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Chapter 7: Q27 E (page 394)

Write the Lewis structure for the diatomic molecule \({{\rm{P}}_{\rm{2}}}\), an unstable form of phosphorus found in high temperature phosphorus vapor.

Short Answer

Expert verified

The Lewis structure for the diatomic molecule \({{\rm{P}}_{\rm{2}}}\) is:

Step by step solution

01

Define Chemical Bonding

A chemical bond is a long-term attraction between atoms, ions, or molecules that allows chemical compounds to form.

02

Writing the Lewis structure

(a) The first step is to figure out how many valence electrons there are. As there are two atoms in total, the total amount of valence electrons on each is.

(b) Next, we'll use a single bond to connect both. Due to both atoms using one electron to create a single connection, four valence electrons are left on each atom.

(c) However, each atom's octet is not fulfilled. As a result, both atoms will use their two additional electrons to create a triple bond.

Therefore, the Lewis structure is:

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Most popular questions from this chapter

Identify the atoms that correspond to each of the following electron configurations. Then, write the Lewis symbol for the common ion formed from each atom: (a)\({\text{1}}{{\text{s}}^{\text{2}}}{\text{2}}{{\text{s}}^{\text{2}}}{\text{2}}{{\text{p}}^{\text{5}}}\)(b)\({\text{1}}{{\text{s}}^{\text{2}}}{\text{2}}{{\text{s}}^{\text{2}}}{\text{2}}{{\text{p}}^{\text{6}}}{\text{3}}{{\text{s}}^{\text{2}}}\)(c)\({\text{1}}{{\text{s}}^{\text{2}}}{\text{2}}{{\text{s}}^{\text{2}}}{\text{2}}{{\text{p}}^{\text{6}}}{\text{3}}{{\text{s}}^{\text{2}}}{\text{3}}{{\text{p}}^{\text{6}}}{\text{4}}{{\text{s}}^{\text{2}}}{\text{3}}{{\text{d}}^{{\text{10}}}}\)(d)\({\text{1}}{{\text{s}}^{\text{2}}}{\text{2}}{{\text{s}}^{\text{2}}}{\text{2}}{{\text{p}}^{\text{6}}}{\text{3}}{{\text{s}}^{\text{2}}}{\text{3}}{{\text{p}}^{\text{6}}}{\text{4}}{{\text{s}}^{\text{2}}}{\text{3}}{{\text{d}}^{{\text{10}}}}{\text{4}}{{\text{p}}^{\text{4}}}\)(e)\({\text{1}}{{\text{s}}^{\text{2}}}{\text{2}}{{\text{s}}^{\text{2}}}{\text{2}}{{\text{p}}^{\text{6}}}{\text{3}}{{\text{s}}^{\text{2}}}{\text{3}}{{\text{p}}^{\text{6}}}{\text{4}}{{\text{s}}^{\text{2}}}{\text{3}}{{\text{d}}^{{\text{10}}}}{\text{4}}{{\text{p}}^{\text{1}}}\).

Use the simulation (http://openstaxcollege.org/l/16MolecPolarity) to perform the following exercises for a two-atom molecule: (a) Adjust the electronegativity value so the bond dipole is pointing toward B. Then determine what the electronegativity values must be to switch the dipole so that it points toward A. (b) With a partial positive charge on A, turn on the electric field and describe what happens. (c) With a small partial negative charge on A, turn on the electric field and describe what happens. (d) Reset all, and then with a large partial negative charge on A, turn on the electric field and describe what happens.

A molecule with the formula\({\rm{A}}{{\rm{B}}_{\rm{3}}}\), in which A and B represent different atoms, could have one of three different shapes. Sketch and name the three different shapes that this molecule might have. Give an example of a molecule or ion that has each shape.

Write Lewis structures for the following: (a)\({\rm{Se}}{{\rm{F}}_{\rm{6}}}\)(b)\({\rm{Xe}}{{\rm{F}}_{\rm{4}}}\)(c)\({\rm{SeC}}{{\rm{l}}_{\rm{3}}}^{\rm{ + }}\)(d)\({\rm{C}}{{\rm{l}}_{\rm{2}}}{\rm{BBC}}{{\rm{l}}_{\rm{2}}}\)(contains a\({\rm{B - B}}\)bond).

Use the Molecule Shape simulator (http://openstaxcollege.org/l/16MolecShape) to explore real molecules. On the Real Molecules tab, select H2O. Switch between the “real” and “model” modes. Explain the difference observed.
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