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Chapter 3: Problem 117

Give the electron configuration of the nitrogen atom.

Short Answer

Expert verified
The electron configuration of nitrogen is 1s虏 2s虏 2p鲁.

Step by step solution

01

Identify Atomic Number

Nitrogen has an atomic number of 7, which means it has 7 electrons in its neutral state.
02

Determine Electron Configuration Pattern

Electrons are added to atomic orbitals in a specific order based on energy levels, often following the Aufbau principle. The sequence is typically: 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, and so on.
03

Fill Electrons into Orbitals

Start filling the orbitals using the pattern from Step 2: 1. First, fill the 1s orbital with 2 electrons: 1s虏. 2. Next, fill the 2s orbital with 2 electrons: 2s虏. 3. Finally, add the remaining 3 electrons to the 2p orbital: 2p鲁.
04

Write the Electron Configuration

Combine the filled orbitals into the electron configuration of nitrogen: 1s虏 2s虏 2p鲁.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Understanding the Nitrogen Atom
The nitrogen atom is a fundamental building block of life, as it is a crucial component of amino acids and nucleic acids. Found in Group 15 of the periodic table, nitrogen has an atomic number of 7. This signifies that a neutral nitrogen atom contains 7 protons in its nucleus and, correspondingly, 7 electrons surrounding it.
These electrons dictate the atom's chemical properties and reactivity. The electrons are distributed among various atomic orbitals, which represent regions around the nucleus where electrons are likely to be found. By comprehending its electron configuration, we gain a deeper insight into nitrogen's behavior in chemical reactions.
Exploring Atomic Orbitals
Atomic orbitals are regions in an atom where electrons are likely to be found. They are defined by three parameters: their size, shape, and direction. Orbitals are often grouped into shells (e.g., 1s, 2p) and are oriented in a specific order based on their energy levels.
  • s-orbitals: These are spherical in shape and can hold a maximum of 2 electrons. For example, 1s and 2s orbitals.
  • p-orbitals: These have a more complex shape and can hold up to 6 electrons. In the case of nitrogen, electrons fill the 2p orbital after filling the 1s and 2s orbitals.
The concept of orbitals helps us understand not only where electrons reside in an atom, but also how atoms bond with each other in various chemical reactions.
Applying the Aufbau Principle
The Aufbau principle is a guideline used to determine the electron configuration of an atom. It provides a methodical way of filling electrons into orbitals, based on their energies. This principle states that electrons fill atomic orbitals from the lowest energy level to the highest.
  • For nitrogen, the filling sequence is: 1s, 2s, then 2p.
  • First, 2 electrons fill the 1s orbital (1s虏).
  • Next, 2 electrons go into the 2s orbital (2s虏).
  • The remaining 3 electrons occupy the 2p orbital, reaching a stable half-filled state (2p鲁).
By following the Aufbau principle, one can predict and write the electron configurations for various elements, which is pivotal in understanding their chemical properties and reactivity.

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Most popular questions from this chapter

Which of the following atoms or ions has the largest ionization energy? (a) \(\mathrm{P}\) (b) \(\mathrm{P}^{+}\) (c) \(\mathrm{P}^{2+}\) (d) \(\mathrm{P}^{3+}\) (e) \(\mathrm{P}^{4+}\)

Predict the relative sizes of the \(\mathrm{Fe}^{2+}\) and \(\mathrm{Fe}^{3+}\) ions, which can be found in a variety of proteins, including hemoglobin, myoglobin, and the cytochromes.

Which of the following is the correct electron configuration for the \(\mathrm{P}^{3-}\) ion? (a) [Ne] (b) \([\mathrm{Ne}] 3 \mathrm{~s}^{2}\) (c) \([\mathrm{Ne}] 3 s^{2} 3 p^{3}\) (d) \([\mathrm{Ne}] 3 s^{2} 3 p^{6}\)

Which of the following isoelectronic ions is the largest? Explain. (a) \(\mathrm{Mn}^{7+}\) (b) \(\mathrm{P}^{3-}\) (c) \(\mathrm{S}^{2-}\) (d) \(\mathrm{Sc}^{3+}\) (e) \(\mathrm{Ti}^{4+}\)

Which of the following atoms or ions is the smallest? Explain. (a) \(\mathrm{Na}\) (b) \(\mathrm{Mg}\) (c) \(\mathrm{Na}^{+}\) (d) \(\mathrm{Mg}^{2+}\) (e) \(\mathrm{O}^{2-}\)
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