Physics

Electrostatics
Current Electricity
Magnetic Effects of Current and Magnetism
Electromagnetic Induction and Alternating Currents
Dual Nature of Matter and Radiation
Physical World and Measurement
Kinematics
Vectors
Laws of Motion
Work, Energy and Power
Motion of System of Particles and Rigid Body
Gravitation
Properties of Bulk Matter
Thermodynamics
Behaviour of Perfect Gas and Kinetic Theory
Oscillations and Waves
Electromagnetic Waves
Optics
Atoms and Nuclei
Electronic Devices & Semiconductor
Communication System
Physics

Chemistry

Hydrocarbons
Chemistry
Some Basic Concepts of Chemistry
Structure of Atom
Classification of Elements and Periodicity in Properties
Chemical Bonding and Molecular Structure
States of Matter: Gases and Liquids
Equilibrium
Redox Reactions
Hydrogen
s-Block Element (Alkali and Alkaline earth metals)
Some p-Block Elements
Organic Chemistry- Some Basic Principles and Techniques
Environmental Chemistry
Solid State
Solutions
Thermodynamics
Electrochemistry
Chemical Kinetics
Surface Chemistry
General Principles and Processes of Isolation of Elements
p-Block Elements
d and f Block Elements
Coordination Compounds
Haloalkanes and Haloarenes
Alcohols, Phenols and Ethers
Aldehydes, Ketones and Carboxylic Acids
Organic Compounds Containing Nitrogen
Amines
Biomolecules
Polymers
Chemistry in Everyday Life

Mathematics

Sets, Relations and Functions
Mathematical Reasoning
Statistics and Probability
Properties of Triangle
Vectors and Three-Dimensional Geometry
Linear Programming
Matrices and Determinants
Mathematics
Trigonometric Ratios & Identities
Algebra
Permutations and Combinations
Coordinate Geometry
Circle and System of Circles
Calculus
Logarithm, Indices, Surds and Partial Fraction
Progressions
Correlation and Regression

Q 1.

Correct4

Incorrect-1

Rutherford's experiment on scattering of {tex} { \alpha } {/tex} -particles showed for the first time that the atom has

electrons

protons

nucleus

neutrons

Q 2.

Correct4

Incorrect-1

The wavelength of a spectral line for an electronic transition is inversely related to:

the number of electrons undergoing the transition

the nuclear charge of the atom

the difference in the energy of the energy levels involved in the transition

the velocity of the electron undergoing the transition.

Q 3.

Correct4

Incorrect-1

The orbital diagram in which the Aufbau principle is violated is:

Q 4.

Correct4

Incorrect-1

The correct ground state electronic configuration of chromium atom is:

{tex} [ \mathrm { Ar } ] 3 d ^ { 5 } 4 s ^ { 1 } {/tex}

{tex} [ \text { Ar } ] 3 d ^ { 4 } 4 s ^ { 2 } {/tex}

{tex} [\text {Ar} ] 3 d ^ { 6 } 4 s ^ { 0 } {/tex}

{tex} [ \text {Ar} ] 4 d ^ { 5 } 4 s ^ { 1 } {/tex}

Q 5.

Correct4

Incorrect-1

The correct set of quantum numbers for the unpaired electron of chlorine atom is:

{tex} n : 2,\ l : 1,\ m : 0{/tex}

{tex} n : 2, \ l : 1, \ m : 1 {/tex}

{tex} n : 3 , \ l : 1 , \ m : 1 {/tex}

{tex} n : 3 , \ l : 0 , \ m : 0 {/tex}

Q 6.

Correct4

Incorrect-1

Which of the following does not characterise {tex} X {/tex}-rays?

The radiation can ionise gases

It causes ZnS to fluorescence

Deflected by electric and magnetic fields

Have wavelengths shorter than ultraviolet rays

Q 7.

Correct4

Incorrect-1

A {tex} 3 p {/tex} orbital has:

two non spherical nodes

two spherical nodes

one spherical & one non spherical node

one spherical and two non spherical nodes

Q 8.

Correct4

Incorrect-1

The orbital angular momentum of an electron in 2s orbital is:

{tex} + \frac { 1 } { 2 } \cdot \frac { h } { 2 \pi } {/tex}

{tex}\mathrm {Zero}{/tex}

{tex} \frac { h } { 2 \pi } {/tex}

{tex} \sqrt { 2 } \cdot \frac { h } { 2 \pi } {/tex}

Q 9.

Correct4

Incorrect-1

For a {tex} d {/tex}-electron, the orbital angular momentum is

{tex} \sqrt { 6 } ( h / 2 \pi ) {/tex}

{tex} \sqrt { 2 } ( h / 2 \pi ) {/tex}

{tex} ( h / 2 \pi ) {/tex}

{tex} 2 ( h / 2 \pi ) {/tex}

Q 10.

Correct4

Incorrect-1

The electrons, identified by quantum numbers {tex} n {/tex} and {tex} l , {/tex} (i) {tex} n = 4 , l = 1 , ( \text { ii } ) n = 4 , l = 0 , ( \text { iii) } n = 3 , l = 2 , \text { and (iv) } n = 3, {/tex} {tex} l = 1 {/tex} can be placed in order of increasing energy, from the lowest to highest, as

{tex} ( \mathrm { iv } ) < ( \mathrm { ii } ) < ( \mathrm { iii } ) < ( \mathrm { i } ) {/tex}

{tex}(\mathrm { ii }) < ( \mathrm { iv } ) < ( \mathrm { i } ) < ( \mathrm { iii } ) {/tex}

{tex} ( \text {i} ) < ( \text { iii } ) < ( \text {ii} ) < ( \text {iv} ) {/tex}

{tex} ( \text { iii) } < ( \text {i} ) < ( \text {iv} ) < ( \text {ii} ) {/tex}

Q 11.

Correct4

Incorrect-1

The number of nodal planes in a {tex} p _ { x } {/tex} orbital is

one

two

three

Zero

Q 12.

Correct4

Incorrect-1

The wavelength associated with a golf ball weighing {tex} 200\ \mathrm { g } {/tex} and moving at a speed of {tex} 5\ \mathrm { m } / \mathrm { h } {/tex} is of the order

{tex} 10 ^ { - 10 } \mathrm { m } {/tex}

{tex} 10 ^ { - 20 } \mathrm { m } {/tex}

{tex} 10 ^ { - 30 } \mathrm { m } {/tex}

{tex} 10 ^ { - 40 } \mathrm { m } {/tex}

Q 13.

Correct4

Incorrect-1

The quantum numbers {tex} + 1 / 2 {/tex} and {tex} - 1 / 2 {/tex} for the electron spin represent

rotation of the electron in clockwise and anticlockwise direction respectively

rotation of the electron in anticlockwise and clockwise direction respectively

magnetic moment of the electron pointing up and down respectively

two quantum mechanical spin states which have no classical analogue

Q 14.

Correct4

Incorrect-1

Rurtherford's experiment, which established the nuclear model of the atom, used a beam of

{tex}\beta{/tex}-particles, which impinged on a metal foil and got absorbed

{tex}\gamma{/tex}-rays, which impinged on a metal foil and ejected electrons

helium atoms, which impinged on a metal foil and got scattered

helium nuclei, which impinged on a metal foil and got scattered

Q 15.

Correct4

Incorrect-1

If the nitrogen atom has electronic configuration {tex} 1 s ^ { 7 } , {/tex} it would have energy lower than that of the normal ground state configuration {tex} 1 s ^ { 2 } 2 s ^ { 2 } 2 p ^ { 3 } , {/tex} because the electrons would be closer to the nucleus. Yet {tex} 1 s ^ { 7 } {/tex} is not observed because it violates.

Heisenberg uncertainty principle

Hund's rule

Pauli exclusion principle

Bohr postulate of stationary orbits

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