1st lecture - atomic structure Flashcards

1
Q

what is chemical reactivity determined by

A

the movement of electrons between atoms

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2
Q

atoms cannot be

A

divisible
cannot be divided/separated

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3
Q

atoms consist of

A

charged particles

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4
Q

thompson made

A

plum pudding
electrons are the bits of plum

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5
Q

rutherford model

A

electrons orbit the nucleus

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6
Q

what was wrong with rutherfords model

A
  • made it seem that all electrons are equal - challenged by atomic emission spectra
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7
Q

how does atomic emission spectra challenge rutherford

A

in AES: electrons absorb energy and become excited

they transition to higher energy levels within the atom.

if rutherford was right, this would not happen as there would be no higher energy levels due to all e- being the same.

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8
Q

what is the atomic emission spectra

A

spectra with different lines
light: wave or particle

excited e- transition to higher energy levels then return to their original levels by emitting energy in the form of photons (light)

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9
Q

equation for energy carried by a photon

A

energy =
Plancks constant x frequency
=
planks x speed of light / wavelength

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10
Q

planks constant

A

6.626 x 10^ -34

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11
Q

what does the atomic emission spectra show

A

shows lines that are unique to each element

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12
Q

what is E = hv tell us

A

eneegy = planks x frequency

photon energy isnt continuuous but quantised

its a multiple of “hv” meaning it has a discrete value

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13
Q

bohr atom

A

positive nucleus
e- in orbits at diff distances to the nucleus

e- cannot exist between orbits, they are quantised

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14
Q

what are orbits defined by

A

quantum number ‘n’

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15
Q

e- closer to the nucleus are

A

lower in energy
tightly bound
more stable

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16
Q

what is a transition

A

e- absorb energy
become excited
move to higher energy orbital
release energy in photons
relax back to original orbit

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17
Q

what does each line on the spectra correspond to

A

a transition
this is unique to each element

18
Q

if an e- distance from the nucleus doubles (x2) the attraction

A

1/4s

greater distance = higher attraction

19
Q

equation to find energy released when an H electron moves to diff orbits

A

E =
-2.178 x 10^-18
x (1/nf ^2) - (1/ni ^2)

20
Q

how many orbitals are there in total

21
Q

as u move further from the nucleus, (increasing n value) the energy levels..

A

get closer and closer and closer

22
Q

n=1 series name

A

lyman series
UV light

1= bottom
lyman bc ur lying down at the bottom of the page

23
Q

n=2 series name

A

balmer series
VISIBLE light

2 ashy knees that need balm

24
Q

n=3 series name

A

paschen series
IR light

passion for Christ: father, son, Holy Spirit

25
general rule for guessing which transition involved the greatest release of energy
the one with the lowest final n value eg: 1 or 2 this is bc the orbits are spaced out the most here
26
which electron will emit a photon in the visible light spectrum
n=2 balmer series
27
what is still wrong with the bohr explanation?
- works with H only tbh - doesnt explain periodic properties of the periodic table - atomic spectra results are different using a magnetic/non magnetic field
28
electrons in magnetic field mass spectra
can make a transition to 3 slightly different energy levels
29
electrons in atomic spectra with no magnetic field
can only absorb 1 distinct wavelength of light can only jump 1 distinct energy level
30
was planck studying waves or particles
waves walk the Planck
31
was einstein studying waves or particles
particles
32
plancks equation for waves
energy = plancks constant x frequency
33
is frequency a property of waves or particles
waves
34
einsteins equation for energy
energy = mass x speed of light^2
35
de broglie equation
planks/wavelength = momentum
36
wha does de broglie link
pure particle property and pure wave property. combines planck and einsteins equations for particles and waves.
37
what is constructive interference
when 2 waves are in phase with each other they reinforce eachother and their amplitude doubles
38
what is destructive interference
when 2 waves are out of phase and cancel each other out
39
what property do electrons and light share
wave particle duality. - constructive + destructive interference which is a property of waves. - photoelectric effect: light knocks electrons off a metal - particle property
40
summary of this set
e- have wave particle duality meaning they have wave and particle properties e- can move between orbits when energy is given these are called transitions and show up on atomic emissions spectra.
41