From the list of the elements Na, Mg, Al, Si, predict
The element which belongs to group 2

Answer

To determine which element from the list (Na, Mg, Al, Si) belongs to group 2, we can follow these steps:

### Step 1: Identify the Atomic Numbers
First, we need to know the atomic numbers of the elements:
- Sodium (Na) has an atomic number of 11.
- Magnesium (Mg) has an atomic number of 12.
- Aluminium (Al) has an atomic number of 13.
- Silicon (Si) has an atomic number of 14.

### Step 2: Write the Electronic Configurations
Next, we will write the electronic configurations for each element:
- Sodium (Na): 2, 8, 1
- Magnesium (Mg): 2, 8, 2
- Aluminium (Al): 2, 8, 3
- Silicon (Si): 2, 8, 4

### Step 3: Determine the Number of Electrons in the Outermost Shell
Now, we will look at the number of electrons in the outermost shell for each element:
- Sodium (Na) has 1 electron in its outermost shell.
- Magnesium (Mg) has 2 electrons in its outermost shell.
- Aluminium (Al) has 3 electrons in its outermost shell.
- Silicon (Si) has 4 electrons in its outermost shell.

### Step 4: Identify the Group Based on the Outermost Electrons
Elements are classified into groups based on the number of electrons in their outermost shell:
- Elements with 1 electron in the outermost shell belong to Group 1 (e.g., Na).
- Elements with 2 electrons in the outermost shell belong to Group 2 (e.g., Mg).
- Elements with 3 electrons in the outermost shell belong to Group 13 (e.g., Al).
- Elements with 4 electrons in the outermost shell belong to Group 14 (e.g., Si).

### Conclusion
From the analysis, we can conclude that **Magnesium (Mg)** is the element that belongs to Group 2.

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