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Chapter 7: Q115E (page 406)

Use the Molecule Shape simulator (http://openstaxcollege.org/l/16MolecShape) to explore real molecules. On the Real Molecules tab, select H2O. Switch between the 鈥渞eal鈥� and 鈥渕odel鈥� modes. Explain the difference observed.

Short Answer

Expert verified

The lone pairs are larger in the "real" mode, and hydrogens are compressed as a result. As a result, the smaller angle of\({104.5^\circ }\).

Step by step solution

01

Definition of molecule

A molecule is a particle made up of two or more atoms that are chemically bonded together. The number of atomic nuclei making up a molecule is a determinate number.

02

Explanation

In this case the structures are very similar.

In the "real" mode, the lone pairs are larger, and because of that hydrogens are being compressed. Ultimately that leads to the smaller angle of\({104.5^\circ }\).

In the model mode, each electron group occupies the same amount of space; therefore the bond angle is shown as\({109.5^\circ }\).

Therefore,the structures are nearly identical in this situation.

The lone pairs are larger in the "real" mode, which compresses hydrogens. Finally, a lower angle of \({104.5^\circ }\) is obtained.

The bond angle is shown as \({109.5^\circ }\) in the model mode because each electron group occupies the same amount of space.

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Most popular questions from this chapter

How are single, double, and triple bonds similar? How do they differ?

Determine the formal charge of each element in the following:

(a) \({{\rm{H}}_{\rm{3}}}{{\rm{O}}^{\rm{ + }}}\)

(b) \({\rm{SO}}_{\rm{4}}^{{\rm{2 - }}}\)

(c) \({\rm{N}}{{\rm{H}}_{\rm{3}}}\)

(d) \({\rm{O}}_{\rm{2}}^{{\rm{2 - }}}\)

(e) \({{\rm{H}}_{\rm{2}}}{{\rm{O}}_{\rm{2}}}\)

Which of the following molecules or ions contain polar bonds? (a) \({{\rm{S}}_{\rm{8}}}\) (b) \({{\rm{S}}_{\rm{8}}}\) (c) \({{\rm{O}}_{\rm{2}}}^{{\rm{2 - }}}\) (d) \({\rm{N}}{{\rm{O}}_{\rm{3}}}^{\rm{ - }}\) (e) \({\rm{C}}{{\rm{O}}_{\rm{2}}}\) (f) \({{\rm{H}}_{\rm{2}}}{\rm{S}}\) (g) \({\rm{B}}{{\rm{H}}_{\rm{4}}}^{\rm{ - }}\) .

The lattice energy of \({\rm{KF}}\) is \({\rm{794kJ/mol}}\), and the interionic distance is \({\rm{269 pm}}\). The \({\rm{Na - F}}\) distance in \({\rm{NaF}}\), which has the same structure as \({\rm{KF}}\), is \({\rm{231 pm}}\). Which of the following values is the closest approximation of the lattice energy of \({\rm{NaF}}\): \({\rm{682 kJ/mol, 794 kJ/mol, 924 kJ/mol, 1588 kJ/mol,}}\) or \({\rm{3175 kJ/mol}}\)? Explain your answer.

A compound with a molar mass of about\({\rm{42 g/mol}}\)contains\({\rm{85}}{\rm{.7 \% }}\)carbon and\({\rm{14}}{\rm{.3 \% }}\)hydrogen by mass. Write the Lewis structure for a molecule of the compound.
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