Term
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Definition
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Term
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Definition
| The state when all electrons of an atom are in the lowest possible energy levels |
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Definition
| when an electron jumps to a higher energy level, it is in its.... |
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Definition
| the probability map for the hydrogen electron |
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| Heisenberg Uncertainty Principle |
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Definition
| impossible to know both the velocity and position of an electron at the same time |
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| Pauli exclusion principle |
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Definition
| an atomic orbital can hold a maximum of two electrons, and those two electrons must have opposite spins |
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| Scientific contribution of Planck? |
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Definition
| Energy is emitte in small, specific amounts called quanta. |
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Definition
| minimum amount of energy change |
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| Contribution of Einstein? |
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Definition
| Light has properties of both waves & particles - "wave-particle duality" |
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Term
| Contribution of de Broglie? |
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Definition
| Electrons exhibit wave properties |
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Term
| Contribution of Schrodinger? |
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Definition
| used mathematical equations to describe the location and energy level of an electron. He developed the quantum mechanics model (the widely accepted atomic model today) |
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Term
| Principal quantum number? What does it tell? |
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Definition
| 1. energy level 2. size of the orbital 3. # of orbitals in the energy level |
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Term
| What does the magnetic quantum number tell? |
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Definition
| 1. orientation of orbital 2. the exact orbital within each sublevel |
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Term
| What does the Angular Momentum Quantum Number tell? |
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Definition
| 1. energy sublevel 2. shape of the orbital |
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Term
| What does the Spin Quantum Number tell? |
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Definition
| 1. electron spin (-1/2 or +1/2) |
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Term
| How many electrons can an orbital hold? What must these electrons do? |
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Definition
| can hold 2. must spin in opposite directions |
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Term
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Definition
| electrons fill the lowest energy orbitals first; you have to fill them in order. you cannot jump to higher ones. |
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| How many electrons can each energy level hold? |
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Definition
| 1st - 2 electrons. 2nd - 8 electrons. 3rd - 18 electrons. 4th - 32 electrons. |
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Term
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Definition
| within a sublevel, place one electron per orbital before pairing them |
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| Difference between valence and core electrons? |
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Definition
| Valence - on the outermost energy levels. Core - innermost energy levels. |
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Term
| Difference between cation and anion? |
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Definition
| Cations are positive. Lose electrons. Are smaller. Anions are negative. Gain electrons. Are larger. |
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Term
| How does Bohr's model of the atom explain the line emission spectrum of hydrogen? |
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Definition
| Electrons exist only in orbits w/ specific amounts of energy called energy levels, therefore... 1. electrons can only gain or lose certain amts of energy --> only certain photons are produced |
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Term
| Characteristics of metals? |
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Definition
| hard, good conductors of heat & electricity, found on the left side of the P table, high density, malleable, reflect light, high melting point |
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| Characteristics of nonmetals? |
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Definition
| can be gases, bad conuctors of electricity, low density, non-malleable |
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| Characteristics of metalloids? Name a widely-used element that is a metalloid? |
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Definition
| characteristics of both i.e. Silicon |
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Term
| What is unique about halogens? |
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Definition
| Only family of elements that exist in all 3 states |
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| What is unique about noble gases? |
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Definition
| stable, do not form compounds, octet |
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Term
| Alkali metals are the most what? |
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Definition
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Term
| On the P table, Atomic radius (size of the atom) increases...? |
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Definition
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Term
| First ionization energy is? |
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Definition
| energy required to remove one electron from a neutral atom |
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Term
| Why are atoms larger when going down on the P table? |
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Definition
| 1. higher energy levels have larger orbitals 2. shielding - core electrons block the attraction b/w the nucleus and the valence electron |
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Term
| On the P table, first ionization energy increases...? |
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Definition
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Term
| On the P table, melting/boiling point is highest where? |
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Definition
| Highest in the middle of a period |
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Term
| On the P table, periods are...? Groups are...? |
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Definition
| periods=rows. groups=columns. |
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Term
| Why are atoms smaller to the right? |
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Definition
| Increased nuclear charge w/o additional shielding pulls electrons in tighter |
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Term
| Why are copper and chromium exceptions to electron configuration? |
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Definition
| Cu and Cr are able to obtain a more stable electron configuration when they take an electron from the 4s and add it to 3d. When it does this it becomes either a half full shell (Cr) or a full one (Cu) this results in a more stable compound with lower energy. |
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