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Chapter 21: Problem 64

What intermolecular forces are present in the following? (a) \(\mathrm{Cl}_{2}\) (b) \(\mathrm{HBr}\) (c) \(\mathrm{HF}\) (d) \(\mathrm{HClO}_{4}\) (e) \(\mathrm{MgI}_{2}\)

Short Answer

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Question: Identify the intermolecular forces present in each of the following substances: (a) Cl2, (b) HBr, (c) HF, (d) HClO4, and (e) MgI2. Answer: (a) London dispersion forces, (b) London dispersion forces and dipole-dipole interactions, (c) London dispersion forces, dipole-dipole interactions, and hydrogen bonding, (d) London dispersion forces and dipole-dipole interactions, (e) ionic bonding.

Step by step solution

01

(a) Identify intermolecular forces in Cl2

In Cl2, two chlorine atoms are bound together by a covalent bond, and both have the same electronegativity. There is no permanent dipole, and hydrogen is not present, so hydrogen bonding is not possible. Therefore, the only intermolecular force present in \(\mathrm{Cl}_{2}\) is London dispersion forces.
02

(b) Identify intermolecular forces in HBr

In HBr, hydrogen is bonded to bromine, which has a significantly different electronegativity. The molecule has a permanent dipole, leading to dipole-dipole interactions between molecules. London dispersion forces are also present since they are always present between all molecules. However, hydrogen bonding is not possible because Br is not one of the three most electronegative elements F, O or N. Therefore, the intermolecular forces present in \(\mathrm{HBr}\) are London dispersion forces and dipole-dipole interactions.
03

(c) Identify intermolecular forces in HF

In the HF molecule, hydrogen is bonded to fluorine, which is the most electronegative element, resulting in a strong, permanent dipole. Therefore, dipole-dipole interactions are present. London dispersion forces are also always present. Additionally, since hydrogen is bonded to fluorine, which is one of the three most electronegative elements (F, O, N), hydrogen bonding is possible. Hence, the intermolecular forces present in \(\mathrm{HF}\) are London dispersion forces, dipole-dipole interactions, and hydrogen bonding.
04

(d) Identify intermolecular forces in HClO4

The HClO4 molecule, also known as perchloric acid, contains hydrogen bonded to a chlorine-oxygen bond, creating a polar molecule with a permanent dipole. This leads to dipole-dipole interactions. London dispersion forces are also present. However, hydrogen bonding is not possible because the hydrogen atom is not directly bonded to one of the three most electronegative elements (F, O, N). Thus, the intermolecular forces present in \(\mathrm{HClO}_{4}\) are London dispersion forces and dipole-dipole interactions.
05

(e) Identify intermolecular forces in MgI2

MgI2 is an ionic compound consisting of magnesium ions and iodide ions. The primary intermolecular force present in ionic compounds is the electrostatic attraction between ions, known as ionic bonding. No covalent bonds exist in MgI2, so there are no London dispersion forces or dipole-dipole interactions. Additionally, hydrogen is not present, so hydrogen bonding is not possible. Therefore, the only intermolecular force present in \(\mathrm{MgI}_{2}\) is ionic bonding.

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Most popular questions from this chapter

Complete and balance the following equations. If no reaction occurs, write NR. (a) \(\mathrm{Cl}_{2}(g)+\mathrm{I}^{-}(a q) \longrightarrow\) (b) \(\mathrm{F}_{2}(g)+\mathrm{Br}^{-}(a q) \longrightarrow\) (c) \(\mathrm{I}_{2}(s)+\mathrm{Cl}^{-}(a q) \longrightarrow\) (d) \(\mathrm{Br}_{2}(l)+\mathrm{I}^{-}(a q) \longrightarrow\)

Write the formula for each of the following compounds. (a) potassium bromite (b) calcium bromide (c) sodium periodate (d) magnesium hypochlorite

Give the formula for the acidic oxide of (a) \(\mathrm{HNO}_{3}\) (b) \(\mathrm{HNO}_{2}\) (c) \(\mathrm{H}_{2} \mathrm{SO}_{4}\)

The average concentration of bromine (as bromide) in seawater is \(65 \mathrm{ppm} .\) Calculate (a) the volume of seawater \(\left(d=64.0 \mathrm{lb} / \mathrm{ft}^{3}\right)\) in cubic feet required to produce one kilogram of liquid bromine. (b) the volume of chlorine gas in liters, measured at \(20^{\circ} \mathrm{C}\) and \(762 \mathrm{~mm}\) \(\mathrm{Hg}\), required to react with this volume of sea water.

At equilibrium, a gas mixture has a partial pressure of \(0.7324\) atm for \(\mathrm{HBr}\) and \(2.80 \times 10^{-3}\) atm for both hydrogen and bromine gases. What is \(K\) for the formation of two moles of HBr from \(\mathrm{H}_{2}\) and \(\mathrm{Br}_{2} ?\)
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