Chemistry: Post your doubts here!

[Dark Destination]

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?

Because they are at different energy levels?

 

[Awesome12]

Like, why is there an increase in 3rd to 4th I.E. and 4th to 5th I.E?

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...

 

[Awesome12]

Because they are at different energy levels?

They are degenerate orbitals ; orbitals on the same energy level.

 

[Dark Destination]

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...

What?

Aren't electrons first removed from 3s in magnesium?

 

[Awesome12]

What?

Aren't electrons first removed from 3s in magnesium?

He asked about the difference in I.E between the 3rd and 4 th and 4th and 5th.

 

[MarcoReus]

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...

So you are saying repulsions decrease and that's the reason?
My theory is (once I thought about it) that when one electron leaves, the charge goes to +1 and thus it's the same amount of protons attracting one less electron so the bond between the nucleus and the remaining electrons gets stronger thus rising the I.E.

And Dark Destination, read the question clearly.

 

[Awesome12]

So you are saying repulsions decrease and that's the reason?
My theory is (once I thought about it) that when one electron leaves, the charge goes to +1 and thus it's the same amount of protons attracting one less electron so the bond between the nucleus and the remaining electrons gets stronger thus rising the I.E.

And Dark Destination, read the question clearly.

Would you care to read it again?

 

[MarcoReus]

Would you care to read it again?

I'll just assume you wrote what I wrote in your version of English.

 

[Dark Destination]

He asked about the difference in I.E between the 3rd and 4 th and 4th and 5th.

Okay, Chemistry master.

 

[Dark Destination]

HCL doesn't have Hydrogen bonding? Why? :/

 

[Dark Destination]

What is the difference between Permanent-Dipole attraction and Hydrogen bonding?

 

[Awesome12]

HCL doesn't have Hydrogen bonding? Why? :/

Hydrogen bonding cannot form between H and Cl. The difference in electronegativity isn't that high to allow a very strong hydrogen bond to form. In addition to that, HCl is non-polar; it has induced dipole forces of attraction.

 

[RoOkaYya G]

HCL doesn't have Hydrogen bonding? Why? :/

poor HCl

 

[MarcoReus]

HCL doesn't have Hydrogen bonding? Why? :/

Hydrogen bond only happens with Fluroine, Nitrogen and Oxygen.

 

[MarcoReus]

What kind of questions come in Hybridization?

 

[RoOkaYya G]

What kind of questions come in Hybridization?

drawing of orbitals
e.c
sketchin graph for orbitals
definition simply
shapes of molecules n bond angles
attraction of electrons
polarisation of orbitals

to name a few

 

[MarcoReus]

drawing of orbitals
e.c
sketchin graph for orbitals
definition simply
shapes of molecules n bond angles
attraction of electrons
polarisation of orbitals

to name a few

Whaaaaaaaaaaaaaaaaaaaaaaaaaaaaaaaaaaat? Bond angles of hybridization? What in the hell is that?

Awesome12, how much of this have we studied?

 

[RoOkaYya G]

Whaaaaaaaaaaaaaaaaaaaaaaaaaaaaaaaaaaat? Bond angles of hybridization? What in the hell is that?

Awesome12, how much of this have we studied?

-_- shapes of molecules!!! so with it theres always bond angle...so i wrote it -_-
chain reaction u see
hybridisation --> shape of molecule --> bon angle --> charge densities n all tht

 

[Awesome12]

Whaaaaaaaaaaaaaaaaaaaaaaaaaaaaaaaaaaat? Bond angles of hybridization? What in the hell is that?

Awesome12, how much of this have we studied?

We have done bond angles of hybridization, but it the same as the ones in the shapes of the molecules. Like AB4 has bond angles = 109.5 degress. Thus in hybridization, it will be SP3 also having bond angles = 109.5 degrees. Nothing to worry about.

 

[RoOkaYya G]

btw Dark Destination u dunno wht uve done? u r askin Awesome12