Which of the following represents the electronic configuration of the electropositive element ?

Options

A. `[He]2s^(1)`
B. `[Xe]6s^(1)`
C. `[He]2s^(2)`
D. `[Xe]6s^(2)`

Explanation

To determine which of the given electronic configurations represents the most electropositive element, we will follow these steps:

### Step 1: Identify the Electronic Configurations
We need to analyze the provided electronic configurations and identify the corresponding elements. The configurations mentioned are:
1. Helium 2s1
2. Xenon 6s1
3. Helium 2s2
4. Xenon 6s2

### Step 2: Determine the Elements
Now, let's identify the elements based on the electronic configurations:
- **Helium 2s1** corresponds to Lithium (Li), which has an atomic number of 3.
- **Xenon 6s1** corresponds to Cesium (Cs), which has an atomic number of 55.
- **Helium 2s2** corresponds to Beryllium (Be), which has an atomic number of 4.
- **Xenon 6s2** corresponds to Barium (Ba), which has an atomic number of 56.

### Step 3: Understand Electropositivity
Electropositivity refers to the tendency of an element to lose electrons and form positive ions. Generally, electropositivity increases as you move down a group in the periodic table and decreases as you move from left to right across a period.

### Step 4: Compare Electropositivity of the Elements
Now, we will compare the electropositivity of the identified elements:
- **Lithium (Li)**: Group 1, relatively electropositive.
- **Cesium (Cs)**: Group 1, lower than Lithium but more electropositive due to being lower in the group.
- **Beryllium (Be)**: Group 2, less electropositive than Lithium.
- **Barium (Ba)**: Group 2, less electropositive than Cesium.

### Step 5: Conclusion
Among the elements identified, **Cesium (Cs)** is the most electropositive element because it is located further down in Group 1 of the periodic table, where electropositivity increases.

### Final Answer
The electronic configuration that represents the most electropositive element is **Xenon 6s1 (Cesium)**.

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