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Q. No.The correct statement among the following is/are:
(I)
\( |\Psi|^2 \) is known as a probability density.
(II)
The Schrödinger equation can be easily solved for a multi-electron atom.
(III)
An atomic orbital is the wave function \( \Psi\) for an electron in an atom.
1. (III) only
2. (I) and (III) only
3. (II) and (III) only
4. (I), (II) and (III)
Subtopic: Quantum Numbers & Schrodinger Wave Equation |
59%
Level 3: 35%-60%
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According to the law of photochemical equivalence, the energy absorbed (in ergs/mole) is given as:
(h = 6.62 × 10–27 ergs, c = 3 × 1010 cm s–1, NA = 6.02 × 1023 mol–1)
(h = 6.62 × 10–27 ergs, c = 3 × 1010 cm s–1, NA = 6.02 × 1023 mol–1)
| 1. | \({{1.196\times 10^{8}}\over{\lambda}}\) | 2. | \({{2.859\times 10^{5}}\over{\lambda}}\) |
| 3. | \({{2.859\times 10^{16}}\over{\lambda}}\) | 4. | \({{1.196\times 10^{16}}\over{\lambda}}\) |
Subtopic: Electromagnetic Radiation |
64%
Level 2: 60%+
NEET - 2013
Hints
Lyman series of hydrogen atom falls in which of the following region of the electromagnetic spectrum?
1. Microwave
2. Ultraviolet
3. Visible
4. Infrared
1. Microwave
2. Ultraviolet
3. Visible
4. Infrared
Subtopic: Type of Spectra |
88%
Level 1: 80%+
Hints
Which of the following pair of d-orbitals has zero electron density along the axis?
1. \(d_\text {xy} ~\text{and}~ d_ {{\text x^2} -{\text y^2} } \)
2. \(d_\text {yz} ~\text{and}~d_{z^2} \)
3. \( d_ {{\text x^2} -{\text y^2}} ~\text{and} ~d_{z^2} \)
4. \(d_\text {xy} ~\text{and}~d_\text {yz} \)
1. \(d_\text {xy} ~\text{and}~ d_ {{\text x^2} -{\text y^2} } \)
2. \(d_\text {yz} ~\text{and}~d_{z^2} \)
3. \( d_ {{\text x^2} -{\text y^2}} ~\text{and} ~d_{z^2} \)
4. \(d_\text {xy} ~\text{and}~d_\text {yz} \)
Subtopic: Nodal Plane |
Level 3: 35%-60%
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The threshold frequency \((\nu_0)\) for metal is \(6.0 × 10^{14}~\text {sec}^{-1}\). When radiation of frequency, \(\nu = 1.0 × 10^{15}~\text {sec}^{-1} \) hits the metal, the kinetic energy of the electron emitted is:
[Given: h = 6.62 × 10-34 Js]
1. 3.65 × 10–19 J
2. 2.65 × 10–19 J
3. 1.95 × 10–19 J
4. 2.95 × 10–20 J
[Given: h = 6.62 × 10-34 Js]
1. 3.65 × 10–19 J
2. 2.65 × 10–19 J
3. 1.95 × 10–19 J
4. 2.95 × 10–20 J
Subtopic: Photo Electric Effect |
82%
Level 1: 80%+
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When electromagnetic radiation of wavelength 300 nm falls on the surface of a metal, electrons are emitted with the kinetic energy of 1.68 × 105 J mol–1. The minimum energy needed to remove one mole of electron from the metal is:
(GivenL: h = 6.626 × 10–34 Js, c = 3 × 108 ms–1, NA = 6.022 × 1023 mol–1)
1. 2.31 × 106 J mol–1
2. 3.84 × 104 J mol–1
3. 3.84 × 10–19 J mol–1
4. 2.31 × 105 J mol–1
(GivenL: h = 6.626 × 10–34 Js, c = 3 × 108 ms–1, NA = 6.022 × 1023 mol–1)
1. 2.31 × 106 J mol–1
2. 3.84 × 104 J mol–1
3. 3.84 × 10–19 J mol–1
4. 2.31 × 105 J mol–1
Subtopic: Photo Electric Effect |
Level 3: 35%-60%
NEET - 2022
Hints
Match List-I with List-II:
Choose the correct answer from the options given below:
| List-I (quantum number) |
List-II (Orbital) |
||
| (A) | n = 2, \(\ell\) = 1 | (I) | 2s |
| (B) | n = 3, \(\ell\) = 2 | (II) | 3s |
| (C) | n = 3, \(\ell\) = 0 | (III) | 2p |
| (D) | n = 2, \(\ell\) = 0 | (IV) | 3d |
| (A) | (B) | (C) | (D) | |
| 1. | (III) | (IV) | (I) | (II) |
| 2. | (IV) | (III) | (I) | (II) |
| 3. | (IV) | (III) | (II) | (I) |
| 4. | (III) | (IV) | (II) | (I) |
Subtopic: Shell & Subshell |
84%
Level 1: 80%+
NEET - 2022
Hints
Given below is the probability density graph of an orbital.
The above graph represents the orbital:
1. 1s
2. 2s
3. 2p
4. 3s
The above graph represents the orbital:
1. 1s
2. 2s
3. 2p
4. 3s
Subtopic: Quantum Numbers & Schrodinger Wave Equation |
65%
Level 2: 60%+
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The relation between \(n_m \) (\(n_m \) = number of permissible values of magnetic quantum number (ml) for a given value of azimuthal quantum number (l) is:
1. \(n_m = l+2\)
2. \(l = {\dfrac{n_m -1} 2}\)
3. \(l= 2n_m +1\)
4. \(n_m = 2l^2 + 1 \)
1. \(n_m = l+2\)
2. \(l = {\dfrac{n_m -1} 2}\)
3. \(l= 2n_m +1\)
4. \(n_m = 2l^2 + 1 \)
Subtopic: Shell & Subshell |
70%
Level 2: 60%+
NEET - 2023
Hints
Using the following statements, identify the correct set of statements:
1. (i), (ii), (iii)
2. (i), (ii), (iv)
3. (i), (ii), (iii), (iv)
4. (i), (iii), (iv)
| (i). | n (principal quantum number) can have values 1, 2, 3, 4, ....... |
| (ii). | The number of orbitals for a given value of l is (2l+1). |
| (iii). | The value of spin quantum numbers is always \(\pm\frac12\). |
| (iv). | For l=5, the total number of orbitals is 9. |
1. (i), (ii), (iii)
2. (i), (ii), (iv)
3. (i), (ii), (iii), (iv)
4. (i), (iii), (iv)
Subtopic: Quantum Numbers & Schrodinger Wave Equation |
85%
Level 1: 80%+
JEE
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