The strongest attractive forces between molecules of O_2 are ionic .pdf

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The strongest attractive forces between molecules of O_2 are: ionic covalent hydrogen bonding dipole-dipole attractions dispersion forces Solution The attractive forces between molecules of O2 will be dispersion forces. This is because O2 is a non-polar molecule so there will be no dipole-dipole interactions, also there is no hydrogen atom so no question of Hydrogen bonding. Dispersion forces are exhibited by non-polar molecules because of thecorrelated movements of the electrons in interacting molecules. The electrons in adjacent molecules repel each other and so they run away from their usual place. As a result, electron density in a molecule becomes redistributed in proximity to another molecule, which is according to quantum mechanical theory of dispersion forces. This is frequently described as the formation of instantaneous dipoles that attract each other. These type of Dispersion forces are present between all chemical groups, and usually represent the main part of the total interaction force in condensed matter..

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Intermolecular Forces Definition Intermolecular forces are the forces of attraction that exist between molecules. These forces play a crucial role in determining the physical and chemical properties of substances, such as boiling points, melting points, solubility, and viscosity. Intermolecular Forces The three main types of intermolecular forces are: London dispersion forces (also known as Van der Waals forces): These forces are present in all molecules, whether they are polar or nonpolar. They arise due to temporary fluctuations in electron distribution, creating temporary dipoles. These temporary dipoles induce dipoles in neighboring molecules, resulting in attractive forces. London dispersion forces increase with increasing molecular size and shape. Substances with stronger London dispersion forces tend to have higher boiling points and melting points. London Dispersion force London dispersion forces are the weakest intermolecular forces. They occur due to temporary fluctuations in electron distribution within molecules, creating temporary dipoles. These temporary dipoles induce dipoles in neighboring molecules, resulting in attractive forces. London dispersion forces increase with increasing molecular size and shape. Substances with stronger London dispersion forces tend to have higher boiling points and melting points. Examples of substances with predominant London dispersion forces include noble gases like helium and nonpolar molecules like hydrocarbons. 2 .Dipole-dipole interactions: These forces occur between polar molecules. They arise due to the attraction between the positive end of one polar molecule and the negative end of another polar molecule. Dipole-dipole interactions are stronger than London dispersion forces and contribute significantly to the physical properties of polar substances . Dipole dipole interaction Polar molecules have an uneven distribution of electron density, resulting in a permanent dipole moment. The positive end of one polar molecule is attracted to the negative end of another polar molecule. Dipole-dipole interactions are stronger than London dispersion forces. These forces contribute significantly to the physical properties of polar substances. Examples of substances with predominant dipole-dipole interactions include hydrogen chloride (HCl) and water (H2O). 3.Hydrogen bonding: This is a special type of dipole-dipole interaction that occurs when a hydrogen atom is bonded to a highly electronegative atom (such as nitrogen, oxygen, or fluorine) and is also attracted to another electronegative atom in a different molecule. Hydrogen bonding is exceptionally strong compared to other intermolecular forces and has a significant impact on the properties of substances. It is responsible for many unique properties of water, such as its high boiling point, surface tension, and the ability to form ice with a lower density than liquid water.

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