Ash-M :)
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#1
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#1
Does anyone know a cheat/hack to know all the Ligand substitution and acid-base reactions with transition metals?

Please help

Even if it's a song or something.
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r7kytt
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Lol 8013 this is your thread
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sqrt of 5
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you only need to know 3 monodentate ligands and 2 bidendate
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8013
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(Original post by r7kytt)
Lol 8013 this is your thread
What????
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8013
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(Original post by Ash-M :))
Does anyone know a cheat/hack to know all the Ligand substitution and acid-base reactions with transition metals?

Please help

Even if it's a song or something.
I have a ligands song which has finished a rough draft, a parody of Hammer To Fall, and a half-finished reactions song on transition metals, a parody of Disco 2000. I will have another for multidentate ligands soon. When I am done with all 3 I will post the lyrics and interpretations to them.
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r7kytt
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(Original post by 8013)
What????
Would you mind supplying your great expertise, I know you have plenty of memorable songs for chemistry, for this student?
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Ash-M :)
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(Original post by sqrt of 5)
you only need to know 3 monodentate ligands and 2 bidendate
I'm not talking about those - that's fine.

I'm talking about the Hexa aqua ions reacting with Cl/OH/NH3/CO3 and the colour change (and any other observations, like effervescence or a precipitate)
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Ash-M :)
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(Original post by 8013)
I have a ligands song which has finished a rough draft, a parody of Hammer To Fall, and a half-finished reactions song on transition metals, a parody of Disco 2000. I will have another for multidentate ligands soon. When I am done with all 3 I will post the lyrics and interpretations to them.
Thanks!
When you do post it, can you send a link here?
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Ash-M :)
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#9
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(Original post by r7kytt)
Would you mind supplying your great expertise, I know you have plenty of memorable songs for chemistry, for this student?
Thank you, kind sir, for directing 8013 to my humble thread
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8013
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#10
(This is my ligands song, parody of Hammer To Fall)
Ligand uses a lone pair
Forms dative (bond) with metal ion
Structure in square brackets
Molecules around and charge outside
Complex, metal (joined) to ligands
A charge, ion, how should we name it?
Number then name of ligands
Then ion name and oxi-number

Complexes have unique colours
But how do those colours exist?
They have unfilled d-orbitals
With H2O ligand, it splits into 2
With energy, electron excites
Large difference between, more energy
This causes smaller wavelength
Its complementary colour transmits

Complex 4 types of shapes
With 6, 4 or 2 ligands
Octahedral has six joined in
Tetrahedral 4, linear 2
square planar, 4, 90 angle
As 2 lone pairs repel each other
They have cis-trans isomers, work like alkenes
Charge depends on ion
And number of negatively charged ligands
*And the bond must come from
The element supplying lone pairs for dative bond (x2)

That’s a ligand
Ligand, you know, how ligand works
While you need it to treat your cancer
By Anti-cancer action
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8013
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#11
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#11
Tetsudo shoka (Japanese song) parody for transition metals. The original has 384 verses. This one has 22 and I think it is really good already.

#1 Transition metal is an element which
Forms stable ions with incomplete d orbitals
Ligand is the species with lone pair of electrons
Forms a dative bond with a metal ion

#2 Dative bond is covalent bond between the metal
And an ion which electrons come from the ligand
1 lone pair monodentate, 2 is a bidentate
Find the total lone pairs connected to the metal

#3 Coordinate bonds are the name of the dative bonds
Forms from pair of electrons from one atom
Transition metal donates electron to it
And the ligand mostly water accepts the lone pair

#4 Colour comes from electrons in energy levels
The ligands will split the d orbital to 2
Transition of energy depends on the difference
larger difference more energy absorbed electron

#5 Energy is proportional to light frequency
Larger difference between levels it shifts to the blue
However zinc ion does not emit a colour
Cause all its d orbitals are completely filled

#6 Most of complexes are octahedral shapes
Bond angle is 90, six fold coordination
Draw to the atom with lone pair for the dative bond
Original charge and ligands determine the charge

#7 If Cl’s a ligand it is tetrahedral
Only 4 ligands, while 2 it is linear shape
XeF4 square planar lone pairs top and bottom
Use cis-trans like a double bond for the isomers

#8 Redox reaction changes the oxidation number
Ligand type and number both will remain unchanged
3d5 can’t do it cause the ion is stable
Paired electrons remove easily in repulsion

#9 Transition metal plus charge number of alkali
Forms H2O4 OH2 deprotonation
With excess NH3 some compounds will continue
This is a type of ligand exchange reaction

#10 Cr starts from green to a green precipitate
When you add excess NH3 it will turn purple
The same also goes to the Ni ion
But deep blue solution forms with excess NH3

#11 Cu starts from blue to blue and then to deep blue
Zn colourless to white and back to colourless
Co pink, blue to pale yellow but expose to air
Ppt blue to pink and solution turns to brown

#12 Mn pale pink to pale brown, darker expose to air
Fe 2 pale green to green, brown when exposed to air
Fe 3 yellow brown to brown, they have one common thing
They have nothing more to see with excess NH3

#13 If NaOH excess, some may have effect too
Cr water ligand will form a green solution
Zn forms another colourless solution too
However the other ions all have no effect

#14 Add 4 Cl minus coordination number change
Cu will have blue to green to yellow solution
Co works too but it turns from pink into blue
Hydroxide reacts with acid, base, amphoteric

#15 When Cr is oxidised from plus 3 to plus 6
Add H2O2 solution from green to yellow
Add some acid to dichromate yellow to orange
Add Zn solution will reduce to blue +2

#16 Use the E cell values to explain the redox
You can find out by adding half cells together
It always gives out positive potential
So reaction thermodynamically feasible

#17 Vanadium has four ions from plus 2 to plus 5
The plus 5 can reduce to plus 2 with E cell
Proof is that the E cell values are positive
But 2 to 0 negative and it can’t be done

#18 Transition metals can be used as catalysts
Like V2O5 in the contact process
SO2 adsorbs to it, SO3 then desorbs
O2 with V2O4 back to V2O5

#19 Homogenous Fe2+ S2O82-
Both in aqueous phase Fe is catalyst
As S2O8 and iodine negative repel
So it makes reaction faster in room temperature

#20 Fe2+ not repelled and react together
Fe3+ and SO4 two minus are formed
When Fe3+ reacts with the iodide
Iodine formed and Fe2+ comes out again

#21 MnO4 plus C2O4 and an acid
One of the products formed is Mn2+
It catalyses the reaction, rate faster
Autocatalysis happens in the titration

#22 Here we get all points from all these transition metals
From structure and shape ligand to redox, catalyst
Here we have reactions and the proofs to the redox
All we know the functions of it as a catalyst
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