JEE Main & Advanced Chemistry Structure of Atom / परमाणु संरचना Question Bank

Quantum number, Electronic configuration and Shape of orbitals Total Questions - 228

1)

Be's 4th electron will have four quantum numbers [MNR 1985]

A)
                \[n\]- 1       \[l\]- 0         \[m\]- 0        \[s\]- +1/2

B)
                \[n\]- 1       \[l\]- 1        \[m\]- +1      \[s\]- +1/2

C)
                \[n\]- 2       \[l\]- 0         \[m\]- 0         \[s\]- -1/2

D)
                \[n\]- 2       \[l\]- 1         \[m\]- 0         \[s\]- +1/2
View Solution
2)

The quantum number which specifies the location of an electron as well as energy is      [DPMT 1983]

A)
                Principal quantum number

B)
                Azimuthal quantum number

C)
                Spin quantum number

D)
                Magnetic quantum number
View Solution
3)

The shape of an orbital is given by the quantum number               [NCERT 1984; MP PMT 1996]

A)
                \[n\]

B)
                \[l\]

C)
                \[m\]

D)
                \[s\]
View Solution
4)

In a given atom no two electrons can have the same values for all the four quantum numbers. This is called [BHU 1979; AMU 1983; EAMCET 1980, 83; MADT Bihar 1980; CPMT 1986, 90, 92; NCERT 1978, 84; RPMT 1997; CBSE PMT 1991; MP PET 1986, 99]

A)
                Hund's rule

B)
                Aufbau's principle

C)
                Uncertainty principle

D)
                Pauli's exclusion principle
View Solution
5)

Nitrogen has the electronic configuration \[1{{s}^{2}},2{{s}^{2}}2p_{x}^{1}2p_{y}^{1}2p_{z}^{1}\] and not \[1{{s}^{2}},2{{s}^{2}}2p_{x}^{2}2p_{y}^{1}2p_{z}^{0}\]   which is determined by [DPMT 1982, 83, 89; MP PMT/PET 1988; EAMCET 1988]

A)
                Aufbau's principle

B)
                Pauli's exclusion principle

C)
                Hund's rule

D)
                Uncertainty principle
View Solution
6)

Which one of the following configuration represents a noble gas                              [CPMT 1983, 89, 93; NCERT 1973; MP PMT 1989; DPMT 1984]

A)
                \[1{{s}^{2}},2{{s}^{2}}2{{p}^{6}},3{{s}^{2}}\]

B)
                \[1{{s}^{2}},2{{s}^{2}}2{{p}^{6}},3{{s}^{1}}\]

C)
                \[1{{s}^{2}},2{{s}^{2}}2{{p}^{6}}\]

D)
                \[1{{s}^{2}},2{{s}^{2}}s{{p}^{6}},3{{s}^{2}}3{{p}^{6}},4{{s}^{2}}\]
View Solution
7)

The electronic configuration of silver atom in ground state is [CPMT 1984, 93]

A)
                \[[Kr]3{{d}^{10}}\,4{{s}^{1}}\]

B)
                \[[Xe]\,4{{f}^{14}}5{{d}^{10}}6{{s}^{1}}\]

C)
                \[[Kr]\,4{{d}^{10}}5{{s}^{1}}\]

D)
                \[[Kr]\,4{{d}^{9}}5{{s}^{2}}\]
View Solution
8)

Principal, azimuthal and magnetic quantum numbers are respectively related to               [CPMT 1988; AIIMS 1999]

A)
                Size, shape and orientation

B)
                Shape, size and orientation

C)
                Size, orientation and shape

D)
                None of the above
View Solution
9)

Correct set of four quantum numbers for valence electron of rubidium (Z = 37) is [IIT 1984; JIPMER 1999; UPSEAT 2003]

A)
                \[5,\,0,\,0,\,+\frac{1}{2}\]

B)
                \[5,\,1,\,0,\,+\frac{1}{2}\]

C)
                \[5,\,1,\,1,\,+\frac{1}{2}\]

D)
                \[6,\,0,\,0,\,+\,\frac{1}{2}\]
View Solution
10)

The correct ground state electronic configuration of chromium atom is [IIT 1989, 94; MP PMT 1993; EAMCET 1997; ISM Dhanbad 1994; AFMC 1997; Bihar MEE 1996; MP PET 1995, 97; CPMT 1999; Kerala PMT 2003]

A)
                \[[Ar]\,3{{d}^{5}}\,4{{s}^{1}}\]

B)
                \[[Ar]\,3{{d}^{4}}4{{s}^{2}}\]

C)
                \[[AR]3{{d}^{6}}4{{s}^{0}}\]

D)
                \[[Ar]4{{d}^{5}}4{{s}^{1}}\]
View Solution
11)

2p orbitals have                [NCERT 1981; MP PMT 1993, 97]

A)
                \[n=1,\,l=2\]

B)
                \[n=1,\,l=0\]

C)
                \[n=2,\,l=1\]

D)
                \[n=2,\,l=0\]
View Solution
12)

Electronic configuration of \[{{H}^{-}}\] is             [CPMT 1985]

A)
                \[1{{s}^{0}}\]

B)
                \[1{{s}^{1}}\]

C)
                \[1{{s}^{2}}\]

D)
                \[1{{s}^{1}}\,2{{s}^{1}}\]
View Solution
13)

The quantum numbers for the outermost electron of an element are given below as \[n=2,\,l=0,\,m=0,\,s=+\frac{1}{2}\]. The atoms is                                       [EAMCET 1978]

A)
                Lithium

B)
                Beryllium

C)
                Hydrogen

D)
                Boron
View Solution
14)

Principal quantum number of an atom represents [EAMCET 1979; IIT 1983; MNR 1990;UPSEAT 2000, 02]

A)
                Size of the orbital

B)
                Spin angular momentum

C)
                Orbital angular momentum

D)
                Space orientation of the orbital
View Solution
15)

An element has the electronic configuration \[1{{s}^{2}},2{{s}^{2}}2{{p}^{6}},3{{s}^{2}}3{{p}^{2}}\]. Its valency electrons are [NCERT 1973]

A)
                6

B)
                2

C)
                3

D)
                4
View Solution
16)

The magnetic quantum number specifies [MNR 1986; BHU 1982; CPMT 1989, 94; MP PET 1999; AFMC 1999; AMU (Engg.) 1999]

A)
                Size of orbitals

B)
                Shape of orbitals

C)
                Orientation of orbitals

D)
                Nuclear stability
View Solution
17)

Which of the following sets of quantum numbers represent an impossible arrangement               [IIT 1986; MP PET 1995]

A)
                n ? 3      l ? 2        m - - 2   \[{{m}_{s}}\]- (+)\[\frac{1}{2}\]

B)
                n ? 4      l ? 0        m ? 0     \[{{m}_{s}}\]- (?)\[\frac{1}{2}\]

C)
                n ? 3      l ? 2        m - -3    \[{{m}_{s}}\] - (+)\[\frac{1}{2}\]

D)
              n ? 5      l ? 3        m ? 0     \[{{m}_{s}}\] - (?) \[\frac{1}{2}\]
View Solution
18)

If \[n=3\], then the value of \['l'\] which is incorrect [CPMT 1994]

A)
                0

B)
                1

C)
                2

D)
                3
View Solution
19)

Which orbital is dumb-bell shaped [MP PMT 1986; MP PET/PMT 1998]

A)
                \[s\]-orbital

B)
                \[p\]-orbital

C)
                \[d\]-orbital

D)
                \[f\]-orbital
View Solution
20)

The total number of unpaired electrons in \[d\]- orbitals of atoms of element of atomic number 29 is     [CPMT 1983]

A)
                10

B)
                1

C)
                0

D)
                5
View Solution
21)

The shape of \[2p\]orbital is       [CPMT 1983; NCERT 1979]

A)
                Spherical

B)
                Ellipsoidal

C)
                Dumb-bell

D)
                Pyramidal
View Solution
22)

The magnetic quantum number for an electron when the value of principal quantum number is 2 can have [CPMT 1984]

A)
                3 values

B)
                2 values

C)
                9 values

D)
                6 values
View Solution
23)

Which one is the correct outer configuration of chromium                 [AIIMS 1980, 91; BHU 1995]

A)


B)


C)


D)

View Solution
24)

The following has zero valency [DPMT 1991]

A)
                Sodium

B)
                Beryllium

C)
                Aluminium

D)
                Krypton
View Solution
25)

The number of electrons in the valence shell of calcium is [IIT 1975]

A)
                6

B)
                8

C)
                2

D)
                4
View Solution
26)

The valence electron in the carbon atom are       [MNR 1982]

A)
                0

B)
                2

C)
                4

D)
                6
View Solution
27)

For the dumb-bell shaped orbital, the value of \[l\] is [CPMT 1987, 2003]

A)
                3

B)
                1

C)
                0

D)
                2
View Solution
28)

Chromium has the electronic configuration \[4{{s}^{1}}3{{d}^{5}}\] rather than \[4{{s}^{2}}3{{d}^{4}}\] because

A)
                \[4s\] and \[3d\] have the same energy

B)
                \[4s\] has a higher energy than \[3d\]

C)
                \[4{{s}^{1}}\] is more stable than \[4{{s}^{2}}\]

D)
                \[4{{s}^{1}}3{{d}^{5}}\] half-filled is more stable than \[4{{s}^{2}}3{{d}^{4}}\]
View Solution
29)

The electronic configuration of calcium ion \[(C{{a}^{2+}})\] is [CMC Vellore 1991]

A)
                \[1{{s}^{2}},2{{s}^{2}}2{{p}^{6}},3{{s}^{2}}3{{p}^{6}},4{{s}^{2}}\]

B)
                \[1{{s}^{2}},2{{s}^{2}}s{{p}^{6}},3{{s}^{2}}3{{p}^{6}},4{{s}^{1}}\]

C)
                \[1{{s}^{2}},2{{s}^{2}}2{{p}^{6}},3{{s}^{2}}3{{p}^{6}}3{{d}^{2}}\]

D)
                \[1{{s}^{2}},2{{s}^{2}}s{{p}^{6}},3{{s}^{2}}3{{p}^{6}}3{{d}^{5}}\]

E)
                \[1{{s}^{2}},2{{s}^{2}}2{{p}^{6}},3{{s}^{2}}3{{p}^{6}},4{{s}^{0}}\]
View Solution
30)

The structure of external most shell of inert gases is [JIPMER 1991]

A)
                \[{{s}^{2}}{{p}^{3}}\]

B)
                \[{{s}^{2}}{{p}^{6}}\]

C)
                \[{{s}^{1}}{{p}^{2}}\]

D)
                \[{{d}^{10}}{{s}^{2}}\]
View Solution
31)

The two electrons in K sub-shell will differ in [MNR 1988; UPSEAT 1999, 2000; Kerala PMT 2003]

A)
                Principal quantum number

B)
                Azimuthal quantum number

C)
                Magnetic quantum number

D)
                Spin quantum number
View Solution
32)

A completely filled \[d\]-orbital \[({{d}^{10}})\] [MNR 1987]

A)
                Spherically symmetrical

B)
                Has octahedral symmetry

C)
                Has tetrahedral symmetry

D)
                Depends on the atom
View Solution
33)

If magnetic quantum number of a given atom represented by ?3, then what will be its principal quantum number [BHU 2005]

A)
                2

B)
                3

C)
                4

D)
                5
View Solution
34)

The total number of orbitals in an energy level designated by principal quantum number \[n\] is equal to             [AIIMS 1997; J&K CET 2005]

A)
                \[2n\]

B)
                \[2{{n}^{2}}\]

C)
                \[n\]

D)
                \[{{n}^{2}}\]
View Solution
35)

The number of orbitals in the fourth principal quantum number will be

A)
                4

B)
                8

C)
                12

D)
                16
View Solution
36)

Which set of quantum numbers are not possible from the following

A)
                \[n=3,\,l=2,\,m=0,\,s=-\frac{1}{2}\]

B)
                \[n=3,\,l=2,\,m=-2,\,s=-\frac{1}{2}\]

C)
                \[n=3,\,l=3,\,m=-3,\,s=-\frac{1}{2}\]

D)
                \[n=3,\,l=0,\,m=0,\,s=-\frac{1}{2}\]
View Solution
37)

The four quantum number for the valence shell electron or last electron of sodium (Z = 11) is [MP PMT 1999]

A)
\[n=2,\,l=1,\,m=-1,\,s=-\frac{1}{2}\]

B)
                \[n=3,\,l=0,\,m=0,\,s=+\frac{1}{2}\]

C)
                \[n=3,\,l=2,\,m=-2,\,s=-\frac{1}{2}\]

D)
                \[n=3,\,l=2,\,m=2,\,s=+\frac{1}{2}\]
View Solution
38)

The explanation for the presence of three unpaired electrons in the nitrogen atom can be given by [NCERT 1979; RPMT 1999; DCE 1999, 2002; CPMT 2001; MP PMT 2002; Pb. PMT / CET 2002]

A)
                Pauli's exclusion principle

B)
                Hund's rule

C)
                Aufbau's principle

D)
                Uncertainty principle
View Solution
39)

The maximum energy is present in any electron at

A)
                Nucleus

B)
                Ground state

C)
                First excited state

D)
                Infinite distance from the nucleus
View Solution
40)

The electron density between \[1s\]and \[2s\]orbital is

A)
                High

B)
                Low

C)
                Zero

D)
                None of these
View Solution
41)

For \[ns\] orbital, the magnetic quantum number has value

A)
                2

B)
                4

C)
                ? 1

D)
                0
View Solution
42)

The maximum number of electrons that can be accommodated in the \[{{M}^{th}}\] shell is

A)
                2

B)
                8

C)
                18

D)
                32
View Solution
43)

For a given value of quantum number \[l\], the number of allowed values of \[m\] is given by

A)
                \[l+2\]

B)
                \[2l+2\]

C)
                \[2l+1\]

D)
                \[l+1\]
View Solution
44)

The number of radial nodes of 3s and 2p orbitals are respectively.            [IIT-JEE 2005]

A)
                2, 0

B)
                0, 2

C)
                1, 2

D)
                2, 1
View Solution
45)

Which of the sub-shell is circular

A)
                \[4s\]

B)
                \[4f\]

C)
                \[4p\]

D)
                \[4d\]
View Solution
46)

Which electronic configuration for oxygen is correct according to Hund's rule of multiplicity

A)
                \[1{{s}^{2}},2{{s}^{2}}2p_{x}^{2}2p_{y}^{1}2p_{z}^{1}\]

B)
                \[1{{s}^{2}},2{{s}^{2}}2p_{x}^{2}2p_{y}^{2}2p_{z}^{0}\]

C)
                \[1{{s}^{2}},2{{s}^{2}}2p_{x}^{3}2p_{y}^{1}2p_{z}^{0}\]

D)
                None of these
View Solution
47)

If value of azimuthal quantum number \[l\] is 2, then total possible values of magnetic quantum number will be

A)
                7

B)
                5

C)
                3

D)
                2
View Solution
48)

The type of orbitals present in \[Fe\] is

A)
                \[s\]

B)
                \[s\] and \[p\]

C)
                \[s,\,p\] and \[d\]

D)
                \[s,\,p,\,d\] and \[f\]
View Solution
49)

The shape of \[{{d}_{xy}}\] orbital will be

A)
                Circular

B)
                Dumb-bell

C)
                Double dumb-bell

D)
                Trigonal
View Solution
50)

In any atom which sub-shell will have the highest energy in the following

A)
                \[3p\]

B)
                \[3d\]

C)
                \[4s\]

D)
                \[3s\]
View Solution
51)

Which electronic configuration is not observing the (\[n+l\]) rule

A)
                \[1{{s}^{2}},2{{s}^{2}}2{{p}^{6}},3{{s}^{2}}3{{p}^{6}}3{{d}^{1}},4{{s}^{2}}\]

B)
                \[1{{s}^{2}},2{{s}^{2}}s{{p}^{6}},3{{s}^{2}}3{{p}^{6}}3{{d}^{7}},4{{s}^{2}}\]

C)
                \[1{{s}^{2}},2{{s}^{2}}2{{p}^{6}},3{{s}^{2}}3{{p}^{6}}3{{d}^{5}},4{{s}^{1}}\]

D)
                \[1{{s}^{2}},2{{s}^{2}}2{{p}^{6}},3{{s}^{2}}3{{p}^{6}}3{{d}^{8}},4{{s}^{2}}\]
View Solution
52)

The four quantum numbers of the outermost orbital of \[K\] (atomic no. =19) are           [MP PET 1993, 94]

A)
                \[n=2,\,l=0,\,m=0,\,s=+\frac{1}{2}\]

B)
                \[n=4,\,l=0,\,m=0,\,s=+\frac{1}{2}\]

C)
                \[n=3,\,l=1,\,m=1,\,s=+\frac{1}{2}\]

D)
                \[n=4,\,l=2,\,m=-1,\,s=+\frac{1}{2}\]
View Solution
53)

The angular momentum of an electron depends on                            [BHU 1978; NCERT 1981]

A)
                Principal quantum number

B)
                Azimuthal quantum number

C)
                Magnetic quantum number

D)
                All of these
View Solution
54)

The electronic configuration of copper \[{{(}_{29}}Cu)\] is           [DPMT 1983; BHU 1980; AFMC 1981; CBSE PMT 1991; MP PMT 1995]

A)
                \[1{{s}^{2}},2{{s}^{2}}2{{p}^{6}},3{{s}^{2}}3{{p}^{6}}3{{d}^{9}},4{{s}^{2}}\]

B)
                \[1{{s}^{2}},2{{s}^{2}}2{{p}^{6}},3{{s}^{2}}3{{p}^{6}}3{{d}^{10}},4{{s}^{1}}\]

C)
                \[1{{s}^{2}}.2{{s}^{2}}2{{p}^{6}},3{{s}^{2}}3{{p}^{6}},4{{s}^{2}}4{{p}^{6}}\]

D)
                \[1{{s}^{2}},2{{s}^{2}}2{{p}^{6}},3{{s}^{2}}3{{p}^{6}}3{{d}^{10}}\]
View Solution
55)

The number of orbitals in \[2p\] sub-shell is [NCERT 1973; MP PMT 1996]

A)
                6

B)
                2

C)
                3

D)
                4
View Solution
56)

The number of orbitals in \[d\] sub-shell is           [MNR 1981]

A)
                1

B)
                3

C)
                5

D)
                7
View Solution
57)

A sub-shell \[l=2\] can take how many electrons [NCERT 1973, 78]

A)
                3

B)
                10

C)
                5

D)
                6
View Solution
58)

Pauli's exclusion principle states that [MNR 1983; AMU 1984]

A)
                Two electrons in the same atom can have the same energy

B)
                Two electrons in the same atom cannot have the same spin

C)
                The electrons tend to occupy different orbitals as far as possible

D)
                Electrons tend to occupy lower energy orbitals preferentially

E)
                None of the above
View Solution
59)

For \[d\]electrons, the azimuthal quantum number is [MNR 1983; CPMT 1984]

A)
                0

B)
                1

C)
                2

D)
                3
View Solution
60)

For \[p\]-orbital, the magnetic quantum number has value

A)
                2

B)
                4, ? 4

C)
                ? 1, 0, +1

D)
                0
View Solution
61)

For \[n=3\] energy level, the number of possible orbitals (all kinds) are [BHU 1981; CPMT 1985; MP PMT 1995]

A)
                1

B)
                3

C)
                4

D)
                9
View Solution
62)

Which of the following ions is not having the configuration of neon

A)
                \[{{F}^{-}}\]

B)
                \[M{{g}^{+2}}\]

C)
                \[N{{a}^{+}}\]

D)
                \[C{{l}^{-}}\]
View Solution
63)

Elements upto atomic number 103 have been synthesized and studied. If a newly discovered element is found to have an atomic number 106, its electronic configuration will be [AIIMS 1980]

A)
                \[[Rn]5{{f}^{14}},6{{d}^{4}},7{{s}^{2}}\]

B)
                \[[Rn]5{{f}^{14}},6{{d}^{1}},7{{s}^{2}}7{{p}^{3}}\]

C)
                \[[Rn]5{{f}^{14}},6{{d}^{6}},7{{s}^{0}}\]

D)
                \[[Rn]5{{f}^{14}},6{{d}^{5}},7{{s}^{1}}\]
View Solution
64)

Ions which have the same electronic configuration are those of

A)
                Lithium and sodium

B)
                Sodium and potassium

C)
                Potassium and calcium

D)
                Oxygen and chlorine
View Solution
65)

When the azimuthal quantum number has a value of \[l=0\], the shape of the orbital is [MP PET 1995]

A)
                Rectangular

B)
                Spherical

C)
                Dumbbell

D)
                Unsymmetrical
View Solution
66)

The magnetic quantum number for valency electrons of sodium is           [CPMT 1988; MH CET 1999]

A)
                3

B)
                2

C)
                1

D)
                0
View Solution
67)

The electronic configuration of an element with atomic number 7 i.e. nitrogen atom is [CPMT 1982, 84, 87]

A)
                \[1{{s}^{2}},2{{s}^{1}},2p_{x}^{3}\]

B)
                \[1{{s}^{2}},2{{s}^{2}}2p_{x}^{2}2p_{y}^{1}\]

C)
                \[1{{s}^{2}},2{{s}^{2}}2p_{x}^{1}2p_{y}^{1}2p_{z}^{1}\]

D)
                \[1{{s}^{2}},2{{s}^{2}}2p_{x}^{1}2p_{y}^{2}\]
View Solution
68)

In a multi-electron atom, which of the following orbitals described by the three quantum members will have the same energy in the absence of magnetic and electric fields [AIEEE 2005] (1)          \[n=1,\,l=0,\,m=0\]                         (2)          \[n=2,\,l=0,\,m=0\] (3)          \[n=2,\,l=1,\,m=1\]                         (4)          \[n=3,\,l=2,\,m=0\] (5)          \[n=3,\,l=2,\,m=0\]

A)
                (1) and (2)

B)
                (2) and (3)

C)
                (3) and (4)

D)
                (4) and (5)
View Solution
69)

Which of the following represents the electronic configuration of an element with atomic number 17 [AMU 1982]

A)
                \[1{{s}^{2}},2{{s}^{2}}2{{p}^{6}},3{{s}^{1}}3{{p}^{6}}\]

B)
                \[1{{s}^{2}},2{{s}^{2}}2{{p}^{6}},3{{s}^{2}}3{{p}^{4}},4{{s}^{1}}\]

C)
                \[1{{s}^{2}},2{{s}^{2}}2{{p}^{6}},3{{s}^{2}}3{{p}^{5}}\]

D)
                \[1{{s}^{2}},2{{s}^{2}}2{{p}^{6}},3{{s}^{1}}3{{p}^{4}},4{{s}^{2}}\]
View Solution
70)

The shape of \[s\]-orbital is         [NCERT 1978I]

A)
                Pyramidal

B)
                Spherical

C)
                Tetrahedral

D)
                Dumb-bell shaped
View Solution
71)

When \[3d\] orbital is complete, the new electron will enter the [EAMCET 1980; MP PMT 1995]

A)
                \[4p\]-orbital

B)
                \[4f\]-orbital

C)
                \[4s\]-orbital

D)
                \[4d\]-orbital
View Solution
72)

In a potassium atom, electronic energy levels are in the following order                [EAMCET 1979; DPMT 1991]

A)
                \[4s>3d\]

B)
                \[4s>4p\]

C)
                \[4s<3d\]

D)
                \[4s<3p\]
View Solution
73)

\[Fe\] (atomic number = 26) atom has the electronic arrangement           [NCERT 1974; MNR 1980]

A)
                2, 8, 8, 8

B)
                2, 8, 16

C)
                2, 8,14, 2

D)
                2, 8, 12, 4
View Solution
74)

\[C{{u}^{2+}}\] will have the following electronic configuration [MP PMT 1985]

A)
                \[1{{s}^{2}},2{{s}^{2}}2{{p}^{6}},3{{s}^{2}}3{{p}^{6}}3{{d}^{10}}\]

B)
                \[1{{s}^{2}},2{{s}^{2}}2{{p}^{6}},3{{s}^{2}}3{{p}^{6}}3{{d}^{9}},4{{s}^{1}}\]

C)
                \[1{{s}^{2}},2{{s}^{2}}2{{p}^{6}},3{{s}^{2}}3{{p}^{6}}3{{d}^{9}}\]

D)
                \[1{{s}^{2}},2{{s}^{2}}2{{p}^{6}},3{{s}^{2}}3{{p}^{6}}3{{d}^{10}},4{{s}^{1}}\]
View Solution
75)

Which one is the electronic configuration of \[F{{e}^{+2}}\] [MADT Bihar 1982; AIIMS 1989]

A)
                \[1{{s}^{2}},2{{s}^{2}}2{{p}^{6}},3{{s}^{2}}3{{p}^{6}}3{{d}^{6}}\]

B)
                \[1{{s}^{2}},2{{s}^{2}}2{{p}^{6}},3{{s}^{2}}3{{p}^{6}}3{{d}^{4}},4{{s}^{2}}\]

C)
                \[1{{s}^{2}},2{{s}^{2}}2{{p}^{6}},3{{s}^{2}}3{{p}^{6}}3{{d}^{5}},4{{s}^{1}}\]

D)
                None of these
View Solution
76)

How many electrons can be fit into the orbitals that comprise the \[{{3}^{rd}}\] quantum shell \[n=3\] [MP PMT 1986, 87; Orissa JEE 1997]

A)
                2

B)
                8

C)
                18

D)
                32
View Solution
77)

Which element is represented by the following electronic configuration                                [MP PMT 1987]

A)
                Nitrogen

B)
                Oxygen

C)
                Fluorine

D)
                Neon
View Solution
78)

If the value of azimuthal quantum number is 3, the possible values of magnetic quantum number would be [MP PMT 1987; RPMT 1999; AFMC 2002; KCET 2002]

A)
                0, 1, 2, 3

B)
                0, ? 1, ? 2, ? 3

C)
                0, \[\pm \]1, \[\pm \]2, \[\pm \] 3

D)
                \[\pm \]1, \[\pm \]2, \[\pm \]3
View Solution
79)

Krypton \[{{(}_{36}}Kr)\] has the electronic configuration \[{{(}_{18}}Ar)\] \[4{{s}^{2}},3{{d}^{10}},4{{p}^{6}}\]. The \[{{37}^{th}}\] electron will go into which one of the following sub-levels [CBSE PMT 1989; CPMT 1989; EAMCET 1991]

A)
                \[4f\]

B)
                \[4d\]

C)
                \[3p\]

D)
                \[5s\]
View Solution
80)

If an electron has spin quantum number of \[+\frac{1}{2}\] and a magnetic quantum number of \[-1\], it cannot be presented in an                [CBSE PMT 1989; UPSEAT 2001]

A)
                \[d\]-orbital

B)
                \[f\]-orbital

C)
                \[p\]-orbital

D)
                \[s\]-orbital
View Solution
81)

The azimuthal quantum number is related to [BHU 1987, 95]

A)
                Size

B)
                Shape

C)
                Orientation

D)
                Spin
View Solution
82)

The total number of electrons that can be accommodated in all the orbitals having principal quantum number 2 and azimuthal quantum number 1 is                [CPMT 1971, 89, 91]

A)
                2

B)
                4

C)
                6

D)
                8
View Solution
83)

Electronic configuration of \[C\] is            [CPMT 1975]

A)
                \[1{{s}^{2}},2{{s}^{2}}2{{p}^{2}}\]

B)
                \[1{{s}^{2}},2{{s}^{2}}2{{p}^{3}}\]

C)
                \[1{{s}^{2}},2{{s}^{2}}\]

D)
                \[1{{s}^{2}},2{{s}^{2}}2{{p}^{6}}\]
View Solution
84)

There is no difference between a \[2p\] and a \[3p\]orbital regarding                                    [BHU 1981]

A)
                Shape

B)
                Size

C)
                Energy

D)
                Value of \[n\]
View Solution
85)

The electronic configuration of chromium is [MP PMT 1993; MP PET 1995; BHU 2001; BCECE 2005]

A)
                \[[Ne]3{{s}^{2}}3{{p}^{6}}3{{d}^{4}},4{{s}^{2}}\]

B)
                \[[Ne]3{{s}^{2}}3{{p}^{6}}3{{d}^{5}},4{{s}^{1}}\]

C)
                \[[Ne]3{{s}^{2}}3{{p}^{6}},4{{s}^{2}}4{{p}^{4}}\]

D)
                \[[Ne]3{{s}^{2}}3{{p}^{6}}3{{d}^{1}},4{{s}^{2}}4{{p}^{3}}\]
View Solution
86)

The shape of \[p\]-orbital is        [MP PMT 1993]

A)
                Elliptical

B)
                Spherical

C)
                Dumb-bell

D)
                Complex geometrical
View Solution
87)

The electronic configuration (outermost) of \[M{{n}^{+2}}\] ion (atomic number of \[Mn=25\]) in its ground state is [MP PET 1993]

A)
                \[3{{d}^{5}},4{{s}^{0}}\]

B)
                \[3{{d}^{4}},4{{s}^{1}}\]

C)
                \[3{{d}^{3}},4{{s}^{2}}\]

D)
                \[3{{d}^{2}},4{{s}^{2}}4{{p}^{2}}\]
View Solution
88)

The principal quantum number represents          [CPMT 1991]

A)
                Shape of an orbital

B)
                Distance of electron from nucleus

C)
                Number of electrons in an orbit

D)
                Number of orbitals in an orbit
View Solution
89)

When the azimuthal quantum number has a value of \[l=1\], the shape of the orbital is [MP PET 1993]

A)
                Unsymmetrical

B)
                Spherically symmetrical

C)
                Dumb-bell

D)
                Complicated
View Solution
90)

How many electrons can be accommodated in a sub-shell for which \[n=3,\,l=1\]             [CBSE PMT 1990]

A)
                8

B)
                6

C)
                18

D)
                32
View Solution
91)

For azimuthal quantum number \[l=3\], the maximum number of electrons will be                                          [CBSE PMT 1991; EAMCET 1991; RPMT 2002; CBSE PMT 2002]

A)
                2

B)
                6

C)
                0

D)
                14
View Solution
92)

An ion has 18 electrons in the outermost shell, it is [CBSE PMT 1990]

A)
                \[C{{u}^{+}}\]

B)
                \[T{{h}^{4+}}\]

C)
                \[C{{s}^{+}}\]

D)
                \[{{K}^{+}}\]
View Solution
93)

The order of filling of electrons in the orbitals of an atom will be                                [CBSE PMT 1991]

A)
                \[3d,\,4s,\,4p,\,4d,\,5s\]

B)
                \[4s,\,3d,\,4p,\,5s,\,4d\]

C)
                \[5s,\,4p,\,3d,\,4d,\,5s\]

D)
                \[3d,\,4p,\,4s,\,4d,\,5s\]
View Solution
94)

The quantum number which may be designated by \[s,\,p,\,d\] and \[f\] instead of number is BHU 1980]

A)
                \[n\]

B)
                \[l\]

C)
                \[{{m}_{l}}\]

D)
                \[{{m}_{s}}\]
View Solution
95)

Which of the following represents the correct sets of the four quantum numbers of a \[4d\] electron [MNR 1992; UPSEAT 2001; J&K CET 2005]

A)
                \[4,\,3,\,2,\,\frac{1}{2}\]

B)
                4, 2, 1, 0

C)
                \[4,\,3,\,-2,\,+\frac{1}{2}\]

D)
                \[4,\,2,\,1,\,-\frac{1}{2}\]
View Solution
96)

Which of the following statements is not correct for an electron that has the quantum numbers \[n=4\] and \[m=2\] [MNR 1993]

A)
                The electron may have the quantum number \[s=+\frac{1}{2}\]

B)
                The electron may have the quantum number \[l=2\]

C)
                The electron may have the quantum number \[l=3\]

D)
                The electron may have the quantum number \[l=0,\,1,\,2,\,3\]
View Solution
97)

The set of quantum numbers not applicable for an electron in an atom is                                              [MNR 1994]

A)
                \[n=1,\,l=1,\,{{m}_{l}}=1,\,{{m}_{s}}=+1/2\]

B)
                \[n=1,\,l=0,\,{{m}_{l}}=0,\,{{m}_{s}}=+1/2\]

C)
                \[n=1,\,l=0,\,{{m}_{l}}=0,\,{{m}_{s}}=-1/2\]

D)
                \[n=2,\,l=0,\,{{m}_{l}}=0,\,{{m}_{s}}=+1/2\]
View Solution
98)

Correct configuration of \[F{{e}^{+3}}\] [26] is [CPMT 1994; BHU 1995; KCET 1992]

A)
                \[1{{s}^{2}},2{{s}^{2}}2{{p}^{6}},3{{s}^{2}}3{{p}^{6}}3{{d}^{5}}\]

B)
                \[1{{s}^{2}},2{{s}^{2}}s{{p}^{6}},3{{s}^{2}}3{{p}^{6}}3{{d}^{3}},4{{s}^{2}}\]

C)
                \[1{{s}^{2}},2{{s}^{2}}2{{p}^{6}},3{{s}^{2}}3{{p}^{6}}3{{d}^{6}},4{{s}^{2}}\]

D)
                \[1{{s}^{2}},2{{s}^{2}}2{{p}^{6}},3{{s}^{2}}3{{p}^{6}}3{{d}^{5}},4{{s}^{1}}\]
View Solution
99)

Azimuthal quantum number for last electron of \[Na\] atom is [BHU 1995]

A)
                1

B)
                2

C)
                3

D)
                0
View Solution
100)

A \[3p\]orbital has                                           [IIT 1995]

A)
                Two spherical nodes

B)
                Two non-spherical nodes

C)
                One spherical and one non-spherical nodes

D)
                One spherical and two non-spherical nodes
View Solution
101)

All electrons on the \[4p\] sub-shell must be characterized by the quantum number(s) [MP PET 1996]

A)
\[n=4,\,m=0,\,s=\pm \frac{1}{2}\]

B)
                \[l=1\]

C)
                \[l=0,\,s=\pm \frac{1}{2}\]

D)
                \[s=\pm \frac{1}{2}\]
View Solution
102)

The electronic configuration of the element of atomic number 27 is

A)
                \[1{{s}^{2}},\ 2{{s}^{2}}2{{p}^{6}},\ 3{{s}^{2}}3{{p}^{6}},\ 4s\ (\uparrow \downarrow )\ 4p\ (\uparrow \downarrow )(\uparrow \downarrow )(\uparrow \downarrow )\ 5s\ (\uparrow )\]

B)
                \[1{{s}^{2}},\ 2{{s}^{2}}2{{p}^{6}},\ 3{{s}^{2}}3{{p}^{6}}3d\ (\uparrow \downarrow )(\uparrow \downarrow )(\uparrow \downarrow ),\ 4s\ (\uparrow \downarrow )\ 4p\ (\uparrow )\]

C)
                \[1{{s}^{2}},\ 2{{s}^{2}}2{{p}^{6}},\ 3{{s}^{2}}3{{p}^{6}},\ 3d\ (\uparrow \downarrow )(\uparrow \downarrow )(\uparrow \downarrow )(\uparrow \downarrow ),\ 4s\ (\uparrow )\]

D)
                \[1{{s}^{2}},\ 2{{s}^{2}}2{{p}^{6}},\ 3{{s}^{2}}3{{p}^{6}},\ 3d\ (\uparrow \downarrow )(\uparrow \downarrow )(\uparrow )(\uparrow )(\uparrow )\ 4s\ (\uparrow \downarrow )\]
View Solution
103)

When the value of the principal quantum number \[n\] is 3, the permitted values of the azimuthal quantum numbers \[l\] and the magnetic quantum numbers \[m\] , are

A)
                \[l\]-\[\begin{matrix}    0 \\    1 \\    2 \\ \end{matrix}\]                  \[m\]-\[\begin{matrix}    0 \\    +1,\,0,\,-1 \\ +2,+1,\,\,0,\,-1,-2 \\ \end{matrix}\]

B)
                \[l\]-\[\begin{matrix}    1 \\    2 \\    3 \\ \end{matrix}\]                  \[m\]-\[\begin{matrix}    1 \\    +2,\,1,\,-1 \\    +3,+2,\,\,1,\,-2,-3 \\ \end{matrix}\]

C)
                \[l\]-\[\begin{matrix}    0 \\    1 \\    2 \\ \end{matrix}\]                  \[m\]-\[\begin{matrix}    0 \\    1,\,\,2,\,3 \\    +3,\,+2,\,1,\,-2,-3 \\ \end{matrix}\]

D)
                \[l\]-\[\begin{matrix}    1 \\    2 \\    3 \\ \end{matrix}\]                  \[m\]-\[\begin{matrix}    0,\,\,1 \\    0,\,\,1,\,\,2 \\    0,\,\,1,\,\,2,\,\,3 \\ \end{matrix}\]
View Solution
104)

The number of possible spatial orientations of an electron in an atom is given by its

A)
                Spin quantum number

B)
                Spin angular momentum

C)
                Magnetic quantum number

D)
                Orbital angular momentum
View Solution
105)

Which of the following sets of orbitals may degenerate

A)
                \[2s,\,2{{p}_{x}},\,2{{p}_{y}}\]

B)
                \[3s,\,3{{p}_{x}},3{{d}_{xy}}\]

C)
                \[1s,\,2s,\,3s\]

D)
                \[2{{p}_{x}},\,2{{p}_{y}},\,2{{p}_{z}}\]
View Solution
106)

The set of quantum numbers \[n=3,\,l=0,\,m=0,\,s=-1/2\] belongs to the element

A)
                \[Mg\]

B)
                \[Na\]

C)
                \[Ne\]

D)
                \[F\]
View Solution
107)

An electron has principal quantum number 3. The number of its (i) sub-shells and (ii) orbitals would be respectively [MP PET 1997]

A)
                3 and 5

B)
                3 and 7

C)
                3 and 9

D)
                2 and 5
View Solution
108)

What is the electronic configuration of \[C{{u}^{2+}}(Z=29)\] of least position     [MP PET/PMT 1998; MP PET 2001]

A)
                \[[Ar]\,4{{s}^{1}}3{{d}^{8}}\]

B)
                \[[Ar]\,4{{s}^{2}}3{{d}^{10}}4{{p}^{1}}\]

C)
                \[[Ar]\,4{{s}^{1}}3{{d}^{10}}\]

D)
                \[[Ar]\,3{{d}^{9}}\]
View Solution
109)

The correct electronic configuration of \[Ti(Z=22)\] atom is [MP PMT 1999]

A)
                \[1{{s}^{2}}2{{s}^{2}}2{{p}^{6}}3{{s}^{2}}3{{p}^{6}}4{{s}^{2}}3{{d}^{2}}\]

B)
                \[1{{s}^{2}}2{{s}^{2}}2{{p}^{6}}3{{s}^{2}}3{{p}^{6}}3{{d}^{4}}\]

C)
                \[1{{s}^{2}}2{{s}^{2}}2{{p}^{6}}3{{s}^{2}}3{{p}^{6}}3{{d}^{4}}\]

D)
                \[1{{s}^{2}}2{{s}^{2}}2{{p}^{6}}3{{s}^{2}}3{{p}^{6}}4{{s}^{1}}3{{d}^{3}}\]
View Solution
110)

Which of the following configuration is correct for iron [CBSE PMT 1999]

A)
                \[1{{s}^{2}}2{{s}^{2}}2{{p}^{6}}3{{s}^{2}}3{{p}^{6}}3{{d}^{5}}\]

B)
                \[1{{s}^{2}}2{{s}^{2}}2{{p}^{6}}3{{s}^{2}}3{{p}^{6}}4{{s}^{2}}3{{d}^{5}}\]

C)
                \[1{{s}^{2}}2{{s}^{2}}2{{p}^{6}}3{{s}^{2}}3{{p}^{6}}4{{s}^{2}}3{{d}^{7}}\]

D)
                \[1{{s}^{2}}2{{s}^{2}}2{{p}^{6}}3{{s}^{2}}3{{p}^{6}}4{{s}^{2}}3{{d}^{6}}\]
View Solution
111)

Which of the following set of quantum numbers belong to highest energy                                           [CPMT 1999]

A)
                \[n=4,\,l=0,\,m=0,\,s=+\frac{1}{2}\]

B)
                \[n=3,\,l=0,\,m=0,\,s=+\frac{1}{2}\]

C)
                \[n=3,\,l=1,\,m=1,\,s=+\frac{1}{2}\]

D)
                \[n=3,\,l=2,\,m=1,\,s=+\frac{1}{2}\]
View Solution
112)

Which quantum number will determine the shape of the subshell            [CPMT 1999; Pb. PMT 1998]

A)
                Principal quantum number

B)
                Azimuthal quantum number

C)
                Magnetic quantum number

D)
                Spin quantum number
View Solution
113)

For the \[n=2\] energy level, how many orbitals of all kinds are possible                                                [Bihar CEE 1995]

A)
                2

B)
                3

C)
                4

D)
                5
View Solution
114)

Which one is in the ground state               [DPMT 1996]

A)


B)


C)


D)

View Solution
115)

                When the principal quantum number \[(n=3)\], the possible values of azimuthal quantum number (\[l\]) is [Bihar MEE 1996; KCET 2000]

A)
                0, 1, 2, 3

B)
                0, 1, 2

C)
                ? 2, ? 1, 0, 1, 2

D)
                1, 2, 3

E)
                0, 1
View Solution
116)

Which statement is not correct for \[n=5\], \[m=3\] [CPMT 1996]

A)
                \[l=4\]

B)
                \[l=0,\,1,\,3;\,s=+\frac{1}{2}\]

C)
                \[l=3\]

D)
                All are correct
View Solution
117)

\[1{{s}^{2}}2{{s}^{2}}2{{p}^{6}}3{{s}^{1}}\] shows configuration of          [CPMT 1996]

A)
                \[A{{l}^{3+}}\] in ground state

B)
                \[Ne\] in excited state

C)
                \[M{{g}^{+}}\] in excited state

D)
                None of these
View Solution
118)

Five valence electrons of \[{{p}^{15}}\] are labelled as If the spin quantum of \[B\] and \[Z\] is \[+\frac{1}{2}\], the group of electrons with three of the quantum number same are [JIPMER 1997]

A)
                \[AB,\,XYZ,\,BY\]

B)
                \[AB\]

C)
                \[XYZ,\,AZ\]

D)
                \[AB,\,XYZ\]
View Solution
119)

Electronic configuration of \[S{{c}^{21}}\] is        [BHU 1997]

A)
                \[1{{s}^{2}}2{{s}^{2}}2{{p}^{6}}3{{s}^{2}}3{{p}^{6}}4{{s}^{2}}3{{d}^{1}}\]

B)
                \[1{{s}^{2}}2{{s}^{2}}2{{p}^{6}}3{{s}^{2}}3{{p}^{6}}4{{s}^{1}}3{{d}^{2}}\]

C)
                \[1{{s}^{2}}2{{s}^{2}}2{{p}^{6}}3{{s}^{2}}3{{p}^{6}}4{{s}^{0}}3{{d}^{3}}\]

D)
                \[1{{s}^{2}}2{{s}^{2}}2{{p}^{6}}3{{s}^{2}}3{{p}^{2}}4{{s}^{2}}3{{d}^{2}}\]
View Solution
120)

If \[n+l=6\], then total possible number of subshells would be   [RPMT 1997]

A)
                3

B)
                4

C)
                2

D)
                5
View Solution
121)

An electron having the quantum numbers \[n=4,\,l=3,\,m=0\], \[s=-\frac{1}{2}\] would be in the orbital [Orissa JEE 1997]

A)
                \[3s\]

B)
                \[3p\]

C)
                \[4d\]

D)
                \[4f\]
View Solution
122)

Which of the following sets of quantum numbers is not allowed                                                [Orissa JEE 1997]

A)
                \[n=1,\,l=0,\,m=0,\,s=+\frac{1}{2}\]

B)
                \[n=1,\,l=1,\,m=0,\,s=-\frac{1}{2}\]

C)
                \[n=2,\,l=1,\,m=1,\,s=+\frac{1}{2}\]

D)
                \[n=2,\,l=1,\,m=0,\,s=-\frac{1}{2}\]
View Solution
123)

For which of the following sets of four quantum numbers, an electron will have the highest energy [CBSE PMT 1994]

A)
                \[n\]-3          \[l\]-2             \[m\]-1            \[s\]- +1/2

B)
                \[n\]-4          \[l\]-2             \[m\]-1            \[s\]- +1/2

C)
                \[n\]-4          \[l\]-1             \[m\]- 0            \[s\]- -1/2

D)
                \[n\]-5          \[l\]-0             \[m\]-0            \[s\]- -1/2
View Solution
124)

The electronic configuration of gadolinium (atomic no. 64) is                       [CBSE PMT 1997]

A)
                \[[Xe]4{{s}^{8}}5{{d}^{9}}6{{s}^{2}}\]

B)
                \[[Xe]4{{s}^{7}}5{{d}^{1}}6{{s}^{2}}\]

C)
                \[[Xe]4{{s}^{3}}5{{d}^{5}}6{{s}^{2}}\]

D)
                \[[Xe]4{{f}^{6}}5{{d}^{2}}6{{s}^{2}}\]
View Solution
125)

An \[{{e}^{-}}\] has magnetic quantum number as \[-3\], what is its principal quantum number [BHU 1998]

A)
                1

B)
                2

C)
                3

D)
                4
View Solution
126)

The number of quantum numbers required to describe an electron in an atom completely is      [CET Pune 1998]

A)
                1

B)
                2

C)
                3

D)
                4
View Solution
127)

The electronic configuration \[1{{s}^{2}}2{{s}^{2}}2p_{x}^{1}2p_{y}^{1}2p_{z}^{1}\] [AFMC 1997; Pb. PMT 1999; CBSE PMT 2001; AIIMS 2001]

A)
                Oxygen

B)
                Nitrogen

C)
                Hydrogen

D)
                Fluorine
View Solution
128)

Which one of the following set of quantum numbers is not possible for \[4p\] electron [EAMCET 1998]

A)
                \[n=4,\,l=1,\,m=-1,\,s=+\frac{1}{2}\]

B)
                \[n=4,\,l=1,\,m=0,\,s=+\frac{1}{2}\]

C)
                \[n=4,\,l=1,\,m=2,\,s=+\frac{1}{2}\]

D)
                \[n=4,\,l=1,\,m=-1,\,s=+\frac{1}{2}\]
View Solution
129)

Which of the following orbital is not possible       [RPMT 1999]

A)
                3 f

B)
                4 f

C)
                5 f

D)
                6 f
View Solution
130)

Which set of quantum numbers for an electron of an atom is not possible            [RPMT; DCE 1999]

A)
                \[n=1,\,l=0,\,m=0,\,s=+1/2\]

B)
                \[n=1,\,l=1,\,m=1,\,s=+1/2\]

C)
                \[n=1,l=0,\,m=0,\,s=-1/2\]

D)
                \[n=2,\,l=1,\,m=-1,\,s=+1/2\]
View Solution
131)

Electronic configuration of ferric ion is    [RPET 2000]

A)
                \[[Ar]\,3{{d}^{5}}\]

B)
                \[[Ar]\,3{{d}^{7}}\]

C)
                \[[Ar]\,3{{d}^{3}}\]

D)
                \[[Ar]\,3{{d}^{8}}\]
View Solution
132)

What is the maximum number of electrons which can be accommodated in an atom in which the highest principal quantum number value is 4            [MP PMT 2000]

A)
                10

B)
                18

C)
                32

D)
                54
View Solution
133)

Which of the following electronic configurations is not possible [CPMT 2000]

A)
                \[1{{s}^{2}}\,\,2{{s}^{2}}\]

B)
                \[1{{s}^{2}}2{{s}^{2}}2{{p}^{6}}\]

C)
                \[3{{d}^{10}}4{{s}^{2}}4{{p}^{2}}\]

D)
                \[1{{s}^{2}}2{{s}^{2}}\,2{{p}^{2}}3{{s}^{1}}\]
View Solution
134)

The electronic configuration of an element is \[1{{s}^{2}}2{{s}^{2}}2{{p}^{6}}3{{s}^{2}}3{{p}^{6}}3{{d}^{5}}4{{s}^{1}}\]. This represents its [IIT Screening 2000]

A)
                Excited state

B)
                Ground state

C)
                Cationic form

D)
                Anionic form
View Solution
135)

Which of the following set of quantum numbers is possible [AIIMS 2001]

A)
                \[n=3;\,\,l=2;\,\,m=2\] and \[s=+\frac{1}{2}\]

B)
                \[n=3;\,\,l=4;\,\,m=0\] and \[s=-\frac{1}{2}\]

C)
                \[n=4;\,l=0;\,\,m=2\] and \[s=+\frac{1}{2}\]

D)
                \[n=4;\,\,l=4;\,\,m=3\] and \[s=+\frac{1}{2}\]
View Solution
136)

Which of the following set of quantum number is not valid [AIIMS 2001]

A)
                \[n=1,\,\,l=2\]

B)
                \[3=2,\,\,m=1\]

C)
                \[m=3,\,\,l=0\]

D)
                \[3=4,\,\,l=2\]
View Solution
137)

Which one pair of atoms or ions will have same configuration                                     [JIPMER 2001]

A)
                \[{{F}^{+}}\] and \[Ne\]

B)
                \[L{{i}^{+}}\] and \[H{{e}^{-}}\]

C)
                \[C{{l}^{-}}\] and \[Ar\]

D)
                \[Na\] and K
View Solution
138)

Which of the following sets of quantum number is not possible                                 [MP PET 2001]

A)
                \[n=3;\,l=+2;\,m=0;\,s=+\frac{1}{2}\]

B)
                \[n=3;\,l=0;\,m=0;\,s=-\frac{1}{2}\]

C)
                \[n=3;\,l=0;\,m=-1;\,s=+\frac{1}{2}\]

D)
                \[n=3;\,l=1;\,m=0;\,s=-\frac{1}{2}\]
View Solution
139)

Which of the following set of quantum numbers is correct for the 19th electron of chromium       [DCE 2001]

A)
                n-3         l-0           m-0        s- 1/2

B)
                n-3         l-2           m- ? 2   s- 1/2

C)
                n-4         l-0           m- 0       s- ½

D)
                n-4         l-1           m- ?1    s- ½
View Solution
140)

When the value of azimuthal quantum number is 3, magnetic quantum number can have values              [DPMT 2001]

A)
                + 1, 0, ? 1

B)
                + 2, + 1, 0, ? 1, ? 2

C)
                ? 3, ? 2, ? 1, ? 0, + 1, + 2, + 3

D)
                + 1, ? 1
View Solution
141)

The quantum numbers \[n=2,\,\,l=1\] represent              [AFMC 2002]

A)
                1s orbital

B)
                2s orbital

C)
                2p orbital

D)
                3d orbital
View Solution
142)

The magnetic quantum number of valence electron of sodium (Na) is                                    [RPMT 2002]

A)
                3

B)
                2

C)
                1

D)
                0
View Solution
143)

Azimuthal quantum number defines      [AIIMS 2002]

A)
                e/m ratio of electron

B)
                Spin of electron

C)
                Angular momentum of electron

D)
                Magnetic momentum of electron
View Solution
144)

Quantum numbers of an atom can be defined on the basis of                    [AIIMS 2002]

A)
                Hund?s rule

B)
                Aufbau?s principle

C)
                Pauli?s exclusion principle

D)
                Heisenberg?s uncertainty principle
View Solution
145)

Which of the following has maximum energy      [AIIMS 2002]

A)


B)


C)


D)

View Solution
146)

                The total magnetic quantum numbers for d-orbital is given by                    [Orissa JEE 2002]

A)
                2

B)
                0, ± 1, ± 2

C)
                0, 1, 2

D)
                5
View Solution
147)

The outer electronic structure \[3{{s}^{2}}3{{p}^{5}}\] is possessed by   [Pb. PMT 2002; Pb. CET 2001]

A)
                Cl

B)
                O

C)
                Ar

D)
                Br
View Solution
148)

Which of the following set of quantum number is not possible                                   [Pb. PMT 2002]

A)
                n-3         l-2           \[{{m}_{1}}\]-1 \[{{m}_{2}}\]- +1/2

B)
                n ? 3                      l ? 2                        \[{{m}_{1}}\]-1                  \[{{m}_{2}}\]- ? 1/2

C)
                n ? 3                      l ? 2                        \[{{m}_{1}}\]-1                  \[{{m}_{2}}\]- 0

D)
                n ? 5                      l ? 2                        \[{{m}_{1}}\]- ? 1                             \[{{m}_{2}}\]- + 1/2
View Solution
149)

The configuration \[1{{s}^{2}},\,2{{s}^{2}}2{{p}^{5}},\,3{{s}^{1}}\] shows               [Pb. PMT 2002]

A)
                Excited state of \[O_{2}^{-}\]

B)
                Excited state of neon

C)
                Excited state of fluorine

D)
                Ground state of fluorine atom
View Solution
150)

The quantum number ?m? of a free gaseous atom is associated with                                        [AIIMS 2003]

A)
                The effective volume of the orbital

B)
                The shape of the orbital

C)
                The spatial orientation of the orbital

D)
                The energy of the orbital in the absence of a magnetic field
View Solution
151)

Correct statement is       [BHU 2003]

A)
                \[K=4{{s}^{1}},\,\,Cr=3{{d}^{4}}4{{s}^{2}},\,\,Cu=3{{d}^{10}}4{{s}^{2}}\]

B)
                \[K=4{{s}^{2}},\,\,Cr=3{{d}^{4}}4{{s}^{2}},\,\,Cu=3{{d}^{10}}4{{s}^{2}}\]

C)
                \[K=4{{s}^{2}},\,\,Cr=3{{d}^{5}}4{{s}^{1}},\,\,Cu=3{{d}^{10}}4{{s}^{2}}\]

D)
                \[K=4{{s}^{1}},\,\,Cr=3{{d}^{5}}4{{s}^{1}},\,\,Cu=3{{d}^{10}}4{{s}^{1}}\]
View Solution
152)

Number of orbitats in h sub-shell is         [BHU 2003]

A)
                11

B)
                15

C)
                17

D)
                19
View Solution
153)

Electronic configuration \[1{{s}^{2}},\,2{{s}^{2}}2{{p}^{6}},\,3{{s}^{2}}3{{p}^{6}}3{{d}^{5}},\,4{{s}^{1}}\] represents          [CPMT 2003]

A)
                Ground state

B)
                Excited state

C)
                Anionic state

D)
                All of these
View Solution
154)

Which of the following sets is possible for quantum numbers     [RPET 2003]

A)
                \[n=4,\,l=3,\,m=-2,\,s=0\]

B)
                \[n=4,\,l=4,\,m=+2,\,s=-\frac{1}{2}\]

C)
                \[n=4,\,l=4,\,m=-2,\,s=+\frac{1}{2}\]

D)
                \[n=4,\,l=3,\,m=-2,\,s=+\frac{1}{2}\]
View Solution
155)

For principle quantum number \[n=4\] the total number of orbitals having \[l=3\]            [AIIMS 2004]

A)
                3

B)
                7

C)
                5

D)
                9
View Solution
156)

The number of \[2p\] electrons having spin quantum number \[s=-1/2\] are                                       [KCET 2004]

A)
                6

B)
                0

C)
                2

D)
                3
View Solution
157)

Which of the following sets of quantum numbers is correct for an electron in \[4f\] orbital           [AIEEE 2004]

A)
                \[n=4,\,l=3,\,m=+1,\,s=+\frac{1}{2}\]

B)
                \[n=4,\,l=4,\,m=-4,\,s=-\frac{1}{2}\]

C)
                \[n=4,\,l=3,\,m=+4,\,s=+\frac{1}{2}\]

D)
                \[n=3,\,l=2,\,m=-2,\,s=+\frac{1}{2}\]
View Solution
158)

Consider the ground state of \[(Z=24)\]. The numbers of electrons with the azimuthal quantum numbers, \[l=1\] and 2 are, respectively                                       [AIEEE 2004]

A)
                16 and 4

B)
                12 and 5

C)
                12 and 4

D)
                16 and 5
View Solution
159)

The four quantum numbers of the valence electron of potassium are                                     [DPMT 2004]

A)
                4, 1, 0 and \[\frac{1}{2}\]

B)
                4, 0, 1 and \[\frac{1}{2}\]

C)
                4, 0, 0 and \[+\frac{1}{2}\]

D)
                4, 1, 1 and \[\frac{1}{2}\]
View Solution
160)

Which of the following electronic configuration is not possible according to Hund?s rule                  [Kerala PMT 2004]

A)
                \[1{{s}^{2}}2{{s}^{2}}\]

B)
                \[1{{s}^{2}}2{{s}^{1}}\]

C)
                \[1{{s}^{2}}2{{s}^{2}}2p_{x}^{1}2p_{y}^{1}2p_{x}^{1}\]

D)
                \[1{{s}^{2}}2{{s}^{2}}2p_{x}^{2}\]

E)
                \[1{{s}^{2}}2{{s}^{2}}2p_{x}^{2}2p_{y}^{1}2p_{z}^{1}\]
View Solution
161)

The ground state term symbol for an electronic state is governed by       [UPSEAT 2004]

A)
                Heisenberg?s principle

B)
                Hund?s rule

C)
                Aufbau principle

D)
                Pauli exclusion principle
View Solution
162)

The electronic configuration of element with atomic number 24 is            [Pb. CET 2004]

A)
                \[1{{s}^{2}},2{{s}^{2}}2{{p}^{6}},3{{s}^{2}}3{{p}^{6}}3{{d}^{4}},4{{s}^{2}}\]

B)
                \[1{{s}^{2}},2{{s}^{2}}2{{p}^{6}},3{{s}^{2}}3{{p}^{6}}3{{d}^{10}}\]

C)
                \[1{{s}^{2}},2{{s}^{2}}2{{p}^{6}},3{{s}^{2}}3{{p}^{6}}3{{d}^{6}}\]

D)
                \[1{{s}^{2}},2{{s}^{2}}2{{p}^{6}},3{{s}^{2}}3{{p}^{6}}3{{d}^{5}}4{{s}^{1}}\]
View Solution
163)

The maximum number of electrons in \[p\]-orbital with \[n=5,\,m=1\] is              [Pb. CET 2003]

A)
                6

B)
                2

C)
                14

D)
                10
View Solution
164)

Number of two electron can have the same values of ?? quantum numbers      [UPSEAT 2004]

A)
                One

B)
                Two

C)
                Three

D)
                Four
View Solution
165)

The number of orbitals present in the shell with \[n=4\] is            [UPSEAT 2004]

A)
                16

B)
                8

C)
                18

D)
                32
View Solution
166)

Which of the following electronic configuration is not possible    [MHCET 2003]

A)
                \[1{{s}^{2}}2{{s}^{2}}\]

B)
                \[1{{s}^{2}},2{{s}^{2}}2{{p}^{6}}\]

C)
                \[[Ar]\,3{{d}^{10}},4{{s}^{2}}4{{p}^{2}}\]

D)
                \[1{{s}^{2}},2{{s}^{2}}2{{p}^{2}},3{{s}^{1}}\]
View Solution
167)

\[{{p}_{x}}\] orbital can accommodate [MNR 1990; IIT 1983; MADT Bihar 1995; BCECE 2005]

A)
                4 electrons

B)
                6 electrons

C)
                2 electrons with parallel spins

D)
                2 electrons with opposite spins
View Solution
168)

The maximum number of electrons that can be accommodated in \['f'\] sub shell is [CPMT 1983, 84; MP PET/PMT 1988; BITS 1988]

A)
                2

B)
                8

C)
                32

D)
                14
View Solution
169)

The number of electrons which can be accommodated in an orbital is     [DPMT 1981; AFMC 1988]

A)
                One

B)
                Two

C)
                Three

D)
                Four
View Solution
170)

The number of electrons in the atom which has 20 protons in the nucleus          [CPMT 1981, 93; CBSE PMT 1989]

A)
                20

B)
                10

C)
                30

D)
                40
View Solution
171)

The maximum number of electrons accommodated in \[5f\] orbitals are               [MP PET 1996]

A)
                5

B)
                10

C)
                14

D)
                18
View Solution
172)

The maximum number of electrons in an atom with \[l=2\] and \[n=3\] is                                            [MP PET/PMT 1998]

A)
                2

B)
                6

C)
                12

D)
                10
View Solution
173)

The configuration \[1{{s}^{2}}2{{s}^{2}}2{{p}^{5}}3{{s}^{1}}\] shows        [AIIMS 1997]

A)
                Ground state of fluorine atom

B)
                Excited state of fluorine atom

C)
                Excited state of neon atom

D)
                Excited state of ion \[O_{2}^{-}\]
View Solution
174)

For sodium atom the number of electrons with \[m=0\] will be                  [RPMT 1999]

A)
                2

B)
                7

C)
                9

D)
                8
View Solution
175)

The number of electrons that can be accommodated in \[d{{z}^{2}}\] orbital is                   [Kurukshetra CEE 2002]

A)
                10

B)
                1

C)
                4

D)
                2
View Solution
176)

Number of unpaired electrons in \[1{{s}^{2}}2{{s}^{2}}2{{p}^{3}}\] is [CPMT 1982; MP PMT 1987; BHU 1987; CBSE PMT 1990; CET Pune 1998; AIIMS 2000]

A)
                2

B)
                0

C)
                3

D)
                1
View Solution
177)

Total number of unpaired electrons in an atom of atomic number 29 is                                   [CPMT 1984, 93]

A)
                1

B)
                3

C)
                4

D)
                2
View Solution
178)

The number of unpaired electrons in \[1{{s}^{2}},\,2{{s}^{2}}2{{p}^{4}}\] is [NCERT 1984; CPMT 1991; MP PMT 1996, 2002]

A)
                4

B)
                2

C)
                0

D)
                1
View Solution
179)

The maximum number of electrons that can be accommodated in a \[3d\] subshell is

A)
                2

B)
                10

C)
                6

D)
                14
View Solution
180)

The maximum number of electrons which each sub-shell can occupy is                                  [Pb. CET 1989]

A)
                \[2{{n}^{2}}\]

B)
                \[2n\]

C)
                \[2(2l+1)\]

D)
                \[(2l+1)\]
View Solution
181)

Number of unpaired electrons in the ground state of beryllium atom is

A)
                2

B)
                1

C)
                0

D)
                All the above
View Solution
182)

How many unpaired electrons are present in \[N{{i}^{2+}}\] cation (atomic number = 28)                                            [IIT 1981; MNR 1984; MP PMT 1995; Kerala PMT 2003]

A)
                0

B)
                2

C)
                4

D)
                6
View Solution
183)

The number of unpaired electrons in an \[{{O}_{2}}\] molecule is [MNR 1983]

A)
                0

B)
                1

C)
                2

D)
                3
View Solution
184)

The number of unpaired electrons in a chromic ion \[C{{r}^{3+}}\] (atomic number = 24) is          [MNR 1986; CPMT 1992]

A)
                6

B)
                4

C)
                3

D)
                1
View Solution
185)

\[3{{d}^{10}}4{{s}^{0}}\] electronic configuration exhibits by

A)
                \[Z{{n}^{++}}\]

B)
                \[C{{u}^{++}}\]

C)
                \[C{{d}^{++}}\]

D)
                \[H{{g}^{++}}\]
View Solution
186)

Which of the following metal ions will have maximum number of unpaired electrons      [CPMT 1996]

A)
                \[F{{e}^{+2}}\]

B)
                \[C{{O}^{+2}}\]

C)
                \[N{{i}^{+2}}\]

D)
                \[M{{n}^{+2}}\]
View Solution
187)

Which of the metal ion will have highest number of unpaired electrons

A)
                \[C{{u}^{+}}\]

B)
                \[F{{e}^{2+}}\]

C)
                \[F{{e}^{3+}}\]

D)
                \[C{{o}^{2+}}\]
View Solution
188)

The maximum number of unpaired electron can be present in \[d\]orbitals are

A)
                1

B)
                3

C)
                5

D)
                7
View Solution
189)

The molecule having one unpaired electron is

A)
                \[NO\]

B)
                \[CO\]

C)
                \[C{{N}^{-}}\]

D)
                \[{{O}_{2}}\]
View Solution
190)

A filled or half-filled set of \[p\] or \[d\]-orbitals is spherically symmetric. Point out the species which has spherical symmetry                                           [NCERT 1983]

A)
                \[Na\]

B)
                \[C\]

C)
                \[C{{l}^{-}}\]

D)
                \[Fe\]
View Solution
191)

The atom of the element having atomic number 14 should have                                               [AMU 1984]

A)
                One unpaired electron

B)
                Two unpaired electrons

C)
                Three unpaired electrons

D)
                Four unpaired electrons
View Solution
192)

An atom has 2 electrons in \[K\] shell, 8 electrons in \[L\] shell and 6 electrons in \[M\] shell. The number of \[s\]-electrons present in that element is            [CPMT 1989]

A)
                6

B)
                5

C)
                7

D)
                10
View Solution
193)

The number of unpaired electrons in carbon atom in excited state is                                       [MNR 1987]

A)
                One

B)
                Two

C)
                Three

D)
                Four
View Solution
194)

Maximum number of electrons present in \['N'\] shell is [EAMCET 1984]

A)
                18

B)
                32

C)
                2

D)
                8
View Solution
195)

The number of \[d\] electrons in \[F{{e}^{+2}}\] (atomic number of \[Fe=26\]) is not equal to that of the             [MNR 1993]

A)
                \[p\]-electrons in \[Ne\] (At. No.= 10)

B)
                \[s\]-electrons in \[Mg\] (At. No.= 12)

C)
                \[d\]-electrons in \[Fe\]

D)
                \[p\]-electrons in \[C{{l}^{-}}\] (At. No. of \[Cl\] = 17)
View Solution
196)

A transition metal \[X\] has a configuration \[[Ar]3{{d}^{4}}\] in its \[+3\] oxidation state. Its atomic number is   [EAMCET 1990]

A)
                25

B)
                26

C)
                22

D)
                19
View Solution
197)

The total number of electrons present in all the \[p\]-orbitals of bromine are                                     [MP PET 1994]

A)
                Five

B)
                Eighteen

C)
                Seventeen

D)
                Thirty five
View Solution
198)

Which of the following has the maximum number of unpaired electrons                                               [IIT 1996]

A)
                \[M{{g}^{2+}}\]

B)
                \[T{{i}^{3+}}\]

C)
                \[{{V}^{3+}}\]

D)
                \[F{{e}^{2+}}\]
View Solution
199)

Which of the following has more unpaired \[d\]-electrons [CBSE PMT 1999]

A)
                \[Z{{n}^{+}}\]

B)
                \[F{{e}^{2+}}\]

C)
                \[{{N}^{3+}}\]

D)
                \[C{{u}^{+}}\]
View Solution
200)

Maximum electrons in a \[d\]-orbital are              [CPMT 1999]

A)
                2

B)
                10

C)
                6

D)
                14
View Solution
201)

The number of unpaired electrons in \[F{{e}^{3+}}(Z=26)\] are [KCET 2000]

A)
                5

B)
                6

C)
                3

D)
                4
View Solution
202)

How many unpaired electrons are present in cobalt [Co] metal                                  [RPMT 2002]

A)
                2

B)
                3

C)
                4

D)
                7
View Solution
203)

The number of unpaired electrons in nitrogen is                 [Pb. CET 2002]

A)
                1

B)
                3

C)
                2

D)
                None of these
View Solution
204)

Which of the following has the least energy

A)
                \[2p\]

B)
                \[3p\]

C)
                \[2s\]

D)
                \[4d\]
View Solution
205)

Pauli's exclusion principle states that      [CPMT 1983, 84]

A)
                Nucleus of an atom contains no negative charge

B)
                Electrons move in circular orbits around the nucleus

C)
                Electrons occupy orbitals of lowest energy

D)
                All the four quantum numbers of two electrons in an atom cannot be equal
View Solution
206)

For the energy levels in an atom, which one of the following statements is correct           [AIIMS 1983]

A)
                There are seven principal electron energy levels

B)
                The second principal energy level can have four sub-energy levels and contains a maximum of eight electrons

C)
                The \[M\]energy level can have maximum of 32 electrons

D)
                The \[4s\] sub-energy level is at a higher energy than the \[3d\] sub-energy level
View Solution
207)

The statements                                                [AIIMS 1982] (i)            In filling a group of orbitals of equal energy, it is energetically preferable to assign electrons to empty orbitals rather than pair them into a particular orbital. (ii)           When two electrons are placed in two different orbitals, energy is lower if the spins are parallelare valid for

A)
                Aufbau principle

B)
                Hund's rule

C)
                Pauli's exclusion principle

D)
                Uncertainty principle
View Solution
208)

According to Aufbau's principle, which of the three \[4d,\,5p\]   and \[5s\]will be filled with electrons first           [MADT Bihar 1984]

A)
                \[4d\]

B)
                \[5p\]

C)
                \[5s\]

D)
                \[4d\] and \[5s\] will be filled simultaneously
View Solution
209)

The energy of an electron of \[2{{p}_{y}}\] orbital is        [AMU 1984]

A)
                Greater than that of \[2{{p}_{x}}\] orbital

B)
                Less than that of \[2{{p}_{x}}\] orbital

C)
                Equal to that of \[2s\] orbital

D)
                Same as that of \[2{{p}_{z}}\] orbital
View Solution
210)

Which of the following principles/rules limits the maximum number of electrons in an orbital to two       [CBSE PMT 1989]

A)
                Aufbau principle

B)
                Pauli's exclusion principle

C)
                Hund's rule of maximum multiplicity

D)
                Heisenberg's uncertainty principle
View Solution
211)

The electrons would go to lower energy levels first and then to higher energy levels according to which of the following [BHU 1990; MP PMT 1993]

A)
                Aufbau principle

B)
                Pauli's exclusion principle

C)
                Hund's rule of maximum multiplicity

D)
                Heisenberg's uncertainty principle
View Solution
212)

Energy of atomic orbitals in a particular shell is in the order [AFMC 1990]

A)
                \[s<p<d<f\]

B)
                \[s>p>d>f\]

C)
                \[p<d<f<s\]

D)
                \[f>d>s>p\]
View Solution
213)

Aufbau principle is not satisfied by           [MP PMT 1997]

A)
                \[Cr\] and \[Cl\]

B)
                \[Cu\] and \[Ag\]

C)
                \[Cr\] and \[Mg\]

D)
                \[Cu\] and \[Na\]
View Solution
214)

Which of the following explains the sequence of filling the electrons in different shells [AIIMS 1998; BHU 1999]

A)
                Hund's rule

B)
                Octet rule

C)
                Aufbau principle

D)
                All of these
View Solution
215)

Aufbau principle is obeyed in which of the following electronic configurations    [AFMC 1999]

A)
                \[1{{s}^{2}}2{{s}^{2}}2{{p}^{6}}\]

B)
                \[1{{s}^{2}}3{{p}^{3}}3{{s}^{2}}\]

C)
                \[1{{s}^{2}}3{{s}^{2}}3{{p}^{6}}\]

D)
                \[1{{s}^{2}}2{{s}^{2}}3{{s}^{2}}\]
View Solution
216)

Following Hund?s rule which element contains six unpaired electron                                       [RPET 2000]

A)
                Fe

B)
                Co

C)
                Ni

D)
                Cr
View Solution
217)

Electron enters the sub-shell for which \[(n+l)\] value is minimum. This is enunciated as                 [RPMT 2000]

A)
                Hund?s rule

B)
                Aufbau principle

C)
                Heisenberg uncertainty principle

D)
                Pauli?s exclusion principle
View Solution
218)

The atomic orbitals are progressively filled in order of increasing energy. This principle is called as [MP PET 2001]

A)
                Hund?s rule

B)
                Aufbau principle

C)
                Exclusion principle

D)
                de-Broglie rule
View Solution
219)

The correct order of increasing energy of atomic orbitals is [MP PET 2002]

A)
                \[5p<4f<6s<5d\]

B)
                \[5p<6s<4f<5d\]

C)
                \[4f<5p<5d<6s\]

D)
                \[5p<5d<4f<6s\]
View Solution
220)

The orbital with maximum energy is        [CPMT 2002]

A)
                3d

B)
                5p

C)
                4s

D)
                6d
View Solution
221)

p-orbitals of an atom in presence of magnetic field are [Pb. PMT 2002]

A)
                Two fold degenerate

B)
                Non degenerate

C)
                Three fold degenerate

D)
                None of these
View Solution
222)

Orbital angular momentum for a d-electron is    [MP PET 2003]

A)
                \[\frac{6h}{2\pi }\]

B)
                \[\frac{\sqrt{6}\,h}{2\pi }\]

C)
                \[\frac{12h}{2\pi }\]

D)
                \[\frac{\sqrt{12}\,h}{2\pi }\]
View Solution
223)

Number of nodal centres for 2s orbital   [RPET 2003]

A)
                1

B)
                0

C)
                4

D)
                3
View Solution
224)

The orbital angular momentum of an electron in \[2s\]-orbital is                                [MP PET 2004]

A)
                \[\frac{1}{2}\frac{h}{2\pi }\]

B)
                \[\frac{h}{2\pi }\]

C)
                \[\sqrt{2}\frac{h}{2\pi }\]

D)
                Zero
View Solution
225)

The maximum number of electrons present in an orbit \[l=3\], is                                             [Pb. PMT 2004]

A)
                6

B)
                8

C)
                10

D)
                14
View Solution
226)

Number of unpaired electrons in \[M{{n}^{4+}}\] is         [DPMT 2005]

A)
                3

B)
                5

C)
                6

D)
                4
View Solution
227)

Which of the following sequence is correct as per Aufbau principle                                          [DPMT 2005]

A)
                \[3s<3d<4s<4p\]

B)
                \[1s<2p<4s<3d\]

C)
                \[2s<5s<4p<5d\]

D)
                \[2s<2p<3d<3p\]
View Solution
228)

Electronic configuration of deuterium atom is                                                                    [J&K CET 2005]

A)
                \[1{{s}^{1}}\]

B)
                \[2{{s}^{2}}\]

C)
                \[2{{s}^{1}}\]

D)
                \[1{{s}^{2}}\]
View Solution