S1.3- electron configuration
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descibre emission spectra
light is emitted when excited electrons high energy state fall back down into lower energy levels, energy of light only a particular precise energy, corresponds energy difference between energy levels of electrons emission spectra are produced by atoms emitting photons when electrons in excited states return to lower energy levels
continuos spectrum
a light source that emits light of all frequencies contains all different wavelengths of lihgt, uv-ir
line spectra
discrete lines where light specific wavelength emitted or absorbed ca either be emizzion or aborption
ground state
lowest level
what happens when energy is supplied to an electron
excites it into high energy state
emission line spectrum=
bright lines of specific wavelength (colour in the visible) are produced when an electron in an excited high energy levl falls down to a lower energy level emitting a photon of light of a specific energy
absorption line spectrum
dark lines of a specific wavelength are produced when a light photon of a specific energy (color int eh visible) is absorbed by an electron when it is excited to a higher energy level
what coincides to spectral lines in the visible region
electron transitions from energy level n=3,4,5, or 6 to n=2
describe structure of energy levels
as the energy difference between the energy levels becomes less the further away they are from the nucleus, this means hat the lines in the emission spectra get closer together at higher energy (shorter wavelength or hgiher frequency) from red->yellow->green->purple (increasing frequency, increasing energy, shorter wavelength)
transition of electrons falling back to the first principle energy level occur in
ultraviolet region
electron transitions to the second principle energy level occur in
the visible regions of the spectrum
transitions in the third principle energy level occur in the
infrared region of the spectrum
what is the order of the energy levels
1S 2S 2P 3S 3P 4S 3D 4P 5S
descibre shape of S orbital
spherical shape
descirpe shape of P orbitals
8 figure shaped 3 of them X= horizontal Y=vertical Z=diagonal
why do orbitals fill up in the way they do
Because electrons will first enter the energy level of lowest energy, when this is full then the next level will begin to fill up
why are each suborbitals able to hold 2 electrons
becuase they have differnet spins and this reduces their mutual repulsion
what is chromiums electronic sturcutre
[AR] 4Sˆ1 3Dˆ5
what is coppers electronic sturcutre
[AR] 4Sˆ1 3Dˆ10
what is the most stable configuration for electron arrangement
first for electrons to enter the sub-orbital singly
whats the rule for the transition metal ions
a filled 4s suborbital is at slightly higher energy level than a partically filled 3d suborbital, means that when electrons are lost from transition metal, first lost from teh 4s suborbital before being lost from 3d
how can many electrons exist in same principle energy level
-different spins being in differnet sub orbitals within the principle energy level
what is evidnece for suborbitals
ionization energy of a particular atom
first ionisation energy
is the energy required to remove one mole of electrons from one mole of gaseous atoms