Aqua Metal Ions Flashcards
Write the equation and observed reaction for the reaction between a Copper Aqua complex and a few drops of OH-(aq)
(Excess same as this)
Blue Solution ——-> Blue precipitate
Write the equation and observed reaction for the reaction between a Colbolt Aqua complex and a few drops of OH-(aq)
(Excess same as this)
Pink Solution ——-> Blue Precipitate
Write the equation and observed reaction for the reaction between a Aluminium Aqua complex and a few drops of OH-(aq)
Clear and Colourless Solution ——> White Precipitate
Write the equation and observed reaction for the reaction between a Iron(3+) Aqua complex and a few drops of OH-(aq)
(Excess same as this)
Purple Solution ——-> Brown Precipitate
Write the equation and observed reaction for the reaction between a Iron(2+) Aqua complex and a few drops of OH-(aq)
(Excess same as this)
Green Solution ——> Green Precipitate ——> Brown (on standing)
Write the equation and observed reaction for the reaction between a Aluminium Aqua complex and excess OH-(aq)
Clear and Colourless solution ——> White Precipitate ———> Colourless solution (precipitate dissolves)
+ 3 H2O on products
Write the equation and observed reaction for the reaction between a Copper Aqua complex and a few drops of NH3(aq)
Blue Solution ——-> Blue Precipitate
Write the equation and observed reaction for the reaction between a Colbolt Aqua complex and a few drops of NH3(aq)
Pink Solution ——-> Blue Precipitate
(2NH4+ not one)
Write the equation and observed reaction for the reaction between a Iron(2+) Aqua complex and a few drops of NH3(aq)
Green Solution ———-> Green Precipitate ———> Brown precipitate (on standing)
Write the equation and observed reaction for the reaction between a Aluminium Aqua complex and a few drops of NH3(aq)
(Same as Excess)
Clear and Colourless Solution ——> White Precipitate
Write the equation and observed reaction for the reaction between a Iron(3+) Aqua complex and a few drops of NH3(aq)
Purple Solution ——> Brown Precipitate
Write the equation and observed reaction for the reaction between a Copper Aqua complex and Excess NH3(aq)
Ligand Substitution Reaction
Blue Solution ——> Blue Precipitate —-> Deep Blue Solution
Write the equation and observed reaction for the reaction between a Colbolt 2+ Aqua complex and Excess NH3(aq)
Pink Solution —-> Blue Precipitate —-> Pale Brown Solution
Write the equation and observed reaction for the reaction between a Copper Aqua complex and a Carbonate ion (CO3 2- ) (aq)
Blue Solution ——-> Blue Green Precipitate
Write the equation and observed reaction for the reaction between a Colbolt Aqua complex and a Carbonate ion (CO3 2- ) (aq)
Pink Solution ——-> Purple Precipitate + Water
Write the equation and observed reaction for the reaction between a Iron (2+) Aqua complex and a Carbonate ion (CO3 2- ) (aq)
(2+ on Complex)
Green Solution ——-> Green precipitate + Water
Write the equation and observed reaction for the reaction between a Copper Aqua complex and Hydrochloric Acid (HCl) (aq)
Blue Solution ——-> Yellow Solution with a green tinge
Tetrahedral change in structure
Write the equation and observed reaction for the reaction between a Colbolt Aqua complex and Hydrochloric Acid (HCl) (aq)
Pink Solution ——-> Blue solution
tetrahedral Change in structure
-2 charge on Colbolt chloride
Write the equation and observed reaction for the reaction between a Aluminium Aqua complex and a Carbonate ion (CO3 2- ) (aq)
Clear and Colourless Solution ——-> White Precipitate + effervescence
Write the equation and observed reaction for the reaction between a Iron (3+) Aqua complex and a Carbonate ion (CO3 2- ) (aq)
Purple Solution ——-> Brown precipitate + effervescence
Why are Metal-Aqua Ions Acidic in solution
Complex ions react with water (hydrolysis)
Aqua complex ions Dissociate Weakly
Thus Produces H+ ions
Within Solution H+ ions produce the hydronium ion making the solution more acidic
Why are 3+ Metal-Aqua ions are more acidic then 2+ Metal aqua ions
3+ Metal ions have a larger charge density (larger charge and smaller)
As a result the 3+ ions are more polarising
They attract the electrons in the O-H in the bond more strongly towards the metal ion, which weakens the bond
This means the H+ ion is more readily released which goes on to from more hydroxonium ions
What does Amphoteric Mean?
A substance that can act as a Bronstead-Lowry Acid and Base
Name an example for an amphoteric metal hydroxide
Hydrated Aluminium Hydroxide
Why does Ammonia form Metal hydroxides
When ammonia is in solution, an equilibrium is met as it is a weak base
NH3 dissociates poorly into NH4+ and H-
Metal Aqua complexes react with the H- ions formed to form a hydroxide
What can happen when Excess NH3 is added to a TM ion
Some Metal Hydroxides that from
react with the ammonia via a partial ligand substitution or full , to form a soluble complex
What colour are the following metal aqua ions
Cu2+
Co2+
Cu2+ = Blue
Co2+ = Pink
What colour are the following metal hexaqua ions
Fe2+
Fe3+
Al3+
Fe2+ = Green
Fe3+ = Purple
Al3+ = Clear and Colourless
Write the equation and observed reaction for the reaction between a Iron 3+ Aqua complex and Hydrochloric Acid (HCl) (aq)
Purple Solution —-> Pale Brown Precipitate
D
Gallium is a 3+ ion
when a 3+ ion reacts with a Carbonate a Hydroxide is produced with water and carbon dioxide
Give an ionic equation for the conversation of [CuCl4]2- when exposed to excess aqueous ammonia
What is The colour change observed
Yellow—-> Deep Blue Solution
Why would a solution containing [Al(H20)6] have a ph < 7
Al3+ central metal ion has a high charge density and small size
This weakens the bond and increases the polarisation of the O-H bonds
Releasing H+ ions
State an observation when Sodium Carbonate is added to a solution of [Al(H20)6]
Bubbles of effervescence
Clear and colourless to white precipitate
Write and equation to show how an aluminium aqua complex can act as a Brønsted-lowry Acid with water
What is/are the reagent for reducing a Fe3+ aqua ion to a Fe2+ ion
Zinc with HCl
