To which group, an element with atomic number 88 will belong?

Options

A. Group 12
B. Group 17
C. Group 10
D. Group 2

Explanation

To determine the group to which an element with atomic number 88 belongs, we can follow these steps:

### Step 1: Identify the Element
The element with atomic number 88 is radium (Ra).

### Step 2: Write the Electronic Configuration
To find the group number, we first need to write the electronic configuration of radium. The nearest noble gas preceding radium is radon (Rn), which has an atomic number of 86.

- The electronic configuration of radon (Rn) is:
\[ \text{[Xe]} 4f^{14} 5d^{10} 6s^{2} \]
- To find the electronic configuration of radium (Ra), we add two more electrons to the 7s subshell:
\[ \text{[Rn]} 7s^{2} \]

### Step 3: Determine the Block
The last electron of radium is in the s subshell (7s²). This indicates that radium belongs to the s-block of the periodic table.

### Step 4: Identify the Period
The principal quantum number (n) for the last electron (7s²) is 7, which indicates that radium is in the 7th period of the periodic table.

### Step 5: Determine the Group Number
In the s-block, the group number is determined by the number of electrons in the outermost shell. Since radium has 2 electrons in the 7s subshell, it belongs to Group 2.

### Conclusion
Therefore, the element with atomic number 88 (radium) belongs to Group 2 of the periodic table.

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