Chemical properties and atomic structure

• It is a particle of matter that uniquely defines a chemical element. Atom
• A substance made of only one type of atom. Element
• Is a characteristic or behavior of a substance that may be observed when it undergoes a chemical change or reaction. Chemical Property
• the center of an atom. nucleus
• positive charge. protons
• no charge. neutron
• total number of protons and neutrons. atomic mass
• In the concentric clouds that surround the nucleus, negative charge, very low mass (9.1093837 × 10⁻³¹ kilograms). electron
• the outermost shell, Determine the chemical bonding properties of an atom. Valence Electron
• 19th Century - Devised the periodic table using their knowledge of atomic masses
• 1864 - John Newlands - Every eighth element had similar properties (Law of Octaves)
• 1869: Dmitri Mendeleev & Lothar Meyer - Proposed a more extensive tabulation of the elements
• To date, 118 elements have been identified
• Henry Moseley found out that the atomic number increases in the same order as the atomic mass
• Period - horizontal rows
• Group/Family - vertical columns; elements having similar properties
• Metals: Good conductor of heat
• Metalloids: Exhibit properties intermediate between metals and non-metals
• Non-metals: Poor conductor of heat & electricity
• Electron Configuration - distribution of electrons within the energy levels or electron shells of an atom
• Block Classification: s-block, p-block, d-block, f-block
• 0.1 M nitrate solutions of: Li, Na, K, Ca, Ba, Sr
• 0.1 M solutions of NaCl, NaBr, and NaI
• Noble Gas - elements that have weak interatomic force, and consequently have very low melting and boiling points
• state of matter, where it can be solid, liquid, or gas. Physical State
• Color - a property of chemicals that mostly comes from the excitation of electrons due to an absorption of energy, this is an aspect where elements are described in terms of hue, lightness and saturation
• described as how a mineral’s surface reflect light and how its interior refract or bend light. Luster
• Acid are chemical substances that donates protons in the form of hydrogen ions, and are characterized by a sour taste in an aqueous medium. They turn blue litmus to red.
• Base are chemical substances that forms hydroxide ions when dissolved in water, and are characterized by a bitter taste and are slippery to touch. They turn red litmus to blue.
• Solubility: A measure of how much solute will dissolve in a solvent at a specific temperature
• Polarizability: Refers to the measure of the tendency of an atom/molecule to form a dipole moment when an electric field is applied across it.
• Polar Molecules: Refers to the uneven distribution of electrons between covalently bonded atoms
• Nonpolar Molecules: Refers to the even distribution of electrons between covalently bonded atoms.
• Types of intermolecular forces: Dipole - Dipole Forces, Ion - Dipole Forces, Dispersion Forces, Ion-induced Dipole, Dipole-induced Dipole, Hydrogen Bonding
• Dipole - Dipole Force: The attraction between two polar molecules or between one polar molecule and another charged species (ion).
• Ion - Dipole Force: The interaction between oppositely charged particles.
• Dispersion Force: Also known as London dispersion force, refers to the weak attractive interactions between all types of molecules due to temporary fluctuations in electron density around nuclei.
• Dispersion Force: Also known as London dispersion force, refers to the weak attractive interactions that exist between all substances due to fluctuations in electron density around nuclei.
• Ion-Induced Dipole Force: Occurs when there are ionic compounds present in solution with nonpolar molecules.
• Ion-Induced Dipole Force: A type of electrostatic interaction whereby a permanent dipole induces a temporary dipole on a nearby neutral particle.