Chem 5 Revision Flash Cards.
Quiz yourself by thinking what should be in
each of the black spaces below before clicking
on it to display the answer.
Help!
|
|
||||
|---|---|---|---|---|---|
| What colour is [Co(H2O)6]2+ (Metal Aqua Ion) | show 🗑
|
||||
| What colour is [Cu(H2O)6]2+ (Metal Aqua Ion) | show 🗑
|
||||
| What colour is [Fe(H2O)6]2+ (Metal Aqua Ion) | show 🗑
|
||||
| show | Colourless Solution
🗑
|
||||
| What colour is [Cr(H2O)6]3+ (Metal Aqua Ion) | show 🗑
|
||||
| show | Yellow Solution
🗑
|
||||
| What compound is formed when [Co(H2O)6]2+ is reacted with OH- or NH3 | show 🗑
|
||||
| show | [Cu(H2O)4(OH)2] PRECIPITATE
🗑
|
||||
| What compound is formed when [Fe(H2O)6]2+ is reacted with OH- or NH3 | show 🗑
|
||||
| What compound is formed when [Al(H2O)6]3+ is reacted with OH- or NH3 | show 🗑
|
||||
| show | [Cr(H2O)3(OH)3] PRECIPITATE
🗑
|
||||
| show | [Fe(H2O)3(OH)3] PRECIPITATE
🗑
|
||||
| show | Its a Blue-Green Precipitate
🗑
|
||||
| What colour is [Cu(H2O)4(OH)2] | show 🗑
|
||||
| show | Its a Green Precipitate
🗑
|
||||
| What colour is [Al(H2O)3(OH)3] | show 🗑
|
||||
| What colour is [Cr(H2O)3(OH)3] | show 🗑
|
||||
| show | Its a Brown Precipitate
🗑
|
||||
| What happens when [Co(H2O)6]2+ is reacted with excess OH- | show 🗑
|
||||
| show | NOTHING!, It says the same Blue Solution.
🗑
|
||||
| What happens when [Fe(H2O)6]2+ is reacted with excess OH- | show 🗑
|
||||
| What happens when [Al(H2O)6]3+ is reacted with excess OH- | show 🗑
|
||||
| show | [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- | show 🗑
|
||||
| show | [Co(NH3)6]2+ a straw coloured solution is formed.
🗑
|
||||
| What happens when [Cu(H2O)6]2+ is reacted with excess NH3 | show 🗑
|
||||
| What happens when [Fe(H2O)6]2+ is reacted with excess NH3 | show 🗑
|
||||
| show | No Change, The solution remains colourless
🗑
|
||||
| What happens when [Cr(H2O)6]3+ is reacted with excess NH3 | show 🗑
|
||||
| What happens when [Fe(H2O)6]3+ is reacted with excess NH3 | show 🗑
|
||||
| What compound is formed when [Co(H2O)6]2+ is reacted with Na2CO3 (Sodium Carbonate) | show 🗑
|
||||
| What compound is formed when [Cu(H2O)6]2+ is reacted with Na2CO3 (Sodium Carbonate) | show 🗑
|
||||
| show | FeCO3, A Green Precipitate
🗑
|
||||
| show | Al(H2O)3(OH)3, A White Precipitate
🗑
|
||||
| What compound is formed when [Cr(H2O)6]3+ is reacted with Na2CO3 (Sodium Carbonate) | show 🗑
|
||||
| show | Fe(H2O)3(OH)3, A Brown Precipitate
🗑
|
||||
| show | They become HYDRATED. Water molecules form coordinate bonds with the metal ions, Forming a METAL-AQUA COMPLEX ION. Generally 6 water molecules.
🗑
|
||||
| show | An Electron Pair acceptor
🗑
|
||||
| What is a Lewis Base? | show 🗑
|
||||
| show | A Lewis Acid-Base reaction!
🗑
|
||||
| What do metal ions act as in an aqueous solution | show 🗑
|
||||
| Why is a solution containing metal-aqua ions acidic? | show 🗑
|
||||
| Why do 3+ metal-aqua ions for more acidic solution than 2+ metal-aqua ions? | show 🗑
|
||||
| What metals-aqua ions can be hydrolysed into insoluble metal hydroxides | show 🗑
|
||||
| How are insoluble metal hydroxides made? | show 🗑
|
||||
| show | 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 | show 🗑
|
||||
| show | 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. | show 🗑
|
||||
| show | 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? | show 🗑
|
||||
| What happens to the coordination number and shape of the complex if ligands are exchanged to ones with a similar size? | show 🗑
|
||||
| What happens if the ligands substituted are different sizes. I.e. H20 to Cl- | show 🗑
|
||||
| What is the result of the following reaction.[Cu(H2O)6]2+ + 4Cl- <---> ?? + ?? | show 🗑
|
||||
| show | Tetrahedral, Yellow
🗑
|
||||
| What is the result of the following reaction.[Co(H2O)6]2+ + 4Cl- <---> ?? + ?? | show 🗑
|
||||
| show | 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? | show 🗑
|
||||
| show | [Cu(H2O)6]2+ + 4NH3 > [Cu(NH3)4(H2O)2]2+ +4H20 [Fe(H2O)6]3+ + SCN- -> [Fe(H2O)5(SCN)]2+ +H20
🗑
|
||||
| show | 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 | show 🗑
|
||||
| show | 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 | show 🗑
|
||||
| show | The enthalpy change when 1 mole of gaseous atoms is formed from an element in its standard state.
🗑
|
||||
| show | The enthalpy change when 1 mole of gaseous 1+ ions are formed from 1 mole of gaseous atoms.
🗑
|
||||
| show | The enthalpy change when 1 mole of gaseous 1- ions is made from 1 mole of gaseous atoms
🗑
|
||||
| Define: Enthalpy of Hydration | show 🗑
|
||||
| show | 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 | show 🗑
|
||||
| Define: Second ionisation enthalpy | show 🗑
|
||||
| Define: Second election affinity | show 🗑
|
||||
| show | 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? | show 🗑
|
||||
| show | 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.
🗑
|
||||
| show | 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? | show 🗑
|
||||
| show | They are usually oxidised to their highest oxidation sate. The exception is sulphur.
🗑
|
||||
| show | 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 | show 🗑
|
||||
| Equation for magnesium reacting with oxygen, speed of reaction and flame colour if appropriate | show 🗑
|
||||
| Equation for aluminum reacting with oxygen, speed of reaction and flame colour if appropriate | show 🗑
|
||||
| show | Si + O2 --> SiO2
Slow
No Flame
🗑
|
||||
| Equation for phosphorus(v) reacting with oxygen, speed of reaction and flame colour if appropriate | show 🗑
|
||||
| Equation for sulphur reacting with oxygen, speed of reaction and flame colour if appropriate | show 🗑
|
||||
| What type of bonding do Sodium, Magnesium and Aluminum oxides have? | show 🗑
|
||||
| show | Giant Covalent
Middle-ish melting point.
🗑
|
||||
| What type of bonding does P4O10 and SO2 have? | show 🗑
|
||||
| Are ionic oxides acidic or alkaline? Why? | show 🗑
|
||||
| Are Covalent oxides acidic or alkaline? Why> | show 🗑
|
||||
| show | 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.
🗑
|
||||
| show | 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 | show 🗑
|
||||
| What type of reactions do rechargeable and non rechargeable cells have? | show 🗑
|
||||
| show | Cheaper than rechargeable in short term
Works for longer initially
Less toxic metals are contained.
🗑
|
||||
| show | Cost more in the long term
Works for shorter time in long term
Have to be disposed off
🗑
|
||||
| Benefits of Hydrogen Fuel Cell | show 🗑
|
||||
| Disadvantages of Hydrogen Fuel Cell | show 🗑
|
||||
| show | A metal that can form one ore more stable ions with a partially filled d-subshell.
🗑
|
Review the information in the table. When you are ready to quiz yourself you can hide individual columns or the entire table. Then you can click on the empty cells to reveal the answer. Try to recall what will be displayed before clicking the empty cell.
To hide a column, click on the column name.
To hide the entire table, click on the "Hide All" button.
You may also shuffle the rows of the table by clicking on the "Shuffle" button.
Or sort by any of the columns using the down arrow next to any column heading.
If you know all the data on any row, you can temporarily remove it by tapping the trash can to the right of the row.
To hide a column, click on the column name.
To hide the entire table, click on the "Hide All" button.
You may also shuffle the rows of the table by clicking on the "Shuffle" button.
Or sort by any of the columns using the down arrow next to any column heading.
If you know all the data on any row, you can temporarily remove it by tapping the trash can to the right of the row.
Embed Code - If you would like this activity on your web page, copy the script below and paste it into your web page.
Normal Size Small Size show me how
Normal Size Small Size show me how
Created by:
deadlybanana