The element with electronic configuration `1s^(2)2s^(2)2p^(6)3s^(2)` is

Options

A. member of alkali family
B. a noble gas
C. an alkaline earth metal
D. unpredictable.

Explanation

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

### Step 1: Count the Total Number of Electrons
The electronic configuration is given as `1s^(2)2s^(2)2p^(6)3s^(2)`. We need to count the number of electrons represented in this configuration.

- `1s^(2)` has 2 electrons
- `2s^(2)` has 2 electrons
- `2p^(6)` has 6 electrons
- `3s^(2)` has 2 electrons

Adding these together:
\[ 2 + 2 + 6 + 2 = 12 \]

### Step 2: Identify the Atomic Number
The total number of electrons in a neutral atom is equal to the atomic number. Therefore, the atomic number of the element is 12.

### Step 3: Determine the Element
Now, we need to identify the element with atomic number 12. Referring to the periodic table, the element with atomic number 12 is Magnesium (Mg).

### Step 4: Classify the Element
Since the last electron enters the `3s` subshell, we can classify Magnesium as an s-block element. More specifically, it is an alkaline earth metal because it is in Group 2 of the periodic table.

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

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