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Chapter 11 Exam 5

Wavelengh The distance between two consecutive wave peaks. Longer W-Lower frequency
Frequency # peaks each second m/s
Radiant energy spectrum
Continuous Spectrum
Visible Spectrum Range of wavelengths 400-700 nm
Quantum Concept Energy is present in small discrete bundles (packets)Ex. photons, electron energy levels
Emission Line Spectrum
Atomic fingerprint Line spectrum to identify elements
Energy Sublevels s, p, d, f Same # as the number of the main level
Orbital Place of space where there is a high probability of finding an atom.
Electron Configuration Says the location of electrons by sublevel 1s1 means one e- in the 1s orbital
S block Filling s sublevels Groups IA/1 & IIA/2
D block Filling d sublevels Groups IIIB/3 - IIB/2
Valence electrons E- in the outermost principal energy level of an atom (highest energy)\ Involved in chemical reactions
Atomic radius Size of atoms Big: down & left
Metallic Character Degree of metal character of an element Increases: down & left
Ionization Energy Amount of energy required to remove an electron from an individual atom in the gaseous state Increases: up & Right (Opposite)
Photons Particles of light
Electromagnetic Radiation Energy that is transmitted from one place to antoher by light
Wave mechanical model Electrons move in waves and streams of particles, just like light does
Principal energy levels Discrete energy levels of an atom
Sublevels/ Orbital Subdivision of the principal energy levels 1 has 1, 2 has 2, 3 has 3, 4 has 4 (like triangle upside down)
Pauli Exclusion Principle an atomic orbital can hold a max of 2 e-, and those e- must have opposite spins
Core electrons Inner e- that don't bond atoms
Representative Elements (Main Group) Groups 1,2, 3,4,5,6,7,and 8
Created by: lesliemelissa19