The ejection of the photoelectron from the silver metal can be stopped by applying a voltage of 0.35 eV when the radiation having a wavelength of 256.7 nm is used. The work function for silver metal is: 

1. 3.40 eV

2. 5.18 eV

3. 4.48 eV

4. -4.40 eV

Subtopic:  Photo Electric Effect |
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Property which is same for the following species is:

 N3, O2–, F, Na+, Mg2+ and Al3+ 

1. Ionic radii

2. Number of electrons

3. Nuclear charge

4. None of the above 

Subtopic:  Number of Electron, Proton & Neutron |
 87%
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The ionization energy for H atom in the ground state is \(2.18 \times10^{-18}~ \mathrm J.\) The process energy requirements will be: \(( He^+(g) \rightarrow He^{2+}(g) + e^- )\)

1. \(8.72 \times10^{-18}~\mathrm J\) 2. \(7.54 \times10^{-18}~\mathrm J\)
3. \(5.67 \times10^{-17}~\mathrm J\) 4. \(2.18 \times10^{-17}~\mathrm J\)
Subtopic:  Hydrogen Spectra |
 59%
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The maximum number of emission lines obtained when the excited electron of the H atom jumps from n = 6 to the ground state is -

1. 30

2. 21

3. 15

4. 28

Subtopic:  Hydrogen Spectra |
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Electrons are emitted with zero velocity from a metal surface when it is exposed to radiation of
wavelength 6800 Å. The
 work function (W0 ) of the metal is: 

1. 3.109 x 10-20 J

2. 2.922 x 10-19 J

3. 4.031 x 1019 J

4. 2.319 x 10-18 J

Subtopic:  Photo Electric Effect |
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Match the following species with their corresponding ground state electronic configuration.

Atom/Ion Electronic configuration
A. Cu 1. 1s22s22p63s23p63d10
B. Cu2+ 2. 1s22s22p63s23p63d104s2
C. Zn2+ 3. 1s22s22p63s23p63d104s1
D. Cr3+ 4. 1s22s22p63s23p63d9
5. 1s22s22p63s23p63d3
 
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

Codes
 
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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Match the following:

Column I Column II
A. X-rays 1. v=100-104 Hz
B. Ultraviolet wave (UV) 2. v=1010 Hz
C. Long radio waves 3. v=1016 Hz
D. Microwave 4. v=1018 Hz
 
A B C D
1. 4 1 3 2
2. 1 4 2 3
3. 1 4 3 2
4. 4 3 1 2
Subtopic:  Electromagnetic Radiation |
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Assertion (A): All isotopes of a given element show the same type of chemical behaviour.
Reason (R): The chemical properties of an atom are controlled by the number of electrons in the atom.

1. Both (A) and (R) are true and (R) is the correct explanation of (A).
2. Both (A) and (R) are true but (R) is not the correct explanation of (A).
3. (A) is true but (R) is false.
4. (A) is false but (R) is true.

Subtopic:  Number of Electron, Proton & Neutron |
 64%
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