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**MULTIPLE CHOICE QUESTIONS**

**Q.1. Taking the Bohr radius as a _{0} = 53 pm, the radius of Li^{++} ion in its ground state, on the basis of Bohr’s model, will be about **

Bohr's radius of orbit (for Hydrogen and H

For an electron around a stationary nucleus, the electrostatics force of attraction provides the necessary centripetal force.

i.e., (1/4πε

Also mvr = nh/2π ...(ii)

From equation (i) and (ii), radius of n^{th} orbit

⇒ r_{n} ∝ n^{2}/Z or r_{n} ∝ 1/Z

r_{n} = a_{0}(n^{2}/Z), where a_{0} = the Bohr radius = 53 pm

The atomic number (Z) of lithium is 3.

As

Therefore, the radius of Li^{++} ion in its ground state, on the basis of Bohr’s model, will be about 1/3 times to that of Bohr radius.

Therefore, the radius of lithium ion is near r = 53/3 ≈ 18pm.**Q.2. The binding energy of a H-atom, considering an electron moving around a fixed nuclei (proton), **(m = electron mass).**If one decides to work in a frame of reference where the electron is at rest, the proton would be moving arround it. By similar arguments, the binding energy would be****This last expression is not correct because ****(a) n would not be integral. ****(b) Bohr - quantisation applies only to electron ****(c) The frame in which the electron is at rest is not inertial. ****(d) The motion of the proton would not be in circular orbits, even approximately.****Ans. **(c)**Solution.**

As the mass of an electron is negligible as compared to proton. So the centripetal force cannot provide the electrostatic force, . So the given expression is not true, as it form non-inertial frame of reference due to m_{e}<<<m_{p} or centripetal force on F_{e} <<< F_{p}. So verifies answer (c).**Q.3. The simple Bohr model cannot be directly applied to calculate the energy levels of an atom with many electrons. This is because ****(a) Of the electrons not being subject to a central force****(b) Of the electrons colliding with each other ****(c) Of screening effects ****(d) The force between the nucleus and an electron will no longer be given by Coulomb’s law****Ans. **(a)**Solution.**

The simple Bohr model cannot be directly applied to calculate the energy levels of an atom with many electrons because when we derive the formula for radius/energy levels etc, we make the assumption that centripetal force is provided only by electrostatic force of attraction by the nucleus. Hence, this will only work for single electron atoms. In multi-electron atoms, there will also be repulsion due to other electrons. The simple Bohr model cannot be directly applied to calculate the energy levels of an atom with many electrons.**Q.4. For the ground state, the electron in the H-atom has an angular momentum = ћ, according to the simple Bohr model. Angular momentum is a vector and hence there will be infinitely many orbits with the vector pointing in all possible directions. In actuality, this is not true, ****(a) Because Bohr model gives incorrect values of angular momentum****(b) Because only one of these would have a minimum energy****(c) Angular momentum must be in the direction of spin of electron****(d) Because electrons go around only in horizontal orbits****Ans. **(a)**Solution.**

According to Bohr’s second postulate of atomic model, angular momentum of revolving electron must be some integral multiple of h/2π. so the Bohr’s model does not give correct value of angular momentum. Hence verified answer (a).**Q.5. O _{2} molecule consists of two oxygen atoms. In the molecule, nuclear force between the nuclei of the two atoms(a) is not important because nuclear forces are short-ranged.(b) is as important as electrostatic force for binding the two atoms.(c) cancels the repulsive electrostatic force between the nuclei.(d) is not important because oxygen nucleus have equal number of neutrons and protonsAns. **(a)

Nuclear forces is too much stronger. Only attractive force as compared to electrostatic repulsive force and nuclear force decreases to zero on increasing distance. So in case of oxygen molecule, the distance between atoms of oxygen is larger as compared to the distances between nucleons in a nucleus. So force between the nuclei of two oxygen atoms is not important as nuclear forces are short ranged forces. Hence verified answer (d).

Total energy of two H-atom in ground state

=2(-13.6)=-27.2 eV

The maximum amount by which their combined kinetic energy is reduced when any one H-atom goes into first excited state after the inelastic collision i.e., the total energy of two H-atom after inelastic collision

[ for excited state (n=2)]

=3.4+13.6=17.0 eV

So loss in KE due to inelastic collision

=27.2-17.0=10.2 eV

**Q.7. A set of atoms in an excited state decays. ****(a) in general to any of the states with lower energy****(b) into a lower state only when excited by an external electric field****(c) all together simultaneously into a lower state ****(d) to emit photons only when they collide****Ans. **(a)**Solution. **A set of atoms in an excited state decays in general to any of the states with lower energy.**Q.8. An ionised H-molecule consists of an electron and two protons.The protons are separated by a small distance of the order of angstrom. In the ground state, (a) The electron would not move in circular orbits(b) The energy would be (2)**(a, c)

In H-molecule two nucleus of 2 H-atoms are separated of the order of angstrom, i.e. of order of nuclear forces. One electron will revolve around the protons. Hence verifies answer (a) and (c).

(a) Because of energy conservation.

(b) Without simultaneously releasing energy in the from of radiation.

(c) Because of momentum conservation.

(d) Because of angular momentum conservation.

Ans.

Solution.

The binding energy of H-atom is larger as compared to the energy of free electron. Large amount of energy is required so that electron can reach near the proton which is possible when nuclear force (attractive) acts between e and p become of order of nuclear force, it is not possible without energy conservation (a) and (b).

(a) Will not be applicable to hydrogen in the molecular from

(b) Will not be applicable as it is for a He-atom

(c) Is valid only at room temperature

(d) Predicts continuous as well as discrete spectral lines

Ans.

Solution.

Bohr proposed a-model for hydrogen atom which is also applicable for some lighter atoms in which a single electron revolves around a stationary nucleus of positive charge Ze (called hydrogen like atom, e.g.: H, He

Q.11. The Balmer series for the H-atom can be observed

(a) If we measure the frequencies of light emitted when an excited atom falls to the ground state

(b) If we measure the frequencies of light emitted due to transitions between excited states and the first excited state

(c) In any transition in a H-atom

(d) As a sequence of frequencies with the higher frequencies getting closely packed

When electron jumps from higher energy level to first energy level, the spectrum of light is called Balmer series. Spectrum lines become closer if electron jumps from higher energy level to ground level. Hence verifies answers (b) and (d).

(a) It will not be absorbed at all

(b) Some of atoms will move to the first excited state

(c) All atoms will be excited to the n = 2 state

(d) No atoms will make a transition to the n = 3 state

Ans.

Let E

(a) He

(b) He

(c) He

(d) Electrons are not subject to central forces

Ans.

Bohr’s atomic model is applicable only for one electron and in He

**VERY SHORT ANSWER TYPE QUESTIONS**

**Q.14. The mass of a H-atom is less than the sum of the masses of a proton and electron. Why is this?Ans.** During formation of an atom with neucleon and electrons, it need the energy to bind the nucleons together in nucleus. This energy comes from Einstein mass- energy relation

E=ΔmC

Where Δm=[Zm

So the mass of a H atom is

Where B.E. = 13.6 eV

**Q.15. Imagine removing one electron from He ^{4} and He^{3}. Their energy levels, as worked out on the basis of Bohr model will be very close. Explain why.**Bohr model is applicable for hydrogen atom-and some lighter atoms in which a single electron revolves around a stationary nucleus of positive charge Ze (called hydrogen like atom). If we remove one electron from He

Ans.

Ans.

Ans.

..(i)

Hence the magnitude of electrostatic force F ∞ q

If proton had a charge (+4/3)e and electron a charge (-3/4)e, then the Bohr formula for the H-atom remains same, since the Bohr formula involves only the product of the charges which remain constant for given values of charges.

**Q.18. Consider two different hydrogen atoms. The electron in each atom is in an excited state. Is it possible for the electrons to have different energies but the same orbital angular momentum according to the Bohr model?Ans.** Bohr postulated that an electron in an atom can move around the nucleus in a certain circular stable orbits without emitting radiations.

Bohr found that the magnitude of the electron’s angular momentum is

quantized i.e

where n = 1 , 2, 3...... each value o f n corresponds to a permitted value o f the orbit radius.

r

Thus, the angular momentum (L) of the orbiting electron is quantised

According to Bohr model electrons having different energies belong to different levels haying different values o f n. So, their angular momenta will be different, as

**SHORT ANSWER TYPE QUESTIONS**

**Q.19. Positronium is just like a H-atom with the proton replaced by the positively charged anti-particle of the electron (called the positron which is as massive as the electron). What would be the ground state energy of positronium?Ans.** As in the new H-atom (positronium) proton is replaced by positron of mass m=me/2 as under

Mass of positronium=m =

m=m

As E

E'

Ans.

For He-atom, Z=4 and n=1

Ans.

Radius of orbit=a

So the number of revolutions per second

(-) sign shows that the direction of current is opposite to the direction of motion of electron.

**Q.22. Show that the first few frequencies of light that is emitted when electrons fall to the nth level from levels higher than n, are approximate harmonics (i.e. in the ratio 1 : 2: 3...) when n >>1.Ans.**

Frequency of emitted radiation:

Wave number/wavelength:

Wave number is the number of waves in unit length**Number of spectral lines:** If an electron jumps from higher energy orbit to lower energy orbit to lower energy orbit it emits radiations with various spectral lines.

If electron falls from orbit n_{2} to n_{1} then the number of spectral lines emitted is given by

If electron falls from n^{th} orbit to ground state (i.e. n_{2} = n and n_{1} = 1), then number of spectral lines emitted N_{E} = n(n-1)/2

The frequency of any line in a series in the spectrum of hydrogen like atoms corresponding to the transition of electrons from (n + p) level to nth level can be expressed as a difference of two terms;

where, m = n + p, (p = 1, 2 , 3 , ...) and R is Rydberg constant.

[By Binomial theorem (1 + x )^{n} - 1 + nx if |x| < 1]

Hence, the first few frequencies of light that is emitted when electrons fall to the nth level from levels higher than n, are approximately harmonic (i.e., in the ratio 1 : 2 : 3 ...) when n » 1.**Q.23. What is the minimum energy that must be given to a H atom in ground state so that it can emit an H _{γ} line in Balmer series. If the angular momentum of the system is conserved, what would be the angular momentum of such H_{γ} photon?**

Ans.

corresponds to transition 4 → 2, "H-gamma"

corresponds to transition 5 → 2 and so on.

where H is the element hydrogen. Four of the Balmer lines are in the technically "visible" part of the spectrum, with wavelengths longer than 400 nm and shorter than 700 nm. Parts of the Balmer series can be seen in the solar spectrum. H-alpha is an important line used in astronomy to detect the presence of hydrogen.

From above discussion it is clear that H_{Y} in Balmer series corresponds to transition n = 5 to n = 2. Initially the electron in ground state i.e., from n = 1 must first should be placed in state n = 5.

From above discussion it is clear that H_{γ} in Balmer series corresponds to transition n = 5 to n = 2. Initially the electron in ground state i.e., from n = 1 must first should be placed in state n = 5.

Energy required for the transition from n = 1 to n - 5 is given by

E = E_{5} - E_{1}

As angular momentum should be conserved, hence angular momentum corresponding to H_{γ} photon = change in angular momentum of electron

**LONG ANSWER TYPE QUESTIONS**

**Q.24. The first four spectral lines in the L yman serics of a H-atom are λ = 1218 Å, 1028 Å, 974.3 Å and 951.4 Å. If instead of Hydrogen, we consider Deuterium, calculate the shift in the wavelength of these lines.****Ans. **Reduced mass of H atom (mass defect) μ_{H} then

(M is mass of H atom)

( ∵ M>>>m_{e})

For Deuterium M = 2M

Reduced mass of Deuterium = μ_{D}

Total energy En of the electron revolving in an nth stationary orbit,

m is the reduced mass of the electron and proton in H atom.

So hv = En_{i }- En_{f}

v ∝ m (reduced mass)

For hydrogen and deuterium

So,

λ_{D} = λ_{H}(0.99973)

λ_{H} = Å, Å, Å and Å (Given)

λ_{D1} = Å = 1214 Å

λ_{D2} = 0.9973 x 1028 = 1025Å

λ_{D3} = 0.9973 x 974 = Å

λ_{D4} = 0.9973 x 954 = Å**Q.25. Deutrium was discovered in 1932 by Harold Urey by measuring the small change in wavelength for a particular transition in ^{1}H and ^{2}H. This is because, the wavelength of transition depend to a certain extent on the nuclear mass. If nuclear motion is taken into account then the electrons and nucleus revolve around their common centre of mass. Such a system is equivalent to a single particle with a reduced mass µ, revolving around the nucleus at a distance equal to the electron-nucleus separation. Here µ = m_{e}M /(m_{e} +M) where M is the nuclear mass and m_{e} is the electronic mass. Estimate the percentage difference in wavelength for the 1st line of the Lyman series in ^{1}H and ^{2}H. (Mass of ^{1}H nucleus is 1.6725 × 10^{–27} kg, Mass of ^{2}H nucleus is 3.3374 × 10^{–27} kg, Mass of electron = 9.109 × 10^{–31} kg.)** Total energy of electron in n

Ans.

μ = reduced mass of electron, proton and neutron (mass defect)

The percentage difference in the wavelength =

Percent change in wavelength

% change

∵ ΔE = (E

as μ = mass defect, e,ε, 0 c, and h are constants for an atom.

∴ λ ∝ 1/h

So eqn. Ist can be written as percentage change in the wavelength =

∵ (Given)

∴ Percentage change in wavelength =

Me << M

Decrease in wavelength.

(-) sign shows that λ

Ans.

Here K = 1/4πε

(-) sign shows the force of attraction.

By Bohr’s postulate, angular momentum= nh/2π

mvr

v = nh/2πmr

[From I]

...(II)

For ground state n = 1

= r

(n = 1 for ground state)

K.E. = 0.1373 × 10

P.E. = 27.2 eV

(ii) Now for spherical nucleus of radius, R, electron moves charge inside the nucleus R>>r

q

(By Coulomb’s law)

(By Bohr’s postulate)

Now for ground state of H, n=1 and then

r

= 0.001656 × 10

K.E = 0.167eV

From part (i)

P.E. = 3992.9/1000 = -3.99eV

K.E. = 0.167 eV

Ans.

(for n

Z = 24

R = Rydberg constt.

∴ E

The energy required to eject an electron from n = 4 state is

E

Energy given to electron is converted into K.E. of ejected electron.

Hence, the K.E. of Auger (ejected) electron= E

K.E. = 11 × 36 × 13.6 = 5385.6 eV

Ans.

= 9.1 × 10

Wavelength associated with a photon = h/m

=2.4×10

...(I)

If λ=0, [neglecting r

∵ λ

Taking r

r

(neglecting small term δ

∴ λ and r

V(r) = -27.2 eV remains unchanged

= 13.6 eV (1 + 2λr

Total energy =

=[-27.2+13.6(1+2λr

=-27.2+13.6+27.2λr

Total E= -13.6+27.2 λr

Change in energy =-13.6+27.2λr

Calculate in such a case, the ground state energy of a H-atom, if ε = 0.1, R

Ans.

Let ε = 2 + δ

[q

[(-) ve sign shows force of attraction]

The electrostatic force of attraction between positively charged nucleus and negatively charged electron provides necessary centripetal force.

Let 23.04 × 10

By Bohr’s IInd postulate, angular momentum

[Given in last Q.]

∴ L = nh

mvr = nh

= (n = 1 for ground state)

Where h = 1.05 × 10

R

R

This is a radius of orbit of electron in ground state of hydrogen atom.

By IInd postulate of Bohr’s Atomic model

Case II: n=1,

= 1.44 x 10

v

= 1/2 x 9.1 x 10

= 5.9 eV

P.E. from R

P.E from R

This is the P.E. of electron in ground state R

Put δ = -1.9

= -17.3 eV

Total E = P.E. + K.E.

=(-17.3 + 5.9) eV

Total energy = -11.4eV

This is the required total energy of electron in ground state of H-atom.

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