Atomic Structure Test

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Atomic Structure Test - 1

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Weekly Quiz Competition

Question 1
1 / -0

Which electronic level would allow the hydrogen atom to absorb a photon but not to emit a photon?

A
3s

B
2_P

C
2s

D
1s

Solution

Ground state of hydrogen atom, i.e., 1s, because by absorbing photon it can go upto any higher level, while it cannot emit a photon because lower level than 1s in not possible.
Question 2
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Rutherford’s alpha particle scattering experiment eventually led to the conclusion that

A
mass and energy are related

B
electrons occupy space around the nucleus

C
neutrons are buried deep in the nucleus

D
the point of impact with matter can be precisely determined

Solution

Rutherford’s experiment was to find the position of protons and electrons in the atom.
Question 3
1 / -0

Which of the following does not characterize X-rays?

A
The radiation can ionize gases

B
It causes ZnS to inflorescence

C
Deflected by electric and magnetic fields

D
Have wavelengths shorter than ultraviolet rays

Solution

X- rays are not deflected by electric by and magnatic fields
Question 4
1 / -0

The electrons, identified by quantum numbers n and l, (i) n = 4, l = 1, (ii) n = 4, l = 0, (iii) n = 3, l = 2 and (iv) n = 3, l = 1 can be placed in order of increasing energy, from the lowest to highest, as

A
(iv) < (ii) < (iii) < (i)

B
(ii) < (iv) < (i) < (iii)

C
(i) < (iii) < (ii) < (iv)

D
(iii) < (i) < (iv) < (ii)

Solution

Reason of correctness

On the basis of (n + l) rule

(i) Value of (n + l) = 4 + 1 = 5 (ii)Value of (n + l) = 4 + 0 = 4

(iii) Value of (n + l) = 3 + 2 = 5 (iv)Value of (n + l) = 3 + 1 = 4

On the basis of (n + l) rule

In these (n + l) is lower for (ii) and (iv) but both are equal. In these n is minimum for (iv)

Hence, energy order = (iv) < (ii)

Similarly in (i) and (iii), (iii) < (i)

Hence, correct order of energy (iv) < (ii) < (iii) < (i)
Question 5
1 / -0

If the nitrogen atom had electronic configuration 1s⁷, it would have energy lower than that of the normal ground state configuration 1s² 2s² 2p³, because the electrons would be closer to the nucleus, yet 1s⁷ is not observed because it violets

A
Heisenberg uncertainty principle

B
Hund’s rule

C
Pauli’s exclusion principle

D
Bohr’s postulate of stationary orbits

Solution

On the basis of Pauli’s exclusion principle, not more than two electrons can enter in an orbital. Hence, seven electrons (as 1s⁷) in an orbital violates Pauli’s exclusion principle.
Question 6
1 / -0

Total number of nodes in 5d sub-shell will be

A
2

B
3

C
2

D
4

Solution

Total number of nodes given by (n – 1), hence 4
Question 7
1 / -0

An electron in H-atom in its ground state absorbs 1.50 times as much as energy as the minimum required for its escape (13.6 eV) from the atom. Thus KE given of emitted electron?

A
13.6 eV

B
20.4 eV

C
34.0 eV

D
6.8 eV

Solution

Energy in ground state = 13.6 eV

Energy absorbed = 1.5 × 13.6 eV = 20.4 eV

Kinetic energy of emitted e¯ is = (– 13.6 + 20.4) eV

= 6.8 eV
Question 8
1 / -0

A continuum in spectrum is observed due to the following

A
Once an electron is completely free from the nucleus, it is no longer restricted to quantized discrete energy states

B
Electron takes up continuously the ordinary kinetic energy corresponding to its speed in free space

C
Both the reason are correct

D
None of the two reasons are correct

Solution

Quantized discrete energy states are due to presence of energy levels. Once electron is completely free from nucleus, it will not be associated with discrete energy states.

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Re-Attempt Weekly Quiz Competition

Atomic Structure Test - 1

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Atomic Structure Test - 1

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SHARING IS CARING

Question 1

3s

2P

2s

1s

Solution

Question 2

mass and energy are related

electrons occupy space around the nucleus

neutrons are buried deep in the nucleus

the point of impact with matter can be precisely determined

Solution

Question 3

The radiation can ionize gases

It causes ZnS to inflorescence

Deflected by electric and magnetic fields

Have wavelengths shorter than ultraviolet rays

Solution

Question 4

(iv) < (ii) < (iii) < (i)

(ii) < (iv) < (i) < (iii)

(i) < (iii) < (ii) < (iv)

(iii) < (i) < (iv) < (ii)

Solution

Question 5

Heisenberg uncertainty principle

Hund’s rule

Pauli’s exclusion principle

Bohr’s postulate of stationary orbits

Solution

Question 6

2

3

2

4

Solution

Question 7

13.6 eV

20.4 eV

34.0 eV

6.8 eV

Solution

Question 8

Once an electron is completely free from the nucleus, it is no longer restricted to quantized discrete energy states

Electron takes up continuously the ordinary kinetic energy corresponding to its speed in free space

Both the reason are correct

None of the two reasons are correct

Solution

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