The valence shell of the element X contains 1 electron in 5s subshell and below that shell, 4 electrons in 4d subshell. The element belongs to which group (IUPAC) of periodic table?

Options

A. 4th group
B. 5th group
C. 6th group
D. 7th group

Answer

To determine the group of the element X based on the given electronic configuration, we can follow these steps:

### Step 1: Identify the Valence Shell Configuration
The valence shell of element X has the following configuration:
- 5s subshell: 1 electron (5s¹)
- 4d subshell: 4 electrons (4d⁴)

### Step 2: Write the Complete Valence Shell Configuration
The complete valence shell configuration can be written as:
- Valence shell configuration = 5s¹ 4d⁴

### Step 3: Determine the Group Number
In the periodic table, the group number can be determined by adding the number of electrons in the outermost s subshell and the d subshell.
- For element X:
- Number of electrons in 5s = 1
- Number of electrons in 4d = 4

Now, we add these:
- Total = 1 (from 5s) + 4 (from 4d) = 5

### Step 4: Identify the IUPAC Group
According to the IUPAC numbering system:
- The elements in the d-block (transition metals) are generally classified into groups based on the total number of valence electrons.
- Since we have a total of 5 valence electrons, element X belongs to Group 5.

### Conclusion
Thus, the element X belongs to Group 5 of the IUPAC periodic table.

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