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CHEMISTRY: TOPIC 12 ATOMIC STRUCTURE


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CHEMISTRY: TOPIC 12 ATOMIC STRUCTURE


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[Front]


What is ionisation energy?
[Back]


min amount of energy needed to remove an electron from 1 mole of gaseous atoms under standard conditions M(g) = M+(g) + e-

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12 questions
🇬🇧🇬🇧
What is ionisation energy?
Min amount of energy needed to remove an electron from 1 mole of gaseous atoms under standard conditions M(g) = M+(g) + e-
What is the energy of a photon's formula?
E = hv v= light frequency (Hz) h = plancks constant (6.63*10^-34)
What is the wavelengths formula?
C = V *wavelength c = speed of light (3*10^8) wavelength (m) multiply answer by Avogadro's constant (6.02 *10^23) /1000 = kJ mol-1
Why is the 2nd ionisation energy always higher than the first?
1) once the electron is removed = positive ion = attracts an electron more strongly than a neutral atom = more energy needed to remove the 2nd electron 2) less repulsion among the remaining electrons = pulled closer by nucleus = more strongly attracted = more difficult to remove
Why is the first IE lowest?
Furthest from nucleus and shielded with the other electrons in the atom
What is the general trend for IE ?
Increases from left to right across a period decreases down a group
Why is boron an exception to the IE trend?
Boron has more protons than beryllium but the IE is lower bec the electron removed from Boron is in a 2p level but for Be it is removed from the 2s level. B's electron is farther away from the nucleus , less energy is needed
Why is oxygen an exception to the IE trend?
Oxygen has 2 electrons paired up in teh same p orbital but nitrogen doesnt an electron in the same p orbital is easier to remove bec of the repulsion from the other electron
What does the IE trend across periods show?
Shows the existence of main energy levels and sub-levels in atoms
How can the electron configuration be deduced from an IE graph?
Large jumps in the graph occur bw the main energy levels