Periodic Trends: Ionic Radius (Which ion is smaller?)
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- Опубліковано 5 січ 2017
- The size of an ion can be determined by:
* How many shells have electrons in them. More shells = larger ion
* How many protons the ion has. More protons = smaller ion
* How many electrons the ion has. All else being equal, more electrons = larger ion.
* Metal ions (positive, cations) are smaller than their corresponding elements
* Non-metal ions (negative, anions) are larger than their corresponding elements.
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Excellent my sweet sir 😊.before this vidio ihave lot of problem in ionic radius when same shell
Which one is larger in li + and mg 2+
So helpful!
What about In+ and Br-. In+ has 48 electrons and more shells but it is smalled than Br- which has 36 electrons and less shells?
Actually does it work for Na+ Li+ Mg2+ Be2+
I understood fully now, thanks.
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How about Co2+ or Co3+ what is the larger ion?
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Guys but in the periodic trend across the period inoic radius decreases and Down the group is increases am i right?
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Why the na is larger than na+, can u tell the reason plsssss?
In Na+ one elctron losses so there are only 10 e- in it . But Na has 11e- in it . Thats y .
electron configuration: For Na (2, 8, 1) which is 3 shells
For Na+ (2, 8) which is 2 shells (so it is the first reason in the video @0:33 )
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Nice
But what about non iso electronic species
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F is larger than F- because F- is attaining a stable electronic config hence smaller size please review....
WOW you are correct. All of the other Halogens fit the trend I described, but Fluorine does not. I'll have to read more about this .
@@chemistNATE how do we compare Li+ and Mg+2
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Simple trick: +ve charge is inverse of size and -ve charge is directly to size....... Large positiviy means smaller size but large negativity means larger size 😏