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Chapter 9: Problem 13

How does a trigonal pyramid differ from a tetrahedron so far as molecular geometry is concerned?

Short Answer

Expert verified
A trigonal pyramidal molecular geometry has one central atom with three surrounding atoms at the corners of a pyramid and a lone pair of electrons on the central atom. The bond angles are typically around 107.5 degrees, and the molecule is polar due to the asymmetric electron distribution. In contrast, a tetrahedral molecular geometry has one central atom with four surrounding atoms at the vertices of a regular tetrahedron. The bond angles are always 109.5 degrees, and the molecule is often nonpolar due to the absence of lone pairs on the central atom and symmetrical distribution of outer atoms. Examples include ammonia (NH₃) for trigonal pyramidal and methane (CH₄) for tetrahedral.

Step by step solution

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1. Defining Trigonal Pyramid and Tetrahedron

A trigonal pyramid is a molecular geometry with one atom at the center and three surrounding atoms (3 outer atoms) at the corners of a pyramid, and it also has a lone pair of electrons at the central atom. This shape is also known as a trigonal pyramidal. A tetrahedron, on the other hand, is a molecular geometry with one central atom and four surrounding atoms (4 outer atoms) at the vertices of a regular tetrahedron. This shape is also referred to as a tetrahedral.
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2. Differences in Bond Angles

In a trigonal pyramidal geometry, the bond angles between the surrounding atoms are typically around 107.5 degrees because of the repulsion caused by the lone pair of electrons on the central atom. The ideal angle would be equal if there were no lone pair present, which is 109.5 degrees. In a tetrahedral geometry, the bond angles are always 109.5 degrees because there are no lone pairs on the central atom to cause additional repulsion.
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3. Differences in Symmetry

A trigonal pyramidal molecule is polar because it has an asymmetric electron distribution with the presence of lone pairs. This means that there is a net dipole moment in the molecule, causing them to have a polar nature. In contrast, a tetrahedral molecule is often nonpolar because there are no lone pairs on the central atom, and the distribution of outer atoms is symmetrical. Therefore, in a pure tetrahedral molecule, the net dipole moment is zero, making it nonpolar.
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4. Examples of Trigonal Pyramidal and Tetrahedral Molecules

An example of a trigonal pyramidal molecule is ammonia (NH₃), where nitrogen is the central atom bonded with three hydrogen atoms, and there is a lone pair of electrons on the nitrogen. An example of a tetrahedral molecule is methane (CH₄), where the central atom is carbon bonded to four hydrogen atoms, and there are no lone pairs present on the central atom.
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Conclusion

In summary, although trigonal pyramidal and tetrahedral molecular geometries might seem similar, they have significant differences. The primary differences arise from the presence of a lone pair on the central atom in a trigonal pyramidal, which causes deviations in bond angles, polarity, and symmetric molecular structure compared to a tetrahedral molecule, which has no lone pairs on the central atom.

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Most popular questions from this chapter

Describe the characteristic electron-domain geometry of each of the following numbers of electron domains about a central atom: \((a) 3,(b) 4,(c) 5,(d) 6\)

(a) What does the term paramagnetism mean? (b) How can one determine experimentally whether a substance is paramagnetic? (c) Which of the following ions would you expect to be paramagnetic: \(\mathrm{O}_{2}^{+}, \mathrm{N}_{2}^{2-}, \mathrm{Li}_{2}^{+}, \mathrm{O}_{2}^{2-} ?\) For those ions that are paramagnetic, determine the number of unpaired electrons.

How many nonbonding electron pairs are there in each of the following molecules: (a) \(\left(\mathrm{CH}_{3}\right)_{2} \mathrm{~S},\) (b) \(\mathrm{HCN},\) (c) \(\mathrm{H}_{2} \mathrm{C}_{2}\), (d) \(\mathrm{CH}_{3} \mathrm{~F} ?\)

Would you expect the nonbonding electron-pair domain in \(\mathrm{NH}_{3}\) to be greater or less in size than for the corresponding one in \(\mathrm{PH}_{3}\) ? Explain.

Shown here are three pairs of hybrid orbitals, with each set at a characteristic angle. For each pair, determine the type of hybridization, if any, that could lead to hybrid orbitals at the specified angle.
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