ICSE CHEMISTRY CLASS 10 PRACTICE PAPER-4
ELECTROLYSIS, PERIODIC TABLE, CHEMICAL BONDING and PRACTICAL CHEMISTRY
Section I (40 Marks)
Answer all the questions
Question
1
a) Choose the correct
answers from the words given below 5M
(8, covalent bond,
Sodium, Hydrogen sulphide, 7, Silver)
i)
An element which belongs to Group 1.
ii) The
number of valence electrons present in Group 17 elements.
iii) The
type of bond formed by the mutual sharing of electrons.
iv) The
gas with rotten egg smell.
v) The
metal used as anode during the electroplating with Silver.
b) Match the following. Example- vi-D 5M
Part-A
i) Anode
mud
ii) Active electrode
iii) Electrovalent
compound
iv) Element with
highest E.A value
v) Sulphur dioxide
vi) A non polar
covalent compound
Part-B
A) Chlorine
B) Elecrorefining
C) Fluorine
D) CCl4
E) Nickel
F) Acidic gas
G) NaCl
c)
Select the correct answers from the words given below: 10M
i)
The valency of a metal which has 1
valence electron.
A)
2- B) 2+ C) 1+ D) 3+
ii)
The element with highest Electronegativity.
A)
Fluorine B) Chlorine C) Boron D) Carbon
iii) The
atomic size __________ across a period.
A)
Decreases B) Increases C) No change D) increases then decreases
iv) Na+
+ e- --> Na is a __________ reaction.
A)
Oxidation B) reduction C) Redox D) Decomposition
v)
The number of bonds present in one
Oxygen molecule.
A)
1 B) 2 C) 3 D) 4
vi) The
electrolyte used in the electroplating with Nickel.
A)
NiSO4 B)
CuSO4 C) FeSO4 D) NaCl
vii) The
ions that discharge at Cathode during the electrolysis of dil. H2SO4
A)
H+ B)
SO42- C)
OH- D) Cl-
viii) The
number of lone pair of electrons present on Oxygen in a water molecule.
A)
1 B) 3 C) 2 D) 4
ix) The
anion which is discharged with most difficulty at anode:
A)
Cl- B)
SO42- C)
OH- D) Br-
x)
The cathode used during the extraction
of Sodium from fused NaCl.
A)
Copper B) Aluminium C) Iron D) Nickel
d)
Identify A,B,C, D and E in the following reactions. 5M
example:
‘G’ is Oxygen gas
i)
A + Cobalt chloride (blue) --> Cobalt chloride(pink)
ii) B
+ acidified K2Cr2O7
-->Clear green
iii) C
+ Lead acetate --> Silvery black
iv) D
+ Potassium Iodide --> Brown precipitate
v) E
+ Nessler’s reagent --> Brown precipitate.
vi) G
+ alkaline Pyrogallol --> Dark brown
e)
Fill in the blanks:- 5M
i)
Across a period the valence electrons
increase by ________(1/2)
ii) The
electronic configuration of Sodium is ________ (2,8,4/2,8,1)
iii) In
an electrolysis reduction takes place at ___________ (Anode/Cathode)
iv) __________(Ni/Fe)
is an inert electrode.
v) NaOH
solution is an/a ____________ (electrolyte/non electrolyte).
f)
Complete the following statement with correct words. 5M
Metals
are (i)_________ (electropositive/electronegative) elements which
(ii)__________ (gain/lose) electrons to attain stability and form (iii)
_________ (cations/anions). The metallic character (iv) __________ (indreases/decreases)
across a period and metals have (v) ___________ (lower/higher) I.P values.
g)
Choose the odd one out. 5M
i)
A) NaCl B) CaCl2 C) NaOH D) MgO (Nature
of bonds)
ii)
A) H2O B) CS2 C) HCl D) H2SO4 (non-polar compound)
iii)
A) NaOH B) H2SO4 C) HNO3 D) H2O (Non-electrolyte)
iv) A) Li B) Na C) Mg D)
K (A
group 2 element)
v) A) HCl B) SO2 C) NH3 D) NO2 (Basic gas)
Section II (40 Marks)
Answer any four of the
following questions
Question-2
(2+4+4)
a) i)
Name the Noble gas in period 1.
ii)
An element having 2 valence electrons belongs to (Group1/Group 2).
b)
Study the table given below and answer the questions. ( Do not identify the elements)
Group
|
1
|
2
|
13
|
14
|
15
|
16
|
17
|
18
|
Period
2
|
A
|
D
|
E
|
Y
|
J
|
|||
Period
3
|
M
|
G
|
L
|
|||||
Period
4
|
Q
|
R
|
T
|
i) Identify the Noble gas given in
the table.
ii) Write the Electronic configuration
of the element ‘E’.
iii) State the nature of the bond
between M and Y.
iv) The number of valence electrons
in D.
c) State
the trends in the following properties across a period in terms of
(increases/decreases).
i)
Electronegativity ii)
Ionization potential
iii) Nuclear charge iv) Electron affinity.
Question-3 (4+2+4)
a) Write the electronic configurations of the
following elements.
i) Carbon ii) Chlorine iii)
Nitrogen iv) Potassium
b) State the nature of the bonds between:
i) Two non-metals
ii) A non metal and a metal.
c) Classify the following compounds into Covalent
/electrovalent.
i) H2O ii) NaCl iii)
KBr iv) NH3
Question-4 (4+2+4)
a) Study the diagram given and answer the following questions.
i) Name the electrolyte taken in the
electrolytic cell.
ii) The product formed at cathode.
iii) Nature of the electrodes.
iv) Write the balanced equation for the
reaction
at cathode.
b) Give
reason why:
i) The
colour of the Copper sulphate solution fades during the electrolysis using Platinum
electrodes.
ii) Neither
of Sulphate ion and Hydroxyl ion discharge at anode during the electrolysis of
aq. CuSO4
using Copper electrodes.
c) i)
State the Observations seen at cathode during the electrolysis of aq. CuSO4
using
Platinum
electrodes.
ii) A
strong electrolyte contains ions only/
molecules only/ ions and molecules.
iii)
The amount of electricity conducted by the electrolyte depends on the
nature /concentration of the ions.
iv)
Here is an electrode reaction Pb2+ +
2e- à Pb
At
which electrode (anode/cathode) would this reaction take place?
Question-5 (3+3+4)
a) The elements X, Y and Z belong to Group 16, 3 and
18 respectively. Then
i) Classify
the elements X and Y into metals/non-metals.
ii) State
the number of valence electrons present in Z.
b) State whether the following statements are TRUE
or FALSE regarding Group 1 elements.
i) These elements have 1
electron in their valency shell.
ii) The elements have
non-metallic nature.
iii) They lose electrons
most readily.
c)
Answer the following questions with reference to the electrolysis of fused PbBr2.
Give reasons:
i) Platinum is not used as the anode.
ii) Silica crucible is used as the
electrolytic cell.
State
the observations at
iii) anode iv)
cathode
Question-6
(4+2+4)
a) Draw the electron dot structures of the following
molecules.
i)
Water ii) HCl iii) NaCl iv) MgO
b) State the nature of the bonds in :
i) Ammonium ion ii)
Chlorine molecule
c) i) Valency
of Y.
ii)
Nature of ‘Z’ metal/nonmetal.
iii)
Write the formula of the Oxide of ‘X’.
iv) Nature
of the bond between X and Z. (covalent/electrovalent).
Element
|
No.of valence
electrons
|
X
|
2
|
Y
|
3
|
Z
|
7
|
A
|
5
|
Question-7 (4+3+3)
a)
Give reasons:
i) Metals like K, Na, Al etc. are
extracted by electrolysis of their fused salts.
ii) The article which is to be
electroplated is always taken as cathode.
iii) During the electrolysis a low current
for longer time should be passed.
iv) During the electroplating with Silver,
Na[Ag(CN)2] is preferred to AgNO3 as the
electrolyte.
b)
Define the term Electroplating and give two uses.
c)
Write the balanced equations of dissociations during the electrolysis of:
i) dil.H2SO4
ii) fused PbBr2
iii) aq. NiSO4
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