Chapters
Chapter 2: Quantum Mechanical Model of Atom
Chapter 3: Periodic Classification Of Elements
Chapter 4: Hydrogen
Chapter 5: Alkali and Alkaline Earth Metals
Chapter 6: Gaseous State
Chapter 7: Thermodynamics
Chapter 8: Physical and Chemical Equilibrium
Chapter 9: Solutions
Chapter 10: Chemical bonding
Chapter 11: Fundamentals of Organic Chemistry
Chapter 12: Basic concept of organic reactions
Chapter 13: Hydrocarbons
Chapter 14: Haloalkanes and Haloarenes
Chapter 15: Environmental Chemistry
Chapter 2: Quantum Mechanical Model of Atom
Tamil Nadu Board Samacheer Kalvi solutions for Class 11th Chemistry Volume 1 and 2 Answers Guide Chapter 2 Quantum Mechanical Model of AtomChoose the best answer [Pages 60 - 63]
Electronic configuration of species M^{2+} is 1s^{2} 2s^{2} 2p^{6} 3s^{2} 3p^{6} 3d^{6} and its atomic weight is 56. The number of neutrons in the nucleus of species M is
26
22
30
24
The energy of light of wavelength 45 nm is
6.67 × 10^{15}J
6.67 × 10^{11}J
4.42 × 10^{–18}J
4.42 × 10^{–15}J
The energies E_{1} and E_{2} of the two radiations are 25 eV and 50 eV respectively. The relation between their wavelengths ie λ_{1} and λ_{2} will be
`λ_1/λ_2` = 1
λ_{1} = 2λ_{2}
λ_{1} = `sqrt(25 xx 50)` λ_{2}
2λ_{1} = λ_{2}
Splitting of spectral lines in an electric field is called __________.
Zeeman effect
Shielding effect
Compton effect
Stark effect
Based on equation E = `-2.178 xx 10^(-18) "J" ("z"^2/"n"^2)`, certain conclusions are written. Which of them is not correct?
Equation can be used to calculate the change in energy when the electron changes orbit.
For n = 1, the electron has a more negative energy than it does for n = 6 which means that the electron is more loosely bound in the smallest allowed orbit.
The negative sign in equation simply means that the energy of electron bound to the nucleus is lower than it would be if the electrons were at the infinite distance from the nucleus.
Larger the value of n, the larger is the orbit radius.
According to the Bohr Theory, which of the following transitions in the hydrogen atom will give rise to the least energetic photon?
n = 6 to n = 1
n = 5 to n = 4
n = 5 to n = 3
n = 6 to n = 5
Assertion: The spectrum of He^{+} is expected to be similar to that of hydrogen.
Reason: He^{+} is also one electron system.
If both assertion and reason are true and reason is the correct explanation of assertion.
If both assertion and reason are true but reason is not the correct explanation of assertion.
If assertion is true but reason is false.
If both assertion and reason are false.
Which of the following pairs of d-orbitals will have electron density along the axes?
`"d"_("z"^2), "d"_"xz"`
`"d"_"xz", "d"_"yz"`
`"d"_("z"^2), "d"_("x"^2-"y"^2)`
`"d"_"xy", "d"_("x"^2-"y"^2)`
Two electrons occupying the same orbital are distinguished by __________.
azimuthal quantum number
spin quantum number
magnetic quantum number
orbital quantum number
The electronic configuration of Eu (Atomic no. 63) Gd (Atomic no. 64) and Tb (Atomic no. 65) are
[Xe] 4f^{6} 5d^{1} 6s^{2}, [Xe] 4f^{7} 5d^{1} 6s^{2} and [Xe] 4f^{8} 5d^{1} 6s^{2}
[Xe] 4f^{7} 6s^{2}, [Xe] 4f^{7} 5d^{1} 6s^{2} and [Xe] 4f^{9} 6s^{2}
[Xe] 4f^{7} 6s^{2}, [Xe] 4f^{8} 6s^{2} and [Xe] 4f^{8} 5d^{1} 6s^{2}
[Xe] 4f^{6} 5d^{1} 6s^{2}, [Xe] 4f^{7} 5d^{1} 6s^{2} and [Xe] 4f^{9} 6s^{2}
The maximum number of electrons in a sub shell is given by the expression
2n^{2}
2l + 1
4l + 2
none of these
For d-electron, the orbital angular momentum is
`(sqrt2"h")/(2π)`
`sqrt(2"h")/(2π)`
`(sqrt(2 xx 4)"h")/(2π)`
`(sqrt6"h")/(2π)`
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
4
6
2
10
Assertion: Number of radial and angular nodes for 3p orbital are 1, 1 respectively.
Reason: Number of radial and angular nodes depends only on principal quantum number.
both assertion and reason are true and reason is the correct explanation of assertion.
both assertion and reason are true but reason is not the correct explanation of assertion.
assertion is true but reason is false.
both assertion and reason are false.
The total number of orbitals associated with the principal quantum number n = 3 is
9
8
5
7
If n = 6, the correct sequence for filling of electrons will be,
ns → (n – 2)f → (n – 1)d → np
ns → (n – 1)d → (n – 2)f → np
ns → (n – 2)f → np → (n – 1)d
none of these are correct
Consider the following sets of quantum numbers:
n | l | m | s | |
(i) | 3 | 0 | 0 | `+1/2` |
(ii) | 2 | 2 | 1 | `-1/2` |
(iii) | 4 | 3 | –2 | `+1/2` |
(iv) | 1 | 0 | –1 | `+1/2` |
(v) | 3 | 4 | 3 | `-1/2` |
Which of the following sets of quantum number is not possible?
(i), (ii), (iii) and (iv)
(ii), (iv) and (v)
(i) and (iii)
(ii), (iii) and (iv)
How many electrons in an atom with atomic number 105 can have (n + 1) = 8?
30
17
15
unpredictable
Electron density in the yz plane of 3d_{xy} orbital is
zero
0.50
0.75
0.90
If uncertainty in position and momentum are equal, then minimum uncertainty in velocity is
`1/"m" sqrt("h"/π)`
`sqrt("h"/π)`
`1/"2m" sqrt("h"/π)`
`"h"/(4π)`
A macroscopic particle of mass 100 g and moving at a velocity of 100 cm s^{–1} will have a de Broglie wavelength of
6.6 × 10^{–29} cm
6.6 × 10^{–30} cm
6.6 × 10^{–31} cm
6.6 × 10^{–32} cm
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
4
0.2
2.5
0.4
The energy of an electron in the 3rd orbit of hydrogen atom is –E. The energy of an electron in the first orbit will be
–3E
`(-"E")/3`
`(-"E")/9`
–9E
Time independent Schrodinger wave equation is
`hat"H" ψ = "E"ψ`
`∇^2ψ + (8π^2"m")/"h"^2 ("E + V")ψ = 0`
`(∂^2ψ)/(∂"x"^2) + (∂^2ψ)/(∂"y"^2) + (∂^2ψ)/(∂"z"^2) + (2"m")/"h"^2 ("E" - "V")ψ = 0`
all of these
Which of the following does not represent the mathematical expression for the Heisenberg uncertainty principle?
`Δ"x".Δ"p" ≥"h"/(4π)`
`Δ"x".Δ"v" ≥"h"/(4π"m")`
`Δ"E".Δ"t" ≥"h"/(4π)`
`Δ"E".Δ"x" ≥"h"/(4π)`
Tamil Nadu Board Samacheer Kalvi solutions for Class 11th Chemistry Volume 1 and 2 Answers Guide Chapter 2 Quantum Mechanical Model of AtomWrite brief answer to the following questions [Pages 64 - 66]
Which quantum number reveal information about the shape, energy, orientation and size of orbitals?
How many orbitals are possible for n = 4?
How many radial nodes for 2s, 4p, 5d and 4f orbitals exhibit? How many angular nodes?
The stabilisation of a half-filled d-orbital is more pronounced than that of the p-orbital why?
Consider the following electronic arrangements for the d^{5} configuration.
⥮ | ⥮ | 1 | ||
(a) |
1 | 1 | 1 | ⥮ | |
(b) |
1 | 1 | 1 | 1 | 1 |
(c) |
- which of these represents the ground state.
- which configuration has the maximum exchange energy.
State and explain Pauli's exclusion principle.
Define orbital?
what are the n and l values for 3p_{x} and `"4d"_("x"^2 - "y"^2)` electron?
Explain briefly the time independent Schrodinger wave equation?
Calculate the uncertainty in position of an electron, if Δv = 0.1% and υ = 2.2 × 10^{6} ms^{-1}
Determine the values of all the four quantum numbers of the 8^{th} electron in the O-atom and 15^{th} electron in Cl atom.
The quantum mechanical treatment of the hydrogen atom gives the energy value:
E_{n} = `(-13.6)/"n"^2` ev atom^{−1}
- use this expression to find ΔE between n = 3 and n = 4
- Calculate the wavelength corresponding to the above transition.
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?
For each of the following, give the sub level designation, the allowable m values and the number of orbitals
- n = 4, l = 2
- n = 5, l = 3
- n = 7, l = 0
Give the electronic configuration of Mn^{2+} and Cr^{3+}
Describe the Aufbau principle.
An atom of an element contains 35 electrons and 45 neutrons. Deduce
- the number of protons
- the electronic configuration for the element
- All the four quantum numbers for the last electron
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.
Calculate the energy required for the process.
\[\ce{He^+_{(g)} -> He^2+_{(g)} + e^-}\]
The ionisation energy for the H atom in its ground state is −13.6 ev atom^{−1}.
An ion with mass number 37 possesses unit negative charge. If the ion contains 11.1% more neutrons than electrons. Find the symbol of the ion.
The Li^{2+} 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 4^{th} orbit.
Protons can be accelerated in particle accelerators. Calculate the wavelength (in Å) of such accelerated proton moving at 2.85 × 10^{8} ms^{−1 }(the mass of proton is 1.673 × 10^{−27} Kg).
What is the de Broglie wavelength (in cm) of a 160 g cricket ball travelling at 140 Km hr^{−1}?
Suppose that the uncertainty in determining the position of an electron in an orbit is 0.6 Å. What is the uncertainty in its momentum?
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 (ΔV) is equal to 1/4π of its velocity (V).
What is the de Broglie wavelength of an electron, which is accelerated from the rest, through a potential difference of 100V?
Identify the missing quantum numbers and the sub energy level
n | l | m | Sub energy level |
? | ? | 0 | 4d |
3 | 1 | 0 | ? |
? | ? | ? | 5p |
? | ? | −2 | 3d |
Chapter 2: Quantum Mechanical Model of Atom
Tamil Nadu Board Samacheer Kalvi solutions for Class 11th Chemistry Volume 1 and 2 Answers Guide chapter 2 - Quantum Mechanical Model of Atom
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Concepts covered in Class 11th Chemistry Volume 1 and 2 Answers Guide chapter 2 Quantum Mechanical Model of Atom are Wave Particle Duality of Matter, Heisenberg’S Uncertainty Principle, Quantum Mechanical Model of Atom – SchröDinger Equation, Quantum Numbers, Filling of Orbitals, Introduction to Atom Models.
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