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Chapter 11 Exam 5
Question | Answer |
---|---|
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 |