S1.3- electron configuration Flashcards
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
describe first ionization energy across a period
increase in ionization energy, number of protons in nucleus increases increase in electrostatic attraction of nucleus for electrons
describe first ionization energy down a group
decrease in ionization energy, distance of electrons in valence shells increases reduces electrostatic attraction, electron inner energy levels shield attraction of nucleus for electrons
what is the frequency or wavelength of the convergence limit
the frequency or wavelength of light emitted by an electron when it falls from the n=infinite to the outermost energy
what type of spectrum is it when a light source goes through a cold gas cloud
absorption
what type of spectrum is it when a light source goes through a hot gas cloud
emission
why does most helium nucleis pass straigh through gold atoms
an atom is mostly made of empty space only composed of a very small nuclei
why do very few helium nuclei deviate largerly from theri path whens hot at gold atoms
even though most of atom made of air, very small nucleus it has a positive charge which repels fold atoms
what is the difference between diagrams 1s and 2s
1s is smaller than 2s
diagram of 2p
a simple 8 drawing
explain why the first ionization energy of sulfur is lower than that o phosphorous
because sulfur has an extra electron, meaning that in the p sub orbital one of the suborbitals pair up the electrons, while in phosphorous every electron is alone meaning electron-electron repulsion is smaller than that of sulfur
does cu have a greater ionization energy than cu2+ and why
cu2+ has greater ionization energy, because there are less electrons present thus the outer electrons, their orbitals are closer to nucleus thus the proton electrostatic attraction is greater needing a greater ioniztion energy
what type of radiation in spectrum has longest wavelength and lowest frequency
infrared radiation
order of atomic orbitals in decreasing energy (highest to lowest).
f
d
p
s
Emission and absorption line spectra both provide evidence for
the existence of energy levels within the atom
Which electron transition represents the first ionisation of a hydrogen atom?
electron transition from n=1 to n=infinite
Such emission spectra provide evidence that electrons are moving from
higher to lower energy levels with the higher energy levels being closer together.
