The electronnegativity of the following elements increases in the order

Options

A. `C,N,Si,P`
B. `N,Si,C,P`
C. `Si, P,C,N`
D. `P,Si,N,C`

Explanation

To determine the order of increasing electronegativity for the elements carbon (C), nitrogen (N), silicon (Si), and phosphorus (P), we can follow these steps:

### Step 1: Understand Electronegativity Trends
Electronegativity is the tendency of an atom to attract electrons in a chemical bond. The trends in electronegativity can be summarized as follows:
- **Across a Period**: Electronegativity increases from left to right across a period due to increasing nuclear charge and decreasing atomic radius.
- **Down a Group**: Electronegativity decreases down a group as atomic size increases, which makes the attraction of the nucleus for bonding electrons weaker.

### Step 2: Identify the Group and Period of Each Element
- **Carbon (C)**: Group 14, Period 2
- **Nitrogen (N)**: Group 15, Period 2
- **Silicon (Si)**: Group 14, Period 3
- **Phosphorus (P)**: Group 15, Period 3

### Step 3: Compare Electronegativity Values
Using known electronegativity values (Pauling scale):
- Nitrogen (N): 3.04
- Carbon (C): 2.55
- Phosphorus (P): 2.19
- Silicon (Si): 1.90

### Step 4: Arrange the Elements in Order of Increasing Electronegativity
Based on the values:
1. Silicon (Si) - 1.90
2. Phosphorus (P) - 2.19
3. Carbon (C) - 2.55
4. Nitrogen (N) - 3.04

Thus, the order of increasing electronegativity is:
**Si < P < C < N**

### Step 5: Identify the Correct Option
From the options provided, we can see that the correct answer corresponds to the order we derived: **Option C**.

### Final Answer
The electronegativity of the elements increases in the order: **Si < P < C < N**.

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