1.	(2 points)  Which of the following ions contain a bidentate ligand?

	a. [Co(NH3)5(H2O)]3+	    c. [Co(NH3)4(NO2)2]+

	b. [Co(NH3)4CO3]+	    d. [Co(NH3)5NO2]2+

2.	(2 points)  The compound [Co(NH3)4(CN)2]Cl dissolves in water to give?

		2 ions		3 ions		4 ions		5 ions

3.	(2 points)  Which of the following compounds exhibits geometric isomerism?

	a. [Pt(NH3)4]Cl2	            c. [Pt(NH3)2Cl2]

	b. [Pt(NH3)3Cl]Br	    d. [Pt(NH3)Cl3]

4.	(2 points)  Draw all isomers of the complex ion formed from the 
	compound [Cr(H2O)4Br2]Cl:











5.	(2 points)  Complexes of non-transition metal ions such as Al3+ are 
	almost always colorless whereas complexes of transition metal ions 
	are usually highly colored.  Explain why?


6.	(1 point)  The oxidation state on Cr in [Cr(CN)4(NH3)2]- is___?____.

7.	The complex [Cr(CN)6]4- has two unpaired electrons.

	a.	(4 points)  Draw the crystal field diagram:













	b. (1 point)  How many unpaired electrons would you expect in 
	[CrF6]4- if F- is a weak field ligand?

		Why?



8.	(2 points)  If a complex ion appears yellow in solution, it is 
	probably absorbing which color of light?

	a) red		b) orange	c) blue		d) violet

9.	(2 points)  Which of the following complex ions would absorb the

	 highest energy light, [CoCl6]3- or [Co(H2O)6]3+?____________________

	Why?


				KEY

1.	(2 points)  Which of the following ions contain a bidentate ligand.

	a. [Co(NH3)5(H2O)]3+	c. [Co(NH3)4(NO2)2]+

	(b. [Co(NH3)4CO3]+)	d. [Co(NH3)5NO2]2+

2.	(2 points)  The compound [Co(NH3)4(CN)2]Cl dissolves in water to give

		(2 ions)		3 ions		4 ions		5 ions

3.	(2 points)  Which of the following compounds exhibits geometric isomerism?

	a. [Pt(NH3)4]Cl2		(c. [Pt(NH3)2Cl2])

	b. [Pt(NH3)3Cl]Br	d. [Pt(NH3)Cl3]

4.	(2 points)  Draw all isomers of the complex ion formed from 
	the compound [Cr(H2O)4Br2]Cl:

				CIS AND TRANS ISOMERS

5.	(2 points)  Complexes of non-transition metal ions such as Al3+ are 
	almost always colorless whereas complexes of transition metal ions 
	are usually highly colored.  Explain why.

	Al3+ complexes have no e's in the d orbitals and filled p orbitals.  
	No electron transitions occur which involve visible light.

	Most transition metal complexes have only partly-filled d orbitals; 
	as visible light is absorbed, these electrons are excited to higher 
	d orbitals.

6.	(1 point)  The oxidation state on Cr in [Cr(CN)4(NH3)2]- is  "+3" .

7.	The complex [Cr(CN)6]4- has two unpaired electrons.

	a.	(4 points)  Draw the crystal field diagram.

		                        Cr2+	4s03d4
						     

		"Strong" 	dz2__no e-__		dx2-y2__no e-__
                 field                                
		"Large"                                     
		(splitting)		              	          
                                                    
		           dxy__e-up__e-down__	dxz__e-up__	dyz__e-up__


	b.	(1 point)  How many unpaired electrons would you expect in [CrF6]4- 
		if F- is a weak field ligand?     "4"                      
		Why?			     	      
                      "Small"(less) splitting:
                      the four electrons would fill the bottom three orbitals first
                      and one of the upper level orbitals next
                      all would be in the up direction spinning together making the
                      molecule paramagnetic
				     	     	     
                      
8.	(2 points)  If a complex ion appears yellow in solution, 
			it is probably absorbing which color of light?

		a) red		b) orange	c) blue		d) "VIOLET"
	 


9.	(2 points)  Which of the following complex ions would absorb the

	 highest energy light, [CoCl6]3- or [Co(H2O)6]3+?    [Co(H2O)6]3+  
	Why?

	H2O is a stronger field ligand, causes a larger splitting
	and absorption of higher energy light.