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Chapter 9: Problem 22

How many electron domains are surrounding the central atoms which adopt the following geometries? (a) linear (b) trigonal planar (c) trigonal pyramidal (d) trigonal bipyramidal.

Short Answer

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(a) 2, (b) 3, (c) 4, (d) 5

Step by step solution

01

Understanding Electron Domains

Electron domains refer to sets of electrons that occupy space around a central atom. This includes bonded atoms (single, double, or triple bonds count as one domain) and lone pairs of electrons.
02

Identifying Electron Domains for Linear Geometry

In linear geometry, there are 2 electron domains around the central atom. This can be visualized with two bonded atoms in a straight line, such as in carbon dioxide (CO鈧�).
03

Identifying Electron Domains for Trigonal Planar Geometry

For trigonal planar geometry, the central atom has 3 electron domains. These could be three bonded atoms arranged in a triangular shape in the same plane, as seen in boron trifluoride (BF鈧�).
04

Identifying Electron Domains for Trigonal Pyramidal Geometry

In trigonal pyramidal geometry, there are 4 electron domains. This includes three bonded atoms and one lone pair of electrons, leading to a triangular base with a central atom at the apex, exemplified by ammonia (NH鈧�).
05

Identifying Electron Domains for Trigonal Bipyramidal Geometry

The trigonal bipyramidal geometry involves 5 electron domains, which could be five bonded atoms in a shape resembling two pyramids sharing a base, such as in phosphorus pentachloride (PCl鈧�).

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Key Concepts

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

Molecular Geometry
Molecular geometry refers to the three-dimensional arrangement of atoms in a molecule. It is crucial for understanding how molecules interact with one another and their environment. The geometry can influence properties like polarity and reactivity. Imagine molecules like a construction made out of connected rods鈥攊t helps in visualizing how atoms are positioned. For instance, in linear geometry, atoms are arranged in a straight line. In contrast, trigonal planar geometry forms a flat triangular shape. When the molecular structure becomes more complex, like in trigonal bipyramidal, it looks like two pyramids sharing a base.
VSEPR Theory
The VSEPR (Valence Shell Electron Pair Repulsion) theory helps predict the geometry of molecules. It states that electron pairs around a central atom will arrange themselves to minimize repulsion. This means they want to be as far apart as possible. Think of these electron pairs as tiny magnets that repel each other. The theory is named for how these electron pairs behave:
  • They repel each other
  • They try to get as far apart as possible
  • Their repulsion affects molecular shape and bond angles
This core idea helps in understanding why different molecules have different shapes. It explains everything from linear molecules like CO鈧� to more complex structures like PCl鈧�.
Bonding
Bonding is the process of atoms joining together, usually involving electrons. There are different types of bonds, such as single, double, and triple bonds. Each of these counts as one electron domain when figuring out molecular geometry. In simple terms, a bond is like a handshake between atoms that holds them together.
  • Single bonds involve the sharing of one pair of electrons
  • Double bonds share two pairs of electrons
  • Triple bonds involve three pairs of shared electrons
These different types of bonds not only dictate how atoms connect but also influence properties like strength and length of the connection.
Lone Pairs
Lone pairs are pairs of electrons that are not involved in bonding and remain on the central atom. Unlike bonding pairs, these electrons do not connect with other atoms, but they do take up space. Imagine them like reserved spots at the table, affecting how the table is set.
  • Lone pairs occupy space around the central atom
  • They influence the geometry by repelling bonded pairs
  • These can affect molecular properties such as solubility and reactivity
For example, in ammonia (NH鈧�), there is one lone pair, which pushes the three hydrogen atoms down, creating a trigonal pyramidal shape. Understanding lone pairs is vital in predicting and explaining the actual shape of molecules.

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Most popular questions from this chapter

A compound composed of \(6.7 \% \mathrm{H}, 40.0 \% \mathrm{C},\) and \(53.3 \% \mathrm{O}\) has a molar mass of approximately \(60 \mathrm{~g} / \mathrm{mol}\). (a) What is the molecular formula of the compound? (b) What is its Lewis structure if the two \(\mathrm{O}\) are bonded to \(\mathrm{C} ?(\mathbf{c})\) What is the geometry and hybridization of the \(\mathrm{C}\) atom that is bonded to \(2 \mathrm{O}\) atoms? (d) How many \(\sigma\) and how many \(\pi\) bonds are there in the molecule?

Which of the following statements about hybrid orbitals is or are true? (i) After an atom undergoes sp hybridization, there is one unhybridized \(p\) orbital on the atom, (ii) Under \(s p^{2}\) hybridization, the large lobes point to the vertices of an equilateral triangle, and (iii) The angle between the large lobes of \(s p^{3}\) hybrids is \(109.5^{\circ}\).

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

Consider the following \(\mathrm{XF}_{4}\) ions: \(\mathrm{PF}_{4}^{-}, \mathrm{BrF}_{4}^{-}, \mathrm{ClF}_{4}^{+}\), and \(\mathrm{AlF}_{4}^{-}\). (a) Which of the ions have more than an octet of electrons around the central atom? (b) For which of the ions will the electron-domain and molecular geometries be the same? (c) Which of the ions will have an octahedral electron-domain geometry? (d) Which of the ions will exhibit a see-saw molecular geometry?

What are the electron-domain and molecular geometries of a molecule that has the following electron domains on its central atom? (a) Three bonding domains and no nonbonding domains, (b) three bonding domains and one nonbonding domain, (c) two bonding domains and two nonbonding domains.
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