The solubility of given copper (II) salts in water should be identified. Concept introduction: Most of the ionic compounds are soluble in water, very few of the ionic compounds are sparingly soluble, and some of the ionic compounds are insoluble in water. When it is soluble in water ions gets separated in the solution. Soluble compounds in water: Almost all the salts of Na + , K + , NH 4 + , ( NO 3 - ) , ( ClO 3 - ) , ( ClO 4 - ) and ( CH 3 CO 2 - ) are soluble. Almost all the salts of Cl - , Br - , I - ( halides ) are soluble. But some of the halides are ( Ag + , Hg 2 2+ , Pb 2+ ) insoluble. Salts of F - are soluble. But some of the fluoride salt of Mg 2+ , Ca 2+ , Sr 2+ , Ba 2+ , Pb 2+ are insoluble. Salts of sulfate ( SO 4 2- ) are soluble. But sulfates of Ca 2+ , Sr 2+ , Ba 2+ , Pb 2+ , Ag + , are insoluble. Insoluble compounds in water: Most of the salts of ( CO 3 2- ) , ( PO 4 3- ) , ( C 2 O 4 2- ) , ( CrO 4 2- ) and ( S 2- ) are insoluble but some of the salts of NH 4 + , alkali metal cations and BaS are soluble. Most of the metal hydroxides and oxides are insoluble in water but some of the alkali metal hydroxides, Ba ( OH ) 2 and Sr ( OH ) 2 are soluble in water.
The solubility of given copper (II) salts in water should be identified. Concept introduction: Most of the ionic compounds are soluble in water, very few of the ionic compounds are sparingly soluble, and some of the ionic compounds are insoluble in water. When it is soluble in water ions gets separated in the solution. Soluble compounds in water: Almost all the salts of Na + , K + , NH 4 + , ( NO 3 - ) , ( ClO 3 - ) , ( ClO 4 - ) and ( CH 3 CO 2 - ) are soluble. Almost all the salts of Cl - , Br - , I - ( halides ) are soluble. But some of the halides are ( Ag + , Hg 2 2+ , Pb 2+ ) insoluble. Salts of F - are soluble. But some of the fluoride salt of Mg 2+ , Ca 2+ , Sr 2+ , Ba 2+ , Pb 2+ are insoluble. Salts of sulfate ( SO 4 2- ) are soluble. But sulfates of Ca 2+ , Sr 2+ , Ba 2+ , Pb 2+ , Ag + , are insoluble. Insoluble compounds in water: Most of the salts of ( CO 3 2- ) , ( PO 4 3- ) , ( C 2 O 4 2- ) , ( CrO 4 2- ) and ( S 2- ) are insoluble but some of the salts of NH 4 + , alkali metal cations and BaS are soluble. Most of the metal hydroxides and oxides are insoluble in water but some of the alkali metal hydroxides, Ba ( OH ) 2 and Sr ( OH ) 2 are soluble in water.
Solution Summary: The author explains the solubility of copper (II) salts in water.
The solubility of given copper (II) salts in water should be identified.
Concept introduction:
Most of the ionic compounds are soluble in water, very few of the ionic compounds are sparingly soluble, and some of the ionic compounds are insoluble in water. When it is soluble in water ions gets separated in the solution.
Soluble compounds in water:
Almost all the salts of Na+, K+, NH4+,(NO3-),(ClO3-),(ClO4-)and(CH3CO2-) are soluble.
Almost all the salts of Cl-, Br-, I-(halides) are soluble. But some of the halides are (Ag+, Hg22+, Pb2+) insoluble.
Salts of F- are soluble. But some of the fluoride salt of Mg2+, Ca2+, Sr2+, Ba2+, Pb2+ are insoluble.
Salts of sulfate (SO42-) are soluble. But sulfates of Ca2+, Sr2+, Ba2+, Pb2+, Ag+, are insoluble.
Insoluble compounds in water:
Most of the salts of (CO32-),(PO43-),(C2O42-),(CrO42-) and (S2-) are insoluble but some of the salts of NH4+, alkali metal cations and BaS are soluble.
Most of the metal hydroxides and oxides are insoluble in water but some of the alkali metal hydroxides, Ba(OH)2and Sr(OH)2 are soluble in water.
(f) SO:
Best Lewis Structure
3
e group geometry:_
shape/molecular geometry:,
(g) CF2CF2
Best Lewis Structure
polarity:
e group arrangement:_
shape/molecular geometry:
(h) (NH4)2SO4
Best Lewis Structure
polarity:
e group arrangement:
shape/molecular geometry:
polarity:
Sketch (with angles):
Sketch (with angles):
Sketch (with angles):
1.
Problem Set 3b
Chem 141
For each of the following compounds draw the BEST Lewis Structure then sketch the molecule (showing
bond angles). Identify (i) electron group geometry (ii) shape around EACH central atom (iii) whether the
molecule is polar or non-polar (iv)
(a) SeF4
Best Lewis Structure
e group arrangement:_
shape/molecular geometry:
polarity:
(b) AsOBr3
Best Lewis Structure
e group arrangement:_
shape/molecular geometry:
polarity:
Sketch (with angles):
Sketch (with angles):
(c) SOCI
Best Lewis Structure
2
e group arrangement:
shape/molecular geometry:_
(d) PCls
Best Lewis Structure
polarity:
e group geometry:_
shape/molecular geometry:_
(e) Ba(BrO2):
Best Lewis Structure
polarity:
e group arrangement:
shape/molecular geometry:
polarity:
Sketch (with angles):
Sketch (with angles):
Sketch (with angles):
Chapter 3 Solutions
OWLv2 6-Months Printed Access Card for Kotz/Treichel/Townsend's Chemistry & Chemical Reactivity, 9th, 9th Edition
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Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell