electron configuration

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64 Terms

1
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draw a diagram of how the waves look going down an EM spectrum

knowt flashcard image
2
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what side of the em spectrum has the longest wave length give colour and radiation

red, radiowaves

3
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what side of the em spectrum has the shortest wavelength give colour and radiation

purple

gamma

4
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if something has a short wavlength whats its frequency like

high frequenecy

5
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so long wavelength =

low frequency

6
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name the relationship between frequency and wavelength

inversely proportional

7
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3 most damaging wavelengths

ultra violet

x rays

gamma rays

8
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what is the speed of all EM waves

speed of light or c

3.00 x 10^-8

9
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whats the equation linking wavespeed frequency and wavelength

c = fλ

10
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what is a continuous spectrum

a spectrum which shows all the wavelengths/ frequencies/ energies of light

11
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what does a continuous spectrum look like

RAINBOW (so like tom)

<p>RAINBOW (so like tom)</p>
12
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so what does a line spectrum show

specific wavelengths/frequencies of light

13
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what are two types of line spectra

absorption and emission

14
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what does an absorption spectrum show

frequency/wavelength shown when a substance (usually a gas) has white light shone through it to show us what wavelengths and frequencies of light it absorbs

15
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what does an absorption spectrum look like

its all rainbow and it has black lines to show whats being absorbed

<p>its all rainbow and it has black lines to show whats being absorbed</p>
16
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what does an emission spectrum show

the wavelegths/frequencies of light emitted when white light is shone on a substance

17
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what does an emission spectrum look like

all black with rainbow lines

<p>all black with rainbow lines</p>
18
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why do substances emit or absorb light

light is made up of photons = energy stores

when light shines on an object it will absorb certain photons of light

which excites the atom's electrons on the energy levels (shells) causing them to jump up one or more energy levels

when the electrons jump back down from the energy level it causes them to emit photons of light

19
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why do the electrons jump back down

the atom is not stable

20
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can electrons jump more than one shell

yes

21
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the bigger the jump =

the greater the energy of the photon

22
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how is the line spectra of hydrogen specific to hydrogen

the lines converge the same as the energy levels

<p>the lines converge the same as the energy levels</p>
23
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so how does the line emission spectrum of hydrogen come about

white light is shone at a hydrogen atom, exciting electrons causing them to jump energy levels, when they return to their original energy level they release a photon of light which is shown on the hydrogen emission spectrum

24
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what are principle quantum numbers

the numbers on the energy levels of an atom

n = 1 first shell

n = 2 second shell

<p>the numbers on the energy levels of an atom</p><p>n = 1 first shell</p><p>n = 2 second shell</p>
25
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two key words to describe energy levels of atoms

1. converging: at higher energy levels (further from the nucleus) the shells get closer together

2. concentric: they are within one another

26
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describe the lines on the emission spectra of hydrogen

converging at higher energies

<p>converging at higher energies</p>
27
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how does the photon of light released differ when electrons jump back down

depending on which energy level it jumps BACK DOWN TO

e.g if it jumps down to n=1 its different photon of light then if it jumps back down to n=2

28
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where does the electron jump back down to if its got the highest energy

or where does the highest energy jump come back down to

n=1

29
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if an electron jumps back down to n=1 what kind of photon is it

it is a UV photon

30
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why is UV the highest energy

not a damn clue - just learn it

31
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if an electron jumps back down to the n=2 energy level what kind of photon is it

visible light

32
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if an electron jumps back down to the n=3 energy level what kind of photon is it

infared

33
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how do you ionise an atom

by exciting an electron enough to just pop off the atom

34
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what two things can be worked out using the main energy levels

the maximum number of electrons

the number of orbitals

35
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how to work out the maximum number of orbitals from main energy level number

n^2

36
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e.g work out the orbital number of the 5th main energy level

n=5

5^2 = 25

37
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how to work out the maximum number of electrons

2n^2

38
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e.g work out the max number of electrons on the 4th main energy level

n=4

4x2 = 8

8^2 = 64

39
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what are the 4 orbitals

s, p, d, f

40
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what is the lowest energy orbital of the 4

s orbital

41
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shape of s orbital

knowt flashcard image
42
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shape of the p orbital

how many are there

infinity shaped

three px py pz

<p>infinity shaped</p><p>three px py pz</p>
43
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shape of d orbital and how many

each one is like a four leafed clover

D FOR DONUT

<p>each one is like a four leafed clover</p><p>D FOR DONUT</p>
44
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where is s block p block d block and f block on the periodic table

knowt flashcard image
45
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how to work out the electron configuration

find element on periodic table then go from hydrogen across and count in the orbitals e.g

C, 1s2 2s2 3p2

can figure out small number on end by counting along the p orbital to see how far in the element carbon is

46
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how to know the coefficient of the line youre counting across

written on the side !!!!!!!! its the period number !!!!!

well up until the d block elements

47
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whats special about the way we write the electron configuration of elements which have electrons occupying orbitals in the d block

the d block configuration starts from 3d instead of 4 like shown on the period number e.g the electron configuration of Mn is [Ar] 4s2 3d5

48
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how can we shorten electron configuration

by using the nearest noble gas and wacking it in square brackets

49
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what do you need to do when writing electron configuration for ONLY transition elements

swap the order so its 4s and 3d

50
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why should you swap the order of 3d and 4s in transition elements

even though the 4s gets filled first then the 3d when theyre emptied, when ionised and lose electrons they actually lose their 4s ones first due to the similar energies between them

51
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how to draw orbital box diagram (the order of the boxes)

same order as the periodic table

52
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what do the whole number plus boxes represent

subshell

e.g 2p ■■■

is the 2p subshell

53
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so what does one box represent

an orbital which makes sense because there was 3 p orbitals px pz py so it makes up p subshell

54
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whats true about the number of electrons in one oribital

2 electrons

55
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what is hunds rule

electrons fill all orbitals in a subshell singly before forming pairs

56
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what is paulis exclusion principle

2 electrons occupying the same orbital must have opposite spins

57
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whats 2 things to remember if asked to draw orbital box diagram

1. the 1s 2s 3s 4s 5s subshells all sit on one line so do the 2p 3p 4p subshells and 3d 4d

2. theres 1 orbital for s subshells, 3 for p subshells and 5 for d subshells

58
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two exceptions in electron configuration

copper and chromium

Cu and Cr

59
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why is chromium an exception and how does it work

half full/full or empty orbitals are the most stable and energetically favourable

if chromium stayed as it was it would have an electron in four out of the five 3d orbitals meaning its partially filled and the 4s orbital is fully filled however instead the 2nd 4s electron goes to the last orbital on the 3d subshell so theres instead a half filled 3d orbital and a half filled 4s orbital which is more stable and energetically favoured making its elec config 4s1 3d5

60
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why is copper an exception and how does it work

copper's electron config is actually 3d10 4s1 instead of 3d9 4s2 this is because its more ENERGETICALLY FAVOURABLE for copper to fill each 3d orbital and leave the 4s orbital half filled as opposed to full 4s orbital and partially filled 3d orbital

61
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what is the limit of convergence

where the lines on an emission spectrum converge

62
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what are the two equations needed for a limit of convergence question

wave speed (given to you its the speed of light) = wavlength x frequency

ionisation energy = h (constant) x frequency

63
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what do we work out using those equations

which of those things equates to the limit of convergence

the ionisation energy

64
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what should you be worried about in these limit of convergence calcuations

it might ask you for it in moles not one atom so work out in atoms then times it by avogadros constant

if it asks for say 2 moles then you again work out atoms then times by avogadros constant then times 2