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https://drive.google.com/viewerng/v...wp-content/uploads/2012/11/9701_s14_qp_43.pdf
Q4 c_i,ii,iii
Expound please!
Q4 c_i,ii,iii
Expound please!
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Aren't you aware that we are provided with data booklets that have value of certain bonds printed.
What is the definition of Standard Cell Potential according to Cambridge syllabus?A
Amine group is C-NH2,
Our sir made us write that SF6 has the octahedral shape. I should you should check what your sir made you write. In addition to that, you should follow the marking scheme.Is there a difference between square bipyramidal and octahedral? Because Q2(e) of the S11 P22 MS (link below) states the SF6 molecule to have the octahedral shape (not both).
http://papers.xtremepapers.com/CIE/Cambridge International A and AS Level/Chemistry (9701)/9701_s11_ms_22.pdf
It's the same thing, but the term octahedral is preferred.Is there a difference between square bipyramidal and octahedral? Because Q2(e) of the S11 P22 MS (link below) states the SF6 molecule to have the octahedral shape (not both).
http://papers.xtremepapers.com/CIE/Cambridge International A and AS Level/Chemistry (9701)/9701_s11_ms_22.pdf
It's the same thing, but the term octahedral is preferred.
The equation for the enthalpy of solution is. E= hydration energy - lattice energy so if the value of hydration energy is greater than the lattice energy then the enthalpy of solution will be positive. As a general rule, the more positive the enthalpy of solution is, the higher is the solubility. The hydration energy depends on the cations, so the difference in their size is relevant to the change in energy, while for lattice energy, neutral molecules are formed and since the sizes of the cations are negligible compared to the sulfate ion, the size of the molecule remains roughly the same as we decend the group so the lattice energy doesn't change that much, but as the the size of the cation increases down the group l, the hydration energy decreases significantly. Since the decrease in hydration energy is greater than the decrease in LE, the enthalpy of soliton is less positive and the solubility deceasesRe: All Chemistry help here!! Stuck somewhere? Ask here!
explain trend of solubility of group 2 sulphates.....well in anser to this.....we have to write that hydration enthalpy decrese faster than lattice bt i dont undrstnd how
If we remove three electrons from 3 half-filled orbitals from the same p subshell, why is there a small increase in ionization energy in each of them?
After the removal of an electron, the already present electrons tend to get closer to each other. Thus it is becomes harder to remove another electron.
Like, why is there an increase in 3rd to 4th I.E. and 4th to 5th I.E?
They are degenerate orbitals ; orbitals on the same energy level.Because they are at different energy levels?
Another possible explanation. In Magnesium, the p sub-shell is complete with THREE PAIRS. The first electron in the FIRST PAIR is removed at the cost of residual repulsion. This makes removing the electron easier. Then electrons get closer to each other. The other electron in the FIRST PAIR is more difficult to remove...
He asked about the difference in I.E between the 3rd and 4 th and 4th and 5th.What?
Aren't electrons first removed from 3s in magnesium?
After the removal of an electron, the already present electrons tend to get closer to each other. Thus it is becomes harder to remove another electron.
Such questions won't really come. They would rather prefer to ask simplistic statements, like why is there an abrupt increase in the ionization energy between the 2nd and 3rd I.E
Another possible explanation. In Magnesium, the p sub-shell is complete with THREE PAIRS. The first electron in the FIRST PAIR is removed at the cost of residual repulsion. This makes removing the electron easier. Then electrons get closer to each other. The other electron in the FIRST PAIR is more difficult to remove...
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