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Description
Flashcards by ashiana121, updated more than 1 year ago
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Created by ashiana121
about 8 years ago
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| Question | Answer |
| What is the main characteristics of the transition metals? | They have an incomplete d sub-shell |
| When forming ions, what orbital do the transition metals lose electrons from first? | 4s |
| Why isnt Zn2+ a transition metal? | Zn can only form a 2+ ion which has a complete d orbital |
| What is a complex? | A central metal ion surrounded by ligands |
| What is a ligand? | An atom, ion or molecule which can donate a lone pair of electrons |
| What type of bonding is involved in complex formation? | Coordinate |
| What is a coordinate bond? | When the shared pair of electrons in the covalent bond both come from only one of the bonding species |
| What is the coordination number? | The number of coordinate bonds formed to a central metal ion |
| If ligands are ________ they form one coordinate bond each to the central metal ion? | Unidentate |
| What do we call the ligands if they can each make two coordinate bonds because they each have two atoms with lone pairs? | Bidentate |
| If a ligand can make multiple coordinate bonds it is _________ | Multidentate |
| NH2CH2CH2NH2 is a ________ ligand | Bidentate |
| Give another example of a bidentate ligand | ethandioate C2O4 2- |
| Give an example of a multidentate ligand | EDTA 4- |
| If there are 3 bidentate ligands attached to a metal ion, what is the coordination number? | 6 |
| What is haem? | An Iron (II) complex with a multidentate ligand |
| A complex with small ligands (H2O, NH3) commonly forms __________ structures | Octrahedral |
| What shape do complexes form with larger complexes such as Cl-? | Tetrahedral |
| Cisplatin has a _____ ______ structure | Square planar |
| Which ion commonly forms colourless, linear complexes? | Ag+ |
| Colour changes can arise from changes in what three things? | - Oxidation state - Coordination number - Ligand |
| Write the equation for which [Co(H2O)6]2+ changes its ligand to Cl and also its coordination number. Describe the colour change. | [Co(H2O)6]2+ + 4 Cl- ---> [CoCl4]2- + 6 H20 Pink to blue |
| Write an equation and describe the colour change for when [Co(H2O)6]2+ reacts with ammonia. Which, out of the three, is the colour change a result of? | [Co(H2O)6]2+ + 6 NH3 -----> [Co(NH3)6]2+ + 6 H20 Pink to straw Due to change in ligand |
| Write the equation for when [Co(NH3)6]2+ (aq) is oxidised. What two things change? | [Co(NH3)6]2+ (aq) ------> [Co(NH3)6]3+ + e- Colour changes from straw to brown Oxidation state changes from +2 to +3 |
| Colour changes arise from _________ _________ from the ground state to excited states between different d orbitals | Electronic transitions |
| A portion of _______ ______ is absorbed to promote d electrons to higher energy levels | Visable light |
| The light that is not absorbed is _________ to give the substance colour | transmitted |
| Ligands cause the 5d orbitals to split into how many energy levels? | Two |
| What is the equation linking the colour and the freq of light absorbed with the energy difference between the split orbitals? | ΔE = hv v is freq of light absorbed h is Plancks constant 6.62607004 × 10-34 ΔE is the energy difference between the split orbitals |
| What colour will a solution appear if it absorbs orange light? | Blue |
| Changing the lignad/coordination number will alter the energy split between the d orbitals, changing ΔE and hence... | The frequency of light absorbed |
| Explain why Sc (Sc3+) has no colour. | Sc3+ hasnt got any d electrons left to move around, therefore there wont be an enery transfer equal to that of visable light |
| Explain why Zn2+ and Cu+ have no colour. | Their d shells are full so there is no space for the electrons to transfer, therefore there is no energy transfer equal to that of visible light |
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