Download transition metals

Name: _________________________________________
Date:____________________________
Optional Homework 8 – do not turn in!!
1.) Write the electron configurations for the following species:
a. Ag
b. Ag+1
c. Cd+2
d. Ir+3
2.) Find the charge of all species in each of the following coordination compounds, if it is a polyatomic
ion, I just want the overall charge of that ion, not individual oxidation numbers of every element!:
HINT: you may need to go back and review your polyatomic ion charges!!
a. K[CuCl2]
K:
Cu:
Cl:
b. (NH4)2[Ni(CN)4]
NH4:
Ni:
CN:
c. [Ti(H2O)6]2(SO4)3
Ti:
H2O:
SO4:
d. Al4[V(CN)6]3
Al:
V:
CN:
3.) Identify the complex ion and the ligands in the compound K3[Fe(CN)5CO]. Find the oxidation
number of the metal ion in complex ion: be sure to label the inner sphere (ligands bonded
covalently to the metal) and outer sphere ligands (counter ions) in the complex!
4.) Find the charge on the nitrosyl ligand (NO) in the Co(III) compound: Na2[Co(CN)5NO]
5.) If the coordination complex [Cr(NH3)5Cl]Cl2 dissociated into its ions, what ions would be formed?
Write a balanced equation showing this dissociation!
[Cr(NH3)5Cl]Cl2
→ ???
6.) Using the ideas of Lewis and resonance structures, determine which of the following ligands can
participate in linkage isomerism (meaning can they cause a compound to be a linkage isomer).
DRAW the resonance structures in order to explain! Remember that a linkage isomer can bond to
the metal ion from two distinctly different places on the molecule. And in order to have a bond –
you need electrons!!!
a. NO2-1
b. SO2
c. NO3-1
7.) Define/explain the crystal field splitting energy ()?
8.) Sketch a structure for the following complex ions:
a. [PdCl4] -2 (square planar)
b. [Be(OH)4]-2 (tetrahedral)
c. [AgCl2]-1
d. [Co(NH3)5CO3]+1
9.) Nitrogen gas can be prepared by passing gaseous ammonia over solid copper (II) oxide at high
temperatures, as described by the following balanced equation. How many grams of N2 are formed
when 18.1 g of NH3 are reacted with 90.4 g of CuO? What starting material, if any is left over? How
many grams of that material are left over?
2 NH3 (g) + 3 CuO (s)  N2 (g) + 3 Cu (s) + 3 H2O (g)
10.) Given the following information, draw the Lewis structure, determine the molecular shape, VSEPR
shape, hybridization around the central atom, and predicted bond angle for each species.
a. PH3
b. CF4
c. SO4 -2
d. PF5
e. KrF2
f.
TeF5 -1
11.) Does the Qc for the formation of 1 mole of NO from its elements differ from the Qc of the
decomposition of 1 mole of NO into its elements? Explain and give the relationship between the
two Qc values.
12.) Balance the reaction and write the Qc
a. ________NaHCO3 (s)  ________Na2CO3 (s) + ________CO2 (g) + _______H2O (g)
13.) Given the following Qc expressions, write the balanced chemical equation:
a. Q = [CO2]2 [H2O]2
[C2H4][O2]3
____
9.
a.
b.
c.
d.
e.
What is the correct answer to the following expression: 3.33 x 10-5 + 8.13 x 10-7?
3 x 10-5
3.4 x 10-5
3.41 x 10-5
3.411 x 10-5
3.4113 x 10-5
____
10.
a.
b.
c.
d.
Rank the subatomic particles from lowest to highest mass?
electrons < neutrons < protons
electrons < protons  neutrons
neutrons < electrons < protons
electrons = protons < neutrons
___
11.
A substance that contains unpaired electrons is attracted to a magnetic field. This
substance is said to be ________.
Ionic
Ferromagnetic
Paramagnetic
Polar
Diamagnetic
a.
b.
c.
d.
e.