showing valence- shell electrons. (a) How many valence electrons does B have initially? (b) How many bonds F has to make in order to achieve an octet? (c) How many valence electrons surround the \(\mathrm{B}\) in the \(\mathrm{BF}_{3}\) molecule? (d) How many valence electrons surround each \(\mathrm{F}\) in the \(\mathrm{BF}_{3}\) molecule? (e) Does \(\mathrm{BF}_{3}\) obey the octet rule?

Short Answer

Expert verified
(a) B has 3 valence electrons initially. (b) F has to make 1 bond to achieve an octet. (c) In the \(\mathrm{BF}_3\) molecule, B is surrounded by 6 valence electrons. (d) Each F in the \(\mathrm{BF}_3\) molecule is surrounded by 8 valence electrons. (e) \(\mathrm{BF}_3\) does not obey the octet rule, as B has an incomplete octet.

Step by step solution

01

(a) Determine the number of valence electrons for B

To find the number of valence electrons of B, we need to look at its position in the periodic table. Boron (B) belongs to Group 13, which means it has 3 valence electrons.
02

(b) Determine how many bonds F has to make to achieve an octet

Fluorine (F) belongs to Group 17 in the periodic table, meaning it has 7 valence electrons. Since each atom wants to achieve a stable octet (8 valence electrons), F needs to form 1 bond (with 1 more electron) to achieve an octet.
03

(c) Create the Lewis structure for \(\mathrm{BF}_3\) and count valence electrons around B

To create the Lewis structure for \(\mathrm{BF}_3\), we'll follow these steps: 1. Place the least electronegative atom (B) in the center. 2. Surround B with F atoms, connected by single bonds 3. Distribute the remaining valence electrons as lone pairs on the F atoms The Lewis structure will look like this: ``` F | B-F-B | F ``` In the \(\mathrm{BF}_3\) molecule, there are 3 single bonds (each containing 2 valence electrons) attached to B and no lone pair electrons. Thus, B is surrounded by 6 valence electrons.
04

(d) Count valence electrons around each F in \(\mathrm{BF}_3\)

In the \(\mathrm{BF}_3\) molecule, each F is connected to B by a single bond and has 3 lone pairs of electrons. Thus, each F has 2 (from the bond) + 6 (from the lone pairs) = 8 valence electrons, achieving an octet.
05

(e) Determine if \(\mathrm{BF}_3\) obeys the octet rule

The octet rule states that an atom seeks to have a total of 8 valence electrons, either through sharing (covalent bonds) or transferring (ionic bonds). In the \(\mathrm{BF}_3\) molecule, each F atom has achieved an octet with 8 valence electrons. However, the central B atom is surrounded by only 6 valence electrons. Therefore, \(\mathrm{BF}_3\) does not obey the octet rule, as B has an incomplete octet.

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Most popular questions from this chapter

Which ionic compound is expected to form from combining the following pairs of elements? (a) calcium and nitrogen, (b) cesium and bromine, (c) strontium and sulfur, (d) aluminum and selenium.

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

A new compound is made that has a \(\mathrm{C}-\mathrm{N}\) bond length of $118 \mathrm{pm}$. Is this bond likely to be a single, double, or triple C-N bond?

For each of the following molecules or ions of sulfur and oxygen, write a single Lewis structure that obeys the octet rule, and calculate the oxidation numbers and formal charges on all the atoms: (a) \(\mathrm{SO}_{2}\), (b) \(\mathrm{SO}_{3}\) (c) \(\mathrm{SO}_{3}^{2-}\). (d) Arrange these molecules/ions in order of increasing \(\mathrm{S}-\mathrm{O}\) bond length.

Write Lewis structures for the following: (a) \(\mathrm{H}_{2} \mathrm{CO}\) (both \(\mathrm{H}\) atoms are bonded to $\mathrm{C} \mathrm{)},(\mathbf{b}) \mathrm{H}_{2} \mathrm{O}_{2},(\mathbf{c}) \mathrm{C}_{2} \mathrm{~F}_{6}($ contains a \(\mathrm{C}-\mathrm{C}\) bond $),(\mathbf{d}) \mathrm{AsO}_{3}^{3-},(\mathbf{e}) \mathrm{H}_{2} \mathrm{SO}_{3}(\mathrm{H}$ is bonded to \(\mathrm{O})\) (f) \(\mathrm{NH}_{2} \mathrm{Cl}\).
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