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What colour is [Co(H2O)6]2+
(Metal Aqua Ion)
(Metal Aqua Ion)
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What colour is [Cu(H2O)6]2+
(Metal Aqua Ion)
(Metal Aqua Ion)
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Chem 5
Chem 5 Revision Flash Cards.
| Question | Answer |
|---|---|
| What colour is [Co(H2O)6]2+ (Metal Aqua Ion) | Pink Solution |
| What colour is [Cu(H2O)6]2+ (Metal Aqua Ion) | Blue Solution |
| What colour is [Fe(H2O)6]2+ (Metal Aqua Ion) | Green Solution |
| What colour is [Al(H2O)6]3+ (Metal Aqua Ion) | Colourless Solution |
| What colour is [Cr(H2O)6]3+ (Metal Aqua Ion) | Violet Solution |
| What colour is [Fe(H2O)6]3+ (Metal Aqua Ion) | Yellow Solution |
| What compound is formed when [Co(H2O)6]2+ is reacted with OH- or NH3 | [Co(H2O)4(OH)2] PRECIPITATE |
| What compound is formed when [Cu(H2O)6]2+ is reacted with OH- or NH3 | [Cu(H2O)4(OH)2] PRECIPITATE |
| What compound is formed when [Fe(H2O)6]2+ is reacted with OH- or NH3 | [Fe(H2O)4(OH)2] PRECIPITATE |
| What compound is formed when [Al(H2O)6]3+ is reacted with OH- or NH3 | [Al(H2O)3(OH)3] PRECIPITATE |
| What compound is formed when [Cr(H2O)6]3+ is reacted with OH- or NH3 | [Cr(H2O)3(OH)3] PRECIPITATE |
| What compound is formed when [Fe(H20)6]3+ is reacted with OH- or NH3 | [Fe(H2O)3(OH)3] PRECIPITATE |
| What colour is [Co(H2O)4(OH)2] | Its a Blue-Green Precipitate |
| What colour is [Cu(H2O)4(OH)2] | Its a Blue Precipitate |
| What colour is [Fe(H2O)4(OH)2] | Its a Green Precipitate |
| What colour is [Al(H2O)3(OH)3] | Its a White Precipitate |
| What colour is [Cr(H2O)3(OH)3] | Its a Green Precipitate |
| What colour is [Fe(H2O)3(OH)3] | Its a Brown Precipitate |
| What happens when [Co(H2O)6]2+ is reacted with excess OH- | NOTHING!, It says the same Pink Solution. |
| What happens when [Cu(H2O)6]2+ is reacted with excess OH- | NOTHING!, It says the same Blue Solution. |
| What happens when [Fe(H2O)6]2+ is reacted with excess OH- | NOTHING!, It says the same Green Solution. |
| What happens when [Al(H2O)6]3+ is reacted with excess OH- | [Al(H2O)2(OH)4]- colourless solution forms, If excess is added to precipitate formed with [Al(H2O)3(OH)3] it will dissolve |
| What happens when [Cr(H2O)6]3+ is reacted with excess OH- | [Cr(OH)6]3- Green solution is formed, If excess is added to precipitate formed with [Cr(H2O)3(OH)3] then it dissolves |
| What happens when [Cr(H2O)6]3+ is reacted with excess OH- | NOTHING!, It says the same Yellow Solution. |
| What happens when [Co(H2O)6]2+ is reacted with excess NH3 | [Co(NH3)6]2+ a straw coloured solution is formed. |
| What happens when [Cu(H2O)6]2+ is reacted with excess NH3 | [Cu(NH3)4(H2O)2]2+ a deep blue solution is formed. |
| What happens when [Fe(H2O)6]2+ is reacted with excess NH3 | No Change, The solution remains green |
| What happens when [Al(H2O)6]3+ is reacted with excess NH3 | No Change, The solution remains colourless |
| What happens when [Cr(H2O)6]3+ is reacted with excess NH3 | [Cr(NH3)6]3+ is formed. It makes a purple solution |
| What happens when [Fe(H2O)6]3+ is reacted with excess NH3 | No change, The solution remains yellow. |
| What compound is formed when [Co(H2O)6]2+ is reacted with Na2CO3 (Sodium Carbonate) | CoCO3, A Pink precipitate |
| What compound is formed when [Cu(H2O)6]2+ is reacted with Na2CO3 (Sodium Carbonate) | CuCO3, A Green-Blue Precipitate |
| What compound is formed when [Fe(H2O)6]2+ is reacted with Na2CO3 (Sodium Carbonate) | FeCO3, A Green Precipitate |
| What compound is formed when [Al(H2O)6]3+ is reacted with Na2CO3 (Sodium Carbonate) | Al(H2O)3(OH)3, A White Precipitate |
| What compound is formed when [Cr(H2O)6]3+ is reacted with Na2CO3 (Sodium Carbonate) | Cr(H2O)3(OH)3, A Green Precipitate |
| What compound is formed when [Fe(H2O)6]3+ is reacted with Na2CO3 (Sodium Carbonate) | Fe(H2O)3(OH)3, A Brown Precipitate |
| What happens to transitional metal compounds in water? | They become HYDRATED. Water molecules form coordinate bonds with the metal ions, Forming a METAL-AQUA COMPLEX ION. Generally 6 water molecules. |
| What is a Lewis Acid? | An Electron Pair acceptor |
| What is a Lewis Base? | An Electron Pair Donor. |
| If there is a coordinate bond what type of reaction must there have been? | A Lewis Acid-Base reaction! |
| What do metal ions act as in an aqueous solution | Lewis Acids, As they accept electron pairs. All ligands act as lewis bases. |
| Why is a solution containing metal-aqua ions acidic? | [Fe(H2O)6]2+ + H2O <--> [Fe(H2O)5(OH)]+ H3O+ The metal 2+ ions release H+ making the solution acidic but only slight dissociation so WEAKLY ACIDIC |
| Why do 3+ metal-aqua ions for more acidic solution than 2+ metal-aqua ions? | Metal 3+ ions are small and have a big charge, this means they have a high charge density than Metal 2+ ions. This means they polarise the OH bond more weakening so it is more likely more H+ will be released. |
| What metals-aqua ions can be hydrolysed into insoluble metal hydroxides | 3+ metal-aqua ions. Namely Aluminum(III), Chromium(III) and Iron(III). 2+ metal-aqua ions can also but it only requires two additions of OH- |
| How are insoluble metal hydroxides made? | Equilibrium produces [M(H2O)5(OH)]2+ Addition of OH- Shifts equilibrium to right. Result is [M(H2O)4(OH)2]+ Addition of more OH- shifts equilibrium to right again. Result is [M(H2O)3(OH)3] uncharged and insoluble. |
| Can 2+ metal-aqua ions be hydrolysed further in to insoluble metal hydroxides. | Yes, There are only two steps though. [M(H2O)6]2+ + H2O <-> [M(H2O)5(OH)]+ + H30+ [M(H2O)5(OH)]+ + H2O <-> M(H2O)4(OH)2 + H30+ Result is insoluble metal hydroxide |
| What well all metal hydroxides act as when dissolved in acid | Bronsted-Lowery bases. They accept H+ ions reversing the hydrolysis. |
| What does amphoteric mean? | It describes a substances that can act as both a base and and acid. The substance can dissolve in both an excess of acid and base. |
| What else can be used to form metal hydroxides. | Ammonia can be added to solution. The resulting equilibrium formed is NH3 + H2O <--> OH- + NH4+ The result is the same as adding a small amount of OH-, Adding too much ammonia can cause ligand displacement. |
| How do Metal ions react with Sodium Carbonate? | Yes, Metal 2 ions will form insoluble metal carbonates. [M(H2O)6]2+ + [CO3]2- <--> MCO3 + 6H20 |
| Why don't Metal 3+ ions react with sodium carbonate? | They are stronger acids so they always from hydroxide precipitates when you add Sodium Carbonate. The carbonate ions react with H3O+ removing them from solution just like OH- ions. |
| What happens to the coordination number and shape of the complex if ligands are exchanged to ones with a similar size? | The coordination number stays the same and so does the shape. |
| What happens if the ligands substituted are different sizes. I.e. H20 to Cl- | There is a change in coordination number and a change in the shape of the ion. |
| What is the result of the following reaction.[Cu(H2O)6]2+ + 4Cl- <---> ?? + ?? | [CuCl4]2- + 6H2O |
| Describe the shape and colour of [CuCl4]2- | Tetrahedral, Yellow |
| What is the result of the following reaction.[Co(H2O)6]2+ + 4Cl- <---> ?? + ?? | [CoCl4]2- + 6H2O |
| Describe the shape and colour of [CoCl4]2- | Tetrahedral, Blue |
| [Cu(H2O)6]2+ + 4Cl- <---> [CuCl4]2- + 6H2O [Co(H2O)6]2+ + 4Cl- <---> [CoCl4]2- + 6H2O How can the equilibrium be shifted to the right hand side? | The forward reaction is ENDOTHERMIC, the reaction is shifted to the right by heating. It is can shifted to the left by adding water. |
| Give two examples of partial substitution | [Cu(H2O)6]2+ + 4NH3 > [Cu(NH3)4(H2O)2]2+ +4H20 [Fe(H2O)6]3+ + SCN- -> [Fe(H2O)5(SCN)]2+ +H20 |
| What are the 3 types of ligand. | Unidentate - One Pair of lone elections Bidentate - Two pairs of lone election Multidentate - More than one lone pair |
| When is a ligand substitution reaction harder to reverse | If the new ligands form a stronger bond with the central metal ion. If the multidentate ligand is substituted as it forms more than one coordinate bond. |
| What is the Chelate effect | When a unidentate ligand is replaced with a multidentate ligand there is an increase in the number of particles. More particles means a greater ENTROPY. Reactions that result in an INCREASED ENTROPY are more likely to occur. |
| Define: Enthalpy of formation | The enthalpy change when 1 mole of compound is formed from its elements in their standard states. |
| Define: Enthalpy of Atomistation | The enthalpy change when 1 mole of gaseous atoms is formed from an element in its standard state. |
| Define: First ionisation energy | The enthalpy change when 1 mole of gaseous 1+ ions are formed from 1 mole of gaseous atoms. |
| Define: First election affinity | The enthalpy change when 1 mole of gaseous 1- ions is made from 1 mole of gaseous atoms |
| Define: Enthalpy of Hydration | The enthalpy change when 1 mole of aqueous ions is formed from gaseous ions |
| Define: Bond dissociation enthalpy | The enthalpy change when all the bonds of the same type in 1 mole of gaseous molecules are broken |
| Define: Enthalpy change of atomisation of a compound | The enthalpy change when 1 mole of gaseous atoms is formed from a compound in its standard states |
| Define: Second ionisation enthalpy | The enthalpy change when 1 mole of gaseous 2+ ions is formed from 1 mole of gaseous 1+ ions. |
| Define: Second election affinity | The enthalpy change when 1 mole of gaseous 2- ions is formed from 1 mole of gaseous 1- ions |
| Define: Enthalpy change of solution | The enthalpy change when 1 mole of solute is dissolved in sufficient solvent that no further enthalpy change occurs on further dilution. |
| Why is Sodium more reactive than magnesium? | Sodium (Group 1) lose one election, Magnesium (Group 2). Sodium is more reactive as it takes less energy to lose one election compared to so. Mg requires more energy (usually heat). |
| How does sodium react with water? | 2Na + 2H2O -> 2NaOH + H2 VIGOROUS REACTION Reactions with cold water forming a molten ball on the surface. Production of NaOH makes the solution strongly alkaline. |
| How does magnesium react with water? | Magnesium reacts VERY SLOWLY with cold water. Nothing to see but forms a weakly alkaline solution. Magnesium Oxide is not very soluble in water so relatively few OH- ions. Mg + 2H2O --> Mg(OH)2 +H2 |
| How does magnesium react with steam? | Magnesium reacts much faster with steam, to from magnesium oxide. |
| What can be said about the oxidation of period 3 elements with oxygen. | They are usually oxidised to their highest oxidation sate. The exception is sulphur. |
| What is the exception to the oxidation states of period 3 elements. | Sulphur froms SO2 which is only a +4 oxidation state. A high temperature and catalyst is needed to make SO3. |
| Equation for sodium reacting with oxygen, speed of reaction and flame colour if appropriate | 2Na + 1/2O2 --> Na2O Vigorous Reaction Yellow Flame |
| Equation for magnesium reacting with oxygen, speed of reaction and flame colour if appropriate | Mg + 1/2O2 --> Mg2O Vigorous Reaction Brilliant White Flame |
| Equation for aluminum reacting with oxygen, speed of reaction and flame colour if appropriate | 2Al + 3/2O2 --> Al2O3 Slow No Flame |
| Equation for silicon reacting with oxygen, speed of reaction and flame colour if appropriate | Si + O2 --> SiO2 Slow No Flame |
| Equation for phosphorus(v) reacting with oxygen, speed of reaction and flame colour if appropriate | P4 + 5O2 --> P4O10 Spontaneously Combusts Brilliant White Flame |
| Equation for sulphur reacting with oxygen, speed of reaction and flame colour if appropriate | S + O2 --> SO2 Burns Steadily Blue Flame |
| What type of bonding do Sodium, Magnesium and Aluminum oxides have? | Ionic High Melting Points. |
| What type of bonding does SiO2 have? | Giant Covalent Middle-ish melting point. |
| What type of bonding does P4O10 and SO2 have? | Simple Covalent Low Melting Point (Only Van der Waals). |
| Are ionic oxides acidic or alkaline? Why? | They are alkaline. When they dissolve in water they form hydroxide ions. Both result in alkaline solutions but sodium hydroxide is more soluble so forms a more alkaline solution than magnesium. |
| Are Covalent oxides acidic or alkaline? Why> | They are acidic. They react with water forming acids. I.e. S03 + H20 --> H2SO4 |
| Silicon dioxide doesn't dissolve in water, why and why then is it still classed as an acid? | The giant covalent structure of silicon dioxide meas that it is insoluble in water. It is still classed as an acid because it reacts with bases to form a salt. |
| How does Aluminum oxide react when it is introduced to water? | It is partially ionic and partially covalently bonded. (Remember Polarization). It is insoluble in water but will react with BOTH acids AND bases to form salts. It is classed as AMPHOTERIC. |
| Equations for amphoteric oxides neutralising acids and bases | Al2O3 + 3H2SO4 --> Al2(SO4)3 + 3H2O Al2O3 + 2NaOH + 3H2O --> 2NaAl(OH)4 |
| What type of reactions do rechargeable and non rechargeable cells have? | Rechargeable Cells: Have reversible Reactions Non Rechargeable cells: Have irreversible reactions. |
| Advantages of Non-rechargeable batteries | Cheaper than rechargeable in short term Works for longer initially Less toxic metals are contained. |
| Disadvantages of Rechargeable batteries | Cost more in the long term Works for shorter time in long term Have to be disposed off |
| Benefits of Hydrogen Fuel Cell | Don't need electrical recharging No toxic chemicals or CO2 produced Only waste product is water |
| Disadvantages of Hydrogen Fuel Cell | Energy is required to produce a supply of hydrogen and oxygen. This generally comes from fossil fuels. Hydrogen is also highly flammable so has to be carefully stored and transported |
| Define: Transition Metal | A metal that can form one ore more stable ions with a partially filled d-subshell. |
Created by:
deadlybanana