Question

what will the trend of lattice energy, enthalpy of hydration and the enthalpy change of solution be like if I look down the group. Please use more or less exothermic or endothermic, and explain

Answer 1

@amistre64 Do you know about this?

Answer 2

i havent a clue ...

Answer 3

I've looked at the Internet, but the pages just make me more confused

Answer 4

the only thing i might vaguely recall about chemistry is balancing out a reaction equation ... but even that is a bit foggy

Answer 5

Ok' I'll ask you more about math, then

Answer 6

Do you know Sb. who's good at chem? people who use Open, ofcuz

Answer 7

@asmagul Hey,there. could you please give me hand with this one?

Answer 8

yeah im looking at this and wait i will explain u

Answer 9

The lattice energies become less exothermic as the group is descended

· The hydration energies of the cations become less exothermic down the group as well

Answer 10

Therefore, the change in ΔH solution down the group is determined by which quantity (ΔH lattice or hydration enthalpies of the ions) shows the greater decrease.

Answer 11

The entropy of the hydrated ion increases as the ionic radius increases.

Answer 12

As the ΔH solution becomes more exothermic down the group, ΔS° (surroundings) becomes more positive down the group, which favors solubility.

Answer 13

There’s a greater change in the hydration enthalpies of the cations than that of the lattice energy. Therefore, the ΔH solution becomes less exothermic down the group.

Answer 14

It is said that the value of delta(H) solution depends on the size of the anion How so?

Answer 15

we hav't learn about delta S, so please don't confuse me with that

Answer 16

lets take an example so you can understand by this by keeping periodic table in your mind.........The OH- ion is similar in size to the group 2 cations. The sum of the ionic radii of both cations and the OH- increases considerably down the group as the value of the radius of the cation increases down the group. ∴ Change in ΔH lattice is greater than that of the group 2 sulfates.
In addition, the sulfate ion is much larger than any of the group 2 cations. So, the sum of the ionic radii changes only by a small amount. ∴ the change in the hydration enthalpies is greater than the change in ΔH lattice of the group 2 sulfates.

Answer 17

Great!that's helpful!

Answer 18

delta H is enthalpy change..we cant measure enthalpy directly so we measure change in enthalpy 4 endothermic and exothermic reactions

Answer 19

delta S is solubility or enthalpy of solution

Answer 20

wait, I'm confused, is't \[\Delta S\] change in entropy?

Answer 21

sorry u r right it is entropy...i have studied it in physics...my bad habit when im studying a subject i dont relate it to others...i will change myself..hanks 4 noticing this