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The potential energy of an electron in ${H e}^{+}$ ion is $- 12.09 e V$ . In which excited state is the electron is present?

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Important Questions on Atomic Structure

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Chemistry>Physical Chemistry>Atomic Structure>Bohr's Model for the Hydrogen Atom

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

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

EASY

Chemistry>Physical Chemistry>Atomic Structure>Bohr's Model for the Hydrogen Atom

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

MEDIUM

Chemistry>Physical Chemistry>Atomic Structure>Bohr's Model for the Hydrogen Atom

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 :

MEDIUM

Chemistry>Physical Chemistry>Atomic Structure>Bohr's Model for the Hydrogen Atom

The ratio of the shortest wavelength of two spectral series of hydrogen spectrum is found to be about

9

. The spectral series are:

MEDIUM

Chemistry>Physical Chemistry>Atomic Structure>Bohr's Model for the Hydrogen Atom

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>Atomic Structure>Bohr's Model for the Hydrogen Atom

Which of the following series of transitions in the spectrum of hydrogen atom falls in visible region?

MEDIUM

Chemistry>Physical Chemistry>Atomic Structure>Bohr's Model for the Hydrogen Atom

If the shortest wavelength in Lyman series of hydrogen atom is

A

, then the longest wavelength in Paschen series of

{He}^{+}

HARD

Chemistry>Physical Chemistry>Atomic Structure>Bohr's Model for the Hydrogen Atom

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?

EASY

Chemistry>Physical Chemistry>Atomic Structure>Bohr's Model for the Hydrogen Atom

The radii of the first Bohr orbit of

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

and

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

are in the order

EASY

Chemistry>Physical Chemistry>Atomic Structure>Bohr's Model for the Hydrogen Atom

If the radius of the hydrogen atom is

53 pm

, the radius of the

{He}^{+}

ion is closest to:

MEDIUM

Chemistry>Physical Chemistry>Atomic Structure>Bohr's Model for the Hydrogen Atom

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

a_{0},

{Li}^{2 +}

is:

MEDIUM

Chemistry>Physical Chemistry>Atomic Structure>Bohr's Model for the Hydrogen Atom

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:

MEDIUM

Chemistry>Physical Chemistry>Atomic Structure>Bohr's Model for the Hydrogen Atom

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.

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Chemistry>Physical Chemistry>Atomic Structure>Bohr's Model for the Hydrogen Atom

For any given series of spectral lines of atomic hydrogen, let $Δ \bar{v} = {\bar{v}}_{m a x} - {\bar{v}}_{m i n}$ be the difference in maximum and minimum wave number in $c m^{- 1}$ .

The ratio $Δ {\bar{v}}_{L y m a n} / Δ {\bar{v}}_{B a l m a r}$ is

MEDIUM

Chemistry>Physical Chemistry>Atomic Structure>Bohr's Model for the Hydrogen Atom

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?

MEDIUM

Chemistry>Physical Chemistry>Atomic Structure>Bohr's Model for the Hydrogen Atom

The shortest wavelength of

H

atom in the Lyman series is

λ_{1}

. The longest wavelength in the Balmer series of

{He}^{+}

is :

MEDIUM

Chemistry>Physical Chemistry>Atomic Structure>Bohr's Model for the Hydrogen Atom

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>Atomic Structure>Bohr's Model for the Hydrogen Atom

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>Atomic Structure>Bohr's Model for the Hydrogen Atom

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})

MEDIUM

Chemistry>Physical Chemistry>Atomic Structure>Bohr's Model for the Hydrogen Atom

The ground state energy of a hydrogen atom is

- 13 .6 eV

. The energy of second excited state of

{He}^{+}

ion in

eV

is:

The potential energy of an electron in He+ ion is -12.09 eV. In which excited state is the electron is present?

Important Questions on Atomic Structure

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The potential energy of an electron in ${H e}^{+}$ ion is $- 12.09 e V$ . In which excited state is the electron is present?