Zoleo IA

• Spectroscopy is the study of interaction between Radiation and matter, which quantifies and qualifies the type of Radiation absorbed, emitted, or scattered.
• Newton and Huygens formulated the theory of light, stating that matter is formed by small, light-wave particles.
• Absorption, Emission, and Scattering of high-speed particles explain the theory of light.
• By the end of the 19th century, Maxwell exposed the Reflection and Refraction Electromagnetic Theory of Light, formulating a mathematical theory to back up electromagnetic phenomena.
• The Maxwell equations explain the fundamental laws of electromagnetism, also known as Maxwell's equations.
• The term "Uph" (wave speed) helped work out the speed of light from experimentally known electric and magnetic parameters.
• The mathematical discovery demonstrated that light is electromagnetic Radiation.
• Atoms are the basic unit of matter that do not change in a Chemical Reaction of a closed system.
• The nucleus of an atom contains 1 proton and 1 neutron.
• Protons have a small negative charge, while electrons have a negative charge.
• A globally neutral atom is normally there is an equal amount of protons and electrons.
• The atomic number (Z) is the number of protons in the nucleus of an atom.
• The mass number (A) is the number of neutrons and protons in the nucleus of an atom.
• A Chemical Element is any substance formed by chemically identical atoms.
• The periodic table of elements is arranged in ascending atomic number from left to right (periods) and arranged based on similar chemical properties by column (groups).
• The chemical symbol for an element is represented by the mass number (no + pt) or atomic number (pt X).
• When an element is represented in the periodic table, the atomic number is the only top of the chemical symbol.
• An Isotope is an atom with the same atomic number (Z) but different mass number (A) because they have different quantities of neutrons.
• Protons are the identity markers of an element/atom.
• Covalent bonds are strong and make up what we call Molecules, which are a group of 2 or more atoms united by covalent or polar covalent bonds.
• All molecules have specific geometry.
• Quantum Mechanics Theory: Basics of Particle Physics, Wave-particle duality, I
• Matter is composed of particles.
• A particle has a mass (m) and a speed (velocity, v).
• When the initial momentum, position, and energy of a particle are known, the particle has a known trajectory.
• Force is the external influence causing an object's velocity to change.
• A particle can have any speed, therefore, can have any value of energy.
• Each moving particle has an energy, called energy E.
• General Rule of Quantum Mechanics: Particles in a small Region can only have specific values of energy, this is a consequence of the wave behavior of a particle.
• Energy Levels: specific energy values of a given particle.
• Spectroscopy studies how light is modified by the interaction with matter, providing information on the matter itself.
• A spectroscopic event can be an absorption, emission, or scattering.
• Absorption occurs when a molecule jumps from a low energetic level to a high energetic level, absorbing the energy difference as a photon of right frequency.
• Emission occurs when a molecule jumps from a high energetic level to a low energetic level, emitting the energy difference as a photon of right frequency.
• Absorption Spectroscopies and Emission Spectroscopies are different.
• Scattering occurs when two jumps occur to a higher level with photon absorption, followed by a jump to a different (lower) level with photon emission.
• Vibrations refer to the movements of atoms of molecules, making atoms come closer or farther (like a spring).
• Energy levels are not very close and are equally spaced (energy difference is relevant), corresponding to photons in the IR Region (IR spectroscopy; vibrational spectroscopy).
• Electronic energy levels and Molecular Motion are related, considering that chemical bonds in molecules are formed by electrons, electronic transitions relate to the change of energy of 2 electrons.
• Electronic energy levels have a large difference between them, corresponding to photons in the visible & UV Region, widely used for e- involved in bonding.