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Describe how an emission line spectrum is produced
e- in ground state, right amount of energy as heat or electricity, jumps to higher level, excited state is unstable, drops to lower energy level, energy absorbed to make jump released as photon, frequency depends on difference in energy levels. E2-E1 = hf, E2 = excited state, E1 = ground state, h is Planks constant, f is frequency of light
Who unlocked the secret line of spectra?
Bohr
What is an energy level?
Shell which electrons of equal energy can occupy
Which energy level do electrons fall into to produce visible light?
N=2
What is the series of lines called when in n=2?
Balmer series
Give two ways to excite electrons.
High temperature, high voltage electricity
N=1
Gives UV range
N=2
Gives visible range
N=3,4,5
Gives IR range
How is continuous spectrum seen
Incandescent bulb+prism
How is emission line spectrum seen
Excited hydrogen+prism
How is absorption line spectrum seen
Incandescent bulb+cold hydrogen+prism
Continuous spectrum
Contains no bright or dark lines
Absorption spectrum
Interrupted by dark absorption lines
Emission spectrum
Dark except at certain wavelengths where there are emission lines
Sodium
Yellow
Lithium
Crimson
Copper
Blue-green
Strontium
Red
Barium
Green(yellowish)
Flame test
Take wooden splint soaked in deionised water overnight, pick up sample of each salt in turn using fresh splint for each, hold salt into a non-luminous Bunsen flame, now the colours produced
Line absorption spectra
Formed when a white light is passed through a gold gaseous element
Note
Flashcard