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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
(a) In a trigonal planar structure, the bond angle is \(120\,degrees\) as three electron pairs are evenly distributed in a plane. (b) A tetrahedral structure has a bond angle of approximately \(109.5\,degrees\). (c) For an octahedral structure, the bond angle is \(90\,degrees\). (d) In a linear structure, the bond angle is \(180\,degrees\).

Step by step solution

01

(a) Trigonal Planar Bond Angle

In a trigonal planar molecular structure, there are three electron pairs around the central atom. These electron pairs are spread out evenly in a plane. The bond angle for a trigonal planar structure is 120 degrees, as there are 360 degrees in a circle and the three electron pairs are evenly distributed around the central atom. So, the bond angle is \(360\,degrees \div 3 = 120\,degrees\).
02

(b) Tetrahedral Bond Angle

In a tetrahedral molecular structure, four electron pairs are arranged around the central atom. The bond angle for a tetrahedral structure can be calculated using the inverse cosine function: \(\cos^{-1}(\frac{-1}{3}) \approx 109.5\, degrees\). Hence, the bond angle for a tetrahedral structure is approximately 109.5 degrees.
03

(c) Octahedral Bond Angle

In an octahedral molecular structure, there are six electron pairs arranged around the central atom. In this structure, the electron pairs are located at the vertices of an octahedron and are arranged such that there are two sets of three collinear electron pairs. The bond angle for an octahedral structure is 90 degrees since the electron pairs are positioned perpendicular to each other.
04

(d) Linear Bond Angle

In a linear molecular structure, the central atom is surrounded by two electron pairs. The bond angle in a linear structure is 180 degrees, as both electron pairs are directly opposite each other around the central atom along a straight line.

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Most popular questions from this chapter

\mathrm{An} \mathrm{} \mathrm{AB}_{2}\( molecule is described as linear, and the \)\mathrm{A}-\mathrm{B}\( bond length is known. (a) Does this information completely describe the geometry of the molecule? (b) Can you tell how many nonbonding pairs of electrons are around the \)A$ atom from this information?

Write the electron configuration for the first excited state for \(\mathrm{N}_{2}\), that is, the state with the highest-energy electron moved to the next available energy level. (a) Is the nitrogen in its first excited state diamagnetic or paramagnetic? (b) Is the \(\mathrm{N}-\mathrm{N}\) bond strength in the first excited state stronger or weaker compared to that in the ground state?

(a) Methane \(\left(\mathrm{CH}_{4}\right)\) and the perchlorate ion \(\left(\mathrm{ClO}_{4}{ }^{-}\right)\)are both described as tetrahedral. What does this indicate about their bond angles? (b) The \(\mathrm{NH}_{3}\) molecule is trigonal pyramidal, while \(\mathrm{BF}_{3}\) is trigonal planar. Which of these molecules is flat?

Consider the \(\mathrm{H}_{2}^{+}\)ion. (a) Sketch the molecular orbitals of the ion and draw its energy-level diagram. (b) How many electrons are there in the \(\mathrm{H}_{2}^{+}\)ion? (c) Write the electron configuration of the ion in terms of its MOs. (d) What is the bond order in \(\mathrm{H}_{2}^{+}\)? (e) Suppose that the ion is excited by light so that an electron moves from a lower-energy to a higherenergy MO. Would you expect the excited-state \(\mathrm{H}_{2}^{+}\)ion to be stable or to fall apart? (f) Which of the following statements about part (e) is correct: (i) The light excites an electron from a bonding orbital to an antibonding orbital, (ii) The light excites an electron from an antibonding orbital to a bonding orbital, or (iii) In the excited state there are more bonding electrons than antibonding electrons?

(a) What is the physical basis for the VSEPR model? (b) When applying the VSEPR model, we count a double or triple bond as a single electron domain. Why is this justified?
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