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(A) E.C of Pd is [Kr] 4d^(8)5s^(2) (R)...

(A) E.C of Pd is `[Kr] 4d^(8)5s^(2)`
(R) Palladium contains `8e^(-)` in N shell.

A

Both (A) and (R) are true and (R) is the correct explanation of (A)

B

Both (A) and (R) are true and (R) is not the correct explanation of (A)

C

(A) is true but (R) is false

D

Both (A) and (R) are false

Text Solution

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The correct Answer is:
D
Both (A) and (R) are false
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In an atom the number of electrons in M - shell is equal to the number of electrons in the K and L - shell . Answer the question. Explanation : 1) Number of electrons in K-shell (1 s^(2)) = 2 Number of electrons in L-shell (2s^(2) sp^(6)) = 8 Total number of electrons in k & L shells = 10 2) Given that number of electrons in M-shell is equal to number of electrons in K& L- shells 3) Hence number of electrons in M-shell (3s^(2) 3p^(6) 3d^(2)) = 10 4) But , we know that before filling of 3d orbital 4s should be filled (4s^(2)) 5) So , electronic configuration is 1s^(2) 2s^(2) 2p^(6) 3s^(2) 3p^(6) 4s^(2) 3d^(2) What is the atomic number of element ?

In an atom the number of electrons in M - shell is equal to the number of electrons in the K and L - shell . Answer the question. Explanation : 1) Number of electrons in K-shell (1 s^(2)) = 2 Number of electrons in L-shell (2s^(2) sp^(6)) = 8 Total number of electrons in k & L shells = 10 2) Given that number of electrons in M-shell is equal to number of electrons in K& L- shells 3) Hence number of electrons in M-shell (3s^(2) 3p^(6) 3d^(2)) = 10 4) But , we know that before filling of 3d orbital 4s should be filled (4s^(2)) 5) So , electronic configuration is 1s^(2) 2s^(2) 2p^(6) 3s^(2) 3p^(6) 4s^(2) 3d^(2) Which is the outermost cell ?

If int e^(x) (x^(2) - 5x+ 8) " dx = " e^(x) f(x) + c then f(x) =

In an atom the number of electrons in N - Shell is equal to the number of electrons in K, L and M shells. Answer the question. How many electrons are there in its outermost shell ? Explanation : K = 1 s^(2) (2) electrons L = 2s^(2) 2p^(6) (8) electrons M = 3s^(2) 3p^(6) 3d^(10) (18) electrons Total (28) electrons N = 4s^(2) 4p^(6) 4d^(10) 4f^(10) (28) electrons To fill 4f^(10) , 1s^(2) , 2s^(2) 2p^(2) 2p^(6) 3s^(2) 3p^(6) 4s^(2) 3d^(10) 4p^(6) 5s^(2) 4d^(10) 5p^(6) 6s^(2) should be filled Hence , the electronic configuration is 1s^(2) 2s^(2) 2p^(6) 3s^(2) 3p^(6) 4s^(2) 3^(10) 4p^(6) 5s^(2) 4d^(10) 5p^(6) 6s^(2) 4f^(10) .

In an atom the number of electrons in N - Shell is equal to the number of electrons in K, L and M shells. Answer the question. Which is the outermost shell ? Explanation : K = 1 s^(2) (2) electrons L = 2s^(2) 2p^(6) (8) electrons M = 3s^(2) 3p^(6) 3d^(10) (18) electrons Total (28) electrons N = 4s^(2) 4p^(6) 4d^(10) 4f^(10) (28) electrons To fill 4f^(10) , 1s^(2) , 2s^(2) 2p^(2) 2p^(6) 3s^(2) 3p^(6) 4s^(2) 3d^(10) 4p^(6) 5s^(2) 4d^(10) 5p^(6) 6s^(2) should be filled Hence , the electronic configuration is 1s^(2) 2s^(2) 2p^(6) 3s^(2) 3p^(6) 4s^(2) 3^(10) 4p^(6) 5s^(2) 4d^(10) 5p^(6) 6s^(2) 4f^(10) .

In an atom the number of electrons in N - Shell is equal to the number of electrons in K, L and M shells. Answer the question. Write the electronic configuration of the elements. Explanation : K = 1 s^(2) (2) electrons L = 2s^(2) 2p^(6) (8) electrons M = 3s^(2) 3p^(6) 3d^(10) (18) electrons Total (28) electrons N = 4s^(2) 4p^(6) 4d^(10) 4f^(10) (28) electrons To fill 4f^(10) , 1s^(2) , 2s^(2) 2p^(2) 2p^(6) 3s^(2) 3p^(6) 4s^(2) 3d^(10) 4p^(6) 5s^(2) 4d^(10) 5p^(6) 6s^(2) should be filled Hence , the electronic configuration is 1s^(2) 2s^(2) 2p^(6) 3s^(2) 3p^(6) 4s^(2) 3^(10) 4p^(6) 5s^(2) 4d^(10) 5p^(6) 6s^(2) 4f^(10) .

In an atom the number of electrons in N - Shell is equal to the number of electrons in K, L and M shells. Answer the question. What is the atomic number ? Explanation : K = 1 s^(2) (2) electrons L = 2s^(2) 2p^(6) (8) electrons M = 3s^(2) 3p^(6) 3d^(10) (18) electrons Total (28) electrons N = 4s^(2) 4p^(6) 4d^(10) 4f^(10) (28) electrons To fill 4f^(10) , 1s^(2) , 2s^(2) 2p^(2) 2p^(6) 3s^(2) 3p^(6) 4s^(2) 3d^(10) 4p^(6) 5s^(2) 4d^(10) 5p^(6) 6s^(2) should be filled Hence , the electronic configuration is 1s^(2) 2s^(2) 2p^(6) 3s^(2) 3p^(6) 4s^(2) 3^(10) 4p^(6) 5s^(2) 4d^(10) 5p^(6) 6s^(2) 4f^(10) .

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AAKASH SERIES-D-BLOCK ELEMENTS-OBJECTIVE EXERCISE-4 (ASSERTION (A) & REASON (R) TYPE QUESTIONS )
  1. (A) Zn^(+2) is diamagnetic (R) The electrons are lost from 4s orbita...

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  2. (A) d block elements are transitioned between s-block metals and p-blo...

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  3. (A) E.C of Pd is [Kr] 4d^(8)5s^(2) (R) Palladium contains 8e^(-) in ...

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  4. (A) Sc exhibit variable oxidation states. (R) Sc is not a transition...

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  5. (A) : Cu^(+2)(aq) is more stable than Cu^(+)(aq) (R): Heat of hydrat...

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  6. (A) Cr^(+2) is reducing in nature. (R) Half filled t(zg) level in Cr...

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  7. (A) Many copper(I) compounds are unstable in aqueous solution. (R) ...

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  8. (A) The number of unpaired electrons in the following gaseous ion Mn^...

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  9. (A) MnO(4)^(-1) is strong oxidizing agent. (R) Mn^(+2) is stable wit...

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  10. (A) The free gaseous Cr atom has six unpaired electrons. (R) Half fi...

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  11. (A) E^(@) for Mn^(+3)//Mn^(+2) is more positive than Cr^(3+)//Cr^(+2) ...

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  12. (A) K2Cr2O7 is used as primary standard in volumetric analysis. (R) ...

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  13. (A) Solution of Na2CrO4 in water is intensely coloured. (R) Oxidatio...

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  14. (A) Elements of 4f sries are called Lanthanides (R) Lanthanum Belong...

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  15. (A) Silver. Gold and platinum are precious metals. (R) Silver glod a...

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  16. (A) Zn,Cd^(-) and Hg of group 12 are transition metals (R) Partiall...

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  17. (A) Mn & Hg exist in simple crystal structures. (R) Both Mn & Hg are...

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  18. (A) Metals of 4d and 5d series have greater enthalpies of atomization ...

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  19. (A) The enthalpy of atomization of zinc is the highest in 3d series. ...

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  20. (A) Second ionization enthalpies of Cr and Cn are very low (R) Both ...

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