Arrange the following compounds in order of increasing solubility in water: O2, LiCl, Br2, metha

Arrange the following compounds in order of increasing...

Key Concepts

Ionic Compounds in Water

Ionic compounds are composed of positively and negatively charged ions. When introduced to water, the polar water molecules can stabilize these charges through ion-dipole interactions. This process usually results in high solubility, as the interactions between water and the ions effectively overcome the ionic lattice energy of the solid compound.

Hydrogen Bonding

Hydrogen bonding is a specific type of strong dipole-dipole interaction that occurs when hydrogen is bonded to highly electronegative atoms like oxygen, nitrogen, or fluorine. In the context of solubility, compounds capable of forming hydrogen bonds with water molecules typically have enhanced solubility, as these interactions help to stabilize the solute within the solvent.

Nonpolar Substances

Nonpolar substances lack significant regions of positive or negative charge, making them less able to engage in strong interactions with polar solvents like water. Without sufficient interactions such as hydrogen bonding or dipole-dipole attractions, nonpolar molecules typically exhibit lower solubility in water due to the unfavorable energy balance during dissolution.

Solubility in Water

Solubility is the ability of a substance (solute) to dissolve in a solvent, such as water. It is governed by the interactions between solute and solvent molecules, and is influenced by factors including polarity, molecular size, and temperature. This concept is central to understanding how different types of compounds behave when mixed with water.

Polarity

Polarity refers to the distribution of electrical charge around a molecule. Molecules with polar bonds and asymmetrical structure tend to have a net dipole moment, which makes them more likely to interact favorably with polar solvents like water. The degree of molecular polarity plays a crucial role in determining how well a substance will dissolve in water.

Transcript

00:01 Okay, so we have four molecules and we want to know which one will dissolve better in water.

00:10 Okay, so which one will have a higher solubility in water? to answer that, we're going to go through the types of interaction that will be going on between these molecules and water.

00:20 So as we know, as we know, water has a dipole moment, is a polar molecule.

00:25 So that for sure is very important in this analysis.

00:29 So the first two here actually will have the same type of interaction because they're both non -poor.

00:38 So when you have a non -polar molecule interacting with a polar molecule, we call that dipole, induced dipole interaction.

00:50 What is that? it means that the dipole of the water induces the creation of a dipole moment and a bromine or deoxygen.

00:58 Okay.

01:00 So because there's a charge there, the electrons of bromine and oxygen, they move around, and when they do that, a dipole moment is created.

01:10 It's not a permanent dipole.

01:12 If you take away the charge that disappears, that's why it's called an induced dipole.

01:16 Okay.

01:17 So this is our first two interactions here.

01:20 The third interaction will be an ion dipole interaction, because now we're looking at lithium chloride.

01:29 Which is an ionic compound.

01:33 We have ions here of lithium and chloride.

01:36 So when they dissolve in water, the water will interact.

01:40 Dipole moment of water interacts with the ions.

01:45 And finally, we have this molecule, which is methanol and it's polar.

01:49 So at first you would say, oh, that's just a dipole -dipole interaction, which would be okay, but maybe there's a better answer here.

01:59 And you have to pay attention to the o -h group.

02:03 When you have an o -h group in one molecule and an o -h group in another molecule, talking about molecules, okay, not ions.

02:15 This cannot be confused with a hydroxy group.

02:21 When you have that, you can form hydrogen bounds...

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