Which of the following is responsible to rule out the existence of definite paths or trajectories of electrons? 1. Pauli's exclusion principle 2. Heisenberg's uncertainty principle 3. Hund's rule of maximum multiplicity 4. Aufbau principle

Subtopic:  Heisenberg Uncertainty Principle |
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Total number of orbitals associated with third shell will be _____.

1.  2

2.  4

3.  9

4.  3

Subtopic:  Quantum Numbers & Schrodinger Wave Equation |
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Orbital angular momentum depends on _______.

1.  l

2.  n and l

3.  n and ${\mathrm{m}}_{\mathrm{l}}$

4.  ${\mathrm{m}}_{\mathrm{l}}$ and ${\mathrm{m}}_{\mathrm{s}}$

Subtopic:  Quantum Numbers & Schrodinger Wave Equation |
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Chlorine exists in two isotopic forms, Cl-37 and Cl-35, but its atomic mass is 35.5. This indicates the ratio of Cl-37 and Cl-35 is approximately :

1. 1:2

2. 1:1

3. 1:3

4. 3:1

Subtopic:  Number of Electron, Proton & Neutron |
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The pair of ions having the same electronic configuration is -

1.  Cr3+, Fe3+

2.  Fe3+, Mn2+

3.  Fe3+, Co3+

4.  Sc3+, Cr3+

Subtopic:  Pauli's Exclusion Principle & Hund's Rule |
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For the electrons of an oxygen atom. The correct statement among the following is-

1. Zeff for an electron in a 2s orbital is the same as Zeff for an electron in a 2p orbital.

2. An electron in the 2s orbital has the same energy as an electron in the 2p orbital.

3. Zeff for an electron in 1s orbital is the same as Zeff for an electron in a 2s orbital

4. The two electrons present in the 2s orbital have same spin quantum numbers ms but of opposite sign

Subtopic:  Quantum Numbers & Schrodinger Wave Equation | Shell & Subshell |
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If travelling at same speeds, which of the following matter waves have the shortest wavelength?

1. Electron

2. Alpha particle (He2+)

3. Neutron

4. Proton

Subtopic:  De Broglie Equation |
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Match the following species with their corresponding ground state electronic configuration.

 Atom/Ion Electronic configuration A. Cu 1. $1{\mathrm{s}}^{2}2{\mathrm{s}}^{2}2{\mathrm{p}}^{6}3{\mathrm{s}}^{2}3{\mathrm{p}}^{6}3{\mathrm{d}}^{10}$ B. Cu2+ 2. $1{\mathrm{s}}^{2}2{\mathrm{s}}^{2}2{\mathrm{p}}^{6}3{\mathrm{s}}^{2}3{\mathrm{p}}^{6}3{\mathrm{d}}^{10}4{\mathrm{s}}^{2}$ C. Zn2+ 3. $1{\mathrm{s}}^{2}2{\mathrm{s}}^{2}2{\mathrm{p}}^{6}3{\mathrm{s}}^{2}3{\mathrm{p}}^{6}3{\mathrm{d}}^{10}4{\mathrm{s}}^{1}$ D. Cr3+ 4. $1{\mathrm{s}}^{2}2{\mathrm{s}}^{2}2{\mathrm{p}}^{6}3{\mathrm{s}}^{2}3{\mathrm{p}}^{6}3{\mathrm{d}}^{9}$ 5. $1{\mathrm{s}}^{2}2{\mathrm{s}}^{2}2{\mathrm{p}}^{6}3{\mathrm{s}}^{2}3{\mathrm{p}}^{6}3{\mathrm{d}}^{3}$

 A B C D 1. 4 2 5 1 2. 3 4 1 5 3. 3 2 1 4 4. 4 2 1 3
Subtopic:  Pauli's Exclusion Principle & Hund's Rule |
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Match the quantum numbers with the information provided by them:

 Quantum number Information provided A. Principal quantum number 1. Orientation of the orbital B. Azimuthal quantum number 2. Energy and size of orbital C. Magnetic quantum number 3. Spin of electron D. Spin quantum number 4. Shape of the orbital

 A B C D 1. 2 4 1 3 2. 1 2 3 4 3. 1 4 3 2 4. 4 1 3 2
Subtopic:  Quantum Numbers & Schrodinger Wave Equation |
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Match the ensuing rules with the corresponding statements

 Rules Statements A. Hund’s Rule 1. No two electrons in an atom can have the same set of four quantum numbers. B. Aufbau Principle 2. Half-filled and completely filled orbitals have extra stability. C. Pauli's Exclusion Principle 3. Pairing of electrons in the orbitals belonging to the same subshell does not take place until each orbital is singly occupied. D. Heisenberg’s Uncertainty Principle 4. It is impossible to determine the exact position and exact momentum of a subatomic particle simultaneously. 5. In the ground state of atoms, orbitals are filled in the order of their increasing energies.

 A B C D 1. 3 5 1 2 2. 1 2 3 4 3. 3 5 1 4 4. 4 5 3 2
Subtopic:  Pauli's Exclusion Principle & Hund's Rule |
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