Atomic Structure Clarification Questions Part Deux

Q1. Are 5p orbitals filled before 4f, since they are of lower energy level?
A: Yes! In fact the f block elements start at lanthanum in period 6. That means 4f is filled after 6s.

Q2. What are the properties of plasma?
A: What a big question. You can read all about plasmas here.

Q3 What does IE graph of ionization energy after the 3r IE look like?
A: Go and get the data booklet from SEAB. This is part of the exam syllabus and provides the 4th IE of many elements. You can use that to plot a graph and see for yourself. The 4th IEs and all follow the same basic rules. Refer to Qn25 in my earlier post.
Basically IE increase across the period due to Zeff. Trhe irregularities due to s vs p subshell or paired vs unpaired electrons may still be there.
You should also note that the elements having inner shell electrons removed will have high IE due to large Zeff(which is due to the smaller shielding in inner shell electrons)

Q4. If quantum nos are not important, do we need to know all these?
A: Its cause they are the basis for our knowledge of atomic structure

Q5. Why is 4s filled before 3d? If it is a 4th shell how can it be closer to the nucleus?
A: 4s is filled before 3d because it is lower in energy.[ 4s shell is still LARGER than 3d orbitals. But its shape makes 4s orbitals more PENETRATING and allows the electrons to move nearer the nucleus ON THE AVERAGE. This is what makes the 4s orbital lower in energy. The maximum boundary and distance of a 4s electrn is further from the nucleus than 3d electrons]

Q6. Are there any exceptions to the 3 rules for determining electronic configuration?
A: Yes note the electronic configs for Cr and Cu.

Q7. What does the f-orbital look like?
A: Google it.

Q8. Are there hybrid orbitals?
A: Yes! These are used in making bonds. You’d have seen them in chem bonding lessons.

Q9. How do you deduce electronic configuration from successive IE?
A: Please read my notes on Ionisation Energies Discussion

Q10. Why does repulsion for paired electrons matter less in s orbital than in p orbitals?
A: Please read my notes on Ionisation Energies Discussion

Q11. Can electron spins be changed?
A: Yes! This requires energy.

Q12. What is meant by orbitals become more diffuse?
A: The orbitals are larger and so the electron density is spread out and diffuse.

Q13. Are there remedial lessons for clueless pple?
A: we can work on that. But remedial lesson involve a lot of work on your part as well.

Q14. How is the colour change in chemical reactions brought about?
A: In a chemical reaction one compou8nd is transformed to another, and if they have different colours, there is a colour change! But why are compounds coloured? Very often its due to their electronic structure! Most of the time, electrons absorb light energy to transit from ground state to excited states. The energy and therefore colour of light absorbed depends on the particular electronic structure. Light that is not absorbed but reflected is what give the colours of compounds. Refer to qn12 on why beta carotene is orange.