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Chemistry 1 - Atomic Structure of the Periodic Table > Ionisation Energies > Flashcards

Ionisation Energies Flashcards

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1
Q

where did the evidence that different energy levels in which electrons can exist within atoms initially come from

A
  • atomic emission spectra

- done by a spectroscope

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2
Q

what happened when elements in a gaseous state were given energy by heating or having an electric current run through them

A
  • the electrons in their atoms moved to higher energy levels
  • they would eventually move back down to their original energy level
  • while emitting electromagnetic radiation
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3
Q

what is a spectroscope specifically measuring

A

the electromagnetic radiation emitted by the electrons in an atom

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4
Q

a spectroscope shows a series of different coloured lines with a black background behind them. what does this show

A
  • it shows that atoms, specifically electrons, dont emit radiation across the whole of the electromagnetic spectrum
  • instead, only specific frequencies are emitted
  • which are unique to the element
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5
Q

what types of atoms radiate the same set of frequencies

A

atoms of the same element

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6
Q

what is the emission spectrum produced called due to its nature

A

a line spectrum

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7
Q

what does the fact that only certain frequencies of electromagnetic radiation are emitted from electrons support

A
  • the notion that the energy of electrons in atoms can only have certain well defined values
  • rather than a continuous range of values
  • this is the basis of the quantum theory where the energy levels of electrons is said to be quantised
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8
Q

what is ionisation energy

A

the measure of the energy required in order to remove an electron from the atom of an element

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9
Q

how do successive ionisation energies support the existence of quantum shells (simple)

A
  • the successive ionisation energies of an element increases steadily
  • but big jumps occur at defined places
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10
Q

if sodium has an atomic number of 11, why is the ionisation energy of the 2nd electron much higher than the first ionisation energy and the 10th even more of a larger jump in terms of their ease of removal

A
  • the first electrons is easier to remove than the second
  • there is a steady increase in the ionisation energy for the next 8 electrons
  • but then a big jump from the ninth to the tenth and 11th
  • as the tenth is even harder to remove
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11
Q

why do the differences in the ease of removal of the electrons and therefore their ionisation energies vary like so

A
  • the 10th and 211th electron are in the first quantum shell
  • this means that they have the lowest energy
  • meaning it requires alot more ionisation energy to excite them enough to escape
  • the second quantum shell consists of the previous 8 electrons which sit at slightly higher energy levels
  • and therefore require less energy on order to ionise
  • the first electrons is in the third quantum shell so it has the most energy out of all the electrons
  • meaning that it requires the least energy to ionise
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12
Q

what are the three factors that impact the ionisation energy of an electron in an atom or just the energy an electron has

A
  • the nucleus or nuclear charge
  • the shielding
  • the distance between the electron and the nucleus (orbitals)
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13
Q

what does a larger nuclear charge lead to and why

A
  • it leads to a larger ionisation energy
  • because for a given distance and shielding, the electrostatic forces of attraction between the positively charged nucleus and electron is stronger
  • meaning that it would require more energy to overcome this attraction and have the electron escape its pull
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14
Q

what is shielding in an atom

A
  • the repulsion between electrons in an atom

- especially from the electrons at lower quantum shells

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15
Q

what does an increase in the electrons in the lower quantum shells relative to an electron lead to

A

increased shielding

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16
Q

what does an increase in shielding lead to and why

A
  • it leads to less ionisation energy being required
  • because the force repelling the electron, in the outer most shell, outwards and away from the nucleus is stronger
  • meaning that the pull of the nucleus is less influential to the electrons
  • so it can escape from its orbit easier with less energy needed
17
Q

what does an increase in the distance between the electron and the nucleus lead to and why

A
  • it leads to less ionisation energy being required
  • as more distance between them means that the electrostatic force of attraction the electron would feel from the nucleus is weaker
  • meaning it can escape from its orbit with less energy being required
18
Q

what is the mathematical way of defining ionisation energy

A

the energy of the electron when removed - the energy of the electron in its original orbital

19
Q

what can an electron feel an electron-electron repulsion by

A
  • electrons that are in the same orbital (albeit tiny)
  • electrons in different orbitals within a given quantum shell
  • electrons in adjacent quantum shells
20
Q

why does electron- electron repulsion lead to a decreased ionisation energy and what is the false reason

A
  • it is not because it ‘cancels out’ from the electrostatic pull of the nucleus or sets up a barrier
  • it just raises the energy of the electrons involved (the ones above) above the value they would have if there was no repulsion between them
  • which would therefore lead to less ionisation energy that would normally be needed
21
Q

how do the ionisation energies and energy levels of the electrons of elements change across periods

A
  • the ionisation energies generally increase across periods

- due to the energy levels of the electrons decreasing

22
Q

how do the factors that impact the energy levels of electrons and therefore their ionisation energies change across periods

A
  • as you move across a period, the nuclear charge increases
  • which leads to an increase attraction between the electrons and the nucleus
  • so the electrons have a lower energy level meaning an increased ionisation energy
  • however, one more electron is added to the same quantum shell
  • which increases the shielding (electron-electron repulsion)
  • this puts the outer electron about to be ionised at a higher energy level leading to lower ionisation energies
  • the orbital the outer electron is in and therefore the distance doesnt change
23
Q

which of the changing factors proves to be more significant

A
  • the increase in nuclear charge
  • leading to an overall decrease in the energy levels of the electrons across periods
  • and therefore an increase in their ionisation energies
24
Q

what periods does the general increase in ionisation energies apply to and what changes this trend

A
  • it applies to periods 2 and 3 mainly

- until you start to get into d-block elements in the 3rd quantum shell

25
Q

how does the energy of the electrons and therefore their ionisation energies change down groups

A
  • the energy of electrons increase down groups

- which means that the ionisation energy required decreases

26
Q

how do the factors that impact the energy levels of electrons and therefore their ionisation energies change down groups

A
  • as you go down a group the nuclear charge increases
  • this means that the energy level of the outer electron is lower which leads to higher ionisation energies
  • however, one new full quantum shell is added as you go down a group once
  • this means that there is an increase in shielding or electron-electron repulsion
  • meaning the energy level of the outer electron is increased
  • the extra shell also means that the outer electron has moved up an orbital leading to increased distances between it and the nucleus
  • this means that the electron feels less of a pull so it sits at an even higher energy level
27
Q

which of the changing factors proves to be more significant

A
  • the combination of the increased shielding and distance is more significant than the increase in nuclear charge
  • so there is a general increase in the energy of the outer electrons and therefore a decrease in ionisation energy own group 1
28
Q

what groups is this trend repeated in

A
  • 2 beryllium to barium
  • 5, nitrogen to bismuth
  • 6, oxygen to polonium
  • 7, flourine to astatine
  • 8 neon to radon

Chemistry 1 - Atomic Structure of the Periodic Table (4 decks)

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