If an atom has electronic configuration $1s^2 2s^2 2p^6 3s^2 3p^6 3d^3 4s^2$, we will place it in group number

Question

If an atom has electronic configuration $1s^2 2s^2 2p^6 3s^2 3p^6 3d^3 4s^2$, we will place it in group number:

Accepted Answer

1.  **Identify the Block:** The electronic configuration ends with electrons filling the $3d$ orbital ($3d^3$) after the $4s$ orbital ($4s^2$). This indicates the element belongs to the **d-block** (Transition Elements).
2.  **Determine the Group Number:** For d-block elements, the group number is calculated as the sum of electrons in the $(n-1)d$ subshell and the $ns$ subshell.
    *   Group Number = (Number of electrons in $3d$) + (Number of electrons in $4s$)
    *   Group Number = $3 + 2 = 5$
3.  **Identify the Element (Optional):** The total number of electrons is $2+2+6+2+6+3+2 = 23$. The element with atomic number 23 is **Vanadium (V)**, which lies in Group 5.

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