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!

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.

• 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

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.

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.

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.

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.

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.

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.

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.

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

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.