# General Knowledge - Chemistry - Discussion

Discussion Forum : Chemistry - Section 1 (Q.No. 5)

5.

The number of d-electrons in Fe

^{2+}(Z = 26) is not equal to that ofDiscussion:

31 comments Page 1 of 4.
Clevein said:
11 months ago

The electron configurations are as follows:

1. **Fe²⁺ (Z = 26):** [Ar] 3d⁶.

=> The number of d-electrons is 6.

2. **Ne (Z = 10):** 1s² 2s² 2p⁶

=> There are no p-electrons in Ne.

3. **Mg (Z = 12):** 1s² 2s² 2p⁶ 3s²

=> The number of s-electrons is 2.

4. **Fe (Z = 26):** [Ar] 4s² 3d⁶

=> The number of d-electrons is 6.

5. **Cl (Z = 17):** 1s² 2s² 2p⁶ 3s² 3p⁵

=> The number of p-electrons is 5.

In summary:

- The number of d-electrons in Fe²⁺ (Z = 26) is **6**.

- The number of p-electrons in Ne (Z = 10) is **0**.

- The number of s-electrons in Mg (Z = 12) is **2**.

- The number of d-electrons in Fe (Z = 26) is **6**.

- The number of p-electrons in Cl (Z = 17) is **5**.

Therefore, the statement is correct.

The number of d-electrons in Fe²⁺ is not equal to the specified electron counts in Ne, Mg, Fe, and Cl.

1. **Fe²⁺ (Z = 26):** [Ar] 3d⁶.

=> The number of d-electrons is 6.

2. **Ne (Z = 10):** 1s² 2s² 2p⁶

=> There are no p-electrons in Ne.

3. **Mg (Z = 12):** 1s² 2s² 2p⁶ 3s²

=> The number of s-electrons is 2.

4. **Fe (Z = 26):** [Ar] 4s² 3d⁶

=> The number of d-electrons is 6.

5. **Cl (Z = 17):** 1s² 2s² 2p⁶ 3s² 3p⁵

=> The number of p-electrons is 5.

In summary:

- The number of d-electrons in Fe²⁺ (Z = 26) is **6**.

- The number of p-electrons in Ne (Z = 10) is **0**.

- The number of s-electrons in Mg (Z = 12) is **2**.

- The number of d-electrons in Fe (Z = 26) is **6**.

- The number of p-electrons in Cl (Z = 17) is **5**.

Therefore, the statement is correct.

The number of d-electrons in Fe²⁺ is not equal to the specified electron counts in Ne, Mg, Fe, and Cl.

Osama Shata said:
2 years ago

Fe (Z=26) configuration is [Ar]18 4S2,3d6.

Fe2+ means it will lose two electrons from its outer shell which is 4S.

So the configuration is [Ar]18 4s0, 3d6 . here the Fe2+ is stable because orbitals are fully filled or fully empty. d-electrons Numbers are 6.

Ne10 configuration is 1S2,2S2,2p6. p-electrons Numbers are 6

Mg12 configuration is 4s2,2s2,2p6,3s2 so s-electrons Numbers are 6

Cl17 configuration is 4s2,2s2,2p6,3s2,4p5. After applying half filled orbitals rule, the configuration will be 4s2,2s2,2p6,3s1,3p6 so p-electrons Numbers are 12

So, D is the correct answer.

Fe2+ means it will lose two electrons from its outer shell which is 4S.

So the configuration is [Ar]18 4s0, 3d6 . here the Fe2+ is stable because orbitals are fully filled or fully empty. d-electrons Numbers are 6.

Ne10 configuration is 1S2,2S2,2p6. p-electrons Numbers are 6

Mg12 configuration is 4s2,2s2,2p6,3s2 so s-electrons Numbers are 6

Cl17 configuration is 4s2,2s2,2p6,3s2,4p5. After applying half filled orbitals rule, the configuration will be 4s2,2s2,2p6,3s1,3p6 so p-electrons Numbers are 12

So, D is the correct answer.

(3)

Desale Moges said:
4 years ago

The electron configuration of Fe+2 will be [Ar]4S13d5.

(2)

Maria khan said:
5 years ago

Please give the correct answer description.

M. Ganga rajasree said:
6 years ago

Thanks all for explaining the answer.

(1)

M Mishra said:
6 years ago

But I think the question is incorrect, as it asked.

It should be, The number of d-electrons in Fe2+ (Z = 26) is equal to that of.

It should be, The number of d-electrons in Fe2+ (Z = 26) is equal to that of.

(1)

Satyam Rahul said:
7 years ago

I think option C is right.

Since outer most electron that is in the d orbital there number are 10 and also Fe2+ (Z=26) that's outer most electron numbers are 10 in d orbital.

Since outer most electron that is in the d orbital there number are 10 and also Fe2+ (Z=26) that's outer most electron numbers are 10 in d orbital.

Gaurav iitian said:
7 years ago

Answer must be option C) Fe (26).

Ktjo said:
8 years ago

I think the answer is B because, when its Mg=12, it is 1s2 2s2 2p6 3S2 but the Fe=26 is 1s2 2s2 2p6 3s2 3p6 4s2 3D6.

Even after you lose one electron from the 'd' of Fe orbital it still is not equal to that of Mg.

Even after you lose one electron from the 'd' of Fe orbital it still is not equal to that of Mg.

Sagarika said:
8 years ago

I think the answer is correct because after D, orbital looses their one electron it stabilised fully.

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