Periodic Properties of the Elements (Test 3)
Quiz yourself by thinking what should be in
each of the black spaces below before clicking
on it to display the answer.
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| Aufbau procedure | "building up"; adding electrons to one subshell until it's full before moving to the next subshell
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| Pauli Exclusion Principle | a max of 2 electrons per orbital as long as they have opposite spin; no two electrons in an atom can have the same four quantum numbers
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| Hund's Rule | parallel before paired; when filling degenerate orbitals, electrons occupy them singly (one at a time) with parallel spin before pairing up
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| ground state | the lowest energy state
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| excited state | not the lowest energy state
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| degenerate | equal in energy
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| node | a region in space where there is zero probability of finding an electron
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| shell | n (1, 2, 3, ...)
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| subshell | n & l (1s, 2s, 2p, ...)
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| Where is the "s" block found? | the left side
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| Where is the "p" block found? | the right side
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| Where is the "d" block found? | the middle
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| Where is the "f" block found? | the bottom
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| The s block starts with what? | 1s
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| The p block starts with what? | 2p
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| The d block starts with what? | 3d
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| The f block starts with what? | 4f
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| Special electron configurations occur when what are involved? | 1. filled outermost subshells
2. half-filled subshells
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| Which electrons are removed in cations? | the electrons from the outermost shell (which is not necessarily the outermost subshell)
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| isoelectronic | having the same electron configuration
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| paramagnetic | attracted into a magnetic field; having unpaired electrons
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| diamagnetic | slightly repelled by a magnetic field; having all electrons paired
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| valence electrons | outer shell electrons
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| core electrons | inner shell electrons
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| For abbreviated electron configurations... | Put the proceeding noble gas symbol in brackets before writing the valence electrons
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| shielding | the ability of other electrons, especially inner core electrons, to decrease the nuclear attraction for an outer electron
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| effective nuclear charge | the nuclear charge that an electron experiences
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| atomic size trend | increases toward the lower left and decreases toward the upper right
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| ionization energy trend | increases toward the upper right and decreases toward the lower left
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| What is the relationship in size between a cation and its parent atom? | smaller than their parent atom
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| What is the relationship in size between an anion and its parent atom? | larger than their parent atom
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| In an isoelectronic series, what is the trend in size? | size decreases with increasing nuclear charge
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| ionization energy | the energy required to remove an electron from a gaseous atom or ion
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| What are the exceptions in ionization energy? | 1. between column 2 and 13 because it is easier to remove the higher energy p electron than the lower energy s electron.
2. between column 15 and 16 because column 15 has a half-filled subshell
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| When does a "huge jump" occur in ionization energies? | when an inner core electron is removed
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| electron affinity | the energy change (delta E) the occurs when an electron is added to a gaseous atom; some negative and some positive
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| The more electronegative the element, | the more the atom "wants" the electron
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| What groups have positive or near-positive electron affinities? | Groups 2 and 18
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| What group has the most negative/most exothermic electron affinities? | Group 17 (halogens)
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| What do you use to make individual predictions? | electron configuration and nuclear charge
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