Quantum Physics – Flashcards
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| According to the Quantum Mechanics model of the atom, the electron is... |
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| A 3-dimensional wave surrounding the nucleus of an atom. The electrons are in fixed energy states and can move about the nucleus without radiating away their energy. |
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| Principle Quantum Number (n) |
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| Indicates the average distance that an electron is located from the nucleus of the atom. |
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| What is the maximum number of electrons possible in any given energy level where n=the energy level equal to? |
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| 2n^2 |
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| Orbital Quantum Number (l) |
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| Indiactes the shape of the path in which electrons move. These paths are called sublevels. |
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| Where are electrons placed in a given energy sublevel? |
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| The lowest energy sublevel first. |
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| Magnetic Quantum Number (ml) |
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| Indicates the direction and space of the path of a pair of electrons. This direction is called an orbital. |
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| Orbital |
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| A three-dimensional space about the nucleus in which electrons of a given energy are likely to be found. |
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| The maximum number of orbitals in a given energy level is equal to... |
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| n^2 |
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| Spin Quantum Number (ms) |
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| Indicates the spin or rotation of the electron on its axis. |
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| Pauli's Exculsion Principle |
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| States that no more than two electrons can occupy the same orbital in an atom and these two electrons must have opposite spins. |
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| Electron Pair |
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| Two electrons in the same orbital with opposite spins. |
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| Valence Electrons |
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| The electrons in the outermost energy level of the atom. |
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| What is the most important part of the electron configuration? Explain. |
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| The valence electrons are the most important part of the electron configuration. The number and arrangement of the valence electrons determine the chemical properties of an element. |
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| Kernel |
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| The entire electron configuration excluding the valence electrons. |
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| Ground State |
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| The lowest energy state of an atom. The atom's most stable state. |
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| Spectroscopy |
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| The method of studying substances that are exposed to some sort of continous exciting energy. |
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| What causes the bright light spectrum? |
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| If an outside force causes an electron to change orbitals, energy is either given off or absorbed by definate units called Quanta. This change produces the bright light spectrum of the substance. |
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| What is true about spectrums of different substances? |
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| Each is unique. |
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| What is found through studying the spectrum? |
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| The energy diagram for the location of the electrons. |
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| Spectrum |
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| A unique set of wave-lengths absorbed by a substance. |
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| Hund's Rule |
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| When placing electrons in a sublevel that has more than one orbital, one electron of the same spin is placed in each orbital before doubling up. |
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| Aufbau Principle |
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| Electrons are placed one at a time in the lowest energy position. |
