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Chapter 9: Problem 5

Draw the Lewis structure for HCN. Indicate the hybrid orbitals, and draw a picture showing all the bonds between the atoms, labeling each bond as \(\sigma\) or \(\pi\).

Short Answer

Expert verified
The Lewis structure for HCN is H-C鈮, with Carbon and Nitrogen having sp hybrid orbitals. There is one 蟽 bond between Hydrogen and Carbon, and one 蟽 bond and two 蟺 bonds between Carbon and Nitrogen.

Step by step solution

01

Determine the valence electrons

First, we need to find the total number of valence electrons for HCN. Hydrogen (H) has 1 valence electron, Carbon (C) has 4 valence electrons, and Nitrogen (N) has 5 valence electrons. Thus, the total number of valence electrons in HCN is: \(1 + 4 + 5 = 10\)
02

Arrange the atoms and form bonds

Now, arrange the atoms, placing the less electronegative atom (Carbon) in the center, and form a single bond between each pair of atoms: H-C-N
03

Complete the octets for the terminal atoms

After forming single bonds, we'll complete the octet for the terminal atoms - Hydrogen and Nitrogen. Since Hydrogen only needs 2 electrons to have a full shell, it's already satisfied. For Nitrogen, it currently has 2 electrons; we need to add 6 more electrons (3 lone pairs) to complete its octet: H-C鈮
04

Identify the hybrid orbitals for Carbon and Nitrogen atoms

Now, we need to identify the hybrid orbitals for Carbon and Nitrogen. Each of these atoms is connected to the other atoms through a triple bond, which means they are sp hybridized. In an sp hybridization, two orbitals mix to form two new hybrid orbitals, so both Carbon and Nitrogen will form two sp hybrid orbitals.
05

Draw the bonds and label them as 蟽 or 蟺

Finally, we need to draw the bonds between the atoms and label them as 蟽 (sigma) or 蟺 (pi). There will be one 蟽 bond and two 蟺 bonds between Carbon and Nitrogen, and one 蟽 bond between Hydrogen and Carbon. The final structure is: H-C鈮 (蟽 bond between H and C, one 蟽 bond and two 蟺 bonds between C and N) So, the Lewis structure for HCN is H-C鈮, with each of Carbon and Nitrogen atom having sp hybrid orbitals, one 蟽 bond between Hydrogen and Carbon, and one 蟽 bond and two 蟺 bonds between Carbon and Nitrogen.

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Most popular questions from this chapter

For each of the following molecules or ions that contain sulfur, write the Lewis structure(s), predict the molecular structure (including bond angles), and give the expected hybrid orbitals for sulfur. a. \(\mathrm{SO}_{2}\) b. \(\mathrm{SO}_{3}\) e. \(\mathrm{SO}_{3}^{2-}\) f. \(\mathrm{SO}_{4}^{2-}\) g. \(\mathrm{SF}_{2}\) h. \(\mathrm{SF}_{4}\) i. \(\mathrm{SF}_{6}\) j. \(\mathrm{F}_{3} \mathrm{~S}-\mathrm{SF}\) k. \(\mathrm{SF}_{5}{ }^{+}\)

Carbon monoxide (CO) forms bonds to a variety of metals and metal ions. Its ability to bond to iron in hemoglobin is the reason that \(\mathrm{CO}\) is so toxic. The bond carbon monoxide forms to metals is through the carbon atom: \(\mathrm{M}-\mathrm{C} \equiv \mathrm{O}\) a. On the basis of electronegativities, would you expect the carbon atom or the oxygen atom to form bonds to metals? b. Assign formal charges to the atoms in CO. Which atom would you expect to bond to a metal on this basis? c. In the MO model, bonding MOs place more electron density near the more electronegative atom. (See the HF molecule in Figs. \(9.42\) and \(9.43 .\) Antibonding MOs place more electron density near the less electronegative atom in the diatomic molecule. Use the MO model to predict which atom of carbon monoxide should form bonds to metals.

What type of molecular orbital would result from the in-phase combination of two \(d_{x z}\) atomic orbitals shown below? Assume the \(x\) -axis is the internuclear axis.

Acetylene \(\left(\mathrm{C}_{2} \mathrm{H}_{2}\right)\) can be produced from the reaction of calcium carbide \(\left(\mathrm{CaC}_{2}\right)\) with water. Use both the localized electron and molecular orbital models to describe the bonding in the acetylide anion \(\left(\mathrm{C}_{2}^{2-}\right)\)

Many important compounds in the chemical industry are derivatives of ethylene \(\left(\mathrm{C}_{2} \mathrm{H}_{4}\right)\). Two of them are acrylonitrile and methyl methacrylate. Complete the Lewis structures, showing all lone pairs. Give approximate values for bond angles \(a\) through \(f\). Give the hybridization of all carbon atoms. In acrylonitrile, how many of the atoms in the molecule must lie in the same plane? How many \(\sigma\) bonds and how many \(\pi\) bonds are there in methyl methacrylate and acrylonitrile?
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