Question

1. explain why the element carbon (c) has a weaker pull on a bonded electron (lower electronegativity) than the element nitrogen (n), even though both are in row 2 of the periodic table.

your answer

1. based on the trend that are discussed in classroom, which is the most electronegative atom in the periodic table and why?

your answer

Explanation:

Question 19

Electronegativity depends on nuclear charge and atomic radius. Carbon (C) and Nitrogen (N) are in the same period (Row 2), so they have the same number of electron shells (atomic radius trend: C > N as we move right in a period). Nitrogen has a greater nuclear charge (atomic number: C = 6, N = 7) than Carbon. The pull on bonded electrons is due to nuclear charge attracting electrons; with similar atomic radii (same period), higher nuclear charge (N) means a stronger pull. Thus, C has a weaker pull (lower electronegativity) than N.

Electronegativity trends: increases across a period (left to right) and decreases down a group (top to bottom). Fluorine (F) is in the top - right of the periodic table (Period 2, Group 17). It has the highest nuclear charge for its period, the smallest atomic radius in its period, and is at the top of its group. These factors (high nuclear charge, small atomic radius) maximize the attractive force on bonded electrons. So, Fluorine is the most electronegative atom.

Answer:

Carbon has a weaker pull on bonded electrons (lower electronegativity) than Nitrogen because, in the same period (Row 2), Nitrogen has a greater nuclear charge (higher atomic number, 7 vs. Carbon’s 6) and a slightly smaller atomic radius (due to increased nuclear charge pulling electrons closer) than Carbon. The greater nuclear charge in Nitrogen exerts a stronger attractive force on bonded electrons, while Carbon’s lower nuclear charge and larger atomic radius (compared to N in the same period) result in a weaker pull on bonded electrons.

Question 20