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The theoretical and experimental values of Rydberg constant are different.

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Important Questions on Structure of Atom

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Chemistry>Physical Chemistry>Structure of Atom>Bohr's Atomic Model and its Limitations

Which of the following statements is false?

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Chemistry>Physical Chemistry>Structure of Atom>Bohr's Atomic Model and its Limitations

The ground state energy of a hydrogen atom is

- 13 .6 eV

. The energy of second excited state of

{He}^{+}

ion in

eV

is:

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Chemistry>Physical Chemistry>Structure of Atom>Bohr's Atomic Model and its Limitations

If the de Broglie wavelength of the electron in

n^{t h}

Bohr orbit in a hydrogenic atom is equal to

1.5 π a_{0}

(a_{0}

is Bohr radius

)

, then the value of

\frac{n}{z}

is:

EASY

Chemistry>Physical Chemistry>Structure of Atom>Bohr's Atomic Model and its Limitations

If the radius of the hydrogen atom is

53 pm

, the radius of the

{He}^{+}

ion is closest to:

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Chemistry>Physical Chemistry>Structure of Atom>Bohr's Atomic Model and its Limitations

What would be the wavelength of the spectral line in Balmer series of the spectrum, having the longest wavelength? Given

R_{H} = 109677 {cm}^{- 1}

EASY

Chemistry>Physical Chemistry>Structure of Atom>Bohr's Atomic Model and its Limitations

The radii of the first Bohr orbit of

H (r_{H}), {He}^{+} (r_{{He}^{+}}^{})

and

{Li}^{2 +} (r_{{Li}^{2 +}}^{})

are in the order

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Chemistry>Physical Chemistry>Structure of Atom>Bohr's Atomic Model and its Limitations

A particle of mass

m

moves in a circular orbit in a central potential field

U (r) = \frac{1}{2} k r^{2} .

If Bohr's quantization conditions are applied, radii of possible orbitals and energy levels vary with quantum number

n

as:

HARD

Chemistry>Physical Chemistry>Structure of Atom>Bohr's Atomic Model and its Limitations

A neutron moving with a speed 'v' makes a head on collision with a stationary hydrogen atom in ground state. The minimum kinetic energy of the neutron for which perfactly inelastic collision will take place is :

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Chemistry>Physical Chemistry>Structure of Atom>Bohr's Atomic Model and its Limitations

In the atomic spectrum of

H

, lines were observed at

\frac{5}{36} R, \frac{3}{16} R, \frac{21}{100} R and \frac{2}{9} R

(

R =

Rydberg constant). It belongs to....... series

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Chemistry>Physical Chemistry>Structure of Atom>Bohr's Atomic Model and its Limitations

For emission line of atomic hydrogen from

n_{i} = 8

n_{f} = n,

the plot of wave number

(\bar{v})

against

(\frac{1}{n^{2}})

will be: (The Rydberg constant,

R_{H}

is in wave number unit)

EASY

Chemistry>Physical Chemistry>Structure of Atom>Bohr's Atomic Model and its Limitations

The electron in the hydrogen atom undergoes transition from higher orbitals to orbital of radius

211.6 pm

. This transition is associated with

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Chemistry>Physical Chemistry>Structure of Atom>Bohr's Atomic Model and its Limitations

If the wavelength of an electronic transition in

{He}^{+}

23 nm

, the wavelength corresponding to same transition in hydrogen atom in

nm

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Chemistry>Physical Chemistry>Structure of Atom>Bohr's Atomic Model and its Limitations

The energy of an electron in first Bohr's orbit of H atom is

- 13.6 eV .

The energy value of electron in the first excited state of

{Li}^{2+}

is :

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Chemistry>Physical Chemistry>Structure of Atom>Bohr's Atomic Model and its Limitations

The radius of the second Bohr orbit for hydrogen atom is

(Planck's constant,

(h) = 6 .6262 \times 10^{- 34} Js;

mass of electron

= 9 .1091 \times 10^{- 31} kg;

charge of electron

= 1 .60210 \times 10^{- 19} C;

permittivity of vacuum,

(\in_{0}) = 8 .854185 \times 10^{- 12} {kg}^{- 1} m^{- 3} A^{2}

)

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Chemistry>Physical Chemistry>Structure of Atom>Bohr's Atomic Model and its Limitations

The ionization energy of gaseous $Na$ atoms is $495.5 kJ {mol}^{- 1}$ . The lowest possible frequency of light that ionizes a sodium atom is

$(h = 6.626 \times 1 0^{- 34} Js, N_{A} = 6.022 \times 1 0^{23} {mol}^{-1})$

HARD

Chemistry>Physical Chemistry>Structure of Atom>Bohr's Atomic Model and its Limitations

Consider the Bohr's model of a one-electron atom where the electron moves around the nucleus. In the following List-I contains some quantities for the

n^{t h}

orbit of the atom and List-II contains options showing how they depend on

n

List - I	List - II
(I) Radius of the $n^{t h}$ orbit	$(P)$ $\propto n^{- 2}$
(II) Angular momentum of the electron in the $n^{t h}$ orbit	$(Q)$ $\propto n^{- 1}$
(III) Kinetic energy of the electron in the $n^{t h}$ orbit	$(R)$ $\propto n^{0}$
(IV) Potential energy of the electron in the $n^{t h}$ orbit	$(S)$ $\propto n^{1}$
	$(T)$ $\propto n^{2}$
	$(U)$ $\propto n^{1 / 2}$

Which of the following options has the correct combination considering List-I and List-II?

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Chemistry>Physical Chemistry>Structure of Atom>Bohr's Atomic Model and its Limitations

The radius of the second Bohr orbit, in terms of the Bohr radius,

a_{0},

{Li}^{2 +}

is:

EASY

Chemistry>Physical Chemistry>Structure of Atom>Bohr's Atomic Model and its Limitations

Which of the following is the energy of a possible excited state of hydrogen?

EASY

Chemistry>Physical Chemistry>Structure of Atom>Bohr's Atomic Model and its Limitations

With increasing Principal Quantum number, the energy difference between adjacent energy levels in H-atom

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Chemistry>Physical Chemistry>Structure of Atom>Bohr's Atomic Model and its Limitations

For the Balmer series, in the spectrum of

H

atom,

\bar{v} = R_{H} \{\frac{1}{n_{1}^{2}} - \frac{1}{n_{2}^{2}}\},

the correct statements among

(I)

(I V)

are,

(I)

As wavelength decreases, the lines in the series converge.

(I I)

The integer

n_{1}

is equal to

2

(I I I)

The lines of the longest wavelength correspond to

n_{2} = 3

(I V)

The ionization energy of hydrogen can be calculated from the wave number of these lines.

The theoretical and experimental values of Rydberg constant are different.

Important Questions on Structure of Atom

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