Aqua Metal Ions Flashcards by Anthony Royster

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

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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

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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

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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

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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)

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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

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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

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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)

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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)

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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

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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

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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

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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

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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

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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

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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