Periodic Trends: Electronegativity, Ionization Energy, Atomic Radius - TUTOR HOTLINE
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- Опубліковано 31 бер 2019
- This video explains the major periodic table trends such as: electronegativity, ionization energy, electron affinity, atomic radius, ion size and metallic character. I also go over the exceptions to each trend and several periodic trends examples.
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She forgot to mention something very important regarding the Ionization Energy part; Another exception other than the two she named is that the NOBLE GASES are going to have the HIGHEST ionization energy since they are so stable it is going to require the most energy to remove an electron.
Do the noble gases follow the same vertical trend (higher row the noble gas is, higher IE compared to lower noble gases?
@@harmie1743 No, because now another component has to be taken into consideration; orbit size. The bigger the orbit the less energy it’ll need to removed an electron since it’s so far away from the nucleus now and the smaller it is the harder it is to remove an electron since it’s closer to the nucleus. So when you are going down the noble gases periodically they get bigger and bigger thus less IE.
Therefor the most IE will reside with the noble gas of Helium.
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Timestamps:
Electronegativity: 0:25
Ionization Energy: 3:40
Electron Affinity: 10:09
Atomic Radii: 12:37
Ion Size: 14:35
Metallic Character: 21:54
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18:12 - one way I can recognize which is larger is because Br has 35 protons while Kr has 36 protons, the 35 protons in the Br nucleus is going to have less of a pull to the 36 electrons compared to the pull of Kr's 36 protons so Br will be larger. Understanding this requires understanding the shielding effect, but for me it's helpful to know the why behind anions being larger.
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I believe the electronegativity follows the below order. Ne > F > O > N >= Ar > C > Kr > Cl > S >= Xe > Se ~ I ~ Rn> other elements..... Helium's EN is very difficult to predict. Its should be less than that of oxygen.
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