Nitrogen's electronegativity value is between those of phosphorus and oxygen.

Which of the following correctly describes the relationship between the three values?

A. The value for nitrogen is less than that of phosphorus because nitrogen is larger, but greater than that of oxygen because nitrogen has a greater effective nuclear charge.

B. The value for nitrogen is less than that of phosphorus because nitrogen has fewer protons but greater than that of oxygen because nitrogen has less valence electrons.

C. The value for nitrogen is greater than that of phosphorus because nitrogen has fewer electrons, but less than that of oxygen because nitrogen is smaller.

D. The value for nitrogen is greater than that of phosphorus because nitrogen is smaller, but less than that of oxygen because nitrogen has a smaller effective nuclear charge.

The correct relationship between the three values will be the value for nitrogen is greater than that of P because N is smaller, but less than that of O because N has a smaller effective nuclear charge.

Electronegativity is the chemical property which describes the tendency of an atom or a functional group which attract electrons toward itself. The electronegativity of an atom will be affected by both its atomic number as well as the distance that its valence electrons reside from the charged nuclei.

The electronegativity of phosphorus will be 2.19 is much less electronegativity than to the nitrogen. The electronegativity of nitrogen will be 3.04. 4. Phosphorus will expand its valence shell to hold more than eight electrons, but nitrogen cannot.

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