Topic 12 Flashcards
What do trends in the first ionisation energy across periods account for?
The existence of main energy levels and sub-levels
What does the successive ionisation energy data for an element show?
Relations to the electronic configuration
What should be able to deduce from the successive ionisation energy of an element?
The group
What does a large difference between the 1st and 2nd ionisation energy values of an element mean?
The element is in group 1
The jump in ionisation energy shows the existence of what?
Energy levels
Are electrons in the inner shell harder or easier to remove?
harder and require more energy because of the strong electrostatic attraction between the nucleus and inner shell
In an emission spectrum the limit of covergence at a higher frequency corresponds to what?
The 1st ionisation energy
What is the convergence limit?
The frequency at which spectral lines converge
Formula for energy
E=hxV
Formula for speed of light?
C= Vx λ
Explain the large increase in ionization energy from IE3 to IE4.
IE4: electron in lower/inner shell/energy level
IE4: electron closer to nucleus
(i) Explain the convergence of lines in a hydrogen emission spectrum.
(ii) State what can be determined from the frequency of the convergence limit.
(i) The lines/energy levels converge at higher frequencies
(ii) Ionisation energy
i) Outline why there is an increase in ionization energy from electron 3 to electron 5.
in the same sub-shell and there is a decrease in electron-electron repulsion
Explain how the number of electrons in the outer main energy level of phosphorus, P, can be determined using the data of successive ionization energies.
successive ionization energy values increase with removal of each electron;
large increase in ionization energy when sixth electron is removed;
as electron is one energy level/shell closer to the nucleus;
