Download [Zn(NH3)4]SO4 [Cr(NH3)5Cl]Cl2 [Co(en)2Br2]2SO4

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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