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AQA A2 Transition
Transition metals
| Question | Answer |
|---|---|
| What is the shape of [Cu(H2O)6]+2? | Octahedral |
| Name and give the formula of an Octahedral shaped complex | [Cu(H2O)6]+2 hexaaquacopper(II) ions Did you remember the oxidation state in roman numeral? |
| Name a tetrahedral shaped complex | TetraChloroNickel(II) ions; [Ni(Cl)4]-2 Did you remember the oxidation state in roman numeral? Have you worked out correctly the overall charge of the complex? |
| Name a square planar complex | TetraCyanoNickel(II) ions; [Ni(CN)4]-2 Did you remember the oxidation state in roman numeral? Have you worked out correctly the overall charge of the complex? |
| Name a bidentate ligand | ethanedioate ion or 1,2diaminoethane. But can do draw their structure? |
| Name an hexadentate ligand | EDTA |
| Name neutral ligands | H2O,NH3 |
| Define a ligand | a chemical able to donate a lone pair of electron to form a dative covalent bond with a central metal ion |
| What is the shape of a complexe with H2O ligands? | octahedral |
| What is the shape of a complexe with CN- ligands? | square planar |
| What is the shape of a complexe with Cl- ligands? | always tetrahedral (because the chloride ions are so big and repel each other) |
| What is the coordination number of [Cu(H2O)6]+2 ? | 6 |
| What is the coordination number of [CuCl4]-2 ? | 4 |
| What is the coordination number of [Ag(NH3)2]+1 ? | 2 |
| What is the coordination number of [Cr(C2O4)2(H2O)2]-2 ? | 6; did you recognise C2O4 as the ethanedioate ion, a bidentate ligand? |
| What is the coordination number of [Ni(en)3]+2 ? | 6; did you recognise en as NH2CH2CH2NH2 ethanediamine, a bidentate ligand? |
| What type of ligands must you have to have optical isomerism on an octahedral complex? | 3 bidentate ligands OR 2bidentate and 2 monodentate OR one hexadentate |
| How do you draw optical isomers? | draw the octahedral shape first; place the bidentate ligands around the metal; then draw the mirror image |
| What type of ligands must you have to have cis/trans isomerism on an octahedral complex? | 2 Define a cis-isomerism using [CoCl2(NH3)4]+ as an example |
| Define a cis-isomerism using [CoCl2(NH3)4]+ as an example | when two Cl- ligands are at 180 of each other |
| Name and give the formula of the yellow precipitate formed when Sodium Hydroxide is added to a metal ion solution | Iron(III)Hydroxide (have you remembered the charge/oxidation number on the Iron?) Fe(OH)3 |
| Name and give the formula of the blue precipitate formed when Sodium Hydroxide is added to a metal ion solution | Copper(II)Hydroxide (have you remembered the charge/oxidation number on the Iron?) Cu(OH)2 |
| Name and give the formula of the pale green precipitate formed when Sodium Hydroxide is added to a metal ion solution | Iron(II)Hydroxide (have you remembered the charge/oxidation number on the Iron?) Fe(OH)2 |
| Name and give the formula of the deep blue solution formed when concentrated is added to a metal ion solution | TetraAmineCopper(II) [Cu(NH3)4]+2 ; you can also write [Cu(NH3)4(H2O)2]+2 |
| How do you write the electronic configuration of an ion? | you writethe electronic configuration of the atom, as 3dx 4s2; then you remove the 4s first! |
| What is the electronic configuration of Fe+2 ions | [Ar] 3d6 Did you take away the 4s2? Have you written the "6" as a superscript? |
| What is the electronic configuration of Cu+2 ions | [Ar] 3d9 Did you take away the 4s2? Have you written the "9" as a superscript? |
| What is the electronic configuration of Cu atoms | [Ar] 3d10 4s1 It is an exception to the usual electron configuration!!! |
| What is the electronic configuration of Cr atoms | [Ar] 3d5 4s2 It is an exception to the usual electron configuration!!! |
| Why do transition metals form at least +2 ions (except copper who has a stable +1 ion)? | Because the sum of the first two ionisation enthalpies is very low. |
| What must you remember when drawing a complex ion? | most likely to be octahedral (3D) shape; the lone pair on the ligand; the charge & brackets on the overall complex; the oxygen of water faces the metal |
| What happens when you add diluted Hydrochloric acid to a solution of Copper(II) ion? | Nothing! |
| What happens when you add CONCENTRATED Hydrochloric acid to a solution of Copper(II) ion? | There is a ligand exchange (H2O--> Cl-) |
| What is the name of TiCl6-? HexaChloroTitanium(II) | Did you remember the oxidation state in roman numeral? |
| What is the formula of PentaAquaMonoHydroxoChromium(III) ions? | [Cr(H2O)5(OH)]+2 Did you work out the overall charge correctly? |
| What are the colour of Vanadium ions from oxidation states +2 to +5 | Yellow Blue Green Violet |
| Name and give the formula of a blue precipitate when dilute Sodium Hydroxide is added to a metal | Copper(II)Hydroxide; Cu(OH)2 it could also be Cobalt(II)Hydroxide Co(OH)2 |
| Name and give the formula of a blue precipitate (that turns beige when left standing)when dilute Sodium Hydroxide is added to a metal | Cobalt(II)Hydroxide Co(OH)2 |
| Name and give the formula of a green precipitate when dilute Sodium Hydroxide is added to a metal | Iron(II)Hydroxide; Fe(OH)2 |
| Name and give the formula of a yellow precipitate when dilute Sodium Hydroxide is added to a metal | Iron(III) Hydroxide; Fe(OH)3 |
| Name and give the formula of a green precipitate when dilute Ammonia is added to a metal | the green precipitate is key: Iron(II)Hydroxide; Fe(OH)2 Ammonia acted as a weak base and removed protons from the water ligands |
| Name and give the formula of a blue precipitate when dilute Ammonia is added to a metal Copper(II)Hydroxide; Cu(OH)2 | Ammonia acted as a weak base and removed protons from the water ligands |
| Name and give the formula of the species formed when concentrated Ammonia is added to Copper(II)ions | TetraAminoCopper(II) ions; [Cu(NH3)4(H2O)2}+2 |
| Why does a green precipitate turn brown by the next day? | The Iron (II) Fe(OH)2 precipitate is OXIDISED by OXYGEN in the air into Iron(III)/Fe(OH)3 |
| What is the state and colour of Copper(II)Hydroxide; Cu(OH)2 | blue precipitate |
| What is the state and colour of Iron(II)Hydroxide; Fe(OH)2 | green precipitate that turns brown when left standing |
| What is the state and colour of Iron(III) Hydroxide; Fe(OH)3 | brown precipitate |
| Name and give the formula of a green precipitate when dilute Ammonia is added to a metal | the green precipitate is key: Iron(II)Hydroxide; Fe(OH)2 Ammonia acted as a weak base and removed protons from the water ligands |
| Name and give the formula of a blue precipitate when dilute Ammonia is added to a metal Copper(II)Hydroxide; Cu(OH)2 | Ammonia acted as a weak base and removed protons from the water ligands |
| Describe how cisplatin works | by binding to the DNA of fast growing cancer cells |
| What type of isomerism is shown in [Pt(NH3)2(Cl)2], a square planar complexe? | cis-trans |
| What is the transition metal invoved when a solution goes from blue to green on addition of concentrated HCl? | Cu(II); have you learned the colours yet? |
| Define a catalyst | A chemical that speeds up a reaction without getting used up (ie the catalyst is REFORMED at the end) by providing an ALTERNATE ROUTE of a lower activation energy |
| Why do transition metals make good catalyst? | They have different oxidation states and can form complexes with reactants |
| Define homogeneous catalyst | When the reactants and the CATALYST are in the same state (ie both aqueous) |
| What is the formula of Sulfide ion? | S-2 You did not say (SO4)-2, did you? that is SulfATE ions! |
| What is the Oxidation number of Sulfur in Sulfate ions? | (SO4)-2; sulfur is +6 |
| What is the oxidation number of Chromium in (Cr2O7)-2 ions | +7 |
| What is the name of FeCO3 | Iron(II)Carbonate Did you remember the oxidation state in roman numeral? |
| What is the formula of Iron(III)Nitrate | Fe(NO3)3 It is all about swapping the charges; Nitrate is (NO3)- |
| Which ion is pale green in water | [Fe(H2O)6]+2 |
| Which ion is yellow in solution? | [Fe(H2O)6]+3 |
| Describe a redox titration procedure | MnO4- in burette; PIPETTE Fe+2 in conical flask; open tap; drop by drop near end-point; record volume when colour in conical flask changes to PERSISTENT pink; repeat until concordant (within 01.cm3) |
| A 1.2g iron nail is dissolved in 250cm3; 22.4cm3 of 0.005mole.dm-3 is needed to titrate a 25 cm3. What is the concentration? | moles MnO4-=22.4/1000*0.005 moles; Fe+2=5xmolesMnO4;moles in 250cm3=molesFe+2 x 10;mass Fe=moles in 250cm x RAM;%Fe = mass Fe /1.2g x 100 |
| State 3 properties of transition metals | Coloured, Complexes, Catalysts |
| Define a transition metal | When a metal forms an ION with a partially filled in d-block orbital |
| What metal is used as a catalyst in the Haber process? | Iron |
| What metal is used as a catalyst in the Contact process where SO2 becomes SO3? | Vanadium(V)oxide, V2O5 |
| What metal is used as a catalyst in the hydrogenation of AlkEnes? | Nickel |
| What metal is used as a catalyst in the decomposition of H2O2? | Manganese(IV)Oxide MnO2 |
| What is the colour of ZnSO4 solution? | colourless because Zn+2 ions are NOT transition metals (full d-block) |
| Describe the shape of the complexe of the haemoglobin complexe | 4 Nitrogen atoms in a square around the central Fe+2 ion; the globin protein acts as another ligand and the oxygen forms the last dative covalent bond |
| Why are hexadentate complexes so stable? | when they form from a solution by ligand exchange, 6 molecules of H2O are displaced, creating massive entropy change |
| Why are Chloro Complexes tetrahedral? | The chlorIDE IONS are large and repel each other |
| How do you recognise a trans complex? | Two identical ligands are on opposite side of the central metal ion |
| How do you recognise a cis complex? | Two identical ligands are on opposite side of the central metal ion |
| Name a linear complex | [Ag(NH3)2]+ aka Tollens reagent |
| How do you draw a complex with a bidentate ligand such as (C2O4)-2? | 1) Draw the octahedral 3D shape; 2) Draw the TWO oxygen with lone pair attaching on adjacent bonds; 3) join the two oxygen and draw the skeleton O-C-C-O; 4) add the =O (double bond to another oxygen) on the Carbons |
| Why are transition metals coloured? | When involved in a complex, the d-orbitals of the metal split; 2) one e- can move up energy levels 3) to do so, the e- absorbs some light energy from the visible spectrum; 4) whatever wavelength is NOT absorbed is TRANSMITTED |
| Why is Copper solution blue? | Because the Copper aqau complex absorbs ALL wavelengths of the visible spectrum, except blue; wavelength from the blue part of the em spectrum are transmitted |
| Describe the colourimetry procedure | Make up a 5 solutions so the approximate concentration of the unknown falls within the range of the 5 solutions; select a filter of a colour opposite to the unknown on the colour wheel; plot absorbances vs concentr; record unknown absorbance and use graph |
| what is autocatalysis? Give an example | When one of the product of the reaction is also the catalyst of the reactio; MnO4- with ethanedioic acid |
| Fe+2 catalyses the following reaction: S2O8- + 2I- --> I2 + 2(SO4)-2; write the two equations to show the mechanism | Fe+2 + S2O8- --> 2 SO4-2 + Fe+3 Fe+3 + 2I- --> I2 + Fe+2 You should be given the electrode potential for this type of question |
| Why are solution of Metal(III) ions acidic? | Because the metal ion is small and highly charged so it pulls the electrons from the dative covalent bond to H2O; the O-H bond in turn is weakened and H+ is liberated |
| Why is a precipitate of Fe(OH)3 [orFe(OH)2] formed when you add Ammonia to Fe(III) [or Fe(II)]? | Ammonia acts as a base and will take away a proton (H+) from one, two, three water ligand |
| Why is Fe(OH)3 precipitate formed when you add Na2CO3 to a solution of Fe(III)? (rather than Fe2(CO3)3) | As Fe+3 is small and charge ions, it attract e- from the H2O and the O-H bonds become polarised; (CO3)-2 |
| Why does a solution of Fe(III) fizz when you add Na2CO3 but not a solution of Fe(II)? | (write the equations) 2 [Fe(H2O)6]+3 + 3 CO3-2 --> 2 [Fe(H2O)3(OH)3] + 3 CO2 + 3 H2O [Fe(H2O)6]+2 + CO3-2 --> FeCO3 + 6 H2O |
| What is an amphoteric chemical? Give an example | A chemical that can react with both an acid and a base. For example Aluminium Hydroxide Al(OH)3 |
| Write the equation for the reaction between Aluminium Hydroxide and Hydrochloric acid | [Al(H2O)3(OH)3]+3 + 3 HCl --> [Al(H2O)6]+3 + 3 Cl- |
| Write the equation for the reaction between Aluminium Hydroxide and Sodium Hydroxide | [Al(H2O)3(OH)3]+3 + OH- --> [Al(OH)4]- + 3 H2O |
Created by:
UrsulineChem
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