ICSE CHEMISTRY CLASS 10 PRACTICE PAPER-9

ICSE CHEMISTRY CLASS 10 PRACTICE PAPER-9

PERIODIC TABLE, ELECTROLYSIS, AMMONIA, NITRIC ACID and

ACIDS , BASES AND SALTS

Section I (40 Marks)

Answer all the questions

Question 1

a) Select a suitable word from the list given in brackets for each of the following statements.   5M

( Ammonia, Hydroxyl ion, Nitrogen dioxide, 7, Hydronium ion, fused Lead bromide, Acetic acid)

i)        The number of electrons present in the outer most shell of a halogen.

ii)      The ion which is responsible for the acidic nature of an acid.

iii)    A strong electrolyte.

iv)    The basic gas released when Ammonium salts are heated an alkali.

v)      The acidic gas released when Nitric acid undergoes thermal decomposition.

b)   Match the following.                Example-   vi-G                                                                      5M

Part-A

i)   The amount of energy released when

      an element gains an electron

ii)  The amount of energy required to remove an electron from its valence shell

iii) The tendency to attract bond pair of

      electrons

iv) The ease to lose electrons

v)  The element which tend to lose

      electrons

vi) Group I

Part-B

A) Electronegativity

B) Electron affinity

C) Ionisation potential

D) Non metal

E) Electropositivity

F) Metal

G) One valence electron

c) Choose the correct option from A, B, C and D for each of the following statements.            5M

i)           Which one of the following statements is suitable for the Atomic radium?

A)    Increases across a period but decreases down a group

B)    Decreases across a period but increases down a group

C)    Does not change across a period       D) Decreases across a period and down a group

ii)         Which one of the following is not correct about a weak electrolyte

A)    Undergoes partial dissociation                B) Conducts small amounts of electricity

C)    Contains ions and molecules                   D) Contains ions only            

iii)       Acidity of a base is defined as

A) The number of Hydronium ions produced by one molecule of the base

B) The number of Hydrogen ions produced by one molecule of an acid

C) The number of Hydroxyl ions produced per molecule of the base in its solution

D) The number of hydroxyl ions that a base contains

iv)       Ammonia gas is released when warm water is added to

A) Magnesium nitride                                        B) Sodium nitrate        

C) Ammonium nitrtate                                       D) Calcium hydroxide

v)         Conc. HNO₃ is a strong __________ agent.

A)    Oxidising                   B) drying                        C) reducing              D) dehydrating

d) Fill in the blanks:-                                                                                                                     5M

i)        Metals have ________(low/high) ionization potential values.

ii)      Strong acids dissociate ______________( completely/partially)tom give a high concentration of Hydronium ions in their aqueous solutions.

iii)    _______________ (Electrorefining / electroplating) makes an article attractive.

iv)    Aqueous solution of Ammonia is called ______________ (liquor/ liquid) ammonia.

v)      Nitric acid is a _______________(non-volatile/ volatile) acid.

e) Name the following.                                                                                                                  5M

i) The electrolyte used in the electroplating of an article with Silver.

ii) The basic gas which gives white dense fumes with HCl gas.

iii)  The non-volatile acid formed when Conc.HNO₃ reacts with Sulphur.

iv) The acid salt formed when dil. H₂SO₄ is treated with insufficient Sodium hydroxide.

v) The most electronegative element.

f) Correct and rewrite the following statements.                                                                          5M

i) During an electrolysis process metal deposits at anode

ii) Sulphuric acid is a monobasic acid.

iii) Group I elements are least electropositive.

iv) Ammonia gas turns Nessler’s reagent to red.

v) Nitric acid reacts with Copper to produce Nitrogen dioxide.

g) Study the table given and answer the following questions.                                                     5M

At. No.	3	4	5	6	7	8	9	10	11	12
Element	A	D	E	G	J	L	M	Q	R	T

i)     Identify the Noble gas in the table.

ii)   The element which belongs to Group 2 and has 3 shells.

iii) The element which shows a valency of 2-.

iv) Which one of the above elements has the highest Electron affinity?

v)   The element which has 3 valence electrons.

h) A)Calculate the molecular weights of the following compounds:                                     [3+2]

i) Sodium carbonate                       ii) Sulphuric acid                iii) Hydrated copper sulphate

B) Calculate the percentage of Oxygen in Sodium hydroxide.

(At.Wt. H-1, C-12, O-16, Na-23, S-32, Cu-64)

Section II (40 Marks)

Answer any four of the following questions

Question 2                                                                                                                      [4+2+2+2]

a)      The atomic number of an element Z is 16. Then

i)        State the group to which it belongs.

ii)      Is Z a metal or non metal?

iii)    Write the formula of the compound between Z and Sodium.

iv)    State the number of shells present in it.       

b)      If an element M belongs to group I

i)        State the nature of the compounds of it .(Ionic/covalent)

ii)      Write the formula of its oxide.

c)      Give reasons why:

i)  Ionization potential increases across a period.

ii)   Metallic character decreases a group.

d)     E, G and L are the three elements with atomic numbers 13, 11 and 15 respectively.

           i) Arrange them in the decreasing order of their electronegativity.

           ii) Which one among them is an alkali metal.

Question 3                                                                                                                          [4+3+3]

a)      Answer the following questions pertaining to the electrolysis of fused Lead bromide.

i)        State any one appropriate observation.

ii)      Name the product at cathode.

iii)    Give reason why the crucible made of silica is taken as electrolytic cell.

iv)    Write the balanced electrode reaction at anode.

b)      Name the following.

i)        The anode during the electro-refining of Copper metal

ii)      The reduction electrode.

iii)    The anion which gets discharged most easily.

c)      During the process of electroplating the article to be electroplated is made i) ____________ and the metal is made _________ and _________ current should be passed for the effective deposition of the metal on the article.

Question 4

a)                                                                                                                                              5+1+4

Group No. Period No.	1	2	13	14	15	16	17	18
2	A		M			T
3		D		J		W	G	R
4		Q

i)           Identify the most electronegative element in group 2.

ii)         Name the reactants taken in the Round bottom flask.

iii)       Which one of the above elements is a metalloid?

iv)       Identify the Halogen given in the table.

v)         State the type of bonding between Q and W.

b) Arrange the following elements in the decreasing of their Ionization potentials.

      Na, S, Al, Cl

c)   i) Give reason why a low current must be passed for a longer time during electroplating.

ii) State any one observation seen during the electrolysis of Copper sulphate using Platinum (inert) electrodes.

iii) Name the impurities settle down below the anode during electrorefining.

iv) Write the Empirical  formula of Acetic acid.

Question 5                                                                                                                      [3+2+3+2]

a) Name the following.

 i) The negatively charged ion produced when an alkali is dissolved in water.

ii) The salt formed by the partial neutralization of an alkali by an acid.

iii) The characteristic property of a crystalline hydrated salt to lose its water of

crystallization to the atmosphere and turn to an amorphous powder.

b) Identify the metal ions present in the salts A and B.

i)  Salt A gives a pale blue precipitate with Ammonium hydroxide.

ii) Salt B gives chalky white precipitate with Sodium hydroxide solution.

c) Write the balanced equation for the following conversions

            i) PbO à Pb(NO₃)₂ à PbCl₂

            ii) Dil. Suplhuric acid  à  Copper sulpahte (using a metallic oxide)

d) State the nature and the strength of the solutions P and Q.

Solution	pH value
P	7
Q	13.5

Question 6                                                                                                                           [4+3+3]

Answer the questions a) and b) with respect to the laboratory preparation of Ammonia gas.

a) i) Name the reactants taken in the process.

   ii) Name the drying agent used

   iii) State the identification test for Ammonia gas.

   iv) Write balanced equation for the above preparation.

b)   Give reasons

i) Round bottom flask is kept in inclined position.

ii) Conc. Sulphuric acid is not used as a drying agent.

iii) Ammonium nitrate is not used in this method.

c) i) Name the industrial process in which Ammonia is prepared from Nitrogen and Hydrogen.

   ii) State whether the above reaction is exothermic or endothermic.

   iii) State the observation seen when gry Ammonia gas is passed over heated yellow PbO.

Question 7

a)      i) Give balanced equation for the preparation of Nitric acid in laboratory method.

Give reasons why :

ii) Nitric acid prepared in the above process appears in yellow colour.

iii) The entire apparatus is made of glass only in this method.

b)      i) State the composition of Aqua regia.

ii) Name the basic oxide formed when Copper nitrate undergoes thermal decomposition.

iii) Write the balanced equation for the reaction between Conc.HNO₃ and Cu.

c)      State any two uses of acids.

d)     Find the Empirical formula of a compound whose composition is given below.

C-40%, H-6.7% and O-53.3%

At.wt.-H-1, C-12, O-16