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Chapter 6: Problem 66

Using lines, solid wedges, and dashed wedges, draw the three-dimensional shape of chloromethylacetylene, \(\mathrm{C}_{3} \mathrm{H}_{3} \mathrm{Cl}\). Indicate the numeric value of all bond angles.

Short Answer

Expert verified
The three-dimensional structure of chloromethylacetylene (C3H3Cl) can be represented as: H 180° / C≡C-C-Cl 180° 180° The molecule has a linear arrangement with bond angles of 180° between H-C≡C, C≡C-C, and C-C-Cl.

Step by step solution

01

Draw the Central Carbon Atoms

First, draw a line to represent the triple bond between the two carbon atoms and a single bond connecting the central carbon atom (C) with the other carbon atom (C) in a linear arrangement: C≡C-C
02

Add the Hydrogen Atom

Now, let's add the hydrogen atom (H) connected to the first carbon atom by a single bond. Since this hydrogen bond would be coming out of the plane, we draw it using a solid wedge: H / C≡C-C
03

Add the Chlorine Atom

Next, draw the chlorine atom (Cl) bonded to the last carbon atom in linear arrangement by a single bond: H / C≡C-C-Cl
04

Indicate Bond Angles

Now, we will indicate the numeric values of the bond angles. In this molecule, there are three atoms involved: hydrogen (H), carbon (C), and chlorine (Cl). - The bond angle between H, the first C, and the second C is 180° because of the linear arrangement. - The bond angle between the first C, the second C (in the triple bond), and the third C is also 180° because of the linear connection. - The bond angle between the second C, the third C, and Cl is also 180°, again due to the linear arrangement. Add these angle values to the drawing: H 180° / C≡C-C-Cl 180° 180° The final representation of the chloromethylacetylene molecule (C3H3Cl) is as follows: H 180° / C≡C-C-Cl 180° 180°

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Most popular questions from this chapter

Is it possible to predict whether a molecule will be polar? Explain completely what you would need to know about the molecule.

Which should have the largest molecular dipole moment: \(\mathrm{H}_{2}, \mathrm{CO}_{2}, \mathrm{CH}_{3} \mathrm{~F}\), or \(\mathrm{CH}_{7} \mathrm{I}\) ?

Which should have the largest dipole moment: \(\mathrm{O}_{3}, \mathrm{H}_{2} \mathrm{O}\), or \(\mathrm{OF}_{2} ?\)

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Consider the molecule \(\mathrm{N}_{2} \mathrm{O}\) (connected \(\mathrm{N}-\mathrm{N}-\mathrm{O})\) (a) Draw the dot diagram. (b) Draw the molecule's three-dimensional shape, and label the numeric value of all bond angles. (c) What is the shape of this molecule? (d) Draw in the individual bond dipole moments. (e) Is the molecule polar? If yes, draw the molecular dipole moment vector.
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