ATOMIC STRUCTURE Flashcards
What is the angle of deflection dependent on? Why do protons deflect lesser compared to electrons?
Angle of deflection is proportional to the charge/mass. (can be positive or negative depending on the charge)
This is because while they have the same charge, the mass of an electron is lower.
What is the relationship between quantum number and stability of electron shell
The lower the principal quantum number, the closer it is to the nucleus. This results in stronger electrostatic forces of attraction between electrons and the positive nucleus making the electron more stable.(lower energy)
What are the types of orbitals
s,p,d,f
1s
2s 2p
3s 3p 3d
…
What is the anomaly of d and s orbitals
empty 3d orbitals are higher in energy than 4s orbitals but fully filled, it is the other way around
Why must the electrons in the same orbital have opp spins?
Electrons are negatively charged and 2 electrons confined within the same orbital experiences repulsion. To coexist, they must spin in opp directions so they exhibit sufficient magnetic attraction to hold themselves tgt.
What is Hund’s rule?
Hund’s rule states that when there are degenerate orbitals available, electrons occupy them singly first before pairing
What are the exceptions for electronic configuration?
3d5 and 3d10 are associated with higher stability so they are filled up first
What is the definition of IE?
Amt of energy required to remove one mole of electrons from one mole of gaseous atoms to produce one mol of gaseous atoms with a single positive charge
What is the definition of IE?
Amt of energy required to remove one mole of electrons from one mole of gaseous atoms to produce one mol of gaseous atoms with a single positive charge
Why are subsequent IEs more endomthermic?
This is because extra energy is need to over come electrostatic FOA between leaving electron and ion of increasingly positive charge
What affects nuclear charge and shielding effect? What do they have to do with Effective nuclear charge?
Nuclear charge is affected by the number of protons while shielding effect is affect by number of inner shell electrons.
ENC=NC-SE
Explain the trend of IE across a period
Across a period, NC increases due to the increase in protons while there is a negligible increase in the shielding effect as electron is being added to valence shell. Thus, ENC increases so the atomic radius will decrease across the group and so IE increases
Explain the trend of IE down the group
NC increase due to increase in protons. SE increase due to increase of inner shell electrons. Thus, there is negligible change of ENC. However, the dist between the outer-shell electrons and the positively charged nucleus increases due to the increased number of electrons shells resulting in weaker electrostatic FOA
What can u tell about successive ionisation energies for an atom?
Large jumps indicate removal of electrons from different electronic shells while small jumps indicate removal from different subshells
