* Your assessment is very important for improving the workof artificial intelligence, which forms the content of this project
Download Atomic Structure 1. Historical perspective of the model of the atom a
Photoredox catalysis wikipedia , lookup
Livermorium wikipedia , lookup
Marcus theory wikipedia , lookup
Periodic table wikipedia , lookup
Molecular Hamiltonian wikipedia , lookup
Electrical resistivity and conductivity wikipedia , lookup
Condensed matter physics wikipedia , lookup
Elementary particle wikipedia , lookup
Photoelectric effect wikipedia , lookup
X-ray fluorescence wikipedia , lookup
Low-energy electron diffraction wikipedia , lookup
Metastable inner-shell molecular state wikipedia , lookup
History of chemistry wikipedia , lookup
Hypervalent molecule wikipedia , lookup
Electronegativity wikipedia , lookup
Chemistry: A Volatile History wikipedia , lookup
Resonance (chemistry) wikipedia , lookup
Nuclear binding energy wikipedia , lookup
Oxidative phosphorylation wikipedia , lookup
IUPAC nomenclature of inorganic chemistry 2005 wikipedia , lookup
Auger electron spectroscopy wikipedia , lookup
Light-dependent reactions wikipedia , lookup
Molecular orbital diagram wikipedia , lookup
X-ray photoelectron spectroscopy wikipedia , lookup
Metallic bonding wikipedia , lookup
Chemical bond wikipedia , lookup
Hydrogen atom wikipedia , lookup
Photosynthetic reaction centre wikipedia , lookup
Rutherford backscattering spectrometry wikipedia , lookup
History of molecular theory wikipedia , lookup
Atomic orbital wikipedia , lookup
Electron configuration wikipedia , lookup
Atomic Structure 1. Historical perspective of the model of the atom a.) In 1803, John Dalton proposed the atomic theory which stated that all matter is made of atoms, atoms of the same type of element have the same chemical properties, compounds are formed by two or more different types of atoms, and that a chemical reaction involves either, joining, separating, or rearranging atoms. b.) In 1910, Ernest Rutherford passed alpha particles through gold foil which showed that atoms are mostly empty space, and that the positive charge within an atom is centrally located. c.) In 1913, Neils Bohr used classic physics to develop a model of an atom where electrons orbit a central nucleus in concentric circles. d.) The electron cloud model shows the probability of an electron to be in a specific location in an atom. Orbital- are the region where one is most likely to find an electron. 2. Current atomic model a.) Atoms are made of protons, neutrons and electrons. i.) protons have a positive charge, are located in the nucleus, and have a mass of 1 amu. ii.) neutrons have no charge, are also located in the nucleus, and have a mass of 1amu. iii.) electrons have a negative charge, are located outside of the nucleus, and have a mass of 5.486 x 10-4 amu or 1/1837 amu. b.) Atomic number is the number of protons in an atom. The atomic number also represents the nuclear charge of an atom. Mass number is the number of protons plus the number of neutrons. c.) An isotope is an atom with the same number of protons, but different number of neutrons. Examples: Carbon-12 12 6 C Carbon-14 14 6 C d.) Average atomic mass is the weighted average mass of all naturally occurring isotopes of an element. e) An Atomic Mass Unit is defined as 1/12 the mass of a Carbon-12 atom. 3. Electron Configuration a.) electrons fill energy levels in order of lowest energy o highest energy. b.) the first energy level two electrons, the second holds eight, the third holds eighteen, and the fourth holds thirty-two. (Max # electrons = 2n2) or 2-8-18-32 c.) no ground state atom has more than thirty-two electrons in any one energy level. 4. The wave mechanical model of the atom is used to show orbitals defined as regions of probable electron location. 5. Each electron has a distinct amount of energy a.) Electrons can gain energy and jump to an excited state. RESULT: absorption spectra b.) When electrons jump back down to the ground state they emit a specific amount of energy, which can be used to identify the atom. RESULT: bright-line emission spectra 6. The valence electrons affect the chemical properties of an atom.