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Chemistry Unit 7
Unit 7: Electron Structure
| Term | Definition |
|---|---|
| Dual Nature | Displays behavior characteristics of both matter (as a particle) & energy (as a wave) [includes light and electrons] |
| Electromagnetic Radiation | Form of energy that exhibits wavelike behavior as it travels through space |
| Wavelength | Distance between 2 successive points on a wave |
| Frequency | Number of waves that pass through a certain point in a given amount of time |
| Speed | How fast the wave travels |
| Photon | A "particle" of electromagnetic energy that can be absorbed or emitted |
| Photon - Absorbed | Moves from a lower energy state to a higher energy state |
| Photon - Emitted | Moves from a higher energy state to a lower energy state |
| Ground State | State of lowest energy (most stable) |
| Excited State | State which has higher potential energy than the ground state. Electrons can be "excited" using many forms of energy, including heat energy and chemical energy. |
| Atomic Emission Spectrum | The unique set of frequencies of waves emitted by atoms of an element |
| Quantized | Energy of electrons is quantized, only certain energy quantities are allowed. |
| 1st Quantum Number | Also known as "Principle Quantum Number", analogous to rings of a Bohr model diagram, #'s range from 1 through infinity, the larger the number, the greater the distance from the nucleus and the greater the energy of the electron |
| 2nd Quantum Number | Specifies number of sublevels within each principle energy level AND the type of orbitals within the sublevel |
| 3rd Quantum Number | Specifies orientation of orbital in 3-dimensional space. 's' sublevels - one orientation, 'p' sublevels - three orientations, 'd' sublevels - five orientations, 'f' sublevels - seven orienations |
| 4th Quantum Number | Specifies the spin of the electron. Electrons can spin clockwise (↑) or counter-clockwise (↓) |
| Pauli Exclusion Principle | No two electrons in an atom can have the same set of quantum numbers (electron configuration) |
| Noble Gas Abbreviation | Abbreviate with first noble gas before element |
| Orbital Diagrams | Show how electrons (↑ or ↓) are distributed within orbitals. Each orbital can hold a maximum of 2 electrons. |
| Aufbau Principle | Each electron occupies the lowest energy orbital available |
| Hund's Rule | When several orbitals are available, electrons enter singly with parallel spins |
| Valence Electrons | Electrons found in outer energy level (max of 8 valence electrons). |
| Period | Horizontal rows on the periodic table. Elements in the same period have the same number of occupied electron shells/levels. |
| Group | Vertical columns on the periodic table. Elements in the same group have the same number of valence electrons. |
| Group 1 | Alkali Metals |
| Group 2 | Alkaline Earth Metals |
| Group 3-12 | Transition Metals |
| Group 17 | Halogens |
| Group 18 | Noble Gases |
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