S1.3- electron configuration

Question 1

descibre emission spectra

Answer 1

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

Question 2

continuos spectrum

Answer 2

a light source that emits light of all frequencies
contains all different wavelengths of lihgt, uv-ir

Question 3

line spectra

Answer 3

discrete lines where light specific wavelength emitted or absorbed
ca either be emizzion or aborption

Question 4

ground state

Answer 4

lowest level

Question 5

what happens when energy is supplied to an electron

Answer 5

excites it into high energy state

Question 6

emission line spectrum=

Answer 6

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

Question 7

absorption line spectrum

Answer 7

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

Question 8

what coincides to spectral lines in the visible region

Answer 8

electron transitions from energy level n=3,4,5, or 6
to n=2

Question 9

describe structure of energy levels

Answer 9

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)

Question 10

transition of electrons falling back to the first principle energy level occur in

Answer 10

ultraviolet region

Question 11

electron transitions to the second principle energy level occur in

Answer 11

the visible regions of the spectrum

Question 12

transitions in the third principle energy level occur in the

Answer 12

infrared region of the spectrum

Question 13

what is the order of the energy levels

Answer 13

1S 2S 2P 3S 3P 4S 3D 4P 5S

Question 14

descibre shape of S orbital

Answer 14

spherical shape

Question 15

descirpe shape of P orbitals

Answer 15

8 figure shaped
3 of them
X= horizontal
Y=vertical
Z=diagonal

Question 16

why do orbitals fill up in the way they do

Answer 16

Because electrons will first enter the energy level of lowest energy, when this is full then the next level will begin to fill up

Question 17

why are each suborbitals able to hold 2 electrons

Answer 17

becuase they have differnet spins and this reduces their mutual repulsion

Question 18

what is chromiums electronic sturcutre

Answer 18

[AR] 4Sˆ1 3Dˆ5

Question 19

what is coppers electronic sturcutre

Answer 19

[AR] 4Sˆ1 3Dˆ10

Question 20

what is the most stable configuration for electron arrangement

Answer 20

first for electrons to enter the sub-orbital singly

Question 21

whats the rule for the transition metal ions

Answer 21

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

Question 22

how can many electrons exist in same principle energy level

Answer 22

-different spins
being in differnet sub orbitals within the principle energy level

Question 23

what is evidnece for suborbitals

Answer 23

ionization energy of a particular atom

Question 24

first ionisation energy

Answer 24

is the energy required to remove one mole of electrons from one mole of gaseous atoms

Question 25

describe first ionization energy across a period

Answer 25

increase in ionization energy, number of protons in nucleus increases increase in electrostatic attraction of nucleus for electrons

Question 26

describe first ionization energy down a group

Answer 26

decrease in ionization energy, distance of electrons in valence shells increases reduces electrostatic attraction, electron inner energy levels shield attraction of nucleus for electrons

Question 27

what is the frequency or wavelength of the convergence limit

Answer 27

the frequency or wavelength of light emitted by an electron when it falls from the n=infinite to the outermost energy

Question 29

what type of spectrum is it when a light source goes through a cold gas cloud

Answer 29

absorption

Question 30

what type of spectrum is it when a light source goes through a hot gas cloud

Answer 30

emission

Question 31

why does most helium nucleis pass straigh through gold atoms

Answer 31

an atom is mostly made of empty space only composed of a very small nuclei

Question 32

why do very few helium nuclei deviate largerly from theri path whens hot at gold atoms

Answer 32

even though most of atom made of air, very small nucleus it has a positive charge which repels fold atoms

Question 33

what is the difference between diagrams 1s and 2s

Answer 33

1s is smaller than 2s

Question 34

diagram of 2p

Answer 34

a simple 8 drawing

Question 35

explain why the first ionization energy of sulfur is lower than that o phosphorous

Answer 35

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

Question 36

does cu have a greater ionization energy than cu2+ and why

Answer 36

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

Question 37

what type of radiation in spectrum has longest wavelength and lowest frequency

Answer 37

infrared radiation

Question 38

order of atomic orbitals in decreasing energy (highest to lowest).

Answer 38

f
d
p
s

Question 39

Emission and absorption line spectra both provide evidence for

Answer 39

the existence of energy levels within the atom

Question 40

Which electron transition represents the first ionisation of a hydrogen atom?

Answer 40

electron transition from n=1 to n=infinite

Question 41

Such emission spectra provide evidence that electrons are moving from

Answer 41

higher to lower energy levels with the higher energy levels being closer together.