Indicates the orientation of an orbital around the nucleus. Tells us the shapes of the electron orbitals Magnetic quantum number -Symbolized by m. Describes the sub shells within a given principal energy level (s,p,d,f). Azimuthal (angular) Quantum Number -Second quantum number, designated l. Pauli Exclusion Principle -No two electrons in the same atom can have the same set of four quantum numbers. Heisenberg uncertainty principle -it is impossible to know exactly both the velocity and the position of a particle at the same time. Orbitals -Regions around the nucleus in which given electron or electron pair is likely to be found. Electrons do not travel in defined orbits but rather are localized in orbitals. The modern description of the behavior of electrons in atoms. A set of frequencies of electromagnetic waves given off by atoms of an element consists of a series of fine lines of individual colors. Atomic emission spectrum -The pattern formed when light passes through a prism or diffraction grating to separate it into the different frequencies of light it contains. For an electron to jump from a lower energy to a higher one, it must absorb an amount of energy equal to the energy difference between the 2 levels. Atomic absorption spectrum -The unique spectrum of light absorbed when an atom's electrons are excited to higher energy levels. Quantum - The energy difference between energy levels. Stated that energy is emitted as electromagnetic radiation from matter comes in bundles called quanta. Max Planck -Developed quantum theory of matter and energy. Bohr model of the atom -A dense, positively charged nucleus is surrounded by electrons revolving around the nucleus in orbits with distinct energy levels.
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