Relative Electronegativity Quick Check

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Question
Use the periodic table to answer the question.

An illustration shows the periodic table of elements. The elements in the periodic table are arranged in groups (columns numbered 1 through 18) and periods (rows numbered 1 through 7) such that the atomic number increases along a period from left to right. The elements are divided into the following categories: · Alkali metals · Alkaline earth metals · Transition metals · Post-transition metals · Lanthanides · Actinides · Metalloids · Nonmetals · Noble gases · Unknown The elements are also classified on the basis of their physical states as follows: · Solid · Liquid · Gas · Unknown The element sulfur is enlarged with the following properties. · Chemical symbol: S · Name: Sulfur · Atomic Number: 16 · Atomic mass: 32.06 · Common oxidation states: 6, 4, 2, negative 2 · Electronegativity: 2.58 · Ionization energies: 999.589 · Electron configuration: [Ne] 3s2 3p4

How would the electron configuration of nitrogen change to make a stable configuration?

(1 point)
Responses

It would gain two electrons.
It would gain two electrons.

It would gain three electrons.
It would gain three electrons.

It would lose four electrons.
It would lose four electrons.

It would lose five electrons.
It would lose five electrons.
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Answer 1

To determine how the electron configuration of nitrogen (N) would change to achieve a stable configuration, we must first examine nitrogen's current electron configuration and how it achieves stability.

Nitrogen has the atomic number 7, and its electron configuration is: \[ \text{N: [He] 2s}^2 \text{2p}^3 \]

Nitrogen has five valence electrons (2 in the 2s subshell and 3 in the 2p subshell). To achieve a stable configuration (which typically means reaching a full outer shell, like the noble gas configuration), nitrogen would ideally want to gain three additional electrons to fill its p subshell.

Thus, the response would be:

• It would gain three electrons.