CHEMISTRY || ATOMIC STRUCTURE-II - SAMIT SIR || XII ||’25|| ENGLISH

1.

Given below are two statements :
Statement I : the orbitals having same energy are called as degenerate orbitals.

Statement II: In hydrogen atom 3p and 3d orbital are not degenerate orbitals .
In the light of the above statement choose the most appropriate answer from the option given

Statement I is true but Statement II is false

Both Statement I and Statement II are true

Both Statement I and Statement II are false

Statement I is false but Statement II is true

2

Match List I with List II

Choose the correct answer from the options given below

A-III,B-IV,C-I,D-II

A-III,B-IV,C-II,D-I

A-II,B-I,C-IV,D-III

A-I,B-III,C-II,D-IV

3

The number of electrons that can be fit into the orbital for which n=3 and l = 1 is

2

6

10

14

4.

Beryllium's fourth electron will have the four quantum numbers

1

2

3

4

5

The total spin resulting for a \( 3d^7 \)
configuration is

3/2

1/2

2

1

6

Which one of the following statement is not true about the quantum numbers n, l,m and s.

m gives the information on the energy of the electron in a given orbital

l gives idea of the shape of the orbital

n gives information on the size of the orbit

s gives the direction of the speed of the electron in the orbital

7

To give designation to an orbital, we need

principal and azimuthal quantum number

principal and magnetic quantum number

azimuthal and magnetic quantum number

principal,azimuthal and magnetic Quantum numbers

8.

The total number of orbitals having l=3 is

3

7

5

9

The quantum number of the most energetic electron in an Ne atom in the first excited state is

2,1,0,+1/2

3,1,1,+1/2

3,0,0,+1/2

3,1,0,+1/2

10

The maximum number of atomic orbitals associated with a principal quantum umber 5 is

9

12

16

25

11

Which of the following sets of quantum numbers represent an impossible arrangement

1

2

3

4

12

Which of the following is/are not correct with respect to energy of atomic orbitals of hydrogen atom?
A)1s<2p<3d<4s
B)1s<2s=2p<3s=3p
C)1s<2s<2p<3s<3p
D)1s<2s<4s<3d
Choose the correct answer from the options given below

A & C only

B & D only

C & D only

A & B only

13

If \( a_0 \)is denoted as the Bohr radius of hydrogen atom, then what is the De Broglie wavelength( \( \lambda \)
) of the electron present in the second orbit of hydrogen atom [n: any Integer]

\( \frac{8\pi a_0}{n} \)

\( \frac{2a_0}{n\pi} \)

\( \frac{4n}{\pi a_0} \)

\( \frac{4 \pi a_0}{n} \)

14

The quantum number not obtained from scrollinger's Wave Equation is

n

l

m

s

15

Two electrons occupying the same orbital are distinguished by

Magnetic quantum number

Azimuthal quantum number

spin quantum number

principal quantum number

16

Which one of the following sets of ions represents a collection of isoelectronic species
(Given atomic number: F:9 ,Cl 17 ,Na =11 Mg =12 ,Al =13 Ca= 20, Sc= 21)

\( \mathrm{Li}^+, \mathrm{Na}^+, \mathrm{Mg}^+, \mathrm{Ca}^{2+} \)

\( \mathrm{Ba}^{2+}, \mathrm{Sr}^{2+}, \mathrm{K}^+, \mathrm{Ca}^{2+} \)

\( \mathrm{N}^{3-}, \mathrm{O}^{2-}, \mathrm{F}^-, \mathrm{S}^{2-} \)

\( \mathrm{K}^+, \mathrm{Cl}^-, \mathrm{Ca}^{2+}, \mathrm{Sc}^{3+} \)

17

Given below are two statements :
Statement I: For a given shell, the total number of allowed orbitals is given by \( n^2 \)
Statement II: For any subshell the spatial orientation of Orbital is given by -l to +l values including zero.
in the light of the above statements choose the correct answer from the options given below

Both the statement I and statement II are false

statement I is true but statement II is false

both statement I and statement II are true

statement I is false but statement II is true

18

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

1

2

3

4

19

The development of the wave mechanical model of the atom is based on which of the following concepts ?

De Broglie concept of the dual nature of the electron

Heisenberg Uncertainty Principle

Schrodinger's principle

all of the above

20

The correct Schrodinger's wave equation for a electron with total energy E and potential energy V is given by

\[ \frac{\partial^2 \psi}{\partial x^2} + \frac{\partial^2 \psi}{\partial y^2} + \frac{\partial^2 \psi}{\partial z^2} + \frac{8 \pi^2 m}{h^2}(E - V) \psi = 0 \]

\[ \frac{\partial^2 \psi}{\partial x^2} + \frac{\partial^2 \psi}{\partial y^2} + \frac{\partial^2 \psi}{\partial z^2} + \frac{8 \pi m}{h^2}(E - V)\psi = 0 \]

\[ \frac{\partial^2 \psi}{\partial x^2} + \frac{\partial^2 \psi}{\partial y^2} + \frac{\partial^2 \psi}{\partial z^2} + \frac{8 \pi^2 m}{h^2}(E - V)\psi = 0 \]

None of the above

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