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Chapter 4: Problem 10

Give one example of a compound having a linear molecular structure that has an overall dipole moment (is polar) and one example that does not have an overall dipole moment (is nonpolar). Do the same for molecules that have trigonal planar and tetrahedral molecular structures.

Short Answer

Expert verified
Examples of compounds with different molecular geometries: 1. Linear molecular structure - Polar: Hydrogen chloride (HCl) - Nonpolar: Carbon dioxide (CO2) 2. Trigonal planar molecular structure - Polar: Sulfur trioxide (SO3) - Nonpolar: Boron trifluoride (BF3) 3. Tetrahedral molecular structure - Polar: Methane (CH4) - Nonpolar: Carbon tetrachloride (CCl4)

Step by step solution

01

Linear molecular structure - Polar

An example of a linear molecular structure that has an overall dipole moment (polar) is hydrogen chloride (HCl). In HCl, there is a difference in electronegativity between the hydrogen and chlorine atoms, leading to an uneven distribution of electron density and the creation of a dipole moment, making it polar.
02

Linear molecular structure - Nonpolar

An example of a linear molecular structure that does not have an overall dipole moment (nonpolar) is carbon dioxide (CO2). In CO2, the oxygen atoms are more electronegative than the central carbon atom, but since the molecule is linear and the more electronegative atoms are symmetrically arranged, these dipoles cancel each other out and it is a nonpolar molecule.
03

Trigonal planar molecular structure - Polar

An example of a trigonal planar molecular structure with an overall dipole moment (polar) is sulfur trioxide (SO3). This molecule has a trigonal planar geometry, with sulfur in the center and oxygen atoms surrounding it in a triangle. Due to the difference in electronegativity between the sulfur and oxygen atoms, there is an overall dipole moment, and the molecule is polar.
04

Trigonal planar molecular structure - Nonpolar

An example of a trigonal planar molecular structure without an overall dipole moment (nonpolar) is boron trifluoride (BF3). In this molecule, boron is the central atom and is surrounded by three fluorine atoms in a trigonal planar arrangement. Although the fluorine atoms have greater electronegativity than boron, the dipoles created by these differences cancel each other out due to the molecule's symmetry, making it nonpolar.
05

Tetrahedral molecular structure - Polar

An example of a tetrahedral molecular structure with an overall dipole moment (polar) is methane (CH4). In this molecule, carbon is the central atom and is surrounded by four hydrogen atoms in a tetrahedral configuration. The difference in electronegativity between carbon and hydrogen creates a dipole moment, and the overall geometry results in a polar molecule.
06

Tetrahedral molecular structure - Nonpolar

An example of a tetrahedral molecular structure without an overall dipole moment (nonpolar) is carbon tetrachloride (CCl4). In CCl4, carbon is the central atom and is surrounded by four chlorine atoms in a tetrahedral arrangement. Although chlorine atoms are more electronegative than carbon, the symmetric distribution of the chlorine atoms results in the cancellation of the individual dipoles, making this molecule nonpolar.

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Most popular questions from this chapter

What do each of the following sets of compounds/ions have in common with each other? a. \(\mathrm{XeCl}_{4}, \mathrm{XeCl}_{2}\) b. ICls, \(\operatorname{TeF}_{4}, \operatorname{ICl}_{3}, \mathrm{PCl}_{3}, \mathrm{SCl}_{2}, \mathrm{SeO}_{2}\)

The diatomic molecule OH exists in the gas phase. The bond length and bond energy have been measured to be \(97.06 \mathrm{pm}\) and \(424.7 \mathrm{kJ} / \mathrm{mol},\) respectively. Assume that the OH molecule is analogous to the HF molecule discussed in the chapter and that molecular orbitals result from the overlap of a lowerenergy \(p_{z}\) orbital from oxygen with the higher- energy \(1 s\) orbital of hydrogen (the \(\mathrm{O}-\mathrm{H}\) bond lies along the \(z\) -axis). a. Which of the two molecular orbitals will have the greater hydrogen 1s character? b. Can the \(2 p_{x}\) orbital of oxygen form molecular orbitals with the \(1 s\) orbital of hydrogen? Explain. c. Knowing that only the \(2 p\) orbitals of oxygen will interact significantly with the \(1 s\) orbital of hydrogen, complete the molecular orbital energy- level diagram for OH. Place the correct number of electrons in the energy levels. d. Estimate the bond order for OH. e. Predict whether the bond order of \(\mathrm{OH}^{+}\) will be greater than, less than, or the same as that of OH. Explain.

Show how two \(2 p\) atomic orbitals can combine to form a \(\sigma\) or a \(\pi\) molecular orbital.

In the molecular orbital model, compare and contrast \(\sigma\) bonds with \(\pi\) bonds. What orbitals form the \(\sigma\) bonds and what orbitals form the \(\pi\) bonds? Assume the \(z\) -axis is the internuclear axis.

What are molecular orbitals? How do they compare with atomic orbitals? Can you tell by the shape of the bonding and antibonding orbitals which is lower in energy? Explain.
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