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Chapter 13: Problem 182

Bond angle of \(109^{\circ} 28\) ' is found in (a) \(\mathrm{NH}_{3}\) (b) \(\mathrm{H}_{2} \mathrm{O}\) (c) \(\mathrm{CH}_{2}\) (d) \(\mathrm{NH}_{A}^{+}\)

Short Answer

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(d) \(\mathrm{NH}_{4}^{+}\) has a bond angle of \(109^{\circ} 28'\).

Step by step solution

01

Understand the Ideal Bond Angle for Tetrahedral Geometry

A bond angle of \(109^{\circ} 28'\) is a specific characteristic of a tetrahedral molecular geometry. This geometry is common in molecules with a central atom bonded to four other atoms, such as \(\text{CH}_4\).
02

Analyze Each Option for Tetrahedral Geometry

- Option (a), \(\text{NH}_3\), is a trigonal pyramidal molecule with three hydrogen atoms and one lone pair, leading to bond angles close to \(107^{\circ}\). - Option (b), \(\text{H}_2\text{O}\), is bent with two hydrogen atoms and two lone pairs, leading to bond angles around \(104.5^{\circ}\).- Option (c), \(\text{CH}_2\), is not complete since the given formula does not specify an overall tetrahedral framework.- Option (d), \(\text{NH}_4^+\), is a positively charged tetrahedral ion which has exactly \(109^{\circ} 28'\) bond angles between the hydrogen atoms.
03

Conclusion

Among the given options, \(\text{NH}_4^+\) matches the criteria for a tetrahedral geometry bond angle of \(109^{\circ} 28'\). Therefore, the correct answer is option (d).

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Tetrahedral Geometry
In the world of chemistry, tetrahedral geometry is a fundamental concept when examining molecular shapes. Imagine a three-dimensional shape where a central atom is connected to four surrounding atoms, similarly to the corners of a tetrahedron. This configuration is very stable and provides an even distribution of electrons. The angles between these bonds are approximately \(109^{\circ} 28'\), a unique property of tetrahedrally arranged atoms.
The key aspects of tetrahedral geometry include:
  • Four bonded atoms or groups surrounding a central atom.
  • A bond angle of about \(109.5^{\circ}\).
  • Commonly found in compounds like methane (\(\text{CH}_4\)).
Understanding this basic formation helps in predicting the shape of many other molecules.
Molecular Geometry
Molecular geometry gives insight into the 3D arrangement of atoms within a molecule. This arrangement is determined by the number of bonds and lone pairs around a central atom and helps predict physical and chemical properties.
Here's what you need to know about molecular geometry:
  • Determined by the VSEPR theory (Valence Shell Electron Pair Repulsion theory).
  • The arrangement of atoms influences the molecule's properties such as polarity and reactivity.
  • Shapes of molecules include linear, trigonal planar, tetrahedral, trigonal bipyramidal, and octahedral.
By understanding molecular geometry, you can predict how molecules will interact with each other, which is crucial in fields such as biochemistry and pharmaceuticals.
Lone Pairs
Lone pairs, also known as non-bonding pairs, are pairs of valence electrons that are not shared with other atoms. They occupy space around a central atom and significantly affect a molecule鈥檚 geometry by repelling bonding pairs, creating deviations in bond angles.
Key points about lone pairs include:
  • They do not participate in chemical bonding.
  • They can distort bond angles; for example, in \(\text{NH}_3\) causing the bond angle to shrink to \(107^{\circ}\).
  • Affect molecular geometry leading to shapes like bent and trigonal pyramidal.
Understanding their influence is essential to grasp the differences between idealized and actual molecular geometries.
Trigonal Pyramidal
The trigonal pyramidal shape is often seen in molecules where a central atom is bonded to three surrounding atoms and has one lone pair. This geometry is a variation of tetrahedral geometry but with a lone pair causing a distortion.
Characteristics of trigonal pyramidal structures include:
  • An example is ammonia (\(\text{NH}_3\)).
  • Has a bond angle of approximately \(107^{\circ}\), slightly less than the tetrahedral angle due to lone pair-bond pair repulsion.
  • The presence of a lone pair makes the structure asymmetrical.
The trigonal pyramidal shape helps explain many molecular behaviors, including dipole moments which contribute to the molecule's physical properties.
Bent Structure
A bent or angular structure arises when a central atom is connected to two atoms and possesses one or more lone pairs. The lone pairs push the bonded atoms closer together, creating a bent shape.
Notable features of bent structures include:
  • Water (\(\text{H}_2\text{O}\)) is a classic example with a bond angle around \(104.5^{\circ}\).
  • Results from the lone pair-bond pair repulsion compressing bond angles.
  • This structure often leads to polar molecules due to the unequal distribution of charge.
Understanding bent structures is vital in predicting how substances will dissolve, react, and interact in various chemical processes.

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Most popular questions from this chapter

Among the following pairs, the one in which the two species are not isostructural is (a) \(\mathrm{SiF}_{4}\) and \(\mathrm{SF}_{4}\) (b) \(\mathrm{IO}_{3}^{-}\)and \(\mathrm{XeO}_{3}\) (c) \(\mathrm{BH}_{4}\) and \(\mathrm{NH}_{4}\) (d) \(\mathrm{PF}_{6}\) and \(\mathrm{SF}_{6}\)

Which of the following is correct? (a) The rate of ionic reactions are very slow (b) The number of electrons present in the valence shell of \(\mathrm{S}\) in \(\mathrm{SF}_{6}\) is 12 (c) According to VSEPR theory \(\mathrm{SnCl}_{2}\) is a linear molecule (d) The correct order of stability to form ionic compounds among \(\mathrm{Na}^{+}, \mathrm{Mg}^{2+}\) and \(\mathrm{Al}^{3+}\) is \(\mathrm{Al}^{3+}>\) \(\mathrm{Mg}^{2+}>\mathrm{Na}^{+}\)

The species having tetrahedral shape is (a) \(\left[\mathrm{PdCl}_{4}\right]^{2}\) (b) \(\left[\mathrm{Ni}(\mathrm{CN})_{4}\right]^{2}\) (c) \(\left[\mathrm{Pd}(\mathrm{CN})_{4}\right]^{2}\) (d) \(\left[\mathrm{NiCl}_{4}\right]^{2}\)

What is the number of sigma and pi bonds present in a molecule of sulphuric acid? (a) \(6 \sigma, 2 \pi\) (b) \(6 \sigma, 0 \pi\) (c) \(2 \sigma, 4 \pi\) (d) \(2 \sigma, 2 \pi\)

Main axis of a diatomic molecule is z, molecule orbitals \(\mathrm{p}_{\mathrm{x}}\) and \(\mathrm{p}_{\mathrm{y}}\) overlap to form, which of the following orbital? (a) \(\pi\) molecular orbital (b) \(\sigma\) molecular orbital (c) \(\delta\) molecular orbital (d) no bond will form
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