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30 Cards in this Set
- Front
- Back
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Do transition metals have complete orbitals? Name one this and exception and why? |
T metals have incomplete d-sub level in atoms or ions. But Zn isn't a transition metal because it has a complete d orbital. |
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Define trend in effective nuclear charge |
Zeff is the average positive charge experienced by the electron, taking into account shielding of outer electron. |
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Explain what is the trend in effective nuclear charge across a period |
As the atomic no increase the Zeff also increase. Because the no. of protons increase but shielding stays the same because electrons are still in the same orbital. So electrons are pulled closer to the nucleus |
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What are the 2 set of d-orbitals and explain how they are grouped |
Set 1: dz2 and dx2-y2 are grouped because they both lie through (along) the axis. In terms of interactions : strong = along / weak = in-between Set 2 : dxy, dyz and dx2 are grouped because they lie in-between the axis. In terms of interactions : weak = along / strong = in-between. |
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Which out of the 3 orbitals are the best at shielding? |
s>p>d s orbitals are the best at shielding becuase they over the whole space so better shielding. d orbitals are the weakest because so cant' shield valance electrons very well |
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What is the equation for working out Zeff? |
Zeff = Z - S Z = no of protons S = inner shells of electrons |
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What's the Zeff for n=3 in sulphur |
Find the atomic no = 16 so... Z = 16 Draw the dot structure and count the number of electrons in the n=2 shell so... S = 10 |
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What's the trend in melting point for Transition metals ? |
- They have higher mp than s orbital - d orbitals are now involved so stronger IMF - more Valance electrons - stronger metallic bonding and bond - d electrons are more involved in M bonding |
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What does high OS mean... |
tends to be a oxidising agent (strong oxidant) |
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What does low OS mean.... |
tends to be a reducing agent |
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Define oxidation and reduction.. |
- Oxidation is the ability to lose electrons (high OS) - Reduction is the ability to gain electrons (low OS) |
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If a atom is reduced... |
higher no. of electrons (reductions = gain electrons). So it will have a higher OS and will be a strong oxdant eg. O, F O is reduced to O2- (by gaining an electon) O + 2e- = O2- |
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If a transition metal has a low oxidation state... |
then it's very unstable, so has to be stabilised using a reducing agent e.g. CO/CN- |
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Define lewis Acid... |
is an electron pair acceptor |
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Define lewis Base... |
is an electron pair donor |
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In a complex what is the LA and LB |
LA = metal LB = ligand |
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What is a ligand? |
ligand is atom, ion or molecule which can donate lone electron pair |
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What is a complex ? |
is a central metal ion surrounded by ligands |
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What is the coordination no.? |
the number of coordinate bonds formed to a central metal ion |
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What is are unidentate/ monodentate ligands? |
ligands that can form one coordinate bond per ligand. e.g. h20, nh3, cl- |
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What are bidentate ligands? |
Ligands that can form 2 coordinate bond per ligand because it has 2 atom with lone pairs e.g. (en) |
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What are multidentate ligands? |
ligands that can form 6 coordinate bond per ligand. e.g. edta- |
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What are ambidenate ligands? |
ligand that have 2 possible places that they can bind to. e.g. NO2- either N or O |
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Workout the OS of Cl in NaClO3? |
Na = +1 O = -2 so.... (+1) Cl (6*-2) = 0 Cl (-5) = 0 Cl = +5 |
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Workout the OS of Fe in K3Fe(CN)6 ? |
CN = -1 K = +1 so.... Fe^ + (6*-1) (3*1) = 0 Fe ^ (-3) = 0 Fe = +3 |
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Workout the OS for ... 1. [Cr(NH3)6]+3 2. [Fe(SCN)(h20)5]+2 3. W(CO)6 4. K2 [PtCl6] |
Cr = +3 Fe = +3 |
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What is the trend in ionic radius? 1. positive ions 2. negative ions |
The positive ions (TM) the ionic radii decrease as you go across the period. Even though the structure is the same the no. of protons increase so pulls the electrons closer to the nucleus. The negative ions same as + ions but this time they have extra shell of electrons. |
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State 2 stereoisomerism |
1. geometrical (E/Z) 2. optical |
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State 4 structural isomerism (SI) |
1. Coordination isomerism 2. Ionisation isomerism 3. hydrate isomerism 4. Linkage isomerism |
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What are the possible isomerism in... - square planar - octahedral - tetrahedral |
s p = S + - O = S + SI T = - + SI |
