2.2 Electron configuration Flashcards
What is a photon?
A packet of energy that behaves like a particle and a wave
Which end of the visible light spectrum has the most energy?
The violet end
Frequency to wavelength conversion
c = vλ
c - speed of light
v - frequency
λ - wavelength
What is the speed of light
c = 3.0 * 10^8 metres per second
Relationship between wavelength and frequency
The longer the wavelegth, the lower the frequency
The shorter the wavelength, the higher the frequency
Energy equation
E = hv
Energy = Planck’s constant (h) * frequency (v)
Planck’s constant (h)
6.63 * 10^-34
What happens when light passes through or reflects off a medium?
Photons of specific energy are absorbed by each electron to promote it to a higher energy level
What determines the specific photons of specific energy absorbed by the electrons?
The medium’s chemical composition
What happens when an electron returns to its ground state energy level?
It releases a photon of specific energy
What happens during the absorption of photons by an electron?
The electron rises to a higher energy level and stays there
How are the dark lines on the absorption spectrum created?
The specific energies absorbed correspond to specific frequencies and wavelengths of being absorbed
What determines the amount of energy absorbed and emitted by an electron
The distance it moves between energy levels
Which transitions result in high frequency light being emitted or absorbed?
Transitions between energy levels that are further apart
What is unique to each element?
It’s absorption and emission spectra
Why do the absorption and emission spectra have lines at the same points?
The energy absorbed promoting an electron between specific energy levels is the same released when it returns to ground state
What do the different lines on a spectrum correspond to?
Different transitions of electrons
What are line spectra used to prove?
The existence of electron energy levels
How come only certain transitions can occur?
Electrons are in specific energy levels
How is the line spectrum produced by the transitions?
Each transition emits or absorbs light of a particular frequency, producing a line spectrum
What would a continuous spectrum suggest?
That electrons can exist anywhere around the nucleus
Colour of the light hydrogen burns with?
Pale blue
What are the 3 series of wavelengths in the hydrogen emission spectrum?
Paschen, Balmer and Lyman
Why can we only see the Balmer series?
It is part of the visible part of the electromagnetic spectrum.
Lyman is part of ultraviolet and Paschen is part of infrared
