Which compound in each of the following pairs of ionic substances has the most negative lattice

step 1 Latus energy is follows this. So lattice energy is the energy that's required to form ionic comp

Which compound in each of the following pairs of ionic...

Key Concepts

Trends in the Periodic Table

Trends in ionic sizes across periods and down groups affect lattice energy. For example, moving down a group increases the ionic radius, which tends to decrease lattice energy, whereas in the same period, smaller ions will lead to stronger attractions, thereby increasing the lattice energy in magnitude.

Ionic Radius

The distance between ions in an ionic compound is related to their ionic radii. Smaller ions can pack closer together, leading to stronger electrostatic attractions. This results in a larger (more negative) lattice energy. Thus, comparing ionic sizes is essential when predicting which compound has a more negative lattice energy.

Effect of Ionic Charge

The magnitude of the ion’s charges plays a critical role in determining lattice energy because the electrostatic force is directly proportional to the product of the charges. Compounds with ions of higher charges will generally exhibit a more negative lattice energy than those with ions of lower charges.

Lattice Energy

Lattice energy is the energy released when gaseous ions come together to form an ionic solid. Its magnitude is influenced primarily by the charges on the ions and the distances between them. A higher charge and a smaller ionic radius usually lead to stronger electrostatic attractions, resulting in a more negative (exothermic) lattice energy.

Coulomb's Law

Coulomb’s law explains how the force between two charged particles depends on the product of their charges and inversely on the square of the distance between them. In the context of ionic lattices, this means that ions with higher charges and those that are closer together will interact more strongly, thereby increasing the lattice energy in magnitude.

Transcript

00:02 Latus energy is follows this.

00:06 So lattice energy is the energy that's required to form ionic compounds.

00:16 And there's an equation that i love to use when i'm teaching lattice energy.

00:22 And we know that lattice energy is equals to this constant k and the relative charges of the ions divided by the distance.

00:33 So, yeah, distance of between those two.

00:36 So, for example, if we're going to be looking at potassium chloride, here we have two ions here put together, make an ion, or two, yeah, make an ionic compound.

00:48 We're looking at ours, the distance between that is found between these two ions there.

00:54 And then q1 and q2 are the relative charges.

00:57 And so if we kind of show this on in this, in the equation form, we have chlorine, potassium and chlorine, go to make potassium chloride.

01:09 And we know potassium has a positive one charge, chlorine has a negative one charge, and so q1, q2 found right there, and then distance, kind of looking at trends of that, okay? and so this is kind of helpful, and we're looking in comparing two different ionic compounds.

01:27 We want to say, we want to look and see which one has the highest or smallest lattice energy compared to those two.

01:32 Now we can get real technical and look at the actual numbers between those, but sometimes we just want to really just use kind of these trends and this equation and make just a rough guess between the two.

01:43 So, for example, we have potassium chloride, and let's look at magnesium oxide, for example.

01:51 And then using these, let's see if we can calculate which one has a larger or smaller lattice energy.

02:00 Okay, so we just filled that one out.

02:03 Let's do the next one.

02:04 So we have magnesium.

02:05 Magnesium has a positive 2 charge.

02:09 Oxygen has a negative 2 charge to make that magnesium oxide.

02:14 So when we're looking at this equation, there's two rules that we can kind of follow here, or two kind of things that we can assume.

02:20 The first one is if q increases, what impact will that have on the lattice energy? well, the lattice energy, since this is a direct relapse.

02:31 Relationship will also increase.

02:34 The second rule that we can follow is looking at the size or distance between the two.

02:40 So if the distance between the two ions increases, what impact will that have on the lattice energy? we see this being an inverse relationship and so the lab synergy will decrease.

02:53 And so looking at these two, let's look for this problem...

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