Question # 1

In Bohr model of hydrogen atom the distance between adjacent orbits increases away from the nucleus, the energy difference between the orbits

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Increases

Decreases

Reaming same

Orbits coincide

The nature of the positive rays depend on

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The nature of the electrode

The nature of the discharge tube

The nature of the residual gas

All of the above

Which of the following is not a property of cathode rays

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They can produce x-rays when they strike a heavy metal anode

They can cause reduction reaction

They produce fluorescence in rare earth and minerals

They comprise neutral particles

Rutherford's model of atom failed because:

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The atom did o have a nucleus and electrons

It did not account fro the attraction b/w protons and neutrons

It did no account for the stability of the atom.

There is actually no space b/w the nucleus ad the electrons.

Charge to mass ratio (e/m) of the electron is determined by

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R. A. Millikan

J. J. Thompson

G. J, Stoney

None of these

The four quantum numbers of the valency electron of potassium are

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4,1,1,1/2

4,0,0,1/2

4,1,0,1/2

4,4,0,1/2

The rules which describe the distribution of electron in atomic energy levels are Auf-ban principle, Pauli's exclusion principle. Hunds rule. The pauli exclusion principle refers to the

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Orientation of orbital in space

Fact that two electrons in the same orbital should have opposite spins

Energy of the orbital

Spin of the electron

In Millikan method the oil droplet falls under the force of gravity but it moves upward due to

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Electric field

Magnetic field

Incident light

X-rays

The order of distance between the various Bohr orbits is

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r₂- r₁> r₃- r₂> r₄- r₃> ......

r₁> r₂> r₂- r₃> r₄-r₃> .....

r₂-r₁= r₃- r₂= r₄- r₃> .....

r₂- r₁> r₃- r₂< r₄- r₃< ....

In the ground state of an atom, the electron is present:

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In the nucleus.

In the second shell.

Nearest to the nucleus.

farthest from the nucleus.

In the atomic emission spectrum the lines which appear bright, appear dark in absorption spectrum because

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The radiations emitted in emission spectrum are absorbed in absorption spectrum

Atomic emission spectrum is continuous

Atomic absorption spectrum is continuous

Distance between the lines increases

The number of neutrons in the element ⁹₄Be is

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4

5

9

13

The mass of the neutron is of the order of

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10^-23kg

10^-24kg

10^-26kg

10^-27kg

The atomic number of an element is 35 what is the total number of electrons present in all the p-orbitals of the ground state atom of that element?

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6

11

17

23

If the value of azimuthal quantum number is 3, then values of m the magnetic quantum no. will be

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0, 1, 2, 3

+3, +2, +1, -1, -2, -3

0, -1, -2 ,-3

-3, 0, +3

The radius of first orbit of H-atom is

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4.75 A°

3.84 A°

8.4 A°

0.529 A°

The spectrum of helium is expected to be similar to that of

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H

Li⁺

Na

He⁺

Sodium chloride imparts a yellow colour to the Bunsen flame. This can be interpreted due to the

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low ionization energy of sodium

sublimation of metallic sodium to give yellow vapour

emission of excess energy absorbed as a radiation in the visible region as a radiation in the visible region

photosenitivity

Pauli's principle is applicable to

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Degenerate orbits

Two electrons in the same orbital

One electron

None

Which of the following is not charged particle

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Proton

Electron

Neutron

Hydrogen nucleus

Splitting of spectral lines when atoms are subjected to strong electric field is called:

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Zeeman effect.

Stark effect

Photoelectric effect.

Compton effect.

Which one of the following particles has amass 1/1836 time, that of hydrogen?

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Neutron.

Proton.

Electron.

Positron.

Charge to mass ratio of electron was discovered by:

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Millika.

Rutherford.

J.J. Thomson.

Chadwick.

n + l value for 4f will

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2

5

7

9

When the electron jumps form second third, fourth orbit to the fist orbit, the transitions are known as

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Balmer series

Lyman series

Pfund series

Brackett series

What is the packet of energy called?

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Electron

Photon

Positron

Proton

Neutrons was discovered by

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Mosely

Milliken

Chadwick

Ruherford

Electrons in degenerate orbitals are placed in separate orbitals with same spin according to

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Hund's rule

Pauli exclusion principle

Aufbau principle

Mosley's law

The wave number of light emitted by a certain source is 2 x 10⁵m. The wavelength of this light will be:

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500 NM.

500 M.

200 NM.

5 x 10⁷m

When electrons revolve in stationary orbits

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There is no change in energy level

They vecome stationary

They are gaining kinetic energy

There is increase in energy

Which of the following is not isoelectronic?

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Na⁺

Mg²⁺

O^2-

Cl^-

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