Terms : Hide Images
| 13937003818 | Definition of a transition element? | Elements that have a partially filled d- or f- shell, in their most common compounds and stable ions | 0 | |
| 13937019805 | What is the first row of f- block elements called? | Lanthanoids | 1 | |
| 13937026276 | What is the second row of f- block elements called? | actinoids | 2 | |
| 13937038667 | How are molecular entities represented? | square brackets | 3 | |
| 13937049533 | what is primary valance? | oxidation number | 4 | |
| 13937051655 | What is secondary valence? | coordination number | 5 | |
| 13937067893 | what coordination number is most common in d-block complexes? | 6 | 6 | |
| 13937073076 | What coordination number is most common in f-block complexes? | 9 | 7 | |
| 13937080042 | What are the ions/molecules surrounding a metal ion in a complex called? | ligands | 8 | |
| 13937082865 | What are ligands? | They are electron pair donors | 9 | |
| 13937093829 | what bonding do ligands use? | sigma bonding | 10 | |
| 13937098784 | What type of bonding do X ligands do? | Covalent | 11 | |
| 13937101789 | What type of bonding do L ligands do? | ionic | 12 | |
| 13937108793 | How do you know if it is a X or L ligand? | replace the metal with hydrogen and if it is a feasible compound it is an X ligand, and bonds covalently. | 13 | |
| 13937118871 | What is a coordination number? | This is the number of atoms attached to the metal ion | 14 | |
| 13937138067 | what is the usual d- configuration of a square planar? | d8 | 15 | |
| 13937149353 | how do you determine the valence electrons of the metal? | the group number | 16 | |
| 13937158608 | What is the assumption when calculating d- configuration? | that d- and s- orbital electrons are in the d-block | 17 | |
| 13937166869 | what is oxidation number? | the charge remaining on the metal atom when all ligands are removed in closed shell configuration | 18 | |
| 13937184862 | what is the total electron count? | the number of metal valence electrons plus the electrons donated by the ligands. | 19 | |
| 13937195933 | what is the total electron count is an odd number? | The complex will have unpaired electrons i.e paramagnetism | 20 | |
| 13937205261 | What bonding does the crystal field approach represent? | ionic | 21 | |
| 13937210465 | What bonding does the molecular orbital theory represent? | covalent | 22 | |
| 13937216159 | What are the 3 assumptions in crystal field theory? | 1. The metal is the point of positive charge 2. The ligands are the point of negative charge 3. Bonding energy comes from the electrostatic interactions between the anions and cation. | 23 | |
| 13937238478 | How many d-orbitals are there? | 5 | 24 | |
| 13937241496 | Which d-orbital is this? | dx2-y2 |  | 25 |
| 13937403181 | Which d-orbital is this? | dxy |  | 26 |
| 13937408128 | Which d-orbital is this? | dxz |  | 27 |
| 13937413274 | Which d-orbital is this? | dyz |  | 28 |
| 13937413656 | Which d-orbital is this? | dz2 |  | 29 |
| 13937478648 | describe octahedral crystal field splitting? | -dx2-y2 and dz2, are effected more strongly, due to their presence directly on the axis, so their energy increases. -dxy, dxz, and dzy orbitals point between the axis so their energy decreases. |  | 30 |
| 13937525471 | Describe tetrahedral crystal field splitting? | -dxy, dxz and dyz orbitals increase in energy -dx2-y2 and dz2 decrease in energy |  | 31 |
| 13937569314 | How do you convert between ∆Tet and ∆Oct? | ∆Tet= 4/9 ∆Oct | 32 | |
| 13937597156 | Define high spin | if ∆Oct is smaller than the pairing energy it is better to put the electrons in the higher energy orbitals | 33 | |
| 13937604042 | Define low spin | if ∆Oct is greater than pairing energy it is better to pair the electrons in lower energy orbitals | 34 | |
| 13937616426 | When is pairing energy added? | Pairing energy is only added if the electrons were not previously paired before splitting. If they were already paired, no pairing energy is required. | 35 | |
| 13937631152 | What is a tetrahedral complex more likely to be? | high spin | 36 | |
| 13945283287 | Why are most tetrahedral complexes high spin? | ∆tet is smaller than ∆oct making pairing energy much greater so electrons are put in higher energy orbitals | 37 | |
| 13945283658 | Describe the square planar crystal field splitting. | If the orbital is associated with z, then it drops in energy. Dxz and dzy do not drop as much as dz2. This is due to the fact they are associated with less z. |  | 38 |
| 13945455436 | What is the most common geometry for d-block? | Octahedron | 39 | |
| 13945455437 | Why do some complexes have color? | The light needs the same energy as ∆oct to make the electron jump to a higher energy orbital. The light therefore has the right frequency for the electron to jump to a higher energy orbital. | 40 | |
| 13945455438 | What are selection rules? | They govern whether a transition between 2 energy levels can occur. | 41 | |
| 13945455439 | When does Laportes selection rule apply? | When the molecule has a Centre of symmetry. Octahedral obey these rules but tetrahedral don't. | 42 | |
| 13945455440 | What does laportes rule state? | In molecules with a Centre of symmetry, gerade to ungerade orbital tansitions can occur (d-p), ungerade to gerade orbital transitions are also allowed (p-d). However gerade to gerade transitions are forbidden. (d-d) | 43 | |
| 13945455441 | How do octahedron complexes have colour? | At one point in solution the octahedron may not be completely symmetrical, therefore the selection rules will not be obeyed perfectly. Therefore d-d transitions will occur and a colour will be able be presented, however the colour will be relatively weak. | 44 | |
| 13945455442 | What is the spin selection rule? | Spin cannot change during orbital transitions. | 45 | |
| 13945455443 | When does the spin selection rule apply? | To all complexes | 46 | |
| 13945455532 | What is the colour of permanganate down to? | It has a d0 configuration so it is not due to d-d transitions. It is due to the transfer of electrons from the ligand to the metal. This is called the charge transfer spectra |  | 47 |
| 13945455444 | What is the balance that measures magnetism? | Guoy balance | 48 | |
| 13945455445 | What is diamagnetic? | all electrons are paired | 49 | |
| 13945455446 | What is paramagnetic? | at least one unpaired electron | 50 | |
| 13945455447 | Which magnetic effects are stronger? | Paramagnetic effects are stronger and overpower diamagnetic effects. | 51 | |
| 13945455448 | What happens when diamagnetic complexes are weighed on a guoy balance? | They repel the magnetic field so they decrease in weight | 52 | |
| 13945455449 | What happens when paramagnetic complexes are weighed on a guoy balance? | They attract the magnetic field so their weight increases. | 53 | |
| 13945455450 | What is the spin only equation? | √n(n+2) | 54 | |
| 13945455451 | What are the units of magnetic moment? | Bohr magnetons | 55 | |
| 13945455452 | What does increased charge/oxidation number cause? | Increased splitting | 56 | |
| 13945455453 | What is the spectrochemical series? | It describes the effect of the ligands on the splitting of the complex | 57 | |
| 13945455454 | What is an isomer? | It is 2 or more complexes of the same empirical formula, which have different structures | 58 | |
| 13945455455 | What is constitutional isomerism? | Have the same empirical formula but different connectivities | 59 | |
| 13945455456 | What is linkage isomerism? | When different atoms of the same ligand can bond to the metal | 60 | |
| 13945455457 | What is coordination isomerism? | This is when 2 complexes in the same compound swap ligands. The ligands coordinated to them therefore changes | 61 | |
| 13945455458 | What is ionization isomerism? | This is when the ligand group can either be in the complex or bound to the complex. | 62 | |
| 13945455459 | What is solvated isomerism? | This is how many water molecules are associated with the complex. | 63 | |
| 13945455460 | What is ligand isomerism? | This is when the ligand isomerism causes a change in the geometry of the complex. | 64 | |
| 13945455461 | What is polymerisation isomerism? | This is when the complex joins to itself to form chains of polymers. | 65 | |
| 13945455462 | What is steroisomerism? | They have the same atom-atom connections but different spatial arrangement. | 66 | |
| 13945455463 | What is geometric isomerism? | This is dependent on what sides of the compounds the different ligands are on. | 67 | |
| 13945455464 | What isomers have the same ligands on the same side? | Cis and fac | 68 | |
| 13945455465 | What isomers have ligands on different sides? | Trans and mer | 69 | |
| 13945455466 | What is polytonal isomerism? | This is when the same complex has different geometries within the same crystal. | 70 | |
| 13945455467 | What are optical isomers? | These are compounds which have a non-super impossible image of itself. It therefore has a chiral Centre. The 2 isomers are known as enantiomers. | 71 | |
| 13945455468 | What are chelate ligands? | These are polydentate ligands, they have more than 1 set of electrons to donate | 72 | |
| 13945455469 | What are the most stable ligands? | Chelate ligands | 73 |
