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Inorganic Chemistry
A student heated (4.91x10^0) grams of calcium sulfate dihydrate. How many grams of water should be lost if the sample is heated correctly?
Inorganic Chemistry
What is the mass percent of water in a hydrate of copper(II) sulfate that has (1.00x10^0) waters of hydration?
Inorganic Chemistry
It is your first day of work in your new laboratory job. You are asked to prepare 700 mL of PBS (phosphate buffered saline). The PBS needs to be pH 7.40, with 25 mM phosphate and 140 mM NaCl. You are given a bottle of NaCl (FW = 58.45), a 1.00 M Na2HPO4 stock solution, and a 1.00 M NaH2PO4 stock solution. Describe how to prepare this buffer. (For H3PO4: pK1 = 2.12, pK2 = 7.21, pK3 = 12.66)
Inorganic Chemistry
(a) write a note on zone refining
(b) what is the assumption of VBT
(c) describe the clathrates of noble gases
(b) what is the assumption of VBT
(c) describe the clathrates of noble gases
Inorganic Chemistry
Q.1
All questions are compulsory. Marks for the questions are shown against them within
brackets.
Please answer in your own words; do not copy from the course material.
(a)
There are unequal number of elements in the periods in the Periodic Table,
explain.
(5)
(b)
Q.4
What is understood by hydrogen bonding? How does hydrogen bonding? How does
hydrogen bonding affect the properties of compounds? How many types of hydrogen
bonding are there?
(5)
What are alkali metals? Why do these metals not occur in free state in nature? List
the principal ores of alkali metals.
(5)
(a) Why is beryllium hydride polymeric in nature? Discuss the structure of polymeric
beryllium hydride.
(5)
(b)
Q.3
(a) (b)
Q.2
What is meant by effective nuclear charge? What are the factors that determine the
effective nuclear charge? How is it calculated?
(5)
At normal temperature, the trihalides of boron are all monomeric compounds whereas
those of aluminium, except AlF3, are dimeric solids, explain.
All questions are compulsory. Marks for the questions are shown against them within
brackets.
Please answer in your own words; do not copy from the course material.
(a)
There are unequal number of elements in the periods in the Periodic Table,
explain.
(5)
(b)
Q.4
What is understood by hydrogen bonding? How does hydrogen bonding? How does
hydrogen bonding affect the properties of compounds? How many types of hydrogen
bonding are there?
(5)
What are alkali metals? Why do these metals not occur in free state in nature? List
the principal ores of alkali metals.
(5)
(a) Why is beryllium hydride polymeric in nature? Discuss the structure of polymeric
beryllium hydride.
(5)
(b)
Q.3
(a) (b)
Q.2
What is meant by effective nuclear charge? What are the factors that determine the
effective nuclear charge? How is it calculated?
(5)
At normal temperature, the trihalides of boron are all monomeric compounds whereas
those of aluminium, except AlF3, are dimeric solids, explain.
Inorganic Chemistry
What is meant by effective nuclear charge? What are the factors that determine the
effective nuclear charge? How is it calculated?
effective nuclear charge? How is it calculated?
Inorganic Chemistry
What is hydrazoic acid? Why are the ionic azides more stable than the covalent azides
and hydrazoic acid
and hydrazoic acid
Inorganic Chemistry
Describe the structure of sulphuric acid and explain the reasons of shortening of S-O
bonds in the molecule.
bonds in the molecule.
Inorganic Chemistry
Carbon can form acetylides and methanides, while the other elements in the group are
unable to do so.
unable to do so.
Inorganic Chemistry
In nature, the element X consists of two naturally occurring isotopes. 107X with abundance 55.84% and isotopic mass 106.9051 amu and 109X with isotopic mass 108.9048 amu. Use the given information to calculate the atomic mass of the element X to an accuracy of .001% (Report your answer like this yyy.yyyy)
