The element with configuration `1s^(2) 2s^(2) 2p^(6) 3s^(2)` would be

Options

A. a metal
B. a non-metal
C. an inert gas
D. a metalloid

Answer

To determine the element with the electronic configuration `1s^(2) 2s^(2) 2p^(6) 3s^(2)`, we can follow these steps:

### Step 1: Analyze the Electronic Configuration
The given electronic configuration is `1s^(2) 2s^(2) 2p^(6) 3s^(2)`.

### Step 2: Count the Total Number of Electrons
To find the element, we need to count the total number of electrons represented in the configuration:
- `1s^(2)` contributes 2 electrons
- `2s^(2)` contributes 2 electrons
- `2p^(6)` contributes 6 electrons
- `3s^(2)` contributes 2 electrons

Adding these together:
\[ 2 + 2 + 6 + 2 = 12 \]
Thus, the total number of electrons is 12.

### Step 3: Identify the Element
The total number of electrons corresponds to the atomic number of the element. An atomic number of 12 indicates that the element is Magnesium (Mg), which is located in Group 2 of the periodic table, known as the alkaline earth metals.

### Step 4: Confirm the Group and Period
Since the outermost electron configuration ends in `3s^(2)`, it confirms that this element belongs to the s-block of the periodic table and specifically to the alkaline earth metals, which have the general electronic configuration of `ns^(2)`.

### Final Answer
The element with the configuration `1s^(2) 2s^(2) 2p^(6) 3s^(2)` is Magnesium (Mg).

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