Electronic distribution is a fundamental concept in chemistry and physics, and mastering it requires a solid understanding of the underlying principles. In order to test your knowledge and strengthen your skills, we have prepared a series of 12 electronic distribution exercises. In this article, we will explore each of these exercises in detail, focusing on their practical application and providing clear and concise explanations for their resolution. Get ready to challenge your understanding of this key topic and improve your electronic distribution skills!

1. Introduction to electronic distribution in quantum theory

The electron distribution in quantum theory is a fundamental concept for understanding how electrons are organized around the nucleus in an atom. In this section, we will explore the basic principles of this topic and learn how to apply them in different cases.

The first step in understanding electron distribution is to understand the Pauli exclusion principle, which states that no two electrons in the same atom can have exactly the same set of quantum numbers. This means that electrons must occupy different energy levels and sublevels in an atom.

Second, it is important to become familiar with Aufbau's rule, which states the sequence in which orbitals are filled in an atom. This rule helps us determine the order in which electrons are distributed in the different energy levels and sublevels. For example, we know that level 1 fills before level 2, and so on.

2. Basic concepts of electronic distribution in chemistry

Electronic distribution in chemistry is a fundamental tool for understanding the structure and behavior of atoms and molecules. This distribution establishes how the electrons are organized around the atomic nucleus, following certain rules and principles. In this section, we will explore some basic concepts about electronic distribution in chemistry.

One of the fundamental concepts in electronic distribution is the Aufbau principle, which states that electrons are added to lower energy orbitals first before filling higher energy orbitals. This means that the electrons are filled in order of increasing energy, following the orbital diagram and respecting Hund's rule, which states that electrons fill the orbitals individually and in parallel before pairing.

To represent the electronic distribution of an atom, the electronic configuration is used, which shows how the electrons are distributed in the different energy levels and sublevels. For example, the electronic configuration of the oxygen atom is 1s² 2s² 2p⁴, which indicates that it has 2 electrons in the 1s level, 2 electrons in the 2s level, and 4 electrons in the 2p level.

3. What are electronic distribution exercises and why are they important?

Electronic distribution exercises are a fundamental tool in chemistry to understand how electrons are organized in an atom. These exercises allow us to identify the electronic configuration of each element and understand how the orbitals are filled with electrons.

The electronic distribution is important because it allows us to predict the chemical and physical properties of elements. By knowing the electronic configuration of an element, we can determine its reactivity, its ability to form chemical bonds and its behavior in different environments.

There are different methods to solve these exercises, but they all follow a series of common steps. First, you must know the rules for filling orbitals, such as Aufbau's rule, the Pauli exclusion principle, and Hund's rule. The electronic configuration is then organized on a diagram or using number and letter notation. Finally, it is checked that the distribution complies with the filling rules and that the total number of electrons is correct.

4. Challenge your knowledge: 12 electronic distribution exercises to test your skills

In this section, we present 12 challenging electronic distribution exercises that will test your chemistry skills. Each of these exercises will challenge you to apply your knowledge about the distribution of electrons in the different levels and sublevels of an atom. Not only will they help you review the basics, but they will also give you practice solving electronic distribution problems. effectively.

For each of the exercises, we will provide you with a Step by Step detailed how to solve the problem. In addition, we will give you tips and examples to facilitate your understanding. If you need a quick review of the basics of electronic distribution, you can use our interactive tutorials, which will give you a complete overview of the topic.

In addition, we recommend using tools such as periodic tables and Lewis diagrams to visualize the electronic distribution more clearly. These tools will help you accurately identify the number of electrons in each level and sublevel. Remember that the key to solving these exercises is to carefully analyze the electronic configuration of each atom and follow the principles established by the Aufbau principle, Hund's rule and the rule of maximum spin multiplicity.

5. Exercise 1: Electronic distribution of the hydrogen atom

6. Exercise 2: Electronic distribution of the carbon atom

The carbon atom is one of the most important elements in organic chemistry. Its electronic distribution determines the way carbon atoms combine with other elements. To determine the electronic distribution of the carbon atom, some must be followed key steps.

First of all, it is important to remember that the carbon atom has 6 electrons. These electrons are distributed in different energy levels called shells. The first energy level, or shell 1, can contain up to 2 electrons. The second energy level, or shell 2, can contain up to 8 electrons. To determine the electronic distribution of the carbon atom, these shells must be filled in order of increasing energy.

The carbon atom has the following electronic distribution: 1s² 2s² 2p². This means that the first 2 electrons are found in shell 1, in the 1s orbital. The next 2 electrons are found in shell 2, in the 2s orbital. The last 2 electrons are found in shell 2, in the 2p orbital. This electronic distribution tells us how the electrons are arranged in the different orbitals of the carbon atom.

7. Exercise 3: Electronic distribution of the chlorine ion

To determine the electronic distribution of the chlorine ion, we must first remember that the chlorine ion, Cl-, has gained an electron, which means that It now has an excess of a negative charge. This affects the way electrons are distributed across the atom's energy levels. Below is a step by step how to solve this problem:

1. Identify the atomic number of chlorine on the periodic table. Chlorine's atomic number is 17, meaning it has 17 electrons in its original neutral state.

2. After gaining one electron, chlorine now has 18 electrons total. To determine the electron distribution, keep in mind that electrons fill energy levels in a specific order: 2, 8, 8, 1. This means that the first 2 electrons fill energy level 1, the next 8 fill energy level 2. of energy 8, the next 3 fill energy level 4 and the last electron occupies energy level XNUMX. Note that higher energy levels are further from the nucleus and have a greater capacity to hold electrons.

3. Therefore, the electronic distribution of the chlorine ion would be the following: 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p⁶. This result tells us that chlorine has a total of 18 electrons distributed in different energy levels. In addition, by becoming an ion with a charge of -1, it acquires greater stability due to the complete filling of its outermost energy level.

8. Exercise 4: Electronic distribution of the oxygen atom

The oxygen atom has an atomic number of 8, which indicates that it has 8 electrons in its electronic configuration. To determine the electronic distribution of the oxygen atom, we must follow a step-by-step process. First of all, we must remember that electrons are distributed in different energy levels, known as shells. The first shell closest to the nucleus can contain up to 2 electrons, the second up to 8 electrons, and the third up to 8 electrons.

For the oxygen atom, we start by filling the shell closest to the nucleus, which is the first shell. We place 2 electrons in this shell. Then, we move to the next shell and place the remaining 6 electrons. This gives us an electron distribution of 2 in the first layer and 6 in the second layer. One way to represent this is to write the electronic configuration of oxygen as 1s² 2s² 2p⁴.

The electronic distribution of the oxygen atom can be visualized as a configuration in which the electrons fill the different shells and subshells according to Aufbau's rule. It is important to mention that this electronic distribution helps us understand how the negative charge of electrons is organized within the oxygen atom and how they interact with other atoms in chemical bonds. Having this information is essential to understand the chemical mechanisms and properties of oxygen in different chemical reactions.

9. Exercise 5: Electronic distribution of the iron ion (Fe2+)

In this exercise, we will learn to determine the electronic distribution of the iron ion (Fe2+). Iron is a transition element and its electronic configuration can be determined using the aufbau rule and the Pauli exclusion principle.

To start, we must remember that iron has an atomic number of 26, which means it has 26 electrons. By losing two electrons to form the Fe2+ ion, its electronic distribution will change.

The first step is to write the electronic configuration of the neutral iron atom. This is done using the energy level diagram or Aufbau's rule. The electronic configuration of neutral Fe is 1s2 2s2 2p6 3s2 3p6 4s2 3d6. Now, we must take into account that the iron(II) ion has lost two electrons, so we must eliminate the outermost electrons, following the Pauli exclusion principle. The resulting electronic distribution will be 1s2 2s2 2p6 3s2 3p6 3d6. This electronic distribution is the electronic distribution of the iron(II) ion..

10. Exercise 6: Electronic distribution of the calcium ion (Ca2+)

In this exercise, the electronic distribution of the calcium ion (Ca2+) will be analyzed. To solve this problem, it is necessary to understand the electronic configuration of calcium and how it is converted into a positive ion.

Calcium has an atomic number of 20, meaning it has 20 electrons in its neutral state. The electronic configuration of calcium in its ground state is 1s2 2s2 2p6 3s2 3p6 4s2. However, when calcium loses two electrons to form the Ca2+ ion, its electronic distribution changes.

When we lose the two electrons from the 4s shell, the electronic distribution of the calcium ion becomes 1s2 2s2 2p6 3s2 3p6. This means that the calcium ion has an electronic structure similar to that of the noble gas argon. By understanding this electronic distribution, we can understand the behavior and properties of the calcium ion in chemical reactions and in its interaction with other chemical species.

11. Exercise 7: Electronic distribution of the nitrogen atom

To solve the electron distribution exercise for the nitrogen atom, we must follow some key steps. First, it is important to remember that the nitrogen atom has an atomic number of 7, meaning it has 7 electrons.

The next step is to determine the order in which the orbitals are filled. To do this, we use the aufbau principle, which states that orbitals are filled in ascending order of energy. Then, the electrons are distributed in the orbitals following the aufbau principle until the electrons are exhausted.

In the case of nitrogen, we start by filling the 1s orbital, which can hold a maximum of 2 electrons. Next, we fill the 2s orbital with 2 more electrons. Next, we fill the three p orbitals (2px, 2py and 2pz) with the remaining 3 electrons. Finally, we check that we have used the 7 available electrons and have filled all the orbitals from lowest to highest energy.

12. Exercise 8: Electronic distribution of the sulfur atom

Sulfur is a chemical element with atomic number 16 and symbol S. To determine the electronic distribution of the sulfur atom, it is necessary to know the structure of the atom and the electronic configuration. The electronic configuration of sulfur is obtained by following the rule of the Aufbau diagram, which states that the electrons of an atom are filled in increasing order of energy.

The first step to determine the electronic distribution of the sulfur atom is to know its atomic number, which in this case is 16. From there, the electrons must be assigned to different energy levels: level 1 can contain up to 2 electrons , level 2 up to 8 electrons and level 3 up to 6 electrons. Following this rule, electrons are assigned from highest to lowest energy until the atomic number is reached.

In the case of sulfur, the electronic distribution can be represented as follows: 1s²2s²2p⁶3s²3p⁴. This indicates that level 1 contains 2 electrons, level 2 contains 8 electrons, level 3 contains 2 electrons in the s sublevel and 4 electrons in the p sublevel. It is important to note that the number of electrons in each level must be equal to the atomic number of the element.

13. Exercise 9: Electronic distribution of the magnesium ion (Mg2+)

Once the magnesium ion (Mg2+) has been formed, it is important to know its electronic distribution to better understand His properties chemicals. The electronic distribution describes how electrons are distributed in the different shells and subshells of an atom or ion. In the case of the magnesium ion, we can determine its electronic distribution using the principle of constructing or obtaining the electronic configuration.

The magnesium ion (Mg2+) has a positive charge of 2+, meaning it has lost two electrons compared to the neutral magnesium atom. This implies that it now has 10 electrons instead of the original 12. To determine the electronic distribution of Mg2+, we must assign these 10 electrons to the different shells and subshells according to the construction principle.

We start by assigning the electrons to the innermost shell, which is the first (n = 1). Since electrons fill in ascending order of energy, the first electron is assigned to the 1s sublevel. Then, the next eight electrons are assigned to the second shell (n = 2), to the 2s and 2p sublevels. However, since the magnesium ion has lost two electrons, we only have two electrons left to allocate. These are placed in the 2s sublevel, leaving the 2p sublevel empty. Therefore, the electronic distribution of the magnesium ion (Mg2+) is 1s2 2s2.

14. Exercise 10: Electronic distribution of the lithium atom

The lithium atom has a specific electronic configuration that determines how its electrons are distributed in the different energy levels and sublevels. To determine this electronic distribution, we can use Aufbau's rule and Hund's rules and the maximum multiplicity of equal energy rules.

The electronic configuration of the lithium atom can be determined by following the following steps:

1. Determine the atomic number of lithium, which is 3. This tells us that the lithium atom has three electrons.
2. Locate the electrons in the different energy levels and sublevels. The first energy level, known as the K level, can contain a maximum of 2 electrons, while the second energy level, known as the L level, can contain a maximum of 8 electrons.

3. Place the electrons in the K level first. Lithium has a single electron in the K level.

4. Place the remaining electrons in the L level. Lithium has two electrons in the L level.
5. The electronic distribution of the lithium atom is 1s² 2s¹. This indicates that lithium has one electron in the K level and two electrons in the L level.

It is important to note that the electronic distribution of the lithium atom follows the rules of quantum mechanics, which tell us how the different energy levels and sublevels are filled. The electronic configuration of lithium provides us with information about the distribution of its electrons and its stability in its ground state.

In summary, the electronic distribution exercises presented are a fundamental tool to test and strengthen your knowledge in this crucial field of chemistry. Through them, you have had the opportunity to become familiar with the rules that govern the distribution of electrons in the different levels and sublevels of atoms.

By solving these exercises, you have been able to test your ability to apply the fundamental principles of electronic distribution, such as Aufbau's rule, Pauli's exclusion principle, and Hund's rule. Additionally, you have learned to use the periodic table to determine the number of electrons in each level and sublevel.

It is important to highlight that the electronic distribution is crucial to understanding the properties and behavior of chemical elements. By mastering the concepts and skills associated with these exercises, you will be prepared to advance your understanding of atomic structure and chemistry in general.

Remember that constant practice and solving exercises are key to strengthening your knowledge. We recommend that you continue exploring similar exercises and delve into other aspects related to electronic distribution. This will allow you to improve your skills and develop a solid foundation in a field so important like chemistry.

In conclusion, solving these electronic distribution exercises has given you the opportunity to test your knowledge and skills in this vital field of chemistry. By continuing to practice and explore this topic, you will be on your way to becoming an expert in electronic distribution and strengthening your foundation in chemistry in general.

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