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18 Cards in this Set
- Front
- Back
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electron configuration
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describes the arrangement of electrons in an atom
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valence electrons
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the outermost shell electrons, involved in chemical reactions
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quantum mechanical atom
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-developed Bohr's model into a model where electrons are in specific locations. Wave properties of electrons conflict with specific location.
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Schrodinger
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-developed an equation that took wave-particle duality into account.
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Schrodinger's equation
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determines the probability of finding an electron in a specific region in space. Uses quantum numbers to predict energy.
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types of quantum numbers
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principle energy levels (n=1,2,3...)
sublevels defining wave function (s, p, d, f) atomic orbitals defining position in space spin, -1/2 or +1/2 (paired in an orbital) |
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Schrodinger's cat
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our measurement of a particle depends on our intention, not an inherent property of the particle
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principle energy level
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n= 1, 2, 3...
the larger n is, the higher the energy level and farther away from the nucleus. |
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What is the electron capacity of a principle energy level
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2(n)^2
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sublevel
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number of sublevels equal to n
a set of energy equal orbitals within a principle energy level. Subshells increase in energy (s<p<d<f) |
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orbital
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a specific region of a sublevel containing a maximum of 2 electrons. Named by sublevel and principle energy level (1s, 2s, 3s, 2p, etc.)
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orbital shapes
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s is spherical
p is dumbbell d is clover shaped f is a flower, going 3 dimensions |
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subshells and the number of their orbitals
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s, 1 orbital
p, 3 orbitals d, 5 orbitals f, 7 orbitals |
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electron configuration
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the arrangement of electrons in atomic orbitals
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Aufbau principle
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"building up" principle. Electrons fill the lowest level first.
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Pauli Exclusion principle
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no two electrons can have the same 4 quantum numbers in an orbital. Two electrons must have the opposite spin from each other.
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Hund's rule
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each orbital in a subshell is filled half way before it is filled all the way.
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Rules for writing electron configurations
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-obtain the total number of electrons in an atom from the atomic number.
-electrons in atoms occupy the lowest energy orbitals first -each principle energy level n contains only n sublevels -the s sublevel has 1 orbital, p has 3, d has 5, f has 7 -no more than 2 electrons per orbital |
