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11th Chemistry Model Exam

St. Britto Hr. Sec. School - Madurai

11th Chemistry Model Exam-Aug 2020

Time : 3.00 Hours

Part - A

Multiple Choice Question - Answer All Question

Match the list-land list-II using the correct code given below the list.

List-I List-II

A. Z = 100 1. Mendelevium

B Z = 101 2. Lawrencium

C. Z = 102 3. Fermium

D. Z = 103 4. Nobelium

A B C D

4 3 2 1
A B C D

3 1 4 2
A B C D

4 1 3 2
A B C D

3 2 1 4

Chloropicrin is prepared by adding nitric acid to______________,

CCl₄
CH₃CI
CHCI₃
None

The formula of the compound is A₂B₃. The number of electrons in the outermost orbits of A and B respectively are,

3 and 6
3 and 2
2 and 3
5 and 2

Which of the following gas is essential for our survival?

N₂
H₂
O₂
He

Various successive ionisation enthalpies (in kJ mol^-1) of an element are given below.

IE₁ IE₂ IE₃ IE₄ IE₅

577.5 1,810 2,750 11,580 14,820

The element is

phosphorus
Sodium
Aluminium
Silicon

RbO₂ is

superoxide and paramagnetic
peroxide and diamagnetic
superoxide and diamagnetic
peroxide and paramagnetic

The name 'Blue John' is given to which of the following compounds?

CaH₂
CaF₂
Ca₂(PO₄)₂
CaO

Assertion (A): Energy of an electron is taken negative.
Reason (R): Energy of electron at infinity is zero.

Both A and R are true and R is the correct explanation of A
Both A and R are true but R is not the correct explanation of A
Ais true but R is false
Both A and R are false

LiH is an example of _________ hydride.

ionic
saline
covalent
both a and b

7.5 g of a gas occupies a volume of 5.6 litres at 0° C and 1 atm pressure. The gas is

NO
N₂O
CO
CO₂

An element X has the following isotopic Composition ²⁰⁰X = 90%, ¹⁹⁹X = 8% and ²⁰²X=2%The Weighted average atomic mass of the element X is closet to

201 u
202 u
199 u
200 u

A colourless solid substance (A) on heating evolved CO₂ and also gave a white residue, soluble in water. Residue also gave CO₂ when treated with dilute HCI

Na₂CO₃
NaHCO₃
CaCO₃
Ca(HCO₃)₂

For the reaction \(A+3B\rightleftharpoons 2C+D\) initial mole of A is twice that of B.1f at equilibrium moles of B and C are equal, then percent of B reacted is

10%
20%
40%
60%

The branch of science which deals the relation between energy, heat, work and accompanying changes around us is 'called' -------

Thermodynamics
Chemical kinetics
Calorimetry
Potentiometer

Consider the following statements
1. Hard water forms scum with soap.
2. Hard water lathers easily with soap
3. Hard water is unsuitable for laundry and boilers
Which of the following statement(s) given above is are correct?

1 & 3
only 1
2 & 3
only 2

Considering the elements F, CI, O and N, the correct order of their chemical reactivity in terms of oxidizing property is_____

F > CI > O > N
F > O > CI > N
CI > F > O > N
0 > F > N > CI

The correct order of electron gain enthalpy with negative sign of F, Cl, Br and I having atomic number 9, 17, 35 and 53 respectively is

I > Br > Cl > F
F > Cl > Br > I
Cl > F > Br > I
Br > I > Cl > F

Which one of the following is a metalloid?

N
P
Bi
Sb

On the basis of molecular orbital theory, select the most appropriate option.

The bond order of O₂ is 2.5 and it is paramagnetic
The bond order of O₂is 1.5 and it is paramagnetic
The bond order of O₂ is 2 and it is diamagnetic
The bond order of O₂ is 2 and it is paramagnetic

Which of the following is the lewis structure of water?

\(H-\overset { .. }{ \underset { .. }{ O } } -H\)

Match the list I with List II and select the correct answer using. the code given below the lists.

List I List II

A Metalloid 1 Cerium

B Noble gas 2 Nobelium

C Trans uranium element 3 Arsenic

D Lanthanide 4 Argon

A B C D

1 3 2 4
A B C D

4 2 1 3
A B C D

3 4 2 1
A B C D

2 1 4 3

Among the alkali metals which one form compounds with more covalent character?

Sodium
Potassium
Rubidium
Lithium

How does dizzonium salt (C₆H₅N₂+Cl^-) decompose?

C₆HSCI+N₂
C₆H₅Br + N₂
only b
both a& b

The main pigment in plants is chlorophyll which contains ________

iron
calcium
barium
magnesium

Identify the correct order regarding the electro negativity of hybrid orbitals of carbon is

sp < Sp² < Sp³
sp > sp² > sp³
sp > sp² > sp³
sp < sp² > sp³

Statement I. In Haber's process, NH₃ is liquefied and removed.
Statement II. In manufacture of NH₃, liquefied and removal of NH₃, keeps the reaction moving in forward direction.

Statement I and II are correct and II is the correct explanation of I.
Statement I and II are correct but II is not the correct explanation of I.
Statement I is wrong but statement II is correct.
Statement I is correct but statement II is wrong.

Several blocks of magnesium are fixed to the bottom of a ship to

Keep away the sharks
prevent rusting of iron ships
make the ship lighter
prevent puncturing by under sea rocks

Which one of the following is not a covalent hydride?

Ammonia
Methane
Lithium hydride
water

Hess's law can be applied to calculate -------- of reactions.

enthalpy
entropy
free energy
internal energy

For the reaction 2NO₂(g) u21cc 2NO(g) + O₂(g), K_c = 1.8 x 10^-6 at 185°C. At the same temperature the value of K_c for the reaction. NO(g) + \(\frac{1}{2}\) O₂ u21cc NO₂(g) is__________.

0.9 x 10⁶
7.5 x 10²
1.95 x 10^-3
1.95 x 10³

Part - B

Generic 2 - Answer All Question

What are the IUPAC names of the following compounds?
(i)\({ CH }_{ 3 }-{ CH }_{ 2 }-\underset { \overset { | }{ COOH } }{ CH } -CH={ CH }_{ 2 }\)
(ii) \(HOOC-\overset { \underset { | }{ { CH }_{ 3 } } }{ \underset { \overset { | }{ { CH }_{ 3 } } }{ C } } -{ CH }_{ 2 }-{ CH }_{ 2 }-{ CH }_{ 2 }-{ CH }_{ 3 }\)

In an experiment ethyliodide in ether is allowed to stand over magnesium pieces. Magnesium dissolves and product is formed
a) Name the product and write the equation for the reaction.
b) Why all the reagents used in the reaction should be dry? Explain
c) How is acetone prepared from the product obtained in the experiment.

Describe the mechanism of Nitration of benzene.

Which is the radioactive element in group 1 element? What is its half-life period?

How are branched alkanes formed from normal alkanes?
Write the IUPAC names of the following compounds.
(i)

(ii)

You are provided with a solid ‘A’ and three solutions of A dissolved in water - one saturated, one unsaturated, and one super saturated. How would you determine which solution is which?

What are the number of bond pairs and lone pairs of electrons on N-atom in N\({ O }_{ 3}^{ - }\)?

Mention the uses of quick lime

(i) Define critical temperature.
(ii) What is the critical temperature of CO₂ gas?

Explain why BeSO₄ and MgSO₄ are readily soluble in water.

Groups from 13 to 18 in the periodic table are called p-block elements. Give reason.

How does inductive effect plays a vital role in determining the strength of acids and bases.

Classify the following compounds by using aromaticity concepts

Explain why pure liquids and .solids can be ignored while writing the value of equilibrium constants

Li₂CO₃ decomposes readily whereas other carbonates are not. Why?

How will you control photochemical smog?

Why noble gases do not show much of chemical reactivity?

Explain the process of chromatography in chlorophyll.

Why the carbonated drinks are stored in pressurized container?

How is iodoethane converted to ethane?

Part - C

Generic 3 - Answer All Question

How will you derive the molecular structure from the type of hybridisation?

Does one gram mole of a gas occupy 22.4 Lunder all conditions of temperature and pressure.

Do you think that heavy water can be used for drinking purposes?

Give reasons for the following:
(i) Covalent bonds are directional while ionic bonds are non-directional.
(ii) Water molecule has bent structure where as CO₂ has linear structure.
(iii) Ethyne molecule is linear

Give a brief account on
(i) Adsorption chromatography
(ii) Partition chromatography

An electron a proton which one will have a higher velocity to produce matter waves of the same wavelength? Explain it

Given the formula of the species that will be isoelectronic with the following atoms or ions
(i) Ar (ii) F^- (iii) K⁺ (iv) S^-2

What are the uses of freons?

Calculate the molar volume of the following 3.0115 \(\times\)10²³ molecules of SO₂ gas

An atom of an element contains 29 electrons and 35 neutrons. Deduce
(i) the number of protons.
(ii) the electronic configuration of the element.

The energy of an electron in the ground state of the hydrogen atom is -2.18 x10^-18J. Calculate the ionisation energy of atomic hydrogen in J mol^-1

(i) Which is largest in size Cu⁺, Cu²⁺ or Cu and why?
(ii) Which element in periodic table has highest ionisation energy (IE)?
(iii) Which element is more metallic Mg or Al and why?

(i) State (n + 1) rule.
(ii) Arrange the orbials in the increasing order of energies based on (a) principal quantum number and (b) (n + 1) rule.

Explain how nitrobenzene and benzene are separated and purified. (or)
How will you separate the mixture of diethyl ether and ethanol?

Calculate the oxidation number of underlined atoms \(\underline { C } I{ O }_{ 3 }\)^-

Part - D

Generic 5 - Answer All Question

Distinguish between the following.
(i) Atomic and molecular mass
(ii) Atomic mass and atomic weight
(iii) Empirical and molecular formula
(iv) Moles and molecules.

Explain the types of substitution reaction?

How does classical smog differ from photochemical smog?

Give the uses of gypsum
Define ionic bond. Give suitable examples and distinguish between covalent bond and ionic bond.

Discuss in detail about the general methods of preparation of alkenes.

Explain the merits of Moseley's long form of periodic table.

Express mathematically Dalton's law of partial pressures.

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