Question

The correct ground state electronic configuration of chromium atom (Z = 24) is *
a) [Ar] 3d⁵ 4s¹
b) [Ar] 3d⁴ 4s²
c) [Ar] 3d⁶ 4s⁰
d) [Ar] 4s¹ 4p⁵
Q3. What would be the

Answer 1

Answer:

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ANSWER = b) [Ar] 3d⁴ 4s²

Answer 2

Answer:

In writing the electron configuration for Chromium the first two electrons will go in the 1s orbital. Since 1s can only hold two electrons the next 2 electrons for Chromium go in the 2s orbital. The next six electrons will go in the 2p orbital. The p orbital can hold up to six electrons. We'll put six in the 2p orbital and then put the next two electrons in the 3s. Since the 3s if now full we'll move to the 3p where we'll place the next six electrons. We now shift to the 4s orbital where we place the remaining two electrons. After the 4s is full we put the remaining four electrons in the 3d orbital and end with 3d4.

Therefore the expected electron configuration for Chromium will be 1s22s22p63s23p44s23d9.

Note that when writing the electron configuration for an atom like Cr, the 3d is usually written before the 4s. Both of the configurations have the correct numbers of electrons in each orbital, it is just a matter of how the electronic configuration notation is written (here is an explanation why).

Therefore we have (still incorrect) 1s22s22p63s23p63d44s2

Correct Electron Configuration for Chromium (Cr)

Explanation:

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