For each element, indicate the number of valence electrons, core electrons, and unpaired electrons in the ground state: a. nitrogen

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Identify the atomic number of nitrogen, which is 7, indicating it has 7 electrons.

Determine the electron configuration of nitrogen in its ground state: 1s^2 2s^2 2p^3.

Count the valence electrons, which are the electrons in the outermost shell (n=2): 2s^2 2p^3, totaling 5 valence electrons.

Calculate the core electrons, which are the electrons not in the outermost shell: 1s^2, totaling 2 core electrons.

Identify the unpaired electrons in the 2p orbital: 2p^3 has three electrons, with one electron in each of the three p orbitals, resulting in 3 unpaired electrons.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Valence Electrons

Valence electrons are the outermost electrons of an atom and are crucial for determining how an element will react chemically. For nitrogen, which has an atomic number of 7, there are 5 valence electrons located in the second energy level. These electrons are involved in bonding and chemical reactions.

Core Electrons

Core electrons are the electrons that are not involved in bonding and are found in the inner shells of an atom. In nitrogen, there are 2 core electrons in the first energy level. Understanding the distinction between core and valence electrons is essential for predicting an element's chemical behavior.

Unpaired Electrons

Unpaired electrons are those that occupy an orbital alone rather than in pairs. In nitrogen's ground state electron configuration (1s² 2s² 2p³), there are 3 unpaired electrons in the 2p orbitals. The presence of unpaired electrons is significant as it influences the atom's magnetic properties and its ability to form bonds.