F.Sc. Part 1 Chemistry.Ch.05.Test (Malik Xufyan)

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Maliks Chemistry -9 Class
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Maliks Chemistry - F.Sc. l
Maliks Chemistry- F.Sc. ll
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Maliks Chemistry - F.Sc. l
Maliks Chemistry- F.Sc. ll
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Malik Xufyan
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Chapter # Topic Page #
Basic concepts – Unsolved paper1
2
3
4
5
6
7
8
9
10
11
5
6
16
17
24
25
36
37
45
46
54
55
64
65
73
74
83
84
93
94
103
104
Experimental Techniques – Solved Paper
Gases – Unsolved Paper
Gases – Solved Paper
Liquid – Unsolved Paper
Liquid – Solved Paper
Atomic Structure – Unsolved Paper
Atomic Structure – Solved Paper
Chemical Bonding –Unsolved Paper
Chemical Bonding – Solved Paper
Thermochemistry – Unsolved Paper
Thermochemistry – Solved Paper
Chemical Equilibrium – Unsolved Paper
Chemical Equilibrium – Solved Paper
Solu on – Unsolved Paper
Solu on – Solved Paper
Electrochemistry – Unsolved Paper
Electrochemistry – Solved Paper
Chemical Kine cs – Unsolved Paper
Chemical Kine cs – Solved Paper
Basic concepts – Solved Paper
Experimental techniques – Unsolved Paper
INDEX

Chapter#5: Atomic Structure Malik Chemistry
Jhang Institute for Advanced46
Name : CH # Atomic Structure Class 11th
Chemistry Test # 05 , CH # 05 (Complete) Marks : 85
Time : 2 & Half Hour Objective & Subjective JIAS Test System
Section-1: Objective
Choose the correct answer 17 x 1=17
Sr # Statement A B C D
1. The nature of cathode rays depends upon Nature of electrode Nature of
discharge tube
Nature of
residual gas
All
2. When 6d orbital is complete ,entering electron
goes into
7f 7s 7p 7d
3. The nature of positive rays depends on Voltage applied Nature of
discharge tube
Nature of
electrode
Nature of
residual gas
4. If an elecrtron is free from attraction of nucleus
then its energy is
Negative Positive Zero None of these
5. Gases conduct electricity at High pressure Ordinary pressure Low pressure Normal
pressure
6 The quantum number which describes the
shape of an orbital is called
Principal quantum
number
Azimuthal
quantum number
Magnetic
quantum
number
Spin quantum
number
7. Quantum number values for 2p orbital are N=2, l=1 N=1,l=2 N=1 l=0 N=2,l=0
8. Lymann series lies in UV region Visible region IR region None of these
9. Photons of green colour are more energetic than
those of
Violet color Blue colour Red colour Indigo colour
10. An orbital can have maximum number of
electrons is
2 4 6 10
11. Inverse of wavelength is called Frequency Wave number Time period All of these
12. The sub shellwhich has only one orbital is
identified by the letter
s p D F
13. Electron behave like Particle Wave Both Non meterial
14. P-orbital have …….shape Spherical Dumbbell Sausage Even more
complicated
15. If n=3 then l= 0,1,2 1,2,3 _2,_3,0,1,2 -3,-2,-1,3,2,1
16. Energy of photon is inversely proportional to Frequency mass Wave number Wavelength
17. Which atomic orbital has lowest energy? 4f 5d 6p 7s

Jhang Institute for Advanced Studeies 47
Section-Il: Short questions
2. Attempt only EIGHT questions. 8 x 2= 16
i. How the idea of the proton can be verified by taking hy-
drogen gas in the discharge tube?
ii. Why e/m value of the cathode rays is just equal to that of
electron?
iii. Why positive rays are also called canal rays?
iv. The e/m value for positive rays obtained from hydrogen
gas is 1836 times less than that of cathode rays. Justify it.
v. Why is it necessary to decrease the pressure in the dis-
charge tube to get the remains the same?
vi. How do you justify that radius of orbit in H-atom is in-
versely proportional to the number of proton in the nu-
cleus?
vii. What is the function of azimuthal quantum number?
viii.State Pauli’s exclusion principle,
ix. What is stark effect and Zeeman Effect?
x. Define spectrum. Give its two types.
xi. Differentiate between slow and fast neutrons.
xii. Describe electrons in orbital’s of 24
Cu and 29
Cr
3. Attempt only 8 questions 8 X 2 = 16
i. What is aufbau principle?
ii. What is self rotation of electron?
iii. Give the relationship between energy and frequency.
iv. Give two defects of Rutherford atomic model?
v. Why e/m value of cathode rays is the same for all gases?
vi. What is frequency and wavelength?
vii. Write de-Broglie equation .What does it show?
viii.Gases do not conduct electricity at normal pressure.
Why?
ix. What are the bases of Schrodinger wave equation?
x. Define Heisenberg principle. Give mathematical relation?
4. Attempt any 6 questions 6 x 2 = 12
i. Define Hund’s rule and give example.
ii. What particles are formed by the decay of free neutron?
iii. Give two defects of Bohr’s model?
iv. Write balanced equation for two nuclear reaction.
v. Total energy of the bounded electron is also negative?
vi. Compare line emission and line absorption spectrum?
vii. Give the postulates of Bohr’s atomic orbital. Which pos-
tulate tells us that the orbits are stationary and energy is
quantized?
viii.What is the formula for calculating the energy of elec-
tron?
ix. What are quantum numbers give their significance.
x. Give some properties of cathode rays?
Section-lIl: Long Questions.
Attempt any THREE questions. 8 x 3 = 24
5) A) Calculate the value of principal quantum number if an
electron in hydrogen atom revolves in an orbit of energy
-0.242 x10-18
J
b) Justify that the energy difference between 2nd
and 3rd
orbits is approximately five times small-
er than that between 1st
and 2nd
orbit.
6) a ) Derivation of radius of revolving electron in nth or-
bit?
b) Measurement of charge on electron by Mil-
likan oil drop method .
7) a) Write a detailed note on production of x-rays. In-
cluding importance of Mosley’s law?
b) write electronic configuration of elements hav-
ing following atomic numbers
22, 23, 36,30,15,19.29,24,34,11,3. Also name the el-
ements having above mentioned atomic num-
bers.
8) a) Write a note on any two Quantum Numbers.
b) Rutherford’s atomic model is based on the
scattering of alpha particles from a thin gold
foil. Discuss it and explain the conculsion.
9) a) Explain the discovery of neutron and their properties.
b)What is J,J Thomson experiment for determining e/m
value of electron? And explain postulates of Bohr’s
atomic modal.

Section-l: Short questions
2. Attempt only EIGHT questions. 8 x 2= 16
i. How the idea of the proton can be verified by taking hydrogen gas in the discharge tube?
Ans: Positive Rays are produced, when high speed cathode rays (electrons) strike the molecules of a gas
enclosed in the discharge tube. They knock out electrons from the gas molecules and positive ions are
produced, which start moving towards the cathode.
M + e -
M+
+ 2e-
ii. Why e/m value of the cathode rays is just equal to that of electron?
Ans:A cathode ray consists of beam of electrons, so cathode rays are actually electrons. The e/m of cath-
ode rays is 1.7588 x 1011
C/Kg which is equal to e/m of electron. Therefore e/m value of cathode ray is
just equal to that of electron.
iii. Why positive rays are also called canal rays?
Ans: Since positive rays produced in the discharge tube passed through the canals or holes of cathode,
therefore positive rays are also called canal rays.
iv. The e/m value for positive rays obtained from hydrogen gas is 1836 times less than that of cathode
rays. Justify it.
Ans: The mass of hydrogen gas is 1836 times more than that of an electron. Cathode rays consist of beam
of electrons. The e/m value for positive rays depends upon the gas used in the tube, and e/m value for
cathode rays is independent of the nature of the gas. Therefore e/m value for positive rays obtained
from H2
gas is 1836 times less than that of cathode rays. Heavier the gas, the smaller the e/m value for
positive rays.
v. Why is it necessary to decrease the pressure in the discharge tube to get the remains the same?
Ans: The current does not flow through the gas at ordinary pressure even at high voltage about 500 volts.
However when the pressure inside the tube is decreased, the gas in the tube begins to conduct electric-
ity at low pressure. Therefore it is necessary to decrease the pressure in the discharge tube to get the
cathode rays.
vi. How do you justify that radius of orbit in H-atom is inversely proportional to the number of proton
in the nucleus?
Ans: According to radius of orbital:
In the above equation , h , and e are constantfactors and if we also fixed the orbit number ‘n’ then we
can write as
where z is number of protons in nucleus. Hence radius is inversely proportional to the number of protons
in the nucl eus.
vii. What is the function of azimuthal quantum number?

Ans: It determines the shape of orbital. It can have any integer value from 0 to n–l. This quantum number
is used to represent the sub–shells, and these value are l = 0, 1, 2, 3. These values represent different sub–
shells which are designated as s, p, d, and f, with values of l = 0, 1, 2, 3 respectively.
viii. State Pauli’s exclusion principle.
Ans: It is impossible for two electrons residing in the same orbital of a poly-electron atom to have the
same values of four quantum numbers. Or
Two electrons in the same orbitals should have opposite spins (↑↓).
ix.What is stark effect and Zeeman Effect?
Ans:
Zeeman Effect: When the excited atoms of hydrogen are placed in a magnetic field, its spectral lines are
further split up in to closely spaced lines. This type of splitting of spectral lines is called Zeeman Effect.
Stark Effect: When the excited hydrogen atom are placed in an electric field, its spectral lines are further
split up into closely spaced lines. This type of splitting of spectral lines is called stark effect.
x. Define spectrum. Give its two types.
Ans:
Spectrum: The dispersion of the components of white light, when it is passed through prism is called
spectrum. The distribution among various wavelengths of the radiant energy emitted or absorbed by an
object is also called spectrum.
Types: (A) Continuous spectrum (B) Line spectrum
xi. Differentiate between slow and fast neutrons.
Ans:
Sr # Fast Neutrons Slow neutrons
1. Those neutrons which travel with an
energy of 1.2 Mev are called as fast
neutrons.
Those neutrons which travel with
an energy of 1 ev are called slow
neutrons.
2. The fast neutrons are not used in
fission reactions because these are
absorbed by the nucleus of the atom
and simply change their path on
colliding with nucleus, therefore
they don’t cause the fission reaction
The slow neutrons are extensively
used in fission reactions because
these can easily penetrate into the
nucleus and thus cause nuclear
fission reactions.
xii. Describe electrons in orbital’s of 24
Cu and 29
Cr
Ans : 29
Cu = 1s2
, 2s2
, 2p6
, 3s2
3p6
, 3d10
, 4s1
24
Cr = 1s2
, 2s2
, 2p6
, 3s2
3p6
, 3d5
, 4s1
3. Attempt only 8 questions 8 X 2 = 16
i. What is aufbau principle?
Ans: The electrons shall be filled in energy sub shells in order of increasing energy values. The electrons
are first placed in 1s, 2s, 2p and so on.
ii. What is self rotation of electron?
Ans: In 1925, Goudsmit and Uhledbech suggested that an electron while moving in an orbital around the
nucleus also rotates or spin about its own axis either in a clockwise or anti-clockwise direction, this is
called self rotation.
iii. Give the relationship between energy and frequency.
Ans: According to planks quantum theory, the amount of energy associated with a quantum of radiation

is proportional to the frequency (ν) of the radiation.
Mathematically
where h is planks constant and its value is 6.626 x 10-24
js
iv. Give two defects of Rutherford atomic model?
Ans:
Defects of Rutherford’s atomic model:
• In this model, behavior of electrons remained unexplained in the atom.
• Ruther ford’s planet like picture was defective and unsatisfactory because the moving electron must be
accelerated towards the nucleus. Therefore the radius of the orbiting electrons should become smaller
and smaller and the electron should fall into the nucleus. Thus an atomic structure as proposed by
Rutherford would collapse.
v. Why e/m value of cathode rays is the same for all gases?
Ans:
The e/m value of positive rays depends upon the nature of gas used in the discharge tube. The charac-
teristic of the gas varies from gas to gas, but for cathode rays e/m value is independent of the nature of
the gas. Therefore, e/m values of positive rays for different gases are different but those for cathode rays
the e/m value is the same.
vi. What is frequency and wavelength?
Ans: Frequency (V):
The number of waves passing through a point per second is called frequency (ν). Its units are cycles s–1
.
Wavelength (λ):
The distance between two successive crests or troughs is called wavelength “λ” and is expressed in Ao
or nm.
vii. Write de-Broglie equation .what does it show?
According to de Broglei, all matter particles in motion have a dual character. It means that electrons,
protons, neutrons, atoms, and molecules, possess the characteristics of both the material particle and a
wave. This is called wave particle duality in matter.
de-Broglei derived a mathematical equation which relates the wavelength (λ) of the electron to the
momentum of electron (mv)
Where
λ = wavelength
v = velocity of electron
m = mass of electron and
h = Planck’s constant.
viii. Gases do not conduct electricity at normal pressure. Why?
Ans: At low pressure, gases molecules are away from each other, that’s why gases cannot conduct cur-

rent at normal pressure.
ix. What are the bases of Schrodinger wave equation?
Ans:
according to schrodinger, although the position of an electron cannot be found exactly, the probability
of finding an electron at a certain position at any time can be found.
The solution of the wave equation gives probability of an electron at a distance r from the nucleus is
calculated for the hydrogen atom in the ground state is obtained.
x. Define Heisenberg principle. Give mathematical relation?
Ans:
Heisenberg showed that it is impossible to determine simultaneously both the position and momen-
tum of an electron. Suppose that Δx is the uncertainty in the measurement of the position and Dp is
the uncertainty in the measurement of momentum of an electron.
This relationship is called uncertainty principle.
xi. What are continuous and line spectrum?
Ans:
Continuous spectrum:
A spectrum containing light of all wavelengths is called continuous spectrum. In this type of spectrum,
the boundary line between the colours cannot be marked. The colours diffuse into each other. One co-
lour merges into another without any dark space. The best example of continuous spectrum is rainbow.
Line spectrum:
When an element or its compound is volatilized on a flame and the light emitted is seen through, a
spectrometer. We see distinct lines separated by dark spaces. This type of spectrum is called line spec-
trum. This is the characteristic of an atom.
3. Attempt any 6 questions 6 x 2 =12
i. Define Hund’s rule and give example .
Ans:
If, degenerate orbitals are available and more than one electrons are to be placed in them, they should
be placed in separate orbitals with the same spin rather putting them in the same orbital with opposite
spins.
According to the rule, the two electrons in 2p subshell of carbon will be distributed as follows
C = 1s,2s,2px
,2py
,2pz
The three orbitals of 2p subshell are degenerate.
ii. What particles are formed by the decay of free neutron?
iii. Give two defects of Bohr’s model?
Defects:
1. Bohr’s theory can successfully explain the origin of the origin of the spectrum of H-atom and ions
like He+1
Li+2
and Be+3
etc. These are all one electron systems. But this theory is not able to explain
the origin of the spectrum of multi-electrons or poly-electrons system like He , Li and Be etc.
2. Bohr Suggested that circular orbits of electrons around the nucleus of Hydrogen atom, but researches
have shown that the motion of electron is not in a single plane, but takes place in three dimensional

space. Actually, the atomic model is not flat.
iv. Write balanced equation for two nuclear reaction.
Ans:
v. Total energy of the bounded electron is also negative?
Ans: The total energy of bounded electron is negative because the electron is under the force of attraction
of the nucleus to have a stable state of the atom. More over when we calculate the total energy of the
bounded electron, which is the sum of K.E. and P. E comes which is also negative.
vi. Compare line emission and line absorption spectrum.
Ans.
Sr # Line emission spectrum Line absorption spectrum
1. An atomic spectrum which consists of bright
lines against a dark background is called line
emission spectrum.
An atomic spectrum which consists of bright
lines against a dark background is called line
emission spectrum.
2. When solids are volatilized or elements in their
gaseous states are heated to high temperature or
subjected to an electrical discharge, radiation of
certain wavelengths are emitted.
When a beam of white light is passed through
the gaseous sample of element, the element
absorbs certain wavelength while the rest of
wavelengths pass through it.
vii. Give the postulates of Bohr’s atomic orbital. Which postulate tells us that the orbits are station-
ary and energy is quantized?
Ans:
Electrons present in a particular orbit neither emits nor absorbed energy while moving in the same
fixed orbits. The energy is emitted or absorbed only when an electron jumps from one orbit to another.
viii. What is the formula for calculating the energy of electron?
Ans:
The energy of electron in different orbits can be calculated by using the following equation:
Energy of an electron is inversely proportional to n2
ix. What are quantum numbers give their significance.
Ans:
Quantum Numbers:
Quantum numbers are the set of numerical values which give the acceptable solutions to Schrodinger

wave equation for hydrogen atom.
Significance:
a) These numbers describe the behavior of electron in an atom completely.
b) These numbers tells us about the size, shape, spin of shell and subshell of atom.
c) Quantum tells us about the completely address of electron in an atom.
x. Give some properties of cathode rays.
Ans:
Properties of cathode rays:
• They are produced by the negative electrode, or cathode, in an evacuated tube, and travel towards the
anode.
• They travel in straight lines and cast sharp shadows.
• They have energy and can do work.
• They are deflected by electric and magnetic fields and have a negative charge
Section-ll: Long Questions. 8 x 3 = 24
5) a) Calculate the value of principal quantum number if an electron in hydrogen atom revolves in an
orbit of energy -0.242 x10-18
J.
b) Justify that the energy difference between 2nd
and 3rd
orbits is approximately five times smaller than that
between 1st
and 2nd
orbit.
6) a) Derivation of radius of revolving electron in nth
orbit?
b) Measurement of charge on electron by Millikan oil drop method.
7) a) Write a detailed note on production of x-rays including importance of Mosley’s law?
b) Write electronic configuration of elements having following atomic numbers
22, 23, 36, 30, 15, 19, 29, 24, 34, 11, 3.Also name the elements having above mentioned atomic numbers.
8) a) Write a note on any two Quantum Numbers.
b) Rutherford’s atomic model is based on the scattering of alpha particles from a thin gold foil. Discuss it
and explain the conclusion.
9) a) Explain the discovery of neutron and their properties.
b) What is J.J Thomson experiment for determining e/m value of electron? Explain postulates of Bohr’s
atomic modal.

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