S1.3 Flashcards
What units does Wavelengths have
m
What units does frequency have
Hz
Frequency and Wavelength are
Inversely Proportional
Energy and Frequency are
directly proportional
What are the 7 regions of EM spectrum increasing frequency
Radio waves
Microwaves
Infrared
Visible Light
Ultra Violet
X-rays
Gamma rays
What has the highest frequency and highest energy , shortest wavelength in the EM spectrum
Gamma Rays
What has the lowest frequency , lowest energy and longest wavelength
Radio waves
Red is on the right with
lowest energy lowest frequency and longest wavelength
Violet is on the left with
highest energy
highest frequency
shortest wavelength
What is the difference between a continuous spectrum and emission line spectrum
Continuous spectrum shows all the wavelengths or frequencies of visible light
Emission line only shows specific wavelengths or frequencies
Lines converge at
higher frequencies
n= 1 is
and has
closest to the nucleus
lowest energy
n=6 is
and has
furthest from the nucleus
highest energy
Main energy levels
converge at higher energy
How do electrons move between energy levels
By absorbing or emitting energy and getting excited
What happens if an electron absorbs an amount of energy
it will transfer from a lower energy level to a higher energy level and be in its excited state
e.g n=2 to n=3
What happens after the electron becomes excited
It becomes unstable and emits the same amount of energy that it absorbed and it transitions back down to n=2
When the the electron transfers from n=3 to n=2 what colour does it correspond to
red
The amount of energy emitted also depends on the
size of the transition
When is emission line spectra produced
when electrons transition from higher to lower energy levels
Four discrete lines on the spectrum suggest
Electrons can only exist at certain energy levels
What radiation correspond when electron transitions from higher energy levels to n=1
UV radiation
What radiation corresponds when electron transitions from higher energy levels n=2
visible light
What radiation corresponds to when electron transitions from higher energy levels to n=3
Infrared Radiation (lowest energy)
What does n= ♾️ represent
The point when the electron has been completely removed from the attraction of the nucleus and the atom has been ionised
the larger the transition the
more energy emitted
What are the sublevels divided into
s p d f
How many electrons can a single atomic orbital hold
two
How many atomic orbitals are each sublevel made of
s - 1 atomic orbital
p - 3 atomic orbitals
d - 5 atomic orbitals
f - 7 atomic orbitals
How many electrons can each sublevel hold
s - two
p - six
d - ten
f - fourteen
The maximum number of electrons in an energy level is
2n squared
What are the exceptions to the Aufbau Principle
Copper and Chromium
What would you expect electronic configuration of CU 29 to be vs what it actually is
thought : Cu 1s2 2s2 2p6 3s2 3p6 4s2 3d9
Actual : Cu 1s2 2s2 2p6 3s2 3p6 4s1 3d10
What’s would be the actual electronic configuration of Cr 24
1s2 2s2 2p6 3s2 3p6 4s1 3d5
Why does boron have a lower ionisation energy then Be ?
Be has electronic configuration of 1s2 2s2
B has electronic configuration of 1s2 2s2 2p1
Higher nuclear charge
electrons in p orbitals are of higher energy and further from the nucleus than electrons in s orbitals , therefore require less energy to remove (weaker electrostatic forces of attraction)
Why has oxygen got a lower IE than nitrogen
1s2 2s2 2p4
1s2 2s2 2p3
Nitrogen has three singly occupied p orbitals but in oxygen one orbital is doubly occupied. An electron is repelled by the second electron and requires less energy to remove than an electron in a half -filled orbital
What happens at the convergence limit
The electron has been removed from the attraction of the nucleus and the atom has been ionised
What is Energy measured in
J
What is wavelength measured in
m
From energy in joules to ionisation energy what do you do
multiply by avogadros constant and divide by 1000
Define successive ionisation energy
The energies required to remove more and more electrons from an ion that is becoming increasingly positive
What is the first and second ionisation energy equation of Allumium.
Al(g) > Al+ (g) + e- 1st
Al + (g) > Al 2+ (g) + e-
The order in which electrons are removed is from
the higher energy levels first
After the first ionisation energy why do all successive ionisation energies show an increase ?
After the first ionisation, the electrons are being removed from an increasingly positive ion. This leads to an increase in the electrostatic attraction between the nucleus and the remaining electrons and an increase in the IE
How do you determine from the large increase what group an element belongs to
Count the number of electrons before first large increase
How can the number of occupied energy levels be identified ?
By the number of jumps +1
Identify energy levels
n=1
n=2
n=3
n=4
n=5
n=6
