Doesn't Fe2+ form with a filled d-orbital, 3d6 isn't half filled, an atomic orbital by definition is a region around the nucleus that can hold 2 electrons, and the d sub shell contains 5 d orbitals in this case we would have 3 filled d orbitals right? By definition Fe3+ empties to 3d5 making the element Fe a transition element as it forms a stable ion with a partially filled d orbital right?
A transition metal is one that forms an ion with a partially-filled d-_subshell_, not orbital. 6/10 electrons is partially filled, so both, the existence of Fe2+ and Fe3+ make Fe a transition element.
I think i get it now, i watched the end lol, i use diagnol filling rule and end up at 4s^2 4p^6 but it cant be the p bloc so it must move diagonally up to 3d^10 which is full, am i right ???
hey, you r contradicting yourself. Sc and Zn are of course not transitional elements if we take the definition u have just given us. they should form at least 1 ion with an incomplete subshell!!!!! Sc has an empty d shell while Zn has a full d subshell hence they are not transition elements!!!!! who the is ridiculous????
Sc and Zn are not transition elements. i have quoted from two sites, just to avoid typing the whole explanation A transition metal is one which forms one or more stable ions which have incompletely filled d orbitals. On the basis of the definition outlined above, scandium and zinc don't count as transition metals - even though they are members of the d block. Scandium has the electronic structure [Ar] 3d14s2. When it forms ions, it always loses the 3 outer electrons and ends up with an argon structure. The Sc3+ ion has no d electrons and so doesn't meet the definition. Zinc has the electronic structure [Ar] 3d104s2. When it forms ions, it always loses the two 4s electrons to give a 2+ ion with the electronic structure [Ar] 3d10. The zinc ion has full d levels and doesn't meet the definition either. www.chemguide.co.uk/inorganic/transition/features.html Explain why Sc and Zn are not considered to be transition elements. A transition metal element is defined as an element that possesses an incomplete d sub-level in one or more of its oxidation states. Scandium is not a typical transition metal as its common Sc 3+ has no d electrons. Zinc isn’t a transition metal as it contains a full d sub level in all of its oxidation states. acceleratedstudynotes.wordpress.com/tag/13-2-2-explain-why-sc-and-zn-are-not-considered-to-be-transition-elements/ so the guy u heard is not ridiculous after all!!!!
11:42 ok u were just making it up!!! after the first minute I couldn't stand watching the whole thing because I was fully convinced that you are confused!!!!!! Shakalaka's comment forced me to rewatch the conclusion
looool i like the banter at the start :p
I told you that you would get there 2024 is looking good for you James
New iPad yesterday so can get back into making walkthroughs 👍
I will never forget this topic now because of that clearly made-up story about Zinc and Scandium😭
That ending was hilarious, great video!
i guess it's kind of randomly asking but does anybody know a good site to watch new movies online?
@Franco Brecken Meh I use Flixportal. you can find it on google :D -nixon
@Nixon Reece Thanks, signed up and it seems to work =) Appreciate it !!
@Franco Brecken You are welcome xD
@@nixonreece3339 most npc interaction ive ever seen
R.I.P To the people who didnt want till the end...
The ending cracked me up haha
Excellent video
Really helpful, thanks!
Thanks m8, i'm a junior in highschool and never done this, now I get it. :D
How did u get 4s^2 3d^10 on zinc the last one. I got 4s^2 and 4p^6 ?????
pls answer asap
Do we need to learn all of the possible ion charges and their different colours? In page 205 of the textbook?
The ending 👌🏽👌🏽
This video is perfect thanks.
Doesn't Fe2+ form with a filled d-orbital, 3d6 isn't half filled, an atomic orbital by definition is a region around the nucleus that can hold 2 electrons, and the d sub shell contains 5 d orbitals in this case we would have 3 filled d orbitals right?
By definition Fe3+ empties to 3d5 making the element Fe a transition element as it forms a stable ion with a partially filled d orbital right?
A transition metal is one that forms an ion with a partially-filled d-_subshell_, not orbital. 6/10 electrons is partially filled, so both, the existence of Fe2+ and Fe3+ make Fe a transition element.
This came up in the exam about Sc and Zn!!!
So I haven't been wasting my time!
Is it just transition elements that u remove from the 4s before the 3d or is that always the case ?
Just TMs
What about Vanadium 5+? Thanks
Awesome awesome awesome
😂 really fun video sir!
thank u chem man
i'm fasting couldnt be asked to go thru textbook
How did u get 4s^2 3d^10 on zinc the last one. I got 4s^2 and 4p^6 ?????
pls answer asap
I think i get it now, i watched the end lol, i use diagnol filling rule and end up at 4s^2 4p^6 but it cant be the p bloc so it must move diagonally up to 3d^10 which is full, am i right ???
Simon M electrons fill up d sub shells first b4 u go anyway near '4s6,
Hahaaa you sneaky guy! Still I learnt a few things in the process.
you got me theree
hey, you r contradicting yourself. Sc and Zn are of course not transitional elements if we take the definition u have just given us.
they should form at least 1 ion with an incomplete subshell!!!!! Sc has an empty d shell while Zn has a full d subshell hence they are not transition elements!!!!!
who the is ridiculous????
justice munyoro ?????????
Sc and Zn are not transition elements. i have quoted from two sites, just to avoid typing the whole explanation
A transition metal is one which forms one or more stable ions which have incompletely filled d orbitals.
On the basis of the definition outlined above, scandium and zinc don't count as transition metals - even though they are members of the d block.
Scandium has the electronic structure [Ar] 3d14s2. When it forms ions, it always loses the 3 outer electrons and ends up with an argon structure. The Sc3+ ion has no d electrons and so doesn't meet the definition.
Zinc has the electronic structure [Ar] 3d104s2. When it forms ions, it always loses the two 4s electrons to give a 2+ ion with the electronic structure [Ar] 3d10. The zinc ion has full d levels and doesn't meet the definition either.
www.chemguide.co.uk/inorganic/transition/features.html
Explain why Sc and Zn are not considered to be transition elements.
A transition metal element is defined as an element that possesses an incomplete d sub-level in one or more of its oxidation states. Scandium is not a typical transition metal as its common Sc 3+ has no d electrons.
Zinc isn’t a transition metal as it contains a full d sub level in all of its oxidation states.
acceleratedstudynotes.wordpress.com/tag/13-2-2-explain-why-sc-and-zn-are-not-considered-to-be-transition-elements/
so the guy u heard is not ridiculous after all!!!!
11:42 ok u were just making it up!!! after the first minute I couldn't stand watching the whole thing because I was fully convinced that you are confused!!!!!!
Shakalaka's comment forced me to rewatch the conclusion
Glad that's all sorted. My attempt at humour backfired there
lol