Target DPP Test

1.

Which of the following sets of quantum numbers is not possible?
1. n = 1, l=0, m=0, s=1/2
2. n = 2, l=0, m=0, s= -1/2
3. n = 3, l= 3, m = -3, s = 1/2
4. n = 3, l= 1, m = 0, s = -1/2

2.

$ \psi ^{2} \ = \ 0 $ represents:
1. a node
2. an orbital
3. angular wave function
4. wave function

3.

What is the maximum number of orbitals that can be identified with the following quantum numbers?
n = 3, l = 1, m = 0

1.	1	2.	2
3.	3	4.	4

4.

The correct set of four quantum numbers for the valence electron of a rubidium atom (Z =37) is:

1.	$5,1,1,+ {1 \over2}$	2.	$6,0,0,+ {1 \over2}$
3.	$5,0,0,+ {1 \over2}$	4.	$5,1,0,+ {1 \over2}$

5.

Which orbital has the maximum number of total nodes?
1. 5s
2. 5p
3. 5d
4. All have the same number of nodes.

6.

$ψ^{2} (r, θ, ϕ)$ represents: (for Schrodinger wave mechanical model)
1. Amplitude of electron wave
2. Probability density of electron
3. Total probability of finding electron around nucleus
4. Orbit

7.

The quantum number not obtained from Schrodinger’s wave equation is:

1.	$n$	2.	$l$
3.	$m$	4.	$s$

8.

For a 4p orbital, the number of radial and angular nodes respectively are
1. 3, 2
2. 1, 2
3. 2, 4
4. 2, 1

9.

Which of the following match is incorrect?
1. $5 p_{x}$ orbital (4 radial nodes)
2. $3 d_{xy}$ orbital (2 nodal planes)
3. 4s orbital (3 radial nodes)
4. 4f Subshell (maximum 14 electrons)

10. Consider the given two statements:

Assertion (A):	All d orbitals are tetra-lobed structures having two nodal planes.
Reason (R):	Out of five, only four d-orbitals are degenerate orbitals.

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.	Both (A) and (R) are False.

11.

Total number of orbitals associated with third shell will be _____.
(a) 2
(b) 4
(c) 9
(d) 3

12.

The number of radial nodes for 3p orbital is ______.
1. 3
2. 4
3. 2
4. 1

13.

Total number of orbitals associated with third shell will be _____.
1. 2
2. 4
3. 9
4. 3

14.

The number of orbitals indicated by the following set of quantum numbers, n = 3, l = 2, m =+2 is:
1. 1
2. 2
3. 3
4. 4

15.

The set of quantum numbers which represent 3p is :
1. n = 1, l = 0;
2, n = 3; l = 1
3. n = 4; l = 2;
4. n = 4; l = 3

16.

The total number of electrons in an atom with the following quantum numbers would be
(a) n = 4, m_s = – ½
(b) n = 3, l = 0
1. 16, 2
2. 11, 8
3. 16, 8
4. 12, 7

17.

The number of electrons that can be present in the subshells having m_s value of $-\frac{1}{2}$ for n = 4 are:

1.	36	2.	4
3.	16	4.	2

18.

The correct set of quantum numbers among the following is :

	n	l	m
(a)	1	1	+2
(b)	2	1	+1
(c)	3	2	–2
(d)	3	4	–2

1. (a), (d)
2. (b), (c)
3. (c), (d)
4. (b), (d)

19.

The graph that represents the probability density v/s distance of the electron from the nucleus for 2s orbital is:

1.
2.
3.
4.

20.

The graph between ${|ψ|}^{2}$ and r (radial distance) is shown below. This represents:

1. 3s orbital
2. 2s orbital
3. 2p orbital
4. 1s orbital

21.

The orbital having two radial as well as two angular nodes is:

1.	3p	2.	4f
3.	4d	4.	5d

22. Orbitals among the following has the highest energy is -
1. 5d
2. 5f
3. 6s
4. 6p

23. Identify the incorrect statement from the following:

1.	The shapes of d_xy, d_yz, and d_zx orbitals are similar to each other; and d_x²-_y² and d_z² are similar to each other.
2.	All the five 5d orbitals are different in size when compared to the respective 4d orbitals.
3.	All the five 4d orbitals have shapes similar to the respective 3d orbitals.
4.	In an atom, all the five 3d orbitals are equal in energy in free state.

24.

Assertion (A):	Half-filled and fully-filled degenerate orbitals are more stable.
Reason (R):	Extra stability is due to the symmetrical distribution of electrons and high exchange energy.

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.

25. How many sets of quantum numbers are possible?

	n	l	m
(a).	2	2	1
(b).	3	2	-2
(c).	3	2	-1
(d).	2	1	-1

1. 0
2. 1
3. 2
4. 3

26. What is the angular momentum value associated with the 'f' orbital?

1.	$0$	2.	$\frac{h}{\sqrt2}\pi$
3.	$\frac{\sqrt3h}{\pi}$	4.	$\frac{\sqrt3h}{\sqrt2\pi}$

27. Which of the following statement about the quantum mechanical model of the atom is incorrect?

1.	Schrodinger's equation cannot be solved exactly for multi-electron atoms.
2.	Quantum mechanics predicts all aspects of the hydrogen atom spectrum.
3.	The model obeys Heisenberg's uncertainty principle.
4.	The wave function is a mathematical function and has physical meaning.

28. Which set of quantum numbers is not possible?
1. n = 2, l = 1, m_l= +1, m_s = –1⁄2
2. n = 3, l = 2, m_l = +1, m_s= +1⁄2
3. n = 4, l = 4, m_l = –1, m_s = +1⁄2
4. n =5, l = 2, m_l = +2, m_s = –1⁄2

29. Consider the two statements:

Statement I:	Two electrons occupying the same orbital are distinguished by magnetic quantum number.
Statement II:	The energy of the electron in the 3p orbital is less than that in the 4s orbital in the hydrogen.

In the light of the above statements, choose the most appropriate answer from the options given below:

1.	Statement I is correct, and statement II is correct.
2.	Statement I is incorrect, and statement II is correct.
3.	Statement I is correct, and statement II is incorrect.
4.	Statement I is incorrect, and statement II is incorrect.

30. The correct statement among the following is:
1. The number of orbitals in $n^{\text {th }}$ shell is $n^{\text {2 }}$.
2. The number of orbitals in a subshell is $(2l-1) $.
3. The number of subshells in $n^{\text {th }}$ shell is $(n+l) $.
4. The number of electrons in a shell is $2(2l+1) $.

Fill OMR Sheet*

*If above link doesn't work, please go to test link from where you got the pdf and fill OMR from there

CLICK HERE to get FREE ACCESS for 2 days of ANY NEETprep course

1.	\(5,1,1,+ {1 \over2}\)	2.	\(6,0,0,+ {1 \over2}\)
3.	\(5,0,0,+ {1 \over2}\)	4.	\(5,1,0,+ {1 \over2}\)

1.	\(0\)	2.	\(\frac{h}{\sqrt2}\pi\)
3.	\(\frac{\sqrt3h}{\pi}\)	4.	\(\frac{\sqrt3h}{\sqrt2\pi}\)

1.	\(n\)	2.	\(l\)
3.	\(m\)	4.	\(s\)

Please be patient as the PDF generation may take upto a minute.

Fill OMR Sheet*