Chapter 12: Problem 42
What is the strongest interparticle force in each substance? (a) Kr (b) BrF (c) \(\mathrm{H}_{2} \mathrm{SO}_{4}\)
Short Answer
Expert verified
(a) London dispersion forces(b) Dipole-dipole interactions(c) Hydrogen bonds
Step by step solution
01
Identify the type of substance for Kr
Krypton (Kr) is a noble gas, which means it is composed of single atoms and is held together by very weak forces known as dispersion forces or London dispersion forces. These are the weakest type of intermolecular forces that arise due to temporary fluctuations in electron density within atoms.
02
Determine the strongest force in Kr
Given that Kr is a noble gas, the strongest interparticle force present is the London dispersion force.
03
Identify the type of substance for BrF
Bromine monofluoride (BrF) is a diatomic molecule consisting of bromine and fluorine. This is a polar molecule due to the difference in electronegativity between bromine and fluorine.
04
Determine the strongest force in BrF
Since BrF is a polar molecule, the strongest interparticle force present is the dipole-dipole interaction, which is stronger than London dispersion forces but weaker than hydrogen bonding.
05
Identify the type of substance for \(\mathrm{H}\_{2} \mathrm{SO}\_{4}\)
Sulfuric acid (\(\mathrm{H}\_{2} \mathrm{SO}\_{4}\)) is a polar molecule and also has hydrogen atoms bonded to oxygen, which is a very electronegative element.
06
Determine the strongest force in \(\mathrm{H}\_{2} \mathrm{SO}\_{4}\)
The strongest interparticle force in \(\mathrm{H}\_{2} \mathrm{SO}\_{4}\) is hydrogen bonding. This is because hydrogen bonding occurs when hydrogen is bonded to highly electronegative atoms like oxygen (O), which is present in sulfuric acid.
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Key Concepts
These are the key concepts you need to understand to accurately answer the question.
London dispersion forces
London dispersion forces, also known as Van der Waals forces, are the weakest type of intermolecular forces. They arise from temporary fluctuations in the electron density in atoms or molecules. Even if a molecule is non-polar, at any moment, there can be an instantaneous dipole due to the movement of electrons. This temporary dipole can induce a dipole in a neighboring molecule, leading to an attractive force between them.
London dispersion forces get stronger as the size of the molecules increases, because larger molecules have more electrons, which can create larger fluctuations. Although weak individually, these forces collectively play a critical role in the properties of gases, liquids, and solids, especially in noble gases and non-polar molecules like O₂ and N₂.
London dispersion forces get stronger as the size of the molecules increases, because larger molecules have more electrons, which can create larger fluctuations. Although weak individually, these forces collectively play a critical role in the properties of gases, liquids, and solids, especially in noble gases and non-polar molecules like O₂ and N₂.
Dipole-Dipole Interactions
Dipole-dipole interactions occur between polar molecules. These molecules have a permanent net dipole moment due to the uneven distribution of electrons within the molecule. A classic example is hydrochloric acid (HCl), where chlorine is more electronegative than hydrogen, creating a partial negative charge on chlorine and a partial positive charge on hydrogen.
These positive and negative ends of different molecules attract each other, resulting in dipole-dipole interactions. These forces are stronger than London dispersion forces but generally weaker than hydrogen bonding. They significantly affect the boiling points and melting points of substances. For instance, they are responsible for the relatively high boiling point of water compared to other molecules of similar size that don't form hydrogen bonds.
These positive and negative ends of different molecules attract each other, resulting in dipole-dipole interactions. These forces are stronger than London dispersion forces but generally weaker than hydrogen bonding. They significantly affect the boiling points and melting points of substances. For instance, they are responsible for the relatively high boiling point of water compared to other molecules of similar size that don't form hydrogen bonds.
Hydrogen Bonding
Hydrogen bonding is a special, stronger type of dipole-dipole interaction. It occurs when hydrogen is covalently bonded to a highly electronegative atom (like nitrogen, oxygen, or fluorine), creating a strong dipole. The hydrogen bond occurs between the hydrogen of one molecule and the electronegative atom of another.
This type of bonding is responsible for many of the unique properties of water, such as its high boiling and melting points, as well as its ability to dissolve many substances. An example of hydrogen bonding is in water (H₂O) where the hydrogen atoms of one water molecule are attracted to the oxygen atom of another water molecule.
You can also find hydrogen bonding in biological molecules such as DNA and proteins, where they play a crucial role in maintaining the structure and function of these macromolecules.
This type of bonding is responsible for many of the unique properties of water, such as its high boiling and melting points, as well as its ability to dissolve many substances. An example of hydrogen bonding is in water (H₂O) where the hydrogen atoms of one water molecule are attracted to the oxygen atom of another water molecule.
You can also find hydrogen bonding in biological molecules such as DNA and proteins, where they play a crucial role in maintaining the structure and function of these macromolecules.
