SUB: CHEMISTRY – Science Paper 2
Max Marks: 80
GENERAL INSTRUCTIONS:
This question paper is divided into two Sections.
Section - I is Compulsory. Attempt ANY FOUR questions from Section - II.
The intended marks for questions or parts of questions are given in brackets [ ].
SECTION - I [40 Marks]
[Attempt ALL questions from this Section]
Question 1
I.
a.
b.
c.
d.
e.
II.
Choose the correct answer:
[5x1=5]
Which of the following is a common characteristic of a covalent compound?
i.
High melting point
iii. Consists of molecules
ii.
Conducts electricity when it is in molten state
iv. Always soluble in water
Ammonium hydroxide will produce a reddish brown precipitate when added to a solution
of:
i.
CuSO4
ii.
Zn(NO3)2
iii. FeSO4
iv. FeCl3
A salt which in solution gives a bluish white ppt. with NaOH solution and white ppt. with
BaCl2 solution is:
i.
CuSO4
ii.
FeSO4
iii. Fe2(SO4)2
iv. CuCl2
Duralumin is an alloy of:
i.
Al and Cu
ii.
Cu and Sn
iii. Al and Ag
iv. Al and Fe
The element with the highest ionization potential in the periodic table is:
i.
He
ii.
Ne
iii. Ar
iv. Xe
Fill in the blanks with suitable words:
[4x1=4]
An acid is a compound which when dissolved in water forms hydronium ions as the only
__________ (1) ions. A base is a compound which if soluble in water contains
__________ (2) ions. A base reacts with an acid to form a __________ (3) and water only.
This type of reaction is known as __________ (4).
III. The equation for the action of heat on Calcium nitrate is:
[5x1=5]
2CaO + 4NO2 + O2
2Ca(NO3)2
a.
How many moles of NO2 are produced when 1 mole of Ca(NO3)2 decomposes?
b.
What volume of O2 at S.T.P. will be produced on heating 65.6g of Ca(NO3)2?
c.
Find out the mass of Ca(NO3)2 required to produce 5 moles of gaseous products.
d.
Find out the mass of CaO formed when 65.6g of Ca(NO3)2 is heated.
e.
Find out the mass of Ca(NO3)2 required to produce 44.8L of NO2 at S.T.P.
IV.
Name the
reactions:
organic
compound
prepared
a.
CH3COONa + NaOH
b.
C2H5Br + KOH(alc)
c.
C2H5Br + KOH(aq.)
d.
C2H5OH + CH3COOH
V.
a.
b.
c.
d.
e.
Identify the following substances:
[5x1=5]
An acidic gas which gives dense white fumes with NH3.
An alkane whose molecular mass is 58.
A solid which when kept in the open, forms a solution after sometime.
An alloy used in electrical fittings.
A metal which gives hydrogen gas or reacting with both dilute acid and alkali.
VI.
a.
b.
c.
Write equations for the following reactions:
Aluminium oxide and Sodium hydroxide
Zinc and dilute Sulphuric acid
Magnesium nitride and water
𝐶𝐶𝐶𝐶𝐶𝐶
∆
by
each
of
the following
[4x1=4]
𝐶𝐶𝐶𝐶𝐶𝐶𝐶𝐶. 𝐻𝐻2 𝑆𝑆𝑆𝑆4
∆
[5x1=5]
d.
e.
Conc. Sulphuric acid and Sugar
Copper with concentrated nitric acid
VII.
a.
b.
c.
d.
e.
Name the following:
Second member of alkene series.
First member of alkane series.
Third member of aldehyde series.
Second member of Carboxylic acid.
Fourth member of alcohol series.
[5x1=5]
VIII. Write the I.U.D.A.C name of the following:
O
O
||
||
a.
H–C–H
H3C – C – CH3
b.
c.
IX.
a.
b.
OH
|
H3C – CH – CH2 – CH3
[5x1=5]
C2H5COOH
CH3
|
H3C – C – CH3
|
CH3
Name the following:
Promoter used in Haber’s process.
Catalyst used in Ostwald’s process.
[2x1=2]
SECTION - II [40 Marks]
[Attempt ANY FOUR questions]
Question 2
a.
The following questions refers to the periodic table:
[5x1=5]]
i.
Name the second last element of the period 3.
ii.
How many elements are in the second period?
iii. Name the element which has the highest electron affinity.
iv. Name the element which has the highest electro-negativity.
v.
Name the element which may be placed on group 1 but is not a metal.
b.
i.
Metals have __________ ionization potential.
[5x1=5]
ii.
Group 18 elements have __________ valence electrons with the exception of
__________ with __________ electrons in valence shell.
iii. Group 2 elements are called __________ metals.
Question 3
a.
Draw different isomers having the following molecular formula:
i.
C5H12
ii.
C4H8
b.
What is denatured alcohol?
c.
Give two important uses of ethanol.
d.
Write equations for:
i.
Preparation of ethanol by hydration of C2H4.
ii.
Preparation of acetic acid from ethanol.
[5]
[1]
[2]
[2]
Question 4
a.
Name the method by which following compounds can be prepared:
[3]
i.
Sodium Sulphate
ii.
Silver Chloride
iii. Iron Sulphide
b.
How will you distinguish between following pairs of compounds using NH4OH? [3]
i.
Copper sulphate and Iron (II) sulphate
iii. Zinc nitrate and Lead nitrate
ii.
Iron (II) sulphate and Iron (III) sulphate
c.
Name:
[4]
i.
A greenish yellow gas with pungent smell.
ii.
An oxide which is yellow when hot and white when cold.
iii. A gas with a rotten egg smell.
iv. A crystalline salt without water of crystallization.
Question 5
a.
Name one:
[5]
i.
Metal which is ductile
ii.
Non-metal which is a conductor of electricity
iii. Neutral oxide
iv. Metallic oxide which cannot be reduced by hydrogen
v.
Non-metal which has lusture
b.
i.
Name the chief ore of aluminium.
[5]
ii.
Name the process used to concentrate the above mentioned ore.
iii. Why is alumina added to Cryolite in the electrolytic reduction of aluminium?
iv. Give cathode and anode reactions involved in extraction of aluminium from its
above mentioned ore.
v.
Name the process used for the concentration of zinc blende.
Question 6
a.
Draw a neat and well labelled diagram for the silver plating on an iron spoon.
b.
Copy and complete the following table related to electrolysis.
S. No.
c.
Name of Electrolyte
Name of
Cathode
Name of
Anode
1
CuSO4 (aq.)
Copper
Copper
2
PbBr2 (molten)
Platinum
Platinum
Classify the
the reactions.
i.
Cu
following
Cu2+
as
ii.
oxidation
Fe3+
and
reduction
Fe2+
iii.
[3]
[4]
Product at
Cathode
reactions,
Cl-
Product at
Anode
also
complete
[3]
Cl
Question 7
a.
A compound has the following percentage composition by mass:
[5]
Carbon – 54.55%
Hydrogen – 9.09%
Oxygen – 36.26%
Its vapour density is 44. Find the empirical and molecular formula of the compound.
b.
Give the electron dot structure of the following
[3]
ii.
CH4
iii. H3O+
i.
NH3
c.
Compare the properties of covalent and electron valent compounds on the following
points:
[2]
i.
Solubility
ii.
Structure
************