Some of the important properties of ionic compounds are as follows: i. low electrical conductivi

Some of the important properties of ionic compounds are as...

Key Concepts

Brittleness

Brittleness in ionic compounds arises from the rigid and directional nature of the ionic bonds in the crystal lattice. When a stress is applied, layers of ions may shift relative to each other. This misalignment can cause like-charged ions to align and repel one another, resulting in a fracture or breakage of the crystal structure.

Ionic Bonding

Ionic bonding involves the transfer of electrons from one atom to another, resulting in the formation of oppositely charged ions. The electrostatic attraction between these ions creates a strong bond that holds them together in a fixed position within the crystal lattice. This concept is critical in understanding the behavior and inherent properties of ionic compounds.

Crystal Lattice Structure

Ionic compounds form a crystal lattice where ions are arranged in a repeating, orderly pattern held together by strong electrostatic forces. This structure explains many properties of ionic substances, including their high melting and boiling points because a significant amount of energy is required to break the interactions between the large number of closely packed ions.

Electrical Conductivity

In the solid state, the ions in an ionic compound are fixed in place within the lattice, which prevents electrical conduction. However, when the compound is molten or dissolved in polar solvents, the ions become mobile and are able to carry electric charge, leading to high electrical conductivity. This change in conductivity is a direct result of the nature of ionic bonding and the structure it produces.

Solubility in Polar Solvents

The solubility of ionic compounds in polar solvents, such as water, is due to the interaction between the partially charged regions of the solvent molecules and the fully charged ions. The polar molecules can surround and stabilize the individual ions, effectively weakening the strong ionic bonds within the lattice and allowing the substance to dissolve.

Transcript

00:01 So in this video, i'm gonna talk about question 22 from chapter eight, which says some of the important properties of ionic compounds are as follows.

00:08 One low electrical conductivity of solids and high electrical conductivity and solution.

00:13 Or when molten.

00:14 Two relatively high melting and boiling points.

00:17 Three.

00:17 Brittleness and force liability and polar solvents.

00:21 How does the concept of ionic bonding discussed in this chapter account for these properties? so we have the 1st 1 low electrical conductivity is solids in high electrical conductivity in solution or when molten.

00:34 So what do our molten or or dissolved ionic compounds look like? compared to our solid ionic compound? well are solid.

00:43 Ionic compound is a very rigid lattice of positive and negatively charged ions.

00:49 That air, held in place by um by the attractive forces between opposite lee charge opposite lee charged ions and the repulsive forces between ions that have the same charge.

01:02 So the positioning and the lattice on optimizes these, and it's frozen in place in a very rigid structure.

01:10 This is in comparison with with the molten solution, where are charged.

01:17 Ions are now allowed to move around and come into contact with each other in different ways.

01:24 So the fact that we have our eye owns moving around versus frozen in place actually allows us to conduct electricity s oh, that's why are molten or dissolved? ionic compound conduct conducts electricity but are very rigid.

01:39 Um, unmoving, solid cannot conduct electricity.

01:42 It will not allow charge to move through it to relatively high melting in boiling points.

01:51 So melting point.

01:52 That's when we go from a solid to a liquid and boiling point.

01:55 That's when we go from a liquid to a gas.

01:58 And to do either of those, you have to overcome what we whole inter molecular forces, the forces between molecules.

02:05 Eso when we're talking about when we're talking about our ionic compound, we are talking about a lattice of charges, at least when we're a solid uh, so you have the same attractive and repulsive kolanovic force throughout the entire lattice...

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