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Bohr's Model for Hydrogen Atom - (Concept)

Bohr's model and its postulates:

1. The electron in the hydrogen atom can move around the nucleus in a circular path of fixed radius and energy. These paths are called orbits, stationary states or allowed energy states and are arranged concentrically around the nucleus. Force of attraction between the nucleus and an electron provides the centripetal force required by the electron to carry out the circular motion.

2. The energy of an electron in the orbit does not change with time. However, the electron will move from a lower stationary state to a higher stationary state when required amount of energy is absorbed by the electron or energy is emitted when electron moves from higher stationary state to lower stationary state

3. Energy can be absorbed or emitted when electron transitions between two different orbits and the frequency of photon involved can be calculated using the formula:

$\left|E_1-E_2\right|=h \nu$

4. The angular momentum of an electron is quantised. In a given stationary state it can be expressed as

L= mvr= nh/2$\pi$, n = orbit number

So only those energy states (or orbits) are allowed in which the above equation holds true for the angular momentum.

Note: Bohr's model is only valid for Hydrogen like species or unielectronic species which contain only a single electron

Concepts List

- Atomic Models
  - Atomic Number(Z), Mass number(A), Isotopes and Isobars (Concept)
- Developments leading to the Bohr’s model of atom
  - Speed of electromagnetic radiation and EM radiation (Concept)
- Particle Nature of electromagnetic radiation
  - Planck's quantum theory (Concept)
- Photoelectric Effect
  - Photoelectric effect (Concept)
- Line Spectrum of hydrogen
  - Line spectrum of hydrogen (Concept)
- Bohr model for hydrogen atom
- Dual behavior of matter
  - De broglie wavelength (Concept)
- Heisenberg’s uncertainty principle
  - Heisenberg’s uncertainty principle (Concept)
- Elementary ideas of quantum mechanics
  - Orbital frequency (Concept)
- Quantum mechanical model of atom

« Previous Concept List Next »

Exam	Chapter
JEE MAIN	Atomic Structure

A.	$\mathrm{\nu\ \alpha\ n^{-3}}$
B.	$\mathrm{\nu\ \alpha\ n^{-2}}$
C.	$\mathrm{\nu\ \alpha\ n^{3}}$
D.	$\mathrm{\nu\ \alpha\ n^{-\frac{2}{3}}}$

A.	1.1 X 10^-34 Js
B.	2.2 X10^-34 Js
C.	3.3 X 10^-34 Js
D.	4.1 X 10^-34 Js

A.	It is valid for a multi electronic species
B.	Angular momentum of an electron is quantised
C.	Centripetal force of attraction required for circular motion is provided by the electrostatic force of attraction between the electron and the nucleus
D.	Orbits have fixed energy and are referred to as stationary states

A.	Both $\mathbf{A}$ and $\mathbf{R}$ are true and $\mathbf{R}$ is the correct explanation of $\mathbf{A}.$
B.	Both $\mathbf{A}$ and $\mathbf{R}$ are true but $\mathbf{R}$ is NOT the correct explanation of $\mathbf{A}.$
C.	$\mathbf{A}$ is true but $\mathbf{R}$ is false.
D.	$\mathbf{A}$ is false but $\mathbf{R}$ is true.

A.	It is valid for multielectronic species.
B.	Angular momentum of an electron is quantised.
C.	Centripetal force of attraction required for circular motion is provided by electrostatic force of attraction between the electron and the nucleus.
D.	Orbits have fixed energy and are referred as stationary energy.

A.	$3s$ orbital is lower in energy than $3p$ orbital
B.	$3p$ orbital is lower in energy than $3d$ orbital
C.	$3s$ and $3p$ orbital is lower in energy than $3d$ orbital
D.	$3s$ , $3p$ and $3d$ orbitals all have the same energy

A.	$3\rightarrow 2$
B.	$5\rightarrow 2$
C.	$4\rightarrow 1$
D.	$2\rightarrow 5$

A.	1.1 x 10^-34Js
B.	2.2 x 10^-34 Js
C.	3.3 x 10^-34 Js
D.	4.1 x 10^-34 Js

A.	$\nu \alpha n^{-3}$
B.	$\nu \alpha n^{-2}$
C.	$\nu \alpha n^{3}$
D.	$\nu \alpha n^{-\frac{2}{3}}$

A.	$\mathrm{n=4}$
B.	$\mathrm{n=2}$
C.	$\mathrm{n=16}$
D.	$\mathrm{n=3}$

A.	$1.15 \times 10^{-44}m^{3}$
B.	$2.81\times 10^{-44}m^{3}$
C.	$1.52\times 10^{-44}m^{3}$
D.	$3.45\times 10^{-44}m^{3}$

A.	$E_1$ of $H=\frac{1}{2} E_2$ of $\mathrm{He}^{+}=\frac{1}{3} E_3$ of $\mathrm{Li}^{2+}=\frac{1}{4} E_4$ of $\mathrm{Be}^{3+}$
B.	$E_1(H)=E_2\left(H e^{+}\right)=E_3\left(L^{2+}\right)=E_4\left(B e^{3+}\right)$
C.	Both A and B
D.	None of these

A.	$\frac{1.5 h}{\pi}$
B.	$\frac{3 h}{2 \pi}$
C.	$\frac{h}{\pi}$
D.	$\frac{3.5 h}{2 \pi}$

A.	$\mathrm{I} \rightarrow \mathrm{P} ; \mathrm{II} \rightarrow \mathrm{R} ; \mathrm{III} \rightarrow \mathrm{S} ; \mathrm{IV} \rightarrow \mathrm{Q}$
B.	$\mathrm{I} \rightarrow \mathrm{P} ; \mathrm{II} \rightarrow \mathrm{R} ; \mathrm{III} \rightarrow \mathrm{Q} ; \mathrm{IV} \rightarrow \mathrm{S}$
C.	$\mathrm{I} \rightarrow \mathrm{Q} ; \mathrm{II} \rightarrow \mathrm{S} ; \mathrm{III} \rightarrow \mathrm{P} ; \mathrm{IV} \rightarrow \mathrm{R}$
D.	$\mathrm{I} \rightarrow \mathrm{Q} ; \mathrm{II} \rightarrow \mathrm{S} ; \mathrm{III} \rightarrow \mathrm{R} ; \mathrm{IV} \rightarrow \mathrm{P}$

A.	25
B.	1
C.	10
D.	2.5

A.	$\frac{36 x}{5}$
B.	$\frac{12x}{5}$
C.	$\frac{108x}{5}$
D.	$x$

A.	2.12
B.	0.529
C.	1.65
D.	4.76

A.	631
B.	528
C.	422
D.	122

A.	Radius of $3^{\text {rd }}$ orbit is nine times larger than that of $1^{\text {st }}$ orbit.
B.	Radius of $8^{\text {th }}$ orbit is four times larger than that of $4^{\text {th }}$ orbit.
C.	Radius of $6^{\text {th }}$ orbit is three time larger than that of $4^{\text {th }}$ orbit.
D.	Radius of $4^{\text {th }}$ orbit is four times larger than that of $2^{\text {nd }}$ orbit.

A.	An atom in a stationary state does not emit electromagnetic radiation as long as it stays in the same state
B.	An atom can take only certain distinct energies $\mathrm{E}_1, \mathrm{E}_2, \mathrm{E}_3$, etc. These allowed states of constant energy are called the stationary states of atom
C.	When an electron makes a transition from a higher energy stationary state to a lower energy stationary state, then it emits a photon of light
D.	The electron in a H atom's stationary state moves in a circle around the nucleus

A.	The probability density of finding the electron is maximum at the nucleus
B.	The electron can be found at a distance $2a_0$ from the nucleus
C.	The 1s orbital is spherically symmetrical
D.	The total energy of the electron is maximum when it is at a distance $\mathrm{a}_0$ from the nucleus

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Bohr's Model for Hydrogen Atom - (Concept)

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