# Samacheer Kalvi 11th Chemistry Solutions Chapter 2 Quantum Mechanical Model of Atom

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## Tamilnadu Samacheer Kalvi 11th Chemistry Solutions Chapter 2 Quantum Mechanical Model of Atom

### Samacheer Kalvi 11th Chemistry Chapter 2 Quantum Mechanical Model of Atom Textual Evaluation Solved

Question 1.
Electronic configuration of species M2+ is 1s2 2s2 2p63s2 3p6 3d6 and its atomic weight is 56. The number of neutrons in the nucleus of species M is ………..
(a) 26
(b) 22
(c) 30
(d) 24
(c) 30
Solution:
M2+ : 1s2 2s2 2p63s2 3p6 3d6
M : 1s2 2s2 2p63s2 3p6 3d8
Atomic number = 26
Mass number = 56
No. of neutrons = 56 – 26 = 30.

Question 2.
The energy of light of wavelength 45 nm is
(a) 6.67 x 1015 J
(b) 6.67 x 1011 J
(c) 4.42 .x 1018 J
(d) 4.42 x 10-15 J
(c) 4.42 x 1018 J
Solution:
E = hv = hc / λ
$$\frac{6.626 \times 10^{-34} \mathrm{J} \mathrm{s} \times 3 \times 10^{8} \mathrm{ms}^{-1}}{45 \times 10^{-9} \mathrm{m}}$$ = 4.42 .x 1018 J.

Question 3.
The energies E1 and E2 of two radiations are 25 eV and 50 eV respectively. The relation between their wavelengths i.e. λ1 and λ2 will be …………
(a) $$\frac{\lambda_{1}}{\lambda_{2}}=1$$
(b) λ1 = 2 λ2
(c) λ1 = $$\sqrt{25 \times 50} \lambda_{2}$$
(d) 2 λ1 = λ2
(b) λ1 = 2 λ2
Solution:
$$\frac{E l}{E 2}$$ = $$\frac{25eV}{50eV}$$ = $$\frac{1}{2}$$
$$\frac{\mathrm{hc}}{\lambda_{1}} \times \frac{\lambda_{2}}{\mathrm{hc}}$$ = $$\frac{1}{2}$$
2 = λ1.

Question 4.
Splitting of spectral lines in an electric field is called …………….
(a) Zeeman effect
(b) Shielding effect
(c) Compton effect
(d) Stark effect
(d) Stark effect
Solution:
The splitting of spectral lines in a magnetic field is called the Zeeman effect and the splitting of spectral lines in an electric field is called the Stark effect.

Question 5.
Based on equation E = -2.178 x 1018 J $$\left(\frac{z^{2}}{n^{2}}\right)$$ certain conclusions are written. Which of them is not correct? (NEET)
(a) Equation can be used to calculate the change in energy when the electron changes orbit
(b) For n = 1, the electron has more negative energy than it does for n = 6 which means that the electron is more loosely bound in the smallest allowed orbit
(c) The negative sign in the equation simply means that the energy of an electron bound to the nucleus is lower than it would be if the electrons were at an infinite distance from the nucleus.
(d) Larger the value of n, the larger is the orbit radius.
(b) For n = 1, the electron has more negative energy than it does for n = 6 which means that the electron is more loosely bound in the smallest allowed orbit
Solution:
Correct statement:
For n = 6, the electron has more negative energy than it does for n = 6 which means that the electron is strongly bound in the smallest allowed orbit.

Question 6.
According to the Bohr Theory, which of the following transitions in the hydrogen atom will give rise to the least energetic photon?
(a) n = 6 to n = 1
(b) n = 5 to n = 4
(c) n = 5 to n = 3
(d) n = 6 to n = 5
(d) n = 6 to n = 5
Solution:
n = 6 to n = 5
E6 = -13.6 / 62 ; E5 = – 13.6 / 52
E6 – E5 = (-13.6 / 62) – (-13.6 / 52)
= 0.166 eV atom-1
E5 – E4 = (-13.6 / 52) – (-13.6 / 42)
= 0.306 eV atom-1

Question 7.
Assertion: The spectrum of He+ is expected to be similar to that of hydrogen.
Reason: He+ is also a one-electron system.
(a) If both assertion and reason are true and the reason is the correct explanation of assertion.
(b) If both assertion and reason are true but the reason is not the correct explanation of assertion.
(c) If the assertion is true but the reason is false
(d) If both assertion and reason are false
(a) If both assertion and reason are true and the reason is the correct explanation of assertion.

Question 8.
Which of the following pairs of d-orbitals will have electron density along the axes ? (NEET Phase – II)
(a) dz2, dxz
(b) dxz, dyz
(c) dz2, $$d_{x^{2}-y^{2}}$$
(d) dxy, $$d_{x^{2}-y^{2}}$$
(c) dz2, $$d_{x^{2}-y^{2}}$$

Question 9.
Two electrons occupying the same orbital are distinguished by …………
(a) azimuthal quantum number
(b) spin quantum number
(c) magnetic quantum number
(d) orbital quantum number
(b) spin quantum number
Solution:
Spin quantum number For the first electron ms = +$$\frac {1}{2}$$
For the second electron ms = –$$\frac {1}{2}$$.

Question 10.
The electronic configuration of Eu (atomic no. 63) Gd (atomic no. 64) and Tb (atomic no. 65) are (NEET – Phase II)
(a) [Xe] 4f7 5d1 6s2, [Xe] 4f7 5d1 6s2 and [Xe] 4f8 5d1 6s2
(b) [Xe] 4f7, 6s2, [Xe] 4f7 5d1 6s2 and [Xe] 4f9 6s2
(c) [Xe] 4f7 , 6s2, [Xe] 4f8 6s2 and [Xe] 4f8 5d1 6s2
(d) [Xe] 4f8 5d1 6s2[Xe] 4f7 5d1 6s2 and [Xe] 4f9 6s2
(b) [Xe] 4f7, 6s2, [Xe] 4f7 5d1 6s2 and [Xe] 4f9 6s2
Solution:
Eu : [Xe] 4f7, 5d0, 6s2
Gd : [Xe] 4f7, 5d1, 6s2
Tb : [Xe] 4f9, 5d0,6s2

Question 11.
The maximum number of electrons in a subshell is given by the expression …………..
(a) 2n2
(b) 21 + 1
(c) 41 + 2
(d) none of these
(c) 41 + 2
Solution:
2 (21 + 1) = 41 + 2.

Question 12.
For d-electron, the orbital angular momentum is ………….
(a) $$\frac{\sqrt{2} h}{2 \pi}$$
(b) $$\frac{\sqrt{2 \mathrm{h}}}{2 \pi}$$
(c) $$\sqrt{2 \times 4}$$
(d) $$\frac{\sqrt{6} h}{2 \pi}$$
(d) $$\frac{\sqrt{6} h}{2 \pi}$$
Solution:
Orbital angular momentum
= $$\sqrt{(1(1+1)}) \mathrm{h} / 2 \pi$$
For d orbital = $$\sqrt{(2 × 3)} \mathrm{h} / 2 \pi$$ = $$\sqrt{6} \mathrm{h} / 2 \pi$$.

Question 13.
What is the maximum numbers of electrons that can be associated with the following set of quantum numbers ? n = 3,l = 1 and m = -1
(a) 4
(b) 6
(c) 2
(d) 10
(c) 2
Solution:
n = 3; l = 1; m = -1 either 3px or 3py

Question 14.
Assertion: The number of radials and angular nodes for 3p orbital are l, l respectively.
Reason: The number of radials and angular nodes depends only on the principal quantum number.
(a) both assertion and reason are true and the reason is the correct explanation of assertion.
(b) both assertion and reason are true but the reason is not the correct explanation of assertion.
(c) the assertion is true but the reason is false
(d) both assertion and reason are false
(c) assertion is true but reason is false
Solution:
No. of radial node = n- l – 1
No. of angular node = l for 3p orbital
No. of angular node = l = 1
No. of radial node = n – l – 1 = 3 – 1 – 1 = 1.

Question 15.
The total number of orbitals associated with the principal quantum number n = 3 is ………..
(a) 9
(b) 8
(c) 5
(d) 7
(a) 9
Solution:
n = 3; l = 0; m1 = 0 – one s orbital n = 3; l = 1; m1 = -1, 0, 1 – three p orbitals n = 3; l = 2; m1 = -2, -1, 0, 1, 2 – five d orbitals, overall nine orbitals are possible.

Question 16.
If n = 6, the correct sequence for filling of electrons will be, …………
(a) ns → (n – 2) f → (n – 1)d → np
(b) ns → (n – 1) d → (n – 2) f → np
(c) ns → (n – 2) f → np → (n – 1) d
(d) none of these are correct
(a) ns → (n – 2)f → (n – l)d → np
Solution:
n = 6 According Aufbau principle,
6s → 4f → 5d → 6p
ns → (n – 1)f → (n – 2)d → np.

Question 17.
Consider the following sets of quantum numbers:

Which of the following sets of quantum numbers is not possible?
(a) (i), (ii), (iii) and (iv)
(b) (ii), (iv) and (v)
(c) (z) and (iii)
(d) (ii), (iii) and (iv)
(b) (ii), (iv) and (v)
Solution:
(ii) l can have the values from 0 to n – 1 n = 2; possible l values are 0, 1 hence l = 2 is not possible.
(iv) for l = 0; m = -1 not possible
(v) for n = 3 l = 4 and m = 3 not possible.

Question 18.
How many electrons in an atom with atomic number 105 can have (n + 1) = 8?
(a) 30
(6) 17
(c) 15
(d) unpredictable
(b) 17
Solution:
n + 1 = 8
Electronic configuration of atom with atomic number 105 is [Rn] 5f14 6d3 7s2

 Orbital (n+1) No. of electrons 5f 5 + 3 = 8 14 6d 6 + 2 = 8 3 7s 7 + 0 = 0 2 No. of electrons = 14 + 3 = 17

Question 19.
Electron density in the yz plane of 3 dx2-y2 orbitals is …………….
(a) zero
(b) 0.50
(c) 0.75
(d) 0.90
(a) zero

Question 20.
If uncertainty in position and momentum are equal, then minimum uncertainty in velocity is ……….
(a) $$\frac{1}{m} \sqrt{\frac{h}{\pi}}$$
(b) $$\sqrt{\frac{\mathrm{h}}{\pi}}$$
(c) $$\frac{1}{2 m} \sqrt{\frac{h}{\pi}}$$
(d) $$\frac{\mathrm{h}}{4 \pi}$$
(c) $$\frac{1}{2 m} \sqrt{\frac{h}{\pi}}$$
Solution:

Question 21.
A macroscopic particle of mass 100 g and moving at a velocity of 100 cm s-1d will have a de Broglie wavelength of ………….
(a) 6.6 x 10-29 cm
(b) 6.6 x 10-30 cm
(c) 6.6 x 10-31 cm
(d) 6.6 x 10-32 cm
(c) 6.6 x 10-31 cm
Solution:
m = 100 g = 100 x 10-3 kg
v = 100 cm s-1 = 100 x 10-2 m s-1
λ = $$\frac{h}{mv}$$ =
= 6.626 x 10-31 ms-1
= 6.626 x 10-31 cm s-1

Question 22.
The ratio of de Broglie wavelengths of a deuterium atom to that of an α-particle, when the velocity of the former is five times greater than that of later, is ……………
(a) 4
(b) 0.2
(c) 2.5
(d) 0.4
(d) 0.4

Question 23.
The energy of an electron in the 3rd orbit of a hydrogen atom is -E. The energy of an electron in the first orbit will be ……………..
(a) – 3E
(b) – E /3
(c) – E / 9
(d) – 9E
(c) – E / 9
Solution:
En  = $$\frac{-13.6}{n^{2}}$$ eV atom-1
E1 = $$\frac{-13.6}{1^{2}}$$13.6 = $$\frac{-13.6}{9}$$
Given that,
E3 = – E
$$\frac{-13.6}{9}$$ = -E
13.6 = – 9E = E1 = – 9E
E1 = – 9E

Question 24.
Time independent Schrodinger wave equation is ………….

(a) $$\widehat{\mathrm{H}} \psi=\mathrm{E} \psi$$.

Question 25.
Which of the following does not represent the mathematical expression for the Heisenberg uncertainty principle?
(a) ∆E.∆p ≥ h/4π
(b) ∆E.∆v ≥ h/4πm
(c) ∆E.∆t ≥ h/4π
(d) ∆E.∆x ≥ h/4π
(d) ∆E.∆x ≥ h/4π.

II. Write brief answer to the following questions

Question 26.
Which quantum number reveals information about the shape, energy, orientation, and size of orbitals?
The information about the shape, energy, orientation, and size of the orbitals are respectively given by Azimuthal, spin, magnetic, and principal quantum numbers.

Question 27.
How many orbitals are possible for n = 4?
If n = 4, the possible number of orbitals are calculated as follows –
n = 4, main shell = N
If n = 4, l values are 0, 1, 2, 3
If l = 0,  4s orbital = 1 orbital
If l = 1,  m = -1,0, +1 = 3 orbitals
If l = 2,  m = -2,-1,0, +1,+2 = 5 orbitals
If l = 3,  m = -3,-2,-1,0, +1,+2,+3 = 7 orbitals
∴ Total number of orbitals = 16 orbitals

Question 28.
How many radial nodes for 2s, 4p, 5d, and 4f orbitals exhibit? How many angular nodes?
The formula for the total number of nodes = n – 1

1. For 2s orbital: Number of radial nodes =1.

2. For 4p orbital: Number of radial nodes = n – l – 1. = 4 – 1 – 1 = 2
Number of angular nodes = l
∴ Number of angular nodes = 1
So, 4p orbital has 2 radial nodes and 1 angular node.

3. For 5d orbital:
Total number of nodes = n – 1 = 5 – 1 = 4 nodes
Number of radial nodes = n – l – 1 = 5 – 2 – 1 = 2 radial nodes.
Number of angular nodes = l = 2
∴ 5d orbital have 2 radial nodes and 2 angular nodes.

4. For 4f orbital:
Total number of nodes = n – 1 = 4 – 1 = 3 nodes
Number of radial nodes = n – 7 – 1 = 4 – 3 – 1 = 0 node.
Number of angular nodes = l = 3 nodes
∴ 4f orbital have 0 radial node and 3 angular nodes.

Question 29.
The stabilization of a half-filled d-orbital is more pronounced than that of the p-orbital why?
The half-filled orbitals are more stable due to symmetry and exchange energy. In the case of half-filled d-orbitals, there are ten possible exchanges whereas in p-orbitals three possible exchanges only, If more exchanges are possible, more exchange energy is released and more stable. Hence, the stabilization of a half-filled d-orbital is more pronounced than that of the p-orbital.

Question 30.
Consider the following electronic arrangements for the d5 configuration.

(1) Which of these represents the ground state
(2) Which configuration has the maximum exchange energy.
(1)  – This represents the ground state.
(2)   – This represents the maximum exchange energy.

Question 31.
State and explain Pauli’s exclusion principle.
Pauli’s exclusion principle states that “ No two electrons in an atom can have the same set of values of all four quantum numbers”. It means that each electron must have unique values for the four quantum numbers.

For the lone electron present in hydrogen atom, the four quantum numbers are: n = 1, l = 0, m = 0 and s = +1/2. For the two electrons present in helium, one electron has the quantum numbers same as the electron of the hydrogen atom,
n = 1, l = 0, m = 0, and s = +1/2

For other electron, the fourth quantum number is different, i.e., n = 1, l = 0, m = 0 and s = -1/2.

Question 32.
Define orbital? What are the n and l values for 3px and 4 dx2-y2 electron?
(i) Orbital is a three-dimensional space in which the probability of finding the electron is maximum.

Question 33.
Explain briefly the time-independent Schrodinger wave equation?
The time independent Schrodinger equation can be expressed as
$$\widehat{\mathrm{H}}$$ Ψ = EΨ ……………(1)
Where $$\widehat{\mathrm{H}}$$ is called Hamiltonian operator.
Ψ is the wave function.
E is the energy of the system.

Since Ψ is a function of position coordinates of the particle and is denoted by Ψ (x, y, z)
∴ Equation (1) can be written as,

Multiply the equation (3) by $$\widehat{\mathrm{H}}$$ and rearranging

The above equation (4) Schrodinger wave equation does not contain time as a variable and is referred to as time-independent Schrodinger wave equation.

Question 34.
Calculate the uncertainty in position of an electron, if ∆v = 0.1% and n = 2.2 x 106 ms-1.
Mass of an electron = m = 9.1 x 10-31 kg.
∆v = Uncertainty in velocity = $$\frac {0.1}{100}$$ x 2.2 x 103 ms-1 .
∆v = 0.22 x 104 = 2.2 x 103 ms-1
∆x . ∆v . m = $$\frac {h}{4π}$$
∆x = $$\frac {h}{∆v . m x 4π}$$

= 0.02635 x 10-6
∆x = 2.635 x 10-8
Uncertainty in position = 2.635 x 10-8.

Question 35.
Determine the values of all the four quantum numbers of the 8th electron in O – atom and 15th electron in Cl atom and the last electron in chromium.
Electronic configuration of Oxygen (Atomic Number = 8) is 1s2 2s2 2py2 2pz1 2px1
The eighth electron is present in 2px orbital and the quantum numbers are
n = 2, l = 1, m = +1 or -1 and s = +1/2.

Electronic configuration of Chlorine (Atomic Number = 17) is 1s2 1s2 2p6 3s2 3p5. Therefore, 15th (last) electron is present in 3pz orbital and the quantum numbers are n = 32, l = 1, m = +1 or -1 and s = +1/2

Electronic configuration of Chromium (Atomic Number = 24) is 1s2 2s2 2p6 3s2 3p6 3d5 4s1. Therefore, last electron is present in 4s orbital and the quantum numbers are n = 4, l = 0, m = 0 and s = +1/2.

Question 36.
The quantum mechanical treatment of the hydrogen atom gives the energy value:
En = $$\frac{-13.6}{n^{2}}$$ eV atom-1

1. use this expression to find ∆E between n = 3 and n = 4
2. Calculate the wavelength corresponding to the above transition.

(1) When n = 3
E3 = $$\frac{-13.6}{3^{2}}$$ = $$\frac {-13.6}{9}$$ = – 1.511 eV atom-1
When n = 4 E4 = $$\frac{-13.6}{4^{2}}$$ = – 0.85 eV atom-1
∆E = E4 – E3 = – 0.85 – (-1.511) = + 0.661 eV atom
∆E = E3 – E4
= – 1.511 – (-0.85)
= – 0.661 eV atom-1

(2) Wave length = λ
∆E = $$\frac {hc}{ λ}$$
λ = $$\frac {hc}{∆E}$$
h = Planck’s constant = 6.626 x 10-34 Js-1
c = 3 x 108 m/s
λ = $$\frac{6.626 \times 10^{-34} \times 3 \times 10^{8}}{0.661}$$
= 10.02 x 10-34 x 3 x 108
= 30 x 10-26
λ = 3 x 10-25 m.

Question 37.
How fast must a 54 g tennis ball travel in order to have a de Broglie wavelength that is equal to that of a photon of green light 5400 Å?
m = mass of tennis ball = 54 g = 5.4 x 10-2 kg.
λ = de Broglie wavelength = 5400 Å. = 5400 x 10-10 m.
V = velocity of the ball = ?
λ = $$\frac {h}{mV}$$
V = $$\frac {h}{λ.m}$$

= 0.2238 x 10-24
= 2.238 x 10-25 m.

Question 38.
For each of the following, give the sub level designation, the allowable m values and the number of orbitals.

1. n = 4, l = 2,
2. n = 5, l = 3
3. n = 7, l = 0

1. n = 4, l = 2
If l = 2, ‘m’ values are -2, -1, 0, +1, +2
So, 5 orbitals such as dxy,dyz,dxz,$$d_{x^{2}-y^{2}}$$ and dz

2. n = 5 , l = 3
If l = 3, ‘m’ values are -3, -2, -1, 0, +1, +2, +3
So, 7 orbitals such as f z, fxz, fyz, fxyz, fz(x2 y2)’ ^x(x2-3y2)’ ^y(3×2 ??y

3. n = 7 , l = 0
If l = 0, ‘m’ values are 0. Only one value.
So, 1 orbital such as 7s orbital.

Question 39.
Give the electronic configuration of Mn2+ and Cr3+
Mn (z = 25). Electronic configuration of
Mn2+ = 1s2 2s2 2p6 3s2 3p6 4s0 3d5.

Cr (z =24) Electronic configuration of
Cr3+ = 1s2 2s2 2p6 3s2 3p6 4s0 3d3.

Question 40.
Describe the Aufbau principle.
In the ground state of the atoms, the orbitals are filled in the order of their increasing energies. That is the electrons first occupy the lowest energy orbital available to them. Once the lower energy orbitals are completely filled, then the electrons enter the next higher energy orbitals.
The order of filling of various orbitals as per the Aufbau principle is –
1 s < 2s < 2p < 3s < 3p < 4s < 3d < 4p < 5s < 4d ………..
For e.g., K (Z =19)
The electronic configuration is 1s2 2s2 2p6 3s2 3p6 4s1.
After filling 4s orbital only we have to fill up 3d orbital.

Question 41.
An n atom of an element contains 35 electrons and 45 neutrons. Deduce

1. the number of protons
2. the electronic configuration for the element
3. All the four quantum numbers for the last electron

An element X contains 35 electrons, 45 neutrons

1. The number of protons must be equal to the number of electrons. So the number of protons = 35.
2. Number of electrons = 35. So the electronic configuration is 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p5.
3. The last electron i.e. 5th electron in 4p orbital has the following quantum numbers. n = 4, l = 1, m =+1, s = + $$\frac {1}{2}$$

Question 42.
Show that the circumference of the Bohr orbit for the hydrogen atom is an integral multiple of the de Broglie wavelength associated with the electron revolving around the nucleus.
In order for the electron wave to exist in phase, the circumference of the orbit should be an integral multiple of the wavelength of the electron wave. Otherwise, the electron wave is out of phase.
mvr = nh / 2π, 2πr = nλ,
where mvr = angular momentum
where 2πr = circumference of the orbit

n = 3, n = 4

Question 43.
Calculate the energy required for the process.
He+(g) → He2+(g) + e
The ionization energy for the H atom in its ground state is – 13.6 eV atom-1.
The ionization energy for the H atom in its ground state =-13.6 eV atom-1.
Ionization energy = $$\frac{13.6 z^{2}}{n^{2}}$$ eV
Z = atomic number
n = principal quantum number or shell number
For He, n = 1, z = 2
IE = $$\frac{-13.6 \times 2^{2}}{1^{2}}$$eV.

Question 44.
An ion with mass number 37 possesses a unit negative charge. If the ion contains 11.1% more neutrons than electrons. Find the symbol of the ion.
Mass number (A) = Number of Protons + Nnumber of neutrons = 37.
Number of neutrons = Number of electrons (x) + 11.1 % of x.
Given:
(x – 1) ion + 1.111x = 37.
x = $$\frac{38}{2}$$ . 11 = 18 = 18.
Atomic Number(z) = 18 – 1 = 17.
Symbol of the ion is $${ }_{17}^{37} X$$.

Question 45.
The Li2+ ion is a hydrogen-like ion that can be described by the Bohr model. Calculate the Bohr radius of the third orbit and calculate the energy of an electron in 4th orbit.
Li2+ hydrogen-like ion.
Bohr radius of the third orbit = r3 = ?
r3 = $$\frac{(0.529) n^{2}}{Z}$$ A
Where n = shell number, Z = atomic number.
r3 = $$\frac{(0.529) 3^{2}}{3}$$ A [∴for lithium Z = 3, n = 3]
= $$\frac{0.529 x 9}{3}$$
r3 = l.587Å
En = $$\frac{(-13.6) Z^{2}}{n^{2}}$$ eV atom-1.
E4 = Energy of the fourth orbit = ?
E4 = $$\frac{(-13.6) \times 3^{2}}{4^{2}}$$ = $$\frac{-13.6 \times 9}{16}$$ = -7.65 eV atom-1
E4 = – 7.65 eV atom-1

Question 46.
Protons can be accelerated in particle accelerators. Calculate the wavelength (in Å)of such accelerated proton moving at 2.85 × 108 ms-1 (the mass of proton is 1.673 x 10-27 Kg).
m = mass of the proton = 1.673 x 10-27 Kg
v = velocity of the proton = 2.85 x 108 ms-1
λ = $$\frac{h}{mv}$$
h = Planck’s constant = 6.626 x 1034 Kg m2 s-1

Wavelength of proton = λ = 1.389 x 10-15 m.

Question 47.
What is the de Broglie wavelength (in cm) of a 160g cricket ball travelling at 140 Km hr-1.
m = mass of the cricket ball = 160g = 0.16 kg.
v = velocity of the cricket ball =140 Km h-1
= $$\frac {140 x 5}{18}$$ = 38.88 ms-1
de Broglie equation = λ = $$\frac{h}{mv}$$
h = Planck’s constant = 6.626 x 10-34 kg m2 s-1

λ = 1.065 x 10-34m
Wave length in cm = 1.065 x 10-34 x 100
= 1.065 x 10-32 cm.

Question 48.
Suppose that the uncertainty in determining the position of an electron in an orbit is 0.6 A. What is the uncertainty in its momentum?.
∆x = uncertainty in position of an electron = 0.6 Å = 0.6 x 10-10 m.
∆p = uncertainty in momentum = ?
Heisenberg’s uncertainty principle states that,
∆x.∆p ≥ $$\frac{h}{4π}$$
∆p = $$\frac{h}{4π.∆x}$$
h = Planck’s constant = 6.626 x 10-34 kg m2 s-1

Uncertainty in momentum = 0.8792 x 10-24 kg ms-1 (or) = 8.792 x 10-25 kg ms-1

Question 49.
Show that if the measurement of the uncertainty in .the location of the particle is equal to its de Broglie wavelength, the minimum uncertainty in its velocity is equal to its velocity /4π
If, uncertainty in position = ∆x = λ , the value of uncertainty in velocity = $$\frac{v}{4π}$$
Heisenberg’s principle states that
∆x.∆v. m = $$\frac{h}{4π}$$ …………(1)
de Broglie equation states that
λ = $$\frac{h}{mv}$$ ………….(2)
∴ h = λ .m.v …………(3)
∆x = $$\frac{h}{∆v.4π}$$ ………….(4)
Substituting the value of h in equation (4)
∆x = $$\frac{λ x m. v}{∆v.4π.m}$$
if ∆x = λ
∆v =  = $$\frac{v}{4π}$$

Question 50.
What is the de Broglie wave length of an electron, which is accelerated from the rest, through a potential difference of 100V?
Potential difference = V = 100 V
Potential energy = eV = 1.609 x 10-19c x 100V
$$\frac{v}{4π}$$ m v2 = 1.609 x 10-19 x 100
$$\frac{v}{4π}$$ m v2 = 1.609 x 10-19 J
v2 = $$\frac{2 \times 1.609 \times 10^{-17}}{m}$$
m = mass of electron = 9.1 x 10-31 Kg

v = 5.93 x 106 m/s
λ = $$\frac{h}{mv}$$ where h = 6.62 x 10-34 JS
= $$\frac{6.62 \times 10^{-34}}{9.1 \times 10^{-31} \times 5.93 \times 10^{6}}$$
= 1.2x 10-10m
A= 1.2 Å.

Question 51.
Identify the missing quantum numbers and the sub energy level

Samacheer Kalvi 11th Chemistry Quantum Mechanical Model of Atom In-Text Questions – Evaluate Yourself

Question 1.
Calculate the de Broglie wavelength of an electron that has been accelerated from rest through a potential difference of 1 k eV.
λ = $$\frac{h}{mv}$$
Potential difference of an electron = V = 1 keV.
Potential energy = $$\frac{1}{2}$$ mv2 = eV
e = charge of an electron = 1.609 x 10-19c
l k V = 1000 V
:. Potential energy = 1.609 x 10-19 x 1000 = 1.609 x 10-19
$$\frac{1}{2}$$ mv2 = 1.609 x 10-16V
m = 9.1 x 10-31 kg
λ = $$\frac{h}{mv}$$

= 1.2 x 10-11 m
λ = 1.2 x 10-11 m.

Question 2.
Calculate the uncertainty in the position of an electron, if the uncertainty in its velocity is 5.7 x 10 s ms-1.
Uncertainty in velocity = Av = 5.7 x 105 ms-1
Mass of an electron = m = 9.1 x 10-31 kg.
Uncertainty in position = ∆x = ?
∆x.m.∆v = $$\frac{h}{4π}$$

= 1 x 10-10m.
Uncertainty in position = 1 x 10-10 m.

Question 3.
How many orbitals are possible in the 4th energy level? (n = 4)
n = 4
Number of orbitals in 4th energy level = ?
When n = 4, l = 0,1,2,3
If l = 0 orbital = 4s =1
If l = 1 orbital = 4px, 4py, 4pz = 2
If l = 2 orbital = $$4 \mathrm{d}_{\mathrm{xy}}, 4 \mathrm{d}_{\mathrm{yz}}, 4 \mathrm{d}_{\mathrm{zx}}, 4 \mathrm{d}_{\mathrm{x}} 2_{\mathrm{y}}, 2,4 \mathrm{d}_{\mathrm{z}^{2}}$$ = 5
If l = 3 orbital = -3,-2, -1, 0, +1, +2, +3 = 7
Number of orbitals in 4th energy level = 16.

Question 4.
Calculate the total number of angular nodes and radial nodes present in 3d and 4f orbitals.
The number of angular nodes in 3d orbital =?
A number of radial nodes in 3d orbital =?
Number of angular nodes = l
Number of radial nodes = n – l – 1

1. For 3d orbital:
Number of angular nodes = 2 because l = 2
Number of radial nodes = 3 – 2 -1 = 0
Total number of nodes in 3d orbital = 2

2. For 4f orbital:
Number of angular nodes = 3 because l = 3
Number of radial nodes = n – l – l =4 – 3 – 1 = 0
Total number of nodes in 4f orbital = 3.

Question 5.
The energy of an electron in a hydrogen atom in the ground state is -13.6 eV. What is the energy of the electron in the second excited state?
Energy of an electron in ground state = -13.6 eV.
∴ The energy of an electron in the second excited state = E2.
n = 2
E2 = $$\frac{-13.6 \mathrm{eV}}{\mathrm{n}^{2}}$$ = $$\frac{-13.6}{2^{2}}$$ = $$\frac{-13.6}{4}$$ = -3.4 eV.

Question 6.
How many unpaired electrons are present in the ground state of Fe3+ (z = 26), Mn2+ (z = 25) and argon (z=18)?

1s2 2s2 2p6 3s2 3p6 3d6 4s2 for Fe atom.
1s2 2s2 2p6 3s2 3p6 3d6 3d5 for Fe3+ ion.
So, it contains 5 unpaired electrons.
Mn (Z = 25). Electronic configuration is 1s2 2s2 2p6 3s2 3p6 3d6 3d5
Mn → Mn2+ + 2e
Number of unpaired electrons in Mn2+ = 5
Ar (Z = 18). Electronic configuration is 1s2 2s2 2p6 3s2 3p6.
All orbitals are completely filled. So, no unpaired electrons in it.

Question 7.
Explain the meaning of the symbol 4f2. Write all the four quantum numbers for these electrons.
4f2 : It means that the element has 2 electrons in outermost 4f shell.
Quantum number values are,
n = principal quantum number = 4
l = azimuthal quantum number = 3
m = magnetic quantum number = – 3, -2
s = spin quantum number = +$$\frac {1}{2}$$ – $$\frac {1}{2}$$.

Question 8.
Which has the stable electronic configuration? Ni2+ or Fe3+
Ni (Z = 28). 1s2 2s2 2p6 3s2 3p64s23d8
Ni2+ electronic configuration = Is2 2s22p6 3s2 3p6 3d8
Fe (Z = 26). 1s2 2s2 2p6 3s2 3p6 4s2 3d6
Fe3+ Is2 2s2 2p6 3s23p6 3d5
If d orbital is half filled, according to Aufbau principle, it is more stable. So Fe3+ is more stable than Ni2+.

### Samacheer Kalvi 11th Chemistry Solutions Quantum Mechanical Model of Atom Additional Questions Solved

Question 1.
Which of the following experiment proves the presence of an electron in an atom?
(a) Rutherford’s α-ray scattering experiment
(b) Davisson and Germer experiment
(c) J.J. Thomson cathode ray experiment
(d) G.R Thomson gold foil experiment
(c) J.J. Thomson cathode ray experiment.

Question 2.
Consider the following statements regarding Rutherford’s α-ray scattering experiment.
i. Most of the α-particles were deflected through a small angle.
ii. Some of α-particles passed through the foil.
iii. Very few α-particles were reflected back by 180°.
Which of the above statements is/are not correct.
(a) i and ii
(b) ii and iii
(c) i and iii
(d) i ii and iii
(a) i and ii.

Question 3.
Considering Bohr’s model which of the following statements is correct?
(a) The energies of electrons are continuously reduced in the form of radiation.
(b) The electron is revolving around the nucleus in a dynamic orbital.
(c) Electrons can revolve only in those orbits in which the angular momentum (mvr) of the electron must be equal to an integral multiple of h/2 π.
(d) In an atom, electrons are embedded like seeds in watermelon.
(c) Electrons can revolve only in those orbits in which the angular momentum (mvr) of the electron must be equal to an integral multiple of h/2π.

Question 4.
The energy of an electron of hydrogen atom in 2nd main shell is equal to
(a) – 13.6 eV atom-1
(b) – 6.8 eV atom-1
(c) – 0.34 eV atom-1
(d) – 3.4 eV atom-1
(d) -3.4 eV atom-1
Hints:
Energy of an electron in 2nd main shell = $$\frac{(-13.6) Z^{2}}{n^{2}}$$; Z = 1, n = 2
E = $$\frac{-13.6}{2^{2}}$$ = $$\frac{-13.6}{4}$$ = -3.4 atom-1.

Question 5.
The energy of an electron of Li2+ in the 3rd main shell is …………..
(a) – 1.51 eV atom-1
(b) – 6.8 eV atom-1
(c) + 1.51 eV atom-1
(d) – 3.4 eV atom-1
(a) -1.51 eV atom-1
Hints:
E = $$\frac{(-13.6) Z^{2}}{n^{2}}$$ eV atom-1
Li2+= H atom. So Z = 1, n = 3.
E = $$\frac{(-13.6) 1^{2}}{3^{2}}$$ = $$\frac{-13.6}{9}$$ = -1.51 eV atom-1

Question 6.
The energy of an electron of a hydrogen atom in the main shell in terms of U mold is
(a) – 1312.8 k J mol-1
(b) – 82.05 k J mol-1
(c) – 328.2 kJ mol-1
(d) – 656.4 k J mol-1
(b) – 82.05 k J mol-1
Hints:
E = $$\frac{(-13.6) Z^{2}}{n^{2}}$$ kJ mol-1 , Z = 1, n = 4
∴ E = $$\frac{-1312.8}{16}$$ = -82.50 kJ mol-1

Question 7.
The Bohr’s radius of Li2 0f21d orbit is
(a) 0.529 Å
(b) 0.0753 Å
(c) 0.7053 Å
(d) 0.0529 Å
(c) 0.7053 Å
Hints:
rn = $$\frac{(0.529) Z^{2}}{n^{2}}$$Å, n = 2, Z = 3(for Li2+)
r = $$\frac{(0.529) 3^{2}}{2^{2}}$$ = $$\frac{0.529 x 4}{3}$$ = 0.7053 Å.

Question 8.
The formula used to calculate the Boh’s radius is ………..
(a) rn = $$\frac{(-13.6) Z^{2}}{n^{2}}$$ eV atom-1
(b) rn = $$\frac{(0.529) Z^{2}}{n^{2}}$$ A
(c) rn= $$\frac{(-1312.8) Z^{2}}{n^{2}}$$ kJ mol-1
(d) rn = $$\frac{(+1312.8) Z^{2}}{n^{2}}$$ kJ mol-1
(b) rn = $$\frac{(0.529) Z^{2}}{n^{2}}$$ A.

Question 9.
Who proposed the dual nature of light to all forms of matter?
(a) John Dalton
(b) Neils Bohr
(c) Albert Einstein
(d) J.J. Thomson
(c) Albert Einstein

Question 10.
dc Brogue equation is ………..
(a) E = h γ
(b) E = mc2
(c) γ = $$\frac{\mathrm{E}_{2}-\mathrm{E}_{1}}{\mathrm{h}}$$
(d) λ = $$\frac{h}{mv}$$
(d) λ = $$\frac{h}{mv}$$.

Question 11.
The crystal used in Davison and Germer experiment is …………….
(a) nickel
(b) zinc suiphide
(c) gold foil
(d) NaCl
(a) nickel.

Question 12.
Which one of the following is the time independent Schrodinger wave equation?

Question 13.
Match the list-I and list-II correctly using the code given below the list.
List – I
A. Principal quantum number
B. Azimuthal quantum number
C. Magnetic quantum number
D. Spin quantum number

List – II
1. represents the directional orientation of orbital
2. represents the spin of the electron
3. represents the main shell
4. represents the subshell

Question 14.
The maximum number of electrons that can be accommodated in N shell is …………..
(a) 8
(b) 18
(c) 32
(d) 36
(c) 32
Hints:
Number of electrons in the main shell = 2n2 n = 4, for N shell.
∴ Maximum number of electrons in N shell = 2(4)2 = 32.

Question 15.
The maximum number of electrons that can be accommodated in f orbital is ………….
(a) 10
(b) 14
(c) 16
(d) 6
(6) 14
Hints:
f orbital – l = 3.
Maximum number of electrons in sub shell = 2(2l + 1)
∴ For ‘f’ orbital, the maximum number of electrons = 2(2 x 3 + l) = 14.

Question 16.
When l = 0, the number of electrons that can be accommodated in the subshell is ……………..
(a) 0
(b) 2
(c) 6
(d) 8
(b) 2
Hints:
If l = 0, number of electrons = (2l + 1)
= 2 (2 x 0 + 1) = 2.

Question 17.
Which one of the quantum numbers is used to calculate the angular momentum of an atom?
(a) n
(b) m
(c) l
(d) s
(c) l

Question 18.
What is the formula used to calculate the angular momentum?
(a) $$\sqrt{l^{(l+1)}} \frac{h}{2 \pi}$$
(b) $$\frac{\mathrm{mvr}}{2 \pi}$$
(c) $$\frac{mvr}{2}$$
(d) m . ∆v
(a) $$\sqrt{l^{(l+1)}} \frac{h}{2 \pi}$$.

Question 19.
Which of the following provides the experimental justification of magnetic quantum number?
(a) Zeeman effect
(b) Stark effect
(c) Uncertainty principle
(d) Quantum condition
(a) Zeeman effect.

Question 20.
What are the values of n, l, m, and s for 3px electron?
(a) 3, 2, 1, 0
(b) 3, 1,-l, +½
(c) 3, 2, +1, -½
(d) 3, 0, 0, +½]
(b) 3, 1, -1, +½
Hint:
3px electron ; n = 3 (main shell)
for px orbitaI, l = 1, m = -1, s = $$\frac {1}{2}$$.

Question 21.
Identify the quantum number for $$4 d_{x^{2}-y^{2}}$$ electron.
(a) 4, 2, -2, +½
(b) 4, 0, 0, +½
(c) 4, 3, 2, +½
(d) 4, 3, 2, -½
(a) 4, 2, -2, +½.

Question 22.
How many orbitals are possible in 3rd energy level?
(a) 16
(6) 9
(c) 3
(d) 27
(b) 9
Hints:
3rd energy level Number of orbitals = ?
n = 3 main shell = m
l = 0, 1,2 m = 0, -1,0, +1
Total = 9 orbitals.

Question 23.
The region where the probability density function of electron reduces to zero is called
(a) orbit
(b) orbital
(c) nodal surface
(d) subshell
(c) nodal surface.

Question 24.
Consider the following statements.
(i) The region where the probability density of electron is zero, called nodal surface.
(ii) The probability of finding the electron is independent of the direction of the nucleus.
(iii) The number of radial nodes is equal to n + l + 1 Which of the above statements is/are correct?
(a) (i) and (iii)
(b) (i) and (ii)
(c) (iii) only
(d) (ii) and (iii)
(b) (i) and (ii).

Question 25.
Match the list-I and List-II correctly using the code given below the list.
List-I
A. s – orbital
B. p – orbital
C. d – orbital
D. f – orbital

List-II
1. complex three-dimensional shape
2. symmetrical sphere
3. dumb-bell shape
4. cloverleaf shape

Question 26.
Which one of the following is the correct increasing order of effective nuclear charge felt by an electron?
(a) s>p>d>f
(b) s<p<d<f
(c) s>p>f>d
(d) f<p<d<s
(a) s>p>d>f.

Question 27.
The value of n, l, m and s of 8th electron in an oxygen atom are respectively
(a) 1, 0, 0, + ½
(b) 2, 1, +1, – ½
(c) 2, 1, -1, – ½
(d) 2, 1, 0, +½
(a) 2, 1, +1, – ½.

Question 28.
The number of impaired electrons in carbon atom in the gaseous state is
(a) 0
(b) 1
(c) 2
(d) 3
(c) 2

Question 29.
Which of the following is not used in writing electronic configuration of an atom?
(a) Aufbau principle
(b) Hund’s rule
(c) Pauli’s exclusion principle
(d) Heisenberg’s uncertainty principle
(d) Heisenberg’s uncertainty principle.

Question 30.
Which of the following is the expected configuration of Cr (Z = 24)?
(a) 1s2 2s2 2p6 3s2 3p6 3d4 4s2
(b) 1s2 2s2 2p6 3s2 3p6 3d5 4s1
(c) 1s2 2s2 2p6 3s2 3p6 3d6
(d) 1s2 2s2 2p6 3s2 3p6 3d5 4s3
(a) 1s2 2s2 2p6 3s2 3p6 3d4 4s2

Question 31.
Which of the following is the actual configuration of Cr (Z = 24)?
(a) 1s2 2s2 2p6 3s2 3p6 3d4 4s2
(b) 1s2 2s2 2p6 3s2 3p6 3d5 4s1
(c) 1s2 2s2 2p6 3s2 3p6 3d6
(d) 1s2 2s2 2p6 3s2 3p6 3d5 4s3
(b) 1s2 2s2 2p6 3s2 3p6 3d5 4s1

Question 32.
Assertion (A) : Cr with electronic configuration [Ar] 3d5 4s1 is more stable than [Ar] 3d4 4s1.
Reason(R ): Half-filled orbitals have been found to have extra stability than partially filled orbitals.
(a) A and R are correct and R is the correct explanation of A.
(b) A and R are correct but R is not the correct explanation of A.
(c) A is correct but R is wrong.
(d) A is wrong but R is correct.
(a) A and R are correct and R is the correct explanation of A.

Question 33.
Assertion (A): Copper (Z = 29) with electronic configuration [Ar] 4s1 3d10 is more stable than [Ar] 4s1 3d10.
Reason(R): Copper with [Ar] 4s2 3d9 is more stable due to symmetrical distribution and exchange energies of d electrons.
(a) A and R are correct and R is the correct explanation of A.
(b) A and R are correct but R is not the correct explanation of A.
(c) A is correct but R is wrong.
(d) A is wrong but R is correct.
(a) A and R are correct and R is the correct explanation of A.

Question 34.
In a sodium atom (atomic number = 11 and mass number = 23) and the number of neutrons is …………..
(a) equal to the number of protons
(b) less than the number of protons
(c) greater than the number of protons
(d) none of these
(c) greater than the number of protons.

Question 35.
The idea of stationary orbits was first given by …………
(a) Rutherford
(b) J.J. Thomson
(c) Nails Bohr
(d) Max Planck
(c) Niels Bohr.

Question 36.
de Broglie equation is ……………
(a) λ = $$\frac {h}{mv}$$
(b) λ = $$\frac {hv}{m}$$
(c) λ = $$\frac {mv}{h}$$
(d) λ = hmv
(a) λ = $$\frac {h}{mv}$$.

Question 37.
The orbital with n = 3 and l = 2 is …………..
(a) 3s
(b) 3p
(c) 3d
(d) 3J
(c) 3d

Question 38.
The outermost electronic configuration of manganese (at. no. = 25) is …………
(a) 3d5 4s2
(b) 3d6 4s1
(c) 3d7 4s0
(d) 3d6 4s2
(a) 3d5 4s2

Question 39.
The maximum number of electrons in a sub-shell is given by the equation
(a) n2
(b) 2n2
(c) 2l – l
(d) 2l + 1
(d) 2l + 1

Question 40.
Which of the following statements is correct for an electron that has the quantum numbers n = 4 and m = -2.
(a) The electron may be in 2 p orbital
(b) The electron may be in 4 d orbital
(c) The electron is in the second main shell
(d) The electron must have spin quantum number as +$$\frac {1}{2}$$.
(b) The electron may be in 4d orbital.

Samacheer Kalvi 11th Chemistry Quantum Mechanical Model of Atom 2 – Marks Questions

Question 1.
What is a stationary orbit?
The electron is revolving around the nucleus in a certain fixed circular path called the stationary orbit.

Question 2.
Explain the theory of electromagnetic radiation.

• The theory of electromagnetic radiation states that a moving charged particle should continuously lose its energy in the form of radiation.
• Therefore, the moving electron in an atom should continuously lose its energy and finally collide with the nucleus resulting in the collapse of the atom.

Question 3.
Explain how the matter has dual character?

• Albert Einstein proposed that light has dual nature, i.e. like photons behave both like a particle and as a wave.
• Louis de Broglie extended this concept and proposed that all forms of the matter showed dual character.
• He combined the following two equations of the energy of which one represents wave character (hυ) and the other represents the particle nature (mc2).

Question 4.
Explain the significance of the de Broglie equation.

• X = $$\frac {h}{mv}$$. This equation implies that a moving particle can be considered as a wave and a wave can exhibit the properties of a particle.
• For a particle with high linear momentum (mv), the wavelength will be so small and cannot be observed.
• For a microscopic particle such as an electron, the mass is of the order of 10-31 kg, hence the wavelength is much larger than the size of an atom and it becomes significant.
• For the electron, the de Broglie wavelength is significant and measurable while for the iron ball it is too small to measure, hence it becomes insignificant.

Question 5.
How many electrons can be accommodated in the main shell l, m, and n?

Question 6.
How many electrons can be accommodated in the sub-shell s, p, d, f?

Question 7.
Why is de Broglie concept is insignificant for macroscopic particles?
The de Broglie wavelength is too small to measure for macroscopic particles and hence, it becomes insignificant.

Question 8.
How many orbitals are possible in the 3rd energy level?
n = 3, main shell is m.
Total number of orbitals in 3rd energy level = ?

Total number of orbitals = 9.

Question 9.
What are Ψ and Ψ2?

• Ψ itself has no physical meaning but it represents an atomic orbital.
• Ψ2 is related to the probability of finding the electrons within a given volume of space.

Question 10.
What is meant by nodal surface?

• The region, where there is a probability density function, reduces to zero is called nodal surface or a radial node.
• For ns orbital, (n-1) nodes are found in it.

Question 11.
Mention the shape of s, p, d orbitals.

• The shape of s – orbital – sphere
• The shape of p – orbital – dumbbell
• The shape of d – orbital – cloverleaf

Question 12.
What is the physical significance of ψ and ψ2?
The wave function ψ itself has no physical meaning. However, the probability of finding the electron in a small volume dxdydz around a point (x, y, z) is proportional to |ψ(x, y, z)|2 dxdydz. |ψ(x, y, z)|2 is known as probability density and is always positive.

Question 13.
Write the equation to calculate the energy of nth orbit.
En = $$\frac{(-1312.8) Z^{2}}{n^{2}}$$ kJ mol-1
Where Z = atomic number, n = principal quantum number.

Question 14.
what are degenerate orbitals?

• Three different orientations in space that are possible for a p-orbital. All the three p-orbitals, namely px, py and pz have same energies and are called degenerate orbitals.
• In the presence of magnetic or electric field, the degeneracy is lost.

Question 15.
Energy of an electron in hydrogen atom in ground state is -13.6 eV. What is the energy of the electron in the third excited state?
E1 = – 13.6 eV
E3 = $$\frac{-13.6}{n^{2}}$$ Where n = 3
E3 = $$\frac{-13.6}{9}$$ = 1.511 eV
Energy of the electron in the third excited state = 1.511 eV.

Question 16.
What are quantum numbers?
The electron in an atom can be characterized by a set of four quantum numbers, namely principal quantum number(n), azimuthal quantum number (l), magnetic quantum number (m), and spin quantum number (s).

Question 17.
State Hund’s rule of maximum multiplicity.
It states that electron pairing in the degenerate orbitals does not take place until all the available orbitals contain one electron each.

Question 18.
How many unpaired electrons are present in the ground state of –
1. Cr3+ (Z = 24)
2. Ne (Z = 10)
1. Cr3+ (Z = 24) 1s2 2s2 2p6 3s2 3p6 3d5 4s1
Cr3+ – 1s2 2s2 2p6 3s2 3p6 3d4.
It contains 4 unpaired electrons.

2. Ne (Z = 10) 1s22s22p6. No unpaired electrons in it.

Question 19.
What is meant by electronic configuration? Write the electronic configuration of N (Z = 7).
The distribution of electrons into various orbitals of an atom is called its electronic configuration.

Question 20.
Which is the actual configuration of Cr (Z = 24) Why?
Cr (Z = 24) 1s22s22p6.
The reason for this is, Cr with 3d5 configuration is half filled and it will be more stable. Chromium has [Ar] 3d5 4s1 and not [Ar] 3d4 4s2 due to the symmetrical distribution and exchange energies of d electrons.

Question 21.
What is the actual configuration of copper (Z = 29)? Explain about its stability.
Copper (Z = 29)
Expected configuration : 1s2 2s2 2p6 3s2 3p6 3d9 4s2
Actual configuration : 1s2 2s2 2p6 3s2 3p6 3d10 4s1
The reason is that fully filled orbitals have been found to have extra stability. Copper has the electronic configuration [Ar] 3d10 4s1 and not [Ar] 3d9 4s2 due the symmetrical distribution and exchange energies of d electrons. Symmetry leads to stability. The full filled configuration have symmetrical distribution of electrons and hence they are more stable than unsymmetrical configuration.

Samacheer Kalvi 11th Chemistry Quantum Mechanical Model of Atom 3 – Mark Questions

Question 1.
Write the observations of Rutherford’s α-ray scattering experiment.
The observations of the α-ray scattering experiment are
(i) most of the α-particles passed through the foil
(ii) some of them were deflected through a small angle and
(iii) very few a -particles were reflected back by 180°.

Question 2.
What are the limitations of Bohr’s atom model?

• The Bohr’s atom model is applicable only to species having one electron such as hydrogen, Li2+ etc, and not applicable to multi-electron atoms.
• It was unable to explain the splitting of spectral lines in the presence of a magnetic field (Zeeman effect) or an electric field (Stark effect).
• Bohr’s theory was unable to explain why the electron is restricted to revolve around the nucleus in a fixed orbit in which the angular momentum of the electron is equal to nh / 2π.

Question 3.
Illustrate the significance of de Broglie equation with an iron ball and an electron.

1. 6.626 kg iron ball moving with 10 ms-1.
2. An electron moving at 72.73 ms-1.

1. λiron ball = $$\frac{h}{mv}$$

= 1 x 10-35m

2. λiron ball = $$\frac{h}{mv}$$

= $$\frac{6.626}{662.6}$$ x 10-3m = 1 x 105m
For an electron, the de Broglie wavelength is significant and measurable while for iron ball it is too small to measure, hence it becomes insignificant.

Question 4.
What are the limitations of Bohr’s atom model?
The Bohr’s atom model is applicable only to species having one electron such as hydrogen, Li2+, etc., and not applicable to multi-electron atoms. It was unable to explain the splitting of spectral lines in the presence of a magnetic field (Zeeman effect) or an electric field (Stark effect). Bohr’s theory was unable to explain why the electron is restricted to revolve around the nucleus in a fixed orbit in which the angular momentum of the electron is equal to $$\frac{n h}{2 \pi}$$

Question 5.
Bohr radius of 1st orbit of a hydrogen atom is 0.529 Å. Assuming that the position of an electron in this orbit is determined with the accuracy of 0.5% of the radius, calculate the uncertainty in the velocity of the electron in the hydrogen atom.
Uncertainty in position = ∆x
= $$\frac{0.5}{100}$$ x 0.529 Å
= $$\frac{0.5}{100}$$ x 10-10 x 0.529 m
∆x = 2.645 x 10-13 m
From Heisenberg’s uncertainty principle,
∆x.∆p ≥ $$\frac{h}{4π}$$
∆x.m.∆p ≥ $$\frac{h}{4π}$$
∆v ≥ $$\frac{h}{∆x.m.4π}$$
∆v =
∆v = 2.189 x 108m.

Question 6.
State and explain Heisenberg’s principle.
The dual nature of matter imposes a limitation on the simultaneous determination of position and velocity of a microscopic particle. Based on this, Heisenberg arrived at his uncertainty principle, which states that ‘It is impossible to accurately determine both the position as well as the momentum of a microscopic particle simultaneously’. The product of uncertainty in the measurement is expressed as follows.
∆x . ∆p ≥ $$\frac{h}{4 \pi}$$
where, ∆x and ∆p are uncertainties in determining the position and momentum, respectively. The uncertainty principle has negligible effect for macroscopic objects and becomes significant only for microscopic particles such as electrons.

Question 7.
Explain the azimuthal quantum number.

• It is represented by the letter 7′ and can take integral values from zero to n – 1, where n is the principal quantum number.
• Each l value represents a subshell (orbital). l = 0, 1, 2, 3 and 4 represents the s, p, d, f and g orbitals respectively.
• The maximum number of electrons that can be accommodated in a given subshell (orbital) is 2(2l + 1).
It is used to calculate the orbital angular momentum using the expression Angular momentum = $$\sqrt{l(l+1)} \frac{h}{2 \pi}$$.

Question 8.
Draw the shapes of 1s, 2s and 3s orbitals

Question 9.
Explain how effective nuclear charge is related with stability of the orbital.

• In a multi-electron atom, in addition to the electrostatic attractive force between the electron and nucleus, there exists a repulsive force among the electrons.
• These two forces are operating in the opposite direction. This results in the decrease in the nuclear force of attraction on electron.
• The net charge experienced by the electron is called effective nuclear charge.
• The effective nuclear charge depends on the shape of the orbitals and it decreases with increase in azimuthal quantum number l.
• The order of the effective nuclear charge felt by a electron in an orbital within the given shell is s > p > d > f.
• Greater the effective nuclear charge, greater is the stability of the orbital. Hence, within a given energy level, the energy of the orbitals are in the following order s < p < d < f.

Question 10.
Calculate the wavelength of an electron moving with a velocity of 2.05 x 107 ms-1.
According to de Broglie’s equation, λ = $$\frac {h}{mv}$$
Mass of electron (m) = 9.1 x 10-31 kg
Velocity of electron (υ) = 2.05 x 107 ms-1
Planck’s constant (h) = 6.626 x 10-34 kg m2 s-1
λ =  =355 x 10-4m.

Question 11.
The mass of an electron is 9.1 x 10-31 kg. If its kinetic energy is 3.0 x 10-25 J, calculate its wavelength.
Step I.
Calculation of the velocity of electron
Kinetic energy = 1 / 2 mυ2 = 3.0 x 10-25 kg m2 s-2
υ2 = 65.9 x 104 m2 s-2
υ = (65.9 x 104 m s-2) = 8.12 x 102 ms-1

Step II.
Calculation of wavelength of the electron
According to de Broglie’s equation,
λ = $$\frac {h}{mv}$$ =
=  0.08967 x l0-5 m = 8967 x 10-10 m = 8967 Å (∴1Å = 10-10m).

Question 12.
From the following sets of quantum numbers, state which are possible. Explain why the others are not possible.

1. n = 0, l = 0, ml = 0, ms = + $$\frac {1}{2}$$
2. n = 1, l = 0, ml = 0, ms = – $$\frac {1}{2}$$
3. n = 1, l = 1, ml = 0, ms = + $$\frac {1}{2}$$
4. n = 1, l = 0, ml = +1, ms= +$$\frac {1}{2}$$
5. n = 3, l = 3, ml = -3, ms = + $$\frac {1}{2}$$
6. n = 3, l = 1, ml = 0, ms = +$$\frac {1}{2}$$

1. The set of quantum numbers is not possible because the minimum value of n can be 1 and not zero.
2. The set of quantum numbers is possible.
3. The set of quantum numbers is not possible because, for n = 1,1 cannot be equal to 1. It can have 0 value.
4. The set of quantum numbers is not possible because for l = 0, ml; cannot be +1. It must be zero.
5. The set of quantum numbers is not possible because, for n = 3, l = 3.
6. The set of quantum numbers is possible.

Question 13.
How many electrons in an atom may have the following quantum numbers?
(a) n = 4; ms = – ½
(b) n = 3, l = 0.
(a) For n = 4
1 Total number of electrons = 2n2 = 2 x 16 = 32
Half out of these will have ms = – $$\frac {1}{2}$$
Total electrons with ms (-½) = 16.

(b) For n = 3
l = 0; m1 = 0, ms = + ½ – ½ (two e).

Question 14.
Show that the circumference of the Bohr orbit for the hydrogen atom is an integral multiple of the de Broglie wavelength associated with the electron revolving around the orbit.
According to Bohr’s theory,
mυr = $$\frac {nh}{2π}$$ (n = 1,2,3, …… so on)
or 2πr = $$\frac {nh}{mυ}$$ or mυ = $$\frac {nh}{2πr}$$ ………..(i)
According to de Brogue equation,
λ = $$\frac {h}{mυ}$$ or mυ = $$\frac {h}{λ}$$ ……….(ii)
Comparing (i) and (ii),
$$\frac {nh}{2πr}$$ = $$\frac {h}{λ}$$ or 2πr = nλ
Thus, the circumference (2πr) of the Bohr orbit for hydrogen atom is an into the de Broglie wave length.

Question 15.
An ion with mass number 56 contains 3 units of positive charge and 30.4% more neutrons than electrons. Assign symbol to the ion.
Let the no. of electrons in the ion = x
the no. of the protons = x + 3 (as the ion has three units positive charge)
and the no. of neutrons = x + $$\frac {30.4x }{100}$$ = x + 0.304 x
Now, mass number of ion = Number of protons + Number of neutrons
= (x + 3) + (x + 0.304 x)
∴ 56 = (x + 3) + (x + 0.304 x) or 2.304 x = 56 – 3 = 53
x = $$\frac {53}{2.304}$$ = 23
Atomic number of the ion (or element) = 23 + 3 = 26
The element with atomic number 26 is iron (Fe) and the corresponding ion is Fe3+.

Question 16.
The uncertainty in the position of a moving bullet of mass 10 g is 10 s m. Calculate the uncertainty in its velocity?
According to uncertainty principle,
∆x.m∆υ = $$\frac {h}{4π}$$ or ∆υ = $$\frac {h}{4πm∆x}$$;
h = 6.626 x 1o-34 kg m2 s-1; m = 10 g = 10-2 kg
∆x = 10-5m; ∆v =  = 5.27 x 10-28mv
= 1.6 x 10-15 kg m2 s-15
Or
$$\frac {1}{2}$$ mv2 = 1.6 x 10-15kg m2s-2
v =  = 5.93 x 107m-1

Question 17.
The uncertainty in the position and velocity of a particle are 10-10 m and 5.27 × 10-24 ms-1 respectively. Calculate the mass of the particle.
According to uncertainty principle.
∆x. m∆υ = $$\frac {h}{4π}$$
or
m = $$\frac {h}{4π∆x.∆υ}$$;
h = 6.626 x 10-34 kg m2 s-1
∆x = 10-10 m; ∆x = 5.27 x 10-24ms-1
m  = 0.1 kg.

Question 18.
With what velocity must an electron travel so that its momentum Is equal to that of a photon of wave length = 5200 A?
According to de Brogue equation, λ = $$\frac {h}{mv}$$
Momentum of electron, mv = $$\frac {h}{λ}$$
= 1.274 x 10-27 kg ms-1 ………(i)
The momentum of electron can also be calculated as = mv = (9.1 x 10-31kg) x v ………(ii)
Comparing (i) and (ii)
(9.1 X 10-31kg) v = (1.274 x 10-27 kg ms-1)
= 1.4 x 103 ms-1

Question 19.
Using Aufbau principle, write the ground state electronic configuration of following atoms.

1. Boron (Z = 5)
2. Neon (Z = 10)
3. Aluminium (Z = 13)
4. Chlorine (Z = 17)
5. Calcium (Z = 20)
6. Rubidium (Z = 37)

1. Boron (Z = 5) ; 1s2 2s2 2p1
2. Neon (Z = 10) ; 1s2 2s2 2p6
3. Aluminium (Z = 13) ; 1s2 2s2 2p6 3s2 3p1
4. Chlorine(Z = 17) ; 1s2 2s2 2p6 3s2 3p5
5. Calcium (Z = 20) ; 1s2 2s2 2p6 3s2 3p6 4s2
6. Rubidium (Z = 37) ; 1s2 2s22p6 3s2 3p63d10 4s2 4p6 5s1

Question 20.
Calculate the de Broglie wavelength of an electron moving with 1 % of the speed of light?
According to de Brogue equation, A = $$\frac {h}{mv}$$
Mass of electron = 9.1 x 10-31 kg; Planck’s constant 6.626 x 10-34 kg m2 s-1
Velocity of electron = 1% of speed of light = 3.0 x 108 x 0.01 = 3 106 ms-1
Wavelength of electron (λ) = $$\frac {h}{mv}$$
= 2.43 x 10-10m.

Question 21.
What is the wavelength for the electron accelerated by 1.0 X i0 volts?
Step I.
Calculation of the velocity of electron
Energy (kinetic energy) of electron = 1.0 x 104 volts.
= 1.0 x 104 x 1.6 x 10-19 J = 1.6 x 10-15J.

Step II.
Calculation of wavelength of the electron
According to de Broglie equation,
λ = $$\frac {h}{mυ}$$; λ
= 1.22 x 10-11m .

Question 22.
In a hydrogen atom, the energy of an electron in first Bohr’s orbit is 13.12 x 105 J mol-1. What is the energy required for its excitation to Bohr’s second orbit?

The energy required for the excitation is:
∆E = E2 – E1 = (-3.28 x l05) – (- 13.12 x 105) = 9.84 x 105 J mol-1

Question 23.
Dual behavior of matter proposed by de Broglie led to the discovery of electron microscope often used for the highly magnified images of biological molecules and other type of material. If the velocity of the electron in this microscope is 1.6 x 106 ms-1, calculate de Broglie wavelength associated with this electron.
λ = $$\frac {h}{mυ}$$; λ =
= 0.455 x 10-34 + 25 m = 0.455 nm = 455 pm.

Question 24.
An element with mass number 81 contains 31.7% more neutrons as compared to protons. Assign the symbol to the element.
An element can be identified by its atomic number only. Let us find the atomic number.
Let the number of protons = x
∴ Number of neutrons = x + $$\frac {x × 31.7}{100}$$ = (x + 0.317 x)
Now, Mass no. of element = No. of protons + No. of neutrons
81 = x + x + 0.317 x = 2.317 x
Or
x = $$\frac {81}{2.317}$$ = 35
∴ No. of protons = 35, No. of neutrons = 81 – 35 = 46
Atomic number of element (Z) = Number of protons = 35
The element with atomic number (Z) 35 is bromine 8135Br.

Question 25.
The electron energy in hydrogen atom is given by En = (- 2.18 × 10-18) / n2 J. Calculate the energy required to remove an electron completely from the n = 2 orbit. What is the longest wavelength of light in cm that can be used to cause this transition?
Step I.
Calculation of energy required
The energy required is the difference in the energy when the electron jumps from orbit with
n = ∞ to orbit with n = 2.
The energy required (∆E) = E – E2
= 0 – $$\left(-\frac{2.18 \times 10^{-18}}{4} \mathrm{J}\right)$$ = 5.45 x 10-19 J.

Step II.
Calculation of the longest wavelength of light in cm used to cause the transition
∆E = hv = hc / λ.
λ = $$\frac {hc}{∆E}$$ = n= 3.644 x 10-7
m = 3.644 x 10-7 x 102 = 3.645 x 10-5 cm.

Samacheer Kalvi 11th Chemistry Quantum Mechanical Model of Atom 5-Mark Questions

Question 1.
Assumptions of Bohr atom model.
1. The energies of electrons are quarantined

2. The electron is revolving around the nucleus in a certain fixed circular path called the stationary orbit.

3. Electron can revolve only in those orbits in which the angular momentum (mvr) of the electron must be equal to an integral multiple of h/2π
mvr = $$\frac {nh}{2π}$$ where n = 1,2,3,…etc.,

4. As long as an electron revolves in a fixed stationary orbit, it doesn’t lose its energy. But if an electron jumps from a higher energy state (E2) to a lower energy state (E1), the excess energy is emitted as radiation. The frequency of the emitted radiation is E2 – E1= hv.
∴ v = $$\frac{\mathrm{E}_{2}-\mathrm{E}_{1}}{\mathrm{h}}$$
Conversely, when suitable energy is supplied to an electron, it will jump from lower energy orbit to a higher energy orbit.

5. Bohr’s postulates are applied to a hydrogen like atom (H, He+ and Li2+ etc..) the radius of the nth orbit and the energy of the electron revolving in the th orbit were derived.
rn = $$\frac{(0.529) n^{2}}{Z}$$ A(0.529) n2
En = $$\frac{(-1 3.6) Z^{2}}{n}$$ eV atom-1
En = $$\frac{(1312.8) Z^{2}}{n}$$ kJ mol-1

Question 2.
Derive de Brogue equation and give its significance.
1. Louis de Brogue extended the concept of dual nature of light to all forms of matter. To quantify this relation, he derived an equation for the wavelength of a matter-wave.

2. He combined the following two equations of the energy of which one represents wave character (hu) and the other represents the particle nature (mc2).
Planck’s quantum hypothesis:
E = hv ……….(1)
Einsteins mass-energy relationship:
E = mc2 ………(2)
From (1) and (2)
hv = mc2
hc/λ = mc2
∴ λ = $$\frac{h}{mc}$$ ………(3)
The equation (3) represents the wavelength of photons whose momentum is given by mc. (Photons have zero rest mass).

3. For a particle of matter with mass m and moving with a velocity y, the equation (3) can be written as λ = $$\frac{h}{mc}$$ ………(4)

4. This is valid only when the particle travels at speed much less than the speed of Light.

5. This equation implies that a moving particle can be considered as a wave and a wave can exhibit the properties of a particle (i.e momentum).

6. Significance of de Brogue equation:
For a particle with high linear momentum, the wavelength will be too small and cannot be observed. For a microscopic particle such as an electron, the mass is 9.1 x 10-31 kg. Hence the wavelength is much larger than the size of atom and it becomes significant.

Question 3.
What are the main features of the quantum mechanical model of an atom.
1. The energy of electrons in an atom is quarantined.

2. The existence of quarantined electronic energy levels is a direct result of the wave-like properties of electrons. The solutions of the Schrodinger wave equation gives the allowed energy levels (orbits).

3. According to Heisenberg’s uncertainty principle, the exact position and momentum of an electron cannot be determined with absolute accuracy. As a consequence, quantum mechanics introduced the concept of orbital. Orbital is a three-dimensional space in which the probability of finding the electron is maximum.

4. The solution of the Schrodinger wave equation for the allowed energies of an atom gives the wave function Ψ, which represents an atomic orbital. The wave nature of the electron present in an orbital can be well defined by the wave function Ψ.

5. The wave function Ψ itself has no physical meaning. However, the probability of finding the electron in a small volume dx, dy, dz around a point (x,y,z) is proportional to |Ψ (x,y,z)|2 dx dy dz |Ψ (x,y,z)|2 is known as probability density and is always positive.

Question 4.
(1) Magnetic quantum number
(2) Spin quantum number
(1) Magnetic quantum number:

• It is denoted by the letter ml. It takes integral values ranging from – l to +l through 0.
i.e. if l = 1; m = -1, 0 and +1.
• The Zeeman Effect (the splitting of spectral lines in a magnetic field) provides the experimental justification for this quantum number.
• The magnitude of the angular momentum is determined by the quantum number l while its direction is given by magnetic quantum number.

(2) Spin quantum number:

• The spin quantum number represents the spin of the electron and is denoted by the letter ‘ms‘.
• The electron in an atom revolves not only around the nucleus but also spins. It is usual to write this as electron spins about its own axis either in a clockwise direction or in anti-clockwise direction.
• Corresponding to the clockwise and anti-clockwise spinning of the electron, maximum two values are possible for this quantum number.
• The values of ‘ms‘ is equal to –$$\frac {1}{2}$$ and +$$\frac {1}{2}$$.

Question 5.
Explain about the shape of orbitals.
Orbital: The solution to Schrodinger equation gives the permitted energy values called eigen values and the wave functions corresponding to the eigen values are called atomic orbitals.

Shape of orbital:
s – orbital:
For Is orbital, l = 0, m = 0, f(θ) = 1√2 and g(φ) = 1/√2π. Therefore, the angular distribution function is equal to 1/√2π. i.e. it is independent of the angle θ and φ. Hence, the probability of finding the electron is independent of the direction from the nucleus. So, the shape of the s orbital is spherical.

p – orbital:
For p orbitals l = 1 and the corresponding m values are -1, 0 and +1. The three different m values indicates that there are three different orientations possible for p orbitals. These orbitals are designated as px, py and pz. The shape of p orbitals are dumb bell shape.

d – orbital:
For ‘d’ orbital 1 = 2 and the corresponding m values are -2, -1, 0, +l,+2. The shape of the d orbital looks like a clover leaf. The five m values give rise to five d orbitals namely dxy, dyz, dzx, dx2-y2 and dz2 The 3d orbitals contain two nodal planes.

f – orbital
For f orbital, 1 = 3 and the m values are -3, -2,-1, 0, +1, +2, +3 corresponding to seven f orbitals, $$\mathrm{f}_{\mathrm{z}^{3}}, \mathrm{f}_{\mathrm{xz}^{2}}, \mathrm{f}_{\mathrm{yz}^{2}}, \mathrm{f}_{\mathrm{xyz}}, \mathrm{f}_{\mathrm{z}\left(\mathrm{x}^{2}-\mathrm{y}^{2}\right)}, \mathrm{f}_{\mathrm{x}\left(\mathrm{x}^{2}-3 \mathrm{y}^{2}\right)}, \mathrm{f}_{\mathrm{y}\left(3 \mathrm{x}^{2}-\mathrm{y}^{2}\right)}$$. They contain 3 nodal planes.

Question 6.
What is exchange energy? How it is related with stability of atoms? Explain with suitable examples.