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Name: _________________________________________ Date:____________________________ Homework 5 Insert space or answer questions on a separate sheet of paper NO OWL homework this weekend – only paper HW – catch up on OWL!!! 1.) Give systematic names for the following: a. [Ni(H2O)6]Cl2 hexaaquanickel(II) chloride b. [Cr(en)3](ClO4)3 trisethylenediaminechromium (III) perchlorate c. K4[Mn(CN)6] potassium hexacyanomanganate (II) d. [V(H2O)6]SO4 hexaaquavanadium (II) sulfate e. [Pt(NH3)2Cl2F2] diamminedichlorodifluoroplatinum (IV) 2.) Write the formulas for the following compounds: a. Tetraamminezinc sulfate Zn+2 SO4-2 NH3 [Zn(NH3)4]SO4 b. Pentaamminechlorochromium(III) chloride NH3 Cl-1 Cr+3 Cl-1 [Cr(NH3)5Cl]Cl2 c. Dibromobis(ethylenediamine)cobalt(III) sulfate (en) Co+3 SO4-2 2Br-1 [Co(en)2Br2]2SO4 3.) Draw the indicated isomers for the following compounds: a. Geometric: [Pt(CH3NH2)2Br2] the N is attached to platinum: identify which is cis/trans H3CH2N Br Pt Br Br NH2CH3 Br Trans: 180o apart Pt NH2CH3 NH2CH3 Cis: 90o apart b. Linkage: [Cr(NH3)5(NO2)]+2 NH3 H3N Cr NH3 H3 N NH3 NO2 NH3 H3N Cr NH3 H 3N NH3 O NO c. Coordination isomers: [Pt(CH3NH2)3Br]Cl and [Pt(CH3NH2)3Cl]Br Cl H3CH2N Br Pt Br NH2CH3 H3CH2N NH2CH3 Cl Pt NH2CH3 NH2CH3 4.) Draw the splitting diagram for an octahedral complex Draw the splitting diagram for a tetrahedral complex Draw the splitting diagram for a square planar complex Be SURE to identify which d orbitals are located where!! ☺ Octahedral: ligands come in ON axes which repulses x2-y2 and the dz2 orbitals 5.) What is the distinction between a weak field and a strong field ligand? What does it mean for electrons filling the d orbitals? Give an example of a weak field ligand. Give an example of a strong field ligand A weak field ligand can be thought of as a species that does not have enough strength to separate the d orbitals much from one another. It creates a small ∆ value, which means that electrons will fill in all the d orbitals, even the higher energy d orbitals before the electrons pair up. 6.) Draw orbital energy splitting diagrams and use the ligand strength series to show how the electrons would fill the d orbitals (orbital occupancy) for each of the following: Are the species high spin or low spin complexes: Hint: the ligand tells you if the ∆ is large or small. The d orbitals electrons come from the metal ION. a. [Cr(CN)6]-4 x2-y2 z2 Cr+2: 1s22s22p63s23p64s03d4 CN is a strong field ligand, this creates a large ∆ This would be a low spin complex xy xz yz b. [Rh(CO)6]+3 x2-y2 Rh+3: 1s22s22p63s23p64s23d104p65s04d6 z2 CO is a strong field ligand, this creates a large ∆ This would be a low spin complex as ∆ is large so the electrons will pair before going to the higher d orbitals xy xz yz c. [Fe(Cl)6]-4 Fe+2: 1s22s22p63s23p64s03d6 x2-y2 Cl-1 is a weak field ligand, this creates a small ∆ z2 This would be a high spin complex as ∆ is small so the electrons will NOT pair pair and will go to the higher d orbitals xy d. [Fe(CO)6]+2 xz x2-y2 yz z2 Fe+2: 1s22s22p63s23p64s23d104p65s04d6 CO is a strong field ligand, this creates a large ∆ This would be a low spin complex as ∆ is large so the electrons will pair before going to the higher d orbitals xy xz yz 7.) Consider the series Cl2, Br2, and I2. What trend is observed in bond strength? Considering the sizes of the atoms, what trend would you predict for bond length? Bond strength decreases from Cl2 to Br2 to I2. As atoms get larger, their bond lengths get longer. And longer bonds tend to be weaker bonds