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In the Bohr's orbit, what is the ratio of total kinetic energy and the total energy of the electron?

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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

The difference between the radii of $3^{rd}$ and $4^{th}$ orbits of ${Li}_{}^{2 +}$ is ${ΔR}_{1}$ . The difference between the radii of $3^{rd}$ and $4^{th}$ orbits of ${He}^{+}$ is $Δ R_{2} .$ Ratio of $Δ R_{1} : Δ R_{2}$ is :

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

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 wavelength corresponding to maximum energy for hydrogen is

91.2 nm

. The corresponding wavelength for

{He}^{+}

ion is

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

Energy of an electron is given by

E = - 2.178 \times 1 0^{- 18} (\frac{Z^{2}}{n^{2}}) J

. Wavelength of light required to excite an electron in a hydrogen atom from level n=1 to n=2 will be :

(h = 6.62 \times 10^{- 34} J s a n d c = 3.0 \times 10^{8} m s^{- 1})

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

[\frac{0.53 \times 10^{- 10}}{4}]

metre is the radius of smallest electron orbit in hydrogen like atom, then the atom is

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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 :

EASY

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

The radius of the

2^{nd}

orbit of

B^{4^{+}}

ion 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}

)

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

1000

-Watt bulb emits a monochromatic light of wavelength

400 nm .

Calculate the number of photons emitted per second by the bulb.

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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

For which of the following species, the electronic transition from

n = 5

state to

n = 2

state will produce the shortest wavelength in

nm

HARD

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

The figure below is the plot of potential energy versus internuclear distance $(d)$ of $H_{2}$ molecule in the electronic ground state. The value of the net potential energy $E_{0}$ (as indicated in the figure) is $- 5.24649 \times 10^{n}$ $kJ {mol}^{- 1},$ for $d = d_{0}$ at which the electron-electron repulsion and the nucleus-nucleus repulsion energies are absent, find the value of $n$ to the nearest integer value.

As reference, the potential energy of $H$ atom is taken as zero when its electron and the nucleus are infinitely far apart.

Use Avogadro constant as $6 .023 \times 10^{23} {mol}^{- 1} .$ Give an answer to the nearest integer value.

Question Image

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

The energy of an electron in the

3 rd

orbit of

H

-atom (in

J

) is approximately:

HARD

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

If the velocity of the revolving electron of

{He}^{+}

in the first orbit

(n = 1)

v,

the velocity of the electron in the second orbit is:

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

The radius (in

pm

) of the

3^{rd}

orbit of

{He}^{+}

{Li}^{2 +}

is respectively _____

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

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

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

In the Bohr's orbit, what is the ratio of total kinetic energy and the total energy of the electron?

Important Questions on Structure of Atom

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