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Chapter 1: Problem 39

Use VSEPR to predict bond angles about each atom of carbon, nitrogen, and oxygen in these molecules. a. b. c. d. e. f.

Short Answer

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Question: Predict the bond angles around the carbon, nitrogen, and oxygen atoms in a given molecule using the VSEPR theory. Answer: To predict bond angles, follow the steps outlined in the provided solution: Determine the electronic geometry of the atom, deduce the VSEPR notation, identify the molecular shape, and determine the corresponding bond angles for that shape. Once you know the bond angles, you can compare them for the carbon, nitrogen, and oxygen atoms in your specific molecule.

Step by step solution

01

Determine the electronic geometry of the atom

To predict bond angles, we first need to know the electronic geometry associated with the central atom. In this case, we will analyze carbon, nitrogen, and oxygen atoms. Each atom has a specific number of valence electrons (carbon has 4, nitrogen has 5, and oxygen has 6). You need to determine the total number of valence electrons around the atom, considering any shared electrons from bonds.
02

Deduce the VSEPR notation

Based on the number of bonding electron pairs and lone electron pairs surrounding the atom, deduce the VSEPR notation. The notation follows the format AXnEm, where A is the central atom, Xn represents the number of bonded atoms (n), and Em represents the number of lone pairs (m).
03

Identify the molecular shape

Using the VSEPR notation, identify the shape of the molecule which is directly associated with the atom. Common shapes include linear, trigonal planar, tetrahedral, trigonal bipyramidal, and octahedral.
04

Determine the bond angles

Finally, determine the bond angles that correspond to the molecular shape you identified in step 3. The bond angles will vary based on the number of bonding and lone electron pairs around the central atom. Here are some general bond angles for common shapes: - Linear: 180° - Trigonal planar: 120° - Tetrahedral: 109.5° - Trigonal bipyramidal: 90° and 120° - Octahedral: 90° Keep in mind that lone pairs can affect bond angles slightly, causing them to be slightly smaller than the typical angles listed above. Once you have determined the bond angles for the atom, you can then compare them to the atoms in your specific molecules.

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Most popular questions from this chapter

Draw structural formulas for the three tertiary \(\left(3^{\circ}\right)\) amines with the molecular formula \(\mathrm{C}_{5} \mathrm{H}_{13} \mathrm{~N}\).

Draw Lewis structures and condensed structural formulas for the four alcohols with the molecular formula \(\mathrm{C}_{4} \mathrm{H}_{10} \mathrm{O}\). Classify each alcohol as primary, secondary, or tertiary.

Draw Lewis structures, showing all valence electrons, for these molecules. (a) \(\mathrm{C}_{2} \mathrm{H}_{6}\) (b) \(\mathrm{CS}_{2}\) (c) \(\mathrm{HCN}\)

Cyanic acid, HOCN, and isocyanic acid, HNCO, dissolve in water to yield the same anion on loss of \(\mathrm{H}^{+}\). (a) Write a Lewis structure for cyanic acid. (b) Write a Lewis structure for isocyanic acid. (c) Account for the fact that each acid gives the same anion on loss of \(\mathrm{H}^{+}\). 1.71 In Chapter 6, we study a group of organic cations called carbocations. Following is the structure of one such carbocation, the tert-butyl cation. (a) How many electrons are in the valence shell of the carbon bearing the positive charge? (b) Using VSEPR, predict the bond angles about this carbon. (c) Given the bond angle you predicted in (b), what hybridization do you predict for this carbon?

Classify each bond as nonpolar covalent or polar covalent or state that ions are formed. (a) \(\mathrm{S}-\mathrm{H}\) (b) \(\mathrm{P}-\mathrm{H}\) (c) \(\mathrm{C}-\mathrm{F}\) (d) \(\mathrm{C}-\mathrm{Cl}\)
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