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Chapter 12: Problem 126

(a) What are the \(\mathrm{C}-\mathrm{C}-\mathrm{C}\) bond angles in diamond? (b) What are they in graphite (in one sheet)? (c) What atomic orbitals are involved in the stacking of graphite sheets with each other?

Short Answer

Expert verified
In diamond, the C-C-C bond angle is approximately 109.47° due to its tetrahedral structure. In one sheet of graphite, the C-C-C bond angle is 120° because carbon atoms form planar hexagonal rings. The stacking of graphite sheets with each other involves the unhybridized 2p orbitals forming π bonds, resulting in weak Van der Waals forces between the adjacent π clouds.

Step by step solution

01

Determine the bond structure in diamond

In diamond, each Carbon atom is covalently bonded to four other Carbon atoms in a tetrahedral structure.
02

Use tetrahedral angle

The bond angle in a tetrahedral structure is approximately 109.47°. Therefore, in diamond, the C-C-C bond angle is 109.47°. b) Calculate Graphite C-C-C bond angle in one sheet
03

Determine the bond structure in graphite

In graphite, each Carbon atom is covalently bonded to three neighboring Carbon atoms, forming planar hexagonal rings.
04

Use trigonometry to find bond angle

The hexagonal ring contains 6 Carbon atoms and its internal angles are 120°. Thus, C-C-C bond angle in one sheet of graphite is 120°. c) Identify the atomic orbitals involved in the stacking of graphite sheets
05

Determine the hybridization of carbon in graphite

In graphite, each Carbon atom is bonded to three neighboring Carbon atoms. This configuration corresponds to an sp2 hybridization, where three (2p and 1s) orbitals form three sp2 hybrid orbitals for bonding.
06

Identify the remaining orbital

Since each Carbon atom contributes one 2p orbital for hybridization, there's one 2p orbital remaining for each Carbon atom. These remaining 2p orbitals form π bonds.
07

Determine the atomic orbitals involved in stacking

The stacking of graphite sheets with each other is due to weak Van der Waals forces between the adjacent π clouds formed by the unhybridized 2p orbitals. These forces allow the sheets in graphite to slide over each other, resulting in its characteristic slipperiness. In summary, the C-C-C bond angles are 109.47° in diamond, 120° in a single sheet of graphite, and the atomic orbitals involved in the stacking of graphite sheets are the unhybridized 2p orbitals forming the π bonds.

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Most popular questions from this chapter

Proteins are naturally occurring polymers formed by condensation reactions of amino acids, which have the general structure In this structure, \(-\mathrm{R}\) represents \(-\mathrm{H},-\mathrm{CH}_{3},\) or another group of atoms; there are 20 different natural amino acids, and each has one of 20 different R groups. (a) Draw the general structure of a protein formed by condensation polymerization of the generic amino acid shown here. (b) When only a few amino acids react to make a chain, the product is called a "peptide" rather than a protein; only when there are 50 amino acids or more in the chain would the molecule be called a protein. For three amino acids (distinguished by having three different R groups, R1, R2, and R3), draw the peptide that results from their condensation reactions. (c) The order in which the R groups exist in a peptide or protein has a huge influence on its biological activity. To distinguish different peptides and proteins, chemists call the first amino acid the one at the \({ }^{\prime \prime} \mathrm{N}\) terminus" and the last one the one at the "C terminus." From your drawing in part (b) you should be able to figure out what "N terminus" and "C terminus" mean. How many different peptides can be made from your three different amino acids?

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