CHEMISTRY: TOPIC 12 ATOMIC STRUCTURE
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CHEMISTRY: TOPIC 12 ATOMIC STRUCTURE - Leaderboard
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| 🇬🇧 | 🇬🇧 |
| 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 |
| When do the large differences in IE happen? | Bw energy levels |
| 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 convergence limit at higher frequency correspond to? | First ionization energy |
| 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 |