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Chapter 9: Problem 15

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

Short Answer

Expert verified
The main differences between a trigonal pyramid and a tetrahedron in molecular geometry are the presence of a lone pair of electrons on the central atom in a trigonal pyramid, resulting in an asymmetrical shape with bond angles slightly less than 109.5 degrees, while a tetrahedral geometry is symmetrical with bond angles of approximately 109.5 degrees and no lone pairs on the central atom. Additionally, a trigonal pyramid has a central atom connected to three other atoms, whereas a tetrahedron has a central atom connected to four other atoms.

Step by step solution

01

Trigonal Pyramid Geometry

In a trigonal pyramid geometry, there is one central atom connected to three other atoms, and there is also a lone pair of electrons on the central atom. This geometric arrangement leads to an overall asymmetrical shape. The bond angles of a trigonal pyramid are slightly less than 109.5 degrees due to the presence of the lone pair-electron repulsion. This is an important feature found in the molecular geometry of trigonal pyramids.
02

Tetrahedron Geometry

In a tetrahedron (tetrahedral) geometry, there is one central atom connected to four other atoms. There are no lone pairs of electrons on the central atom in this case, and it has a symmetrical shape. The bond angles in a tetrahedron are approximately 109.5 degrees. A tetrahedral geometry is more symmetrical and provides equal distribution of electrons around the central atom.
03

Differences

The key differences between a trigonal pyramid and a tetrahedron in terms of molecular geometry are: 1. Presence of Lone Pair: Trigonal pyramid has one lone pair of electrons on the central atom, while a tetrahedron has no lone pairs on the central atom. 2. Bond Angles: The bond angles in a trigonal pyramid are slightly less than 109.5 degrees due to the presence of the lone pair-electron repulsion, whereas the bond angles in a tetrahedron are approximately 109.5 degrees. 3. Geometry: A trigonal pyramid has an asymmetrical shape, while a tetrahedron has a symmetrical shape. 4. Number of Atoms: Trigonal pyramid consists of a central atom connected to three other atoms, while a tetrahedron consists of a central atom connected to four other atoms.

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Most popular questions from this chapter

Consider the molecule \(\mathrm{PF}_{4} \mathrm{Cl}\) (a) Draw a Lewis structure for the molecule, and predict its electron-domain geometry. (b) Which would you expect to take up more space, a \(\mathrm{P}-\mathrm{F}\) bond or a \(\mathrm{P}-\mathrm{Cl}\) bond? Explain. (c) Predict the molecular geometry of \(\mathrm{PF}_{4} \mathrm{Cl} .\) How did your answer for part (b) influence your answer here in part \((\mathrm{c}) ?(\mathbf{d})\) Would you expect the molecule to distort from its ideal electron-domain geometry? If so, how would it distort?

The phosphorus trihalides \(\left(\mathrm{PX}_{3}\right)\) show the following variation in the bond angle \(\mathrm{X}-\mathrm{P}-\mathrm{X} : \mathrm{PF}_{3}, 96.3^{\circ} ; \mathrm{PCl}_{3}, 100.3^{\circ}\) ; \(\mathrm{PBr}_{3}, 101.0^{\circ} ; \mathrm{PI}_{3}, 102.0^{\circ} .\) The trend is generally attributed to the change in the electronegativity of the halogen. (a) Assuming that all electron domains are the same size, what value of the \(X-P-X\) angle is predicted by the VSEPR model? (b) What is the general trend in the \(X-P-X\) angle as the halide electronegativity increases? (c) Using the VSEPR model, explain the observed trend in \(X-P-X\) angle as the electronegativity of \(X\) changes. (d) Based on your answer to part (c), predict the structure of \(\mathrm{PBrCl}_{4}\)

Consider a molecule with formula \(\mathrm{AX}_{3}\) . Supposing the \(\mathrm{A}-\mathrm{X}\) bond is polar, how would you expect the dipole moment of the \(\mathrm{AX}_{3}\) molecule to change as the \(\mathrm{X}-\mathrm{A}-\mathrm{X}\) bond angle increases from \(100^{\circ}\) to \(120^{\circ}\)

Dichloroethylene \(\left(\mathrm{C}_{2} \mathrm{H}_{2} \mathrm{Cl}_{2}\right)\) has three forms (isomers), each of which is a different substance. (a) Draw Lewis structures of the three isomers, all of which have a carbon-carbon double bond. ( b) Which of these isomers has a zero dipole moment? (c) How many isomeric forms can chloroethylene, \(\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{Cl}\) have? Would they be expected to have dipole moments?

The structure of borazine, \(\mathrm{B}_{3} \mathrm{N}_{3} \mathrm{H}_{6},\) is a six-membered ring of alternating \(\mathrm{B}\) and \(\mathrm{N}\) atoms. There is one \(\mathrm{H}\) atom bonded to each \(\mathrm{B}\) and to each \(\mathrm{N}\) atom. The molecule is planar. (a) Write a Lewis structure for borazine in which the formal charge on every atom is zero. (b) Write a Lewis structure for borazine in which the octet rule is satisfied for every atom. (c) What are the formal charges on the atoms in the Lewis structure from part (b)? Given the electronegativities of \(\mathrm{B}\) and \(\mathrm{N},\) do the formal charges seem favorable or unfavorable? (d)Do either of the Lewis structures in parts (a) and (b) have multiple resonance structures? (e) What are the hybridizations at the B and N atoms in the Lewis structures from parts (a) and (b)? Would you expect the molecule to be planar for both Lewis structures? (f) The six \(B-N\) bonds in the borazine molecule are all identical in length at 1.44 A. Typical values for the bond lengths of \(\mathrm{B}-\mathrm{N}\) single and double bonds are 1.51 \(\mathrm{A}\) and \(1.31 \mathrm{A},\) respectively. Does the value of the \(\mathrm{B}-\mathrm{N}\) bond length seem to favor one Lewis structure over the other? (g) How many electrons are in the \(\pi\) system of borazine?
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