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Chapter 8: Problem 75

A carbene is a compound that has a carbon bonded to two atoms and a lone pair remaining on the carbon. Many carbenes are very reactive. (a) Draw the Lewis structure for the simplest carbene, \(\mathrm{H}_{2} \mathrm{C}\). (b) Predict the length of the carbon-carbon bond you would expect if two $\mathrm{H}_{2} \mathrm{C}$ molecules reacted with each other by a combination reaction.

Short Answer

Expert verified
The Lewis structure for H2C is: H | C: | H When two H2C molecules react with each other, they will form a single carbon-carbon bond with an approximate bond length of 1.54 Å.

Step by step solution

01

Draw the Lewis structure for H2C

To draw the Lewis structure, we'll start by counting the total number of valence electrons. Carbon has 4 valence electrons, while each hydrogen atom has 1 valence electron. Therefore, H2C has a total of (2 x 1) + 4 = 6 valence electrons. Place carbon in the center, then surround it with hydrogen atoms and a lone pair of electrons. H | C: | H
02

Predict the carbon-carbon bond length for two H2C molecules

If two H2C molecules reacted with each other by a combination reaction, the carbon with the lone pair would bond with the carbon of the other H2C molecule. Since both carbons have a lone pair, they would share these electrons to form a bond. The bond formed between the carbons in this reaction will be a single bond. The length of a single carbon-carbon bond is approximately 1.54 Å. So, we would expect the carbon-carbon bond formed between two H2C molecules to be approximately 1.54 Å in length.

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Most popular questions from this chapter

Although \(\mathrm{I}_{3}^{-}\) is a known ion, \(\mathrm{F}_{3}^{-}\) is not. \((\mathbf{a})\) Draw the Lewis structure for \(I_{3}^{-}\) (it is linear, not a triangle). (b) One of your classmates says that \(\mathrm{F}_{3}^{-}\) does not exist because \(\mathrm{F}\) is too electronegative to make bonds with another atom. Give an example that proves your classmate is wrong. (c) Another classmate says \(\mathrm{F}_{3}^{-}\) does not exist because it would violate the octet rule. Is this classmate possibly correct? (d) Yet another classmate says \(\mathrm{F}_{3}^{-}\) does not exist because \(\mathrm{F}\) is too small to make bonds to more than one atom. Is this classmate possibly correct?

1,2-dihydroxybenzene is obtained when two of the adjacent hydrogen atoms in benzene are replaced with an OH group. A skeleton of the molecule is shown here. (a) Complete a Lewis structure for the molecule using bonds and electron pairs as needed. (b) Are there any resonance structures for the molecule? If so, sketch them. (c) Are the resonance structures in (a) and (b) equivalent to one another as they are in benzene?

Calculate the formal charge on the indicated atom in each of the following molecules or ions: (a) the central oxygen atom in \(\mathrm{O}_{3},(\mathbf{b})\) phosphorus in \(\mathrm{PF}_{6}^{-},(\mathbf{c})\) nitrogen in \(\mathrm{NO}_{2}\), (d) iodine in ICl \(_{3}\), (e) chlorine in \(\mathrm{HClO}_{4}\) (hydrogen is bonded to \(\mathrm{O}\) ).

(a) Is lattice energy usually endothermic or exothermic? (b) Write the chemical equation that represents the process of lattice energy for the case of NaCl. (c) Would you expect salts like \(\mathrm{NaCl}\), which have singly charged ions, to have larger or smaller lattice energies compared to salts like CaO which are composed of doubly-charged ions?

Write Lewis structures that obey the octet rule for each of the following, and assign oxidation numbers and formal charges to each atom: $(\mathbf{a}) \mathrm{OCS},(\mathbf{b}) \mathrm{SOCl}_{2}(\mathrm{~S}$ is the central atom), (c) \(\mathrm{BrO}_{3}^{-}\), (d) \(\mathrm{HClO}_{2}(\mathrm{H}\) is bonded to \(\mathrm{O})\).
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