Chapter 6 - Electron Configuration and Periodic Trends

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Chemistry

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16 Terms

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principle number (n)

describes the shell, starts closest to the nucleus, when the number increases the shell’s energy increases

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angular momentum (L)

a subshell describing the shape (s, p, d, etc)

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magnetic quantum number (mL)

which subshell the electron is in

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spin quantum number (ms)

which direction the electron spins

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angular momentum = 0

the s subshell

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angular momentum = 1

the p subshell

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angular momentum = 2

d subshell

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electron configuration

describes the shell number, subshell, and orbitals

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pauli exclusion principle

states no electron can have the same “address”

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aufbau principle

states electrons fill subshells from lowest to highest energy level

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orbital diagram

visual representation of electron configuration, each box is one orbital, each arrow is an electron, where the arrow points is ms

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hund’s rule

states that electrons spread out when possible

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core electrons

electrons in the inner shells

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atomic size trends

size decreases across periods, size increases down rows

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atomic radii trends

when there are more protons than electrons the electrons are held more tightly

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electron affinity

energy change needed from an electron to form an ion