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This digital mural is about chemistry, specifically about:

Its importance in daily life

States of matter

Atomic theories and models

Sub-particles

Applications of nuclear energy

Information about chemical bonds

Classification of chemical compounds

And personal conclusions

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Protons: They exist in a nucleus and have a positive nuclear charge. The atomic number or proton number is the number of protons present in an atom.

Electrons: Electrons are located in an electron cloud, which is the area surrounding the nucleus of the atom. Electrons can abbreviated as e⁻. Electrons have a negative charge that is equal in magnitude to the positive charge of the protons.

Neutrons: Along with protons, they make up almost all of the mass of the atom. The number of neutrons is called the neutron number and can be found by subtracting the proton number from the atomic mass number. The neutrons in an element determine the isotope of an atom, and often its stability.

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Why is it so important?

As said by many, like Biologist Gustavo Ramirez, "Chemistry is the science that studies the composition, properties, and interactions of matter." Chemistry can be found in every day life, because it's everywhere our eyes can see. Our phones' screen, for example, is a liquid crystal display (LCD for short), which is an invention of chemistry, and circuitry. A couple examples of chemistry in every day life are:

Medications that relieve pain

Preservation techniques for food

Insecticides and cleaning products

Creating dyes and synthetic fibers for clothing

And many others!

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Solid: In a solid, particles are packed tightly together so they don't move much. The electrons of each atom are constantly in motion, so the atoms have a small vibration, but they are fixed in their position. Because of this, particles in a solid have very low kinetic energy.

Liquid: In a liquid, the particles are more loosely packed than in a solid and are able to flow around each other, giving the liquid an indefinite shape. Therefore, the liquid will conform to the shape of its container.

Gas: In a  gas, the particles have a great deal of space between them and have high kinetic energy. A gas has no definite shape or volume. If unconfined, the particles of a gas will spread out indefinitely; if confined, the gas will expand to fill its container.

Plasma: Plasma consists of highly charged particles with extremely high kinetic energy. The noble gases (helium, neon, argon, krypton, xenon and radon) are often used to make glowing signs by using electricity to ionize them to the plasma state.

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The attributes of naturally decaying atoms, known as ‘radioisotopes’, give such atoms several applications across many aspects of modern day life.

The first practical application of a radioisotope was made by a Hungarian man named George de Hevesy in 1911. His was the first use of radioactive tracers - now routine in environmental science.

Radioisotopes, nuclear power process heat and non-stationary power reactors have essential uses across multiple sectors, including consumer products, food and agriculture, industry, medicine and scientific research, transport, and water resources and the environment. The applications of nuclear technology outside of civil electricity production in power plants are less well-known.

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Ramirez, G. (2022, October 13) Chemistry Uses, Importance & Examples. Study.com. https://study.com/academy/lesson/chemistry-uses-importance-examples.html

Bagley, M. (2023, 6 octubre). States of matter: Definition and phases of change. Live Science. https://www.livescience.com/46506-states-of-matter.html

Libretexts. (2023a, enero 30). Sub-Atomic particles. Chemistry LibreTexts. https://chem.libretexts.org/Bookshelves/Physical_and_Theoretical_Chemistry_Textbook_Maps/Supplemental_Modules_(Physical_and_Theoretical_Chemistry)/Atomic_Theory/The_Atom/Sub-Atomic_Particles

The Many Uses of Nuclear Technology - World Nuclear Association. (s. f.). https://world-nuclear.org/information-library/non-power-nuclear-applications/overview/the-many-uses-of-nuclear-technology#:~:text=Radioisotopes%2C%20nuclear%20power%20process%20heat,water%20resources%20and%20the%20environment.

Chemical bonds, types, characteristics, how occur. . . - Ferrovial. (2022, 17 noviembre). Ferrovial. https://www.ferrovial.com/en/stem/chemical-bonds/

Libretexts. (2023, 30 junio). Chemical compounds. Chemistry LibreTexts. https://chem.libretexts.org/Bookshelves/Inorganic_Chemistry/Supplemental_Modules_and_Websites_(Inorganic_Chemistry)/Chemical_Compounds/Chemical_Compounds

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Ross, & Sydney. (2025, 17 marzo). John Dalton | Biography, Discoveries, Atomic Model, & Facts. Encyclopedia Britannica. https://www.britannica.com/biography/John-Dalton/Atomic-theory

Libretexts. (2021, 16 junio). 4.12: Thomson’s Atomic Model. Chemistry LibreTexts. https://chem.libretexts.org/Courses/Modesto_Junior_College/Chemistry_143_-_Bunag/Chemistry_143_-_Introductory_Chemistry_(Bunag)/04%3A_Atomic_Structure/4.12%3A_Thomson's_Atomic_Model

The Editors of Encyclopaedia Britannica. (2025, 5 mayo). Rutherford model | Definition, Description, Image, & Facts. Encyclopedia Britannica. https://www.britannica.com/science/Rutherford-model

Atomic flashback: A century of the Bohr model. (2025, 8 mayo). CERN. https://home.cern/news/news/physics/atomic-flashback-century-bohr-model

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De Broglie’s atomic model (1924 AD) - Rincón educativo. (2024, 17 diciembre). Rincón Educativo. https://rinconeducativo.org/en/recursos-educativos/de-broglies-atomic-model-1924-ad/#:~:text=The%20de%20Broglie%20model%20of,the%20concept%20of%20electronic%20orbital.

Schrödinger’s atomic model (1926 AD) - Rincón educativo. (2024, 17 diciembre). Rincón Educativo. https://rinconeducativo.org/en/recursos-educativos/schrodingers-atomic-model-1926-ad/

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Covalent: Occurs when non-metallic atoms share electrons. In this type of bond, electrons move between atoms, producing polar covalent bonds (sharing electrons unequally) and non-polar ones (when the number of electrons is evenly distributed). Example: water (H₂O) is composed of two hydrogen atoms and one oxygen atom, and in its bond, each hydrogen atom shares an oxygen atom.

Ionic: this occurs when metallic and non-metallic atoms bond and an electron charge is given from one to the other. As a result, both negatively charged ions (anions) and positive ones (cations) are produced, and there is an attraction between their opposite charges.
Example: in sodium chloride (NaCl), which combines a chlorine atom and a sodium atom.

Metallic: These are formed between two metal atoms, whose nuclei gather and are surrounded by their electrons like a cloud. It's spread out like a network. All pure metallic elements consist of metal bonds, for example, gold (Au), iron (Fe), aluminum (Al), etc.

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De la Rosa González Patricio Arturo: In conclusion, I find all of these topics interesting and fun to read about. My favorite is probably the story of Bohr's model and how he worked under Rutherford.

Peña Hinojosa Ana Carolina: Throughout this semester we saw different topics, but my favorite was that of the atomic theories.

Carreño de León Nelly Johana: I enjoyed identifying and distinguishing between different types of compounds, which helped me to better understand chemistry and its application in real life.

Chavez Rodriguez Deyna Fernanda: This project helped me understand the importance of chemistry in everyday life and its connection with other sciences.

Gorostiza Andrade Leonardo: I loved learning about periodic table elements like ionization, electronegativity, and atomic radius.

Elizondo Salinas Fernanda: This lesson was about electronegativity because it helped me understand how atoms interact in a molecule.

Tristan García Oswaldo: In this lesson we learned that electronegativity is the ability of an atom to attract electrons in a chemical bond. It varies across the periodic table, increasing from left to right and decreasing down a group.

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Chemical compounds can generally be classified into two broad groups: molecular compounds and ionic compounds. Molecular compounds involve atoms joined by covalent bonds and can be represented by a variety of formulas. Ionic compounds are composed of ions joined by ionic bonding, and their formulas are generally written using oxidation states.

Molecular compounds are composed of atoms that are held together by covalent bonds. These bonds are formed when electrons are shared between two atoms. The concept of chemical formulas was created to describe many characteristics of molecular compounds in a simple manner.

An empirical formula represents the proportions of atoms in a molecule. It gives important information about a molecule, because it displays the ratios of atoms that are present within the molecule.

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He based his theory of partial pressures on the idea that only like atoms in a mixture of gases repel one another, whereas unlike atoms appear to react indifferently toward each other. his conceptualization explained why each gas in a mixture behaved independently. Although this view was later shown to be erroneous, it served a useful purpose in allowing him to abolish the idea, held by many previous atomists from the Greek philosopher Democritus to the 18th-century mathematician and astronomer Ruggero Giuseppe Boscovich, that atoms of all kinds of matter are alike.

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The electron was discovered by J.J. Thomson in 1897. The existence of protons was also known, as was the fact that atoms were neutral in charge. Since the intact atom had no net charge and the electron and proton had opposite charges, the next step after the discovery of subatomic particles was to figure out how these particles were arranged in the atom.

Following the discovery of the electron, J.J. Thomson developed what became known as the "plum pudding" model in 1904. Plum pudding is an English dessert similar to a blueberry muffin. In Thomson's plum pudding model of the atom, the electrons were embedded in a uniform sphere of positive charge, like blueberries stuck into a muffin.

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Rutherford model, description of the structure of atoms proposed (1911) by the New Zealand-born physicist Ernest Rutherford. The model described the atom as a tiny, dense, positively charged core called a nucleus, in which nearly all the mass is concentrated, around which the light, negative constituents, called electrons, circulate at some distance, much like planets revolving around the Sun.

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Rutherford had made the startling discovery that most of the atom is empty space. The vast majority of its mass is located in a positively charged central nucleus, which is 10,000 times smaller than the atom itself. The dense nucleus is surrounded by a swarm of tiny, negatively charged electrons.

Bohr suggested that instead of buzzing randomly around the nucleus, electrons inhabit orbits situated at a fixed distance away from the nucleus. In this picture, each orbit is associated with a particular energy, and the electron can change orbit by emitting or absorbing energy in discrete chunks (called quanta). In this way, Bohr was able to explain the spectrum of light emitted (or absorbed) by hydrogen, the simplest of all atoms.

Bohr published these ideas in 1913 and over the next decade developed the theory with others to try to explain more complex atoms. In 1922 he was rewarded with the Nobel prize in physics for his work.

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Prince Louis-Victor Pierre Raymond de Broglie, better known as Louis de Broglie, presented, in 1924, his doctoral thesis "Research on quantum theory", in which he asserted the wave-particle duality of electrons, laying the foundations of the wave mechanics.

Later, in 1927, de Broglie's statements were experimentally proven by scientists Clinton Davisson and Lester Germer.

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It is known as the "Quantum-Wave Model" and was proposed by Erwin Schrödinger, in 1926, based on the studies of De Broglie, Bohr and Sommerfeld.

His model conceives of electrons as undulations of matter, that is, it describes the wave behavior of the electron. This allowed the later formulation of a probabilistic interpretation of the wave function (magnitude used to describe the probability of finding a particle in space) by Max Born and meant that the position of an electron or its path could be studied probabilistically. momentum but not both, due to the Heisenberg Uncertainty Principle.

Schrödinger was awarded the Nobel Prize, in 1933, for his contributions to atomic theory, the development of the equation to calculate the probability that an electron is in a specific position.