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Chapter 9: Problem 16

Describe the bond angles to be found in each of the following molecular structures: (a) trigonal planar, (b) tetrahedral, (c) octahedral, (d) linear.

Short Answer

Expert verified
The bond angles for each molecular structure are: (a) Trigonal planar: 120°, (b) Tetrahedral: 109.5°, (c) Octahedral: 90° and 180°, (d) Linear: 180°.

Step by step solution

01

Trigonal planar bond angle

Trigonal planar molecules have three atoms bonded to the central atom and no lone electron pairs on the central atom. These bonded atoms are evenly spaced around the central atom, forming a plane. The bond angle can be found by dividing 360°, which represents a full circle, between the three atoms. In this case: \(Bond angle = \frac{360°}{3} = 120°\) The bond angle in a trigonal planar molecular structure is 120°.
02

Tetrahedral bond angle

Tetrahedral molecules have four atoms bonded to the central atom and no lone electron pairs on the central atom. The bond angle in a tetrahedral molecular structure can be found using the geometry of a regular tetrahedron, where the bond angle is known as the tetrahedral angle. The tetrahedral angle is approximately: \(Bond angle = 109.5°\) The bond angle in a tetrahedral molecular structure is 109.5°.
03

Octahedral bond angle

Octahedral molecules have six atoms bonded to the central atom and no lone electron pairs on the central atom. In an octahedral structure, the atoms form a regular octahedron. The bond angles in an octahedral structure can be found by considering the geometry of the octahedron. There are two types of bond angles in an octahedral structure: 1. The angle between two atoms bonded to the central atom in the same plane: \(90°\) 2. The angle between two atoms bonded to the central atom in opposite planes: \(180°\) The bond angles in an octahedral molecular structure are 90° and 180°.
04

Linear bond angle

Linear molecules have two atoms bonded to the central atom and no lone electron pairs on the central atom. The bonded atoms are in a straight line with the central atom. Since they form a straight line, the bond angle in a linear molecular structure is: \(Bond angle = 180°\) The bond angle in a linear molecular structure is 180°. In conclusion, the bond angles for each molecular structure are: a) Trigonal planar: 120° b) Tetrahedral: 109.5° c) Octahedral: 90° and 180° d) Linear: 180°

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Most popular questions from this chapter

(a) The PH \(_{3}\) molecule is polar. Does this offer experimental proof that the molecule cannot be planar? Explain. (b) It turns out that ozone, \(\mathrm{O}_{3},\) has a small dipole moment. How is this possible, given that all the atoms are the same?

The vertices of a tetrahedron correspond to four alternating corners of a cube. By using analytical geometry, demonstrate that the angle made by connecting two of the vertices to a point at the center of the cube is \(109.5^{\circ},\) the characteristic angle for tetrahedral molecules.

In which of the following \(\mathrm{AF}_{n}\) molecules or ions is there more than one \(\mathrm{F}-\mathrm{A}-\mathrm{Fbond}\) angle: \(\mathrm{SiF}_{4}, \mathrm{PF}_{5}, \mathrm{SF}_{4}, \mathrm{AsF}_{3} ?\)

Dichloroethylene \(\left(\mathrm{C}_{2} \mathrm{H}_{2} \mathrm{Cl}_{2}\right)\) has three forms (isomers), each of which is a different substance. (a) Draw Lewis structures of the three isomers, all of which have a carbon-carbon double bond. ( b) Which of these isomers has a zero dipole moment? (c) How many isomeric forms can chloroethylene, \(\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{Cl}\) have? Would they be expected to have dipole moments?

In ozone, \(\mathrm{O}_{3}\) , the two oxygen atoms on the ends of the molecule are equivalent to one another. (a) What is the best choice of hybridization scheme for the atoms of ozone? (b) For one of the resonance forms of ozone, which of the orbitals are used to make bonds and which are used to hold nonbonding pairs of electrons? (c) Which of the orbitals can be used to delocalize the \(\pi\) electrons? (d) How many electrons are delocalized in the \(\pi\) system of ozone?
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