Programme Code : BDP
Course Code : CHE-O2
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Year : 2012 Views: 876 Submitted By : r.s.banait On 29th September, 2012

Do you have solution for this Question. If yes    I aslo want solution.

Q.


Q1 a) Name the scientists who got Chemistry Nobel prize in 1906 and 1911. (1)

b) Explain Hund’s rule briefly with suitable example. (2)

c) Write down the main features of Mendeleev’s periodic table. (2)

d) What are the factors which affect the ionization energy? (2)

e) Define the following terms

i) Electron affinity

ii) Electronegativity

iii) Van der Waals radius (3)

Q 2 a) What is the difference between intramolecular and intermolecular hydrogen bonding?

Explain with suitable examples. (3)

b) What are ortho and para forms of hydrogen? Discuss the effect of temperature on

ortho and para hydrogens? (2)

c) Explain the following:

i) The alkai metals do not occur in the free state in nature.

ii) The alkali metals are the largest in their corresponding period.

iii) The alkali metals act as strong reducing agent. (3)

d) Discuss briefly anomalous nature of lithium. (2)

Q.3 a) Explain the following

i) The alkaline earth metals are soft metals.

ii) The alkaline earth metals are less reactive than alkali metals.

iii) The halides of beryllium polymerise easily. (3)

b) Briefly discuss the complexation behaviour of alkaline earth metals. (2)

c) Why aluminum can not be extracted from aqueous solution of aluminum salts by the

process of electrolysis? (2)

d) Why does hot and conc. HNO3 render Al and Ga passive? (2)

e) Why are the borohydrides more stable than boranes? (1)

Q.4 a) What are metaborates? Give reaction for the borax-bead test for cobalt and the colour

obtained thereof. (1+2)

b) B-N bond distance in borazine is 144 pm, which is less than the sum of single-bond

covalent radii of B (82 pm) and N (70 pm). What does this indicate? (2)

c) The inert nature of silicones make them useful for what? (1)

d) What is the structure of most acetylides? (2)

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e) Give the reaction of phosphorus with potassium hydroxide. (2)

Q.5 a) How is red lead formed from lead oxide? Give the relevant reactions. What are the

uses of red lead? (4)

b) Give suitable reactions to explain why the pale blue liquid of N2O3 loses its colour on

warming? (2)

c) Hypophosphorous acid is monobasic even though it has three hydrogen atoms. Why? (2)

d) Give one very important use of hydrazine. (1)

e) What is phosphatic slag? (1)

Q.6 a) Explain the paramagnetic behaviour of oxygen on the basis of molecular orbital

theory. Give reasons for a large difference in melting and boiling points between

oxygen and sulphur. (5)

b) How is peroxomonosulphuric acid prepared from peroxodisulphuric acid and how

can the two be distinguished from each other? Illustrate with the help of complete

reactions. (5)

Q.7 a) Enumerate the reasons of delay in the isolation of fluorine. Why is fluorine unable to

exhibit the positive oxidation states? Explain the strongest ability of this element with

the help of Born Haber cycle. (5)

b) Acid strength of oxoacids of halogens increases with increase in the oxidation

number of halogen, explain. (2)

c) The interhalogen, ICl3 has a T-shaped structure, explain. (3)

Q.8 a) How is the ionisation energy, melting point and boiling point of the noble gases

affected by their electronic configuration? (2)

b) Explain the structure of XeOF4 on the basis of VSEPR theory (3)

c) Why do the transition metals exhibit variable oxidation states? How does the stability

of oxidation states of transition metals vary across a series and down the group? (5)

Q.9 a) Properties of transition metals vary from one element to another, whereas the

lanthanide elements resemble one another more closely and occur together in nature,

explain. (5)

b) Why is the range of oxidation states much more restricted in the lanthanide series as

compared to the early actinides, explain. (5)

Q.10 a) What are the main assumptions of crystal field theory? How does it explain the

colours of transition metal complexes? (5)

b) Carbon is theoretically capable of reducing almost all metal oxides at high

temperatures, still some metals can not be obtained by reduction of their oxides with

carbon, explain. (5)


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