# Plus One Chemistry Model Question Paper 1

## Kerala Plus One Chemistry Model Question Paper 1

Time Allowed: 2 hours
Cool off time: 15 Minutes
Maximum Marks: 60

General Instructions to candidates

• There is a ‘cool off time’ of 15 minutes in addition to the writing time.
• Use the ‘cool off time’ to get familiar with questions and to plan your answers.
• Read the instructions carefully.
• Calculations, figures and graphs should be shown in the answer sheet itself.
• Malayalam version of the questions is also provied.
• Give equations wherever necessary.
• Electronic devices except non programmable calculators are not allowed in the Examination Hall.

Answer all questions from question numbers 1 to 7. Each carry one score.

Question 1:
Give the equation showing relation between empirical formula and molecular formula of a compound.

Question 2:
Which of the following transition of electron in the hydrogen atom will emit maximum energy ?
i. n5 → n4
ii. n4 → n3
iii. n3 → n2
iv. same in all transition

Question 3:
The geometry and type of hybridisation of central atom in BF3 are
i. linear, SP
ii. tetrahedral, SP3
iii. trigonal planar,SP2
iv. Pyramidal, SP3

Question 4:
Arrange the following elements in the increasing order of first ionisation energy: Li, Be,B

Question 5:
The compressibility factor of an ideal gas is …………

Question 6:
What is the molecular formula of Buck ministers fullerene ?

Question 7:
Ozone layer depletion in Antarctica is due to the formation of the compound
i. acrolein
ii. formaldehyde
iii. SO2 and SO3
iv. chlorine nitrate

Answer any ten from question numbers 8 to 20. Each carries two scores.

Question 8:
In the two oxides of carbon, the mass ratio of oxygen is 1.33 : 2.66. Identify the law illustrated by the above ratio and state the law.

Question 9:
Using s, p, d notation describe the orbitals with following set of quantum number.

Question 10:
A set of molecules are given below:
NaCl, O2, KCl, BF3, PCl5
a. Classify the molecules into ionic and covalent compounds.
b. Classify the above molecules into those obeying octet rule and those not obeying octet rule.

Question 11:
Identify the extensive and intensive properties from the following :
density, internal energy, heat capacity, molar heat capacity

Question 12:
Match the following:

Question 13:
Derive the relation between Kp and Kc of a gaseous reversible reaction.

Question 14:
a. What is Buffer solution ?
b. How a basic buffer can be prepared ?

Question 15:
Briefly explain the bonding in diborane.

Question 16:
Nitrogen, sulfur, halogen and phosphorous present in an organic compound are detected by Lassaigne’s test. Explain Lass aignes test for detecting nitrogen?

Question 17:
Write Van der Waals equation for one-mole gas and also write the physical significance of Van der Waals constants,

Question 18:
Complete the reaction.

Question 19:
Predict the products formed by addition reaction of HBr to but -1- ene in the presence of peroxide and in the absence of peroxide.

Question 20:
Give any two importance of green chemistry in day-to-day life.

Answer any seven from question numbers 21 to 29. Each carries three scores.

Question 21:
Calculate the number of atoms in each of the following.
a. 14 g of Nitrogen (N2).
b. 14 mole atom Nitrogen (N2)
c. 14 U of Nitrogen (N2).

Question 22:
a. Identify the position of the elements in the periodic table having outer electronic configuration.
i. ns2np4 with n = 3
ii. (n-1)d2 ns2 with n=4.
b. “Removal of electron from an atom become easier on moving down the group.” Give reason.

Question 23:
a. Write the two postulates of Kinetic molecular theory of gases responsible for deviation of real gases from ideal behaviour.
b. What is Boyle point ?

Question 24:
a. Derive the equaion for Gibbs energy change (∆G ) in terms of ∆H and ∆S.
b. Write any two condition for which G becomes negative according to Gibbs equation.

Question 25:
Decomposition of PC15 can be represented as
PCl5(g) → PCl3(g)+ Cl2(g)

∆H = 124.0KJmol-1
Describe the effect of the following on the above equilibrium ?
a. addition of PCl5
b. increase in pressure.
c. increase in temperature

Question 26:
Explain the following reactions.
a. CO is heated with ZnO
b. Boric acid is added to water
c. BF3 with NaH.

Question 27:
Balance the following redox reaction using oxidation number or ion-electron method :

Question 28:
What causes the temporary and permanent hardness of water ? Give one method to remove permanent hardness ?

Question 29:
Analyze the given compound.
C2H5C(CH3) = C(CH3)C2H5
a. Write the IUPAC name of the compound.
b. Draw the structures of the geometrical isomers possible for the compound.

Answer any three from question numbers 30 to 33. Each carries four scores.

Question 30:
a. Write the Schrodinger wave equation and explain the terms.
b. Draw the boundary surface diagrams of any four 3d orbitals.

Question 31:
Compare the relative stability of the following species and indicate their magnetic properties based on molecular orbital theory.
O2 and O2+

Question 32:
By passing Cl2 gas through a solution, gets bleaching powder
a. Write the balanced chemical equation for above reaction.
b. What happens if CO2 gas is passed instead of Cl2 and write the balanced chemical equation.

Question 33:
Which of the following carbocation is most stable ?
(CH3)3C+, (CH3)2CH+, CH3CH2CH2+
b. Write the principle involved in the distillation of organic compound under reduced pressure ? Give an example.

Relation between empirical and molecular formula,
MF = (EF) x n
Where n is a simple whole number

n3 → n2

Triagonal planar, SP2

Be > B > Li

The deviation from ideal behaviour is measured in terms of compressibility factor Z, which is the ratio of product PV and nRT.

C60

Chlorine nitrate

Law of Multiple Proortions
According to this law, if two elements can combine to form more than one compound the masses of one element that combine with a fixed mass of the other element are in the ratio of small whole numbers.

a. 4P
b. 3d

a. lonic : NaCl, KCl
Covalent: BF3, PCl53, O2
b. Obeying octet rule – NaCl, KCl, O2
Not obeying Octet rule : BF3, PCl5

Extensive : Heat capacity, Internal energy
Intensive : density, molar heat capacity

Kp = Kc (RT)∆n

a. The solutions which resist change in pH on dilution or with the addition of small amounts of acid or alkali are called Buffer Solutions.
b. Basic buffer : Buffer mixture of a weak base and its salt with a strong acid,
e.g., NH4OH and NH4Cl (pH = 9.25)

In boron atom lies one plane. Above and below this plane, there are 2 bridging H- atom. Each bridged H atom is bonded to 2 boron atom only by sharing of 2 electrons. Such a bond is called 3 centered 2 electron bond. Thus diborane have two (B-H-B) bonds, ie., two 3-centered 2 electron bond and four (B-H) bonds, ie., four 2 centered 2 electron bond.

By fusing organic compound with sodium metal, the elements present in the compound forms corresponding water soluble salts.

Detection of Nitrogen:
N exist as NaCN in sodium fusion extract.

On heating with con.H2SO4, Fe2+ oxidised to Fe3+ to give prussion blue in colour.

Detection of Halogens:
Halogen exist as halides (max.) in fusion extract. Mien AgNO3 and HNO3 is added they form AgX.
X + Ag+ AgX; (X = Cl, Br, I)
AgCl – white ppt
Agl – yellow ppt
AgBr – pale yellow

Detection of Suphur:
Sulphur as Na2S is fusion extract when sodium nitroprusside added gives violet colour.
Na2S + Na2[Fe(CN)5N0)] → Na4[Fe(CN)5 NOS] (violet colour)

Detection of Phosphorus:
The compound is heated with oxidising reagent (Sodium peroxide). The phosphorous present in the compound is oxidised to phosphate. The solution is boiled with nitric acid and then treated with ammonium molybdate. A yellow colouration or precipitate indicates the presence of phosphorus.

There is deviation from ideal behaviour at high pressure and low temperaure. This is due to two faulty assumptions in kinetic theory of gases. It is corrected by van der Waal’s equation.

where n is the number of moles of the gas a and b are van der Waal’s constants.

Dry cleaning of clothes. Tetra chloro ethene (Toxic and contaminates ground water) which is used as solvent for dry cleaning is replaced by liquified CO2.
• Bleaching of paper. Cl2 gas is replaced H2O2.
• Synthesis of chemicals.

i. 1s2 2s2 2p6 3s2 3p4
Block – p block
Atomic number – 16
Group – 16th group
Period – 3
Element – Sulphur

ii. 1s2 2s2 2p6 3s2 3p6 3d2 4s2
Block – d block
Atomic number – 22
Group – 4 th group
Period – 4
Element – Ti

b. Down a group, the outermost electron being increasingly farther from the nucleus, there is an increased shielding of the nuclear charge by the electrons in the inner levels. In this case increase in shielding out weights the increasing nuclear charge and the removal of the outermost electrons requires less energy down a group.

a. Maxwell, Boltzmann and others put forward a theoretical model of the gas. The theory is known as kinetic molecular theory of gases or microcopic model of gases.

Postulates of kinetic molecular theory are:
• All gases are made up of a large number of extremely small particles called molecules.
• The molecules are separated from one another by large distances so that the actual volume of the molecules is negligible as compared to the total volume of gas.
• The molecules are in a state of continuous rapid motion in all directions. During their motion, they keep on colliding with one another and also with the walls of the container.

b. The temperature at which a real gas obeys ideal gas law over an appreciable range of pressure is called Boyle temperature or Boyle point.

a. Neither decrease in enthalpy nor increase in entropy alone can determine the direction of spontaneous hange for these systems. For this purposes, we define a new thermodynamic function the Gibbs energy or Gibbs function, G as
G = H – TS
The change in Gibbs energy for the system
∆Gsys = ∆Hsys – T∆Ssys – Ssys ∆T
At constant temperature, ∆T = 0
∆Gsys = ∆Hsys

Usually the subscript ‘ system’ is dropped and we simply write this equation as
∆G = ∆H – T∆S
Gibbs energy change = enthalpy change – temperature x entropy change.
It is reffered to as the Gibbs equation.
b. 1. ∆G is always -ve for a spontaneous process.
2. ∆G became negative for a reactions which are spontaneous only at a low temperature.

a. Shift the equilibrium in the forward reaction
b. Increase of pressure shift the equilibrium towards left (backward direction) where then no.of particle is less.
c. Increasing temperature shift the equilibrium in the forward direction as it is endothermic.

a. ZnO(s) + CO (g) $$\underrightarrow { \Delta }$$ Zn(s) + C02
Extraction of metals

b. When boric acid is added to water, it accepts electrons from -OH ion. Boric acid is sparingly soluble in cold water i however fairly soluble in hot water, boric acid behaves as a weak monobasic acid. It doesn’t act as proton donor, beh- 0 aves as a lewis acid, it accepts a pair of electrons.
B(OH)3 + 2HOH → [B(OH)4] + H3O+
450 A:
c. 2BF3 + 6 NaH $$\underrightarrow { 450K }$$ B2H6 + 6 NaF
Diborane is produced on an industrial scale by the reaction of BF3 with sodium hydride.

Temporary hardness is due to presence of bicarbonates of Ca and Mg in water. Permanent hardness is due to presence of chlorides and sulphates of Ca and Mg in water. Permanent hardness re¬moved by ion exchange method or permutit process (Zeolite).

a. Erwin Schrodinger developed an atomic model taking into account both the wave and particle nature of elecron. This equation is known as shrodinger wave equation. For a system the schrodinger equation is written as
H$$\Psi$$ = E$$\Psi$$, where h is a mathematical operatior called Hamiltonian. Schrodinger gave a recipe of constructing this operator from the expression for the total energy of the system. The total energy of the system takes into accountthe kinetic energiesofallthe subatomic particles attractive potential bet-ween the electrons and nuclei and repuisive potential among the electrons and nuclei individually. Solution of this equation gives E and $$\Psi$$.