Spectrums

• white light shine through gaseous atoms
• phontons of certain energy are absorbed by an atom
• causing electrons to move to a higher engry level.
• meaning light of a frequency corresponding to energy of the photon will be removed.
• when shown on spectrometer, electronis transitions appear as dark lines against bright background.

• atoms given energy ( by heating or electrical field)
• electrons are then moved to a higher energy level.
• when source of energy removed, the elctron moves back to lower energy level.
• QUANTUM ENERGY - packet of engry that releases the engry lost.
• corresponds to electromagneticradiation of specific frequency.

• Simplest emission spectrum - one electron.
• Atomic spectrum of hydrogen - separate lines in the ultraviolet (Lyman), visible (Balmer), infrared (Paschen).

• atom excited by absorbing energy - electron jumps to higher energy level.
• electron falls down an enegry level - emits engry in form of electromagnetic radiation.
• line in spectrum is emitted energy - because energy of emitted radiation equal to difference between two energy levels in this electronic transition.
•   E=hf - electron transitions between enegry levels result in emission of radiation of different frequencies - produce different lines in spectrum.

• Balmer series - electrons returing back to n=2 energy level. 
• frequency increases - lines get closer together - enegry difference between the shells decrease. 

This is the hydrogen spectrum of the Balmer series:

• spectral lines closer together as frequency of radiation increases until converge limit.
• Convergence Limit - corresponds to point at which energy of an electron is no longer quantised.
• that point, nucleus has lost all influence over the electron 
• atom has become ionised.

measuring convergent frequency of Lyman series (difference between n=1 and n=inifinty) allows ionisation energy to be calculated using    E=hf.

This if you need to write your own notes:

This if you need to write your own notes: