This homework set is due Monday January 30^th 2016 at the start of class. Please

Question

This homework set is due Monday January 30^th 2016 at the start of class. Please turn in the homework on pages separate from this one. If you have multiple pages make sure they are kept together either by a staple or a paper clip, prior to arriving to class. Turn in the problems in the order they were assigned. Remove any "spiral fringe" from the homework prior to turning in the homework set, failure to do so will result in the loss of 5 points. This homework set is worth 20 points. Using the ammonium cation and potassium cation explain the relationship between solubility and ionic radius? Explain why all the potassium halides crystalize in the NaCl structure type whereas the ammonium halides do not. Predict the 31^P NMR spectrum of PF_2H_2Cl. Carbon monoxide is a widely used ligand in inorganic chemistry. When treated with H+ CO is fairly unreactive as a base, but readily reacts with nickel as a base. Is it possible for CO to be both a weak base and strong base? Looking at Ni(acac)_2 you determine it is not tetragonal. It is paramagnetic. How is this possible?

Explanation / Answer

1. Compounds containing small ions tends to be less soluble than compounds containing large ions.

This can be explained on the basis of attraction forces. Ions with smaller size bond more closely together and therfore harder to be separated in water while ions with larger size relatively loosely bound and can be separated more easily by attraction of water molecules.

When we compare size of K+ and NH4+ ions, NH4+ ion is larger in size therefore will be more soluble.

Potassium halide crystallize in NaCl structure and NH4+ crystallises in CsCl structure because NH4+ and Cs+ ions have comparable sizes.

Related Questions

Navigate

• Browse (All)
• Browse T
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.